SOLUTIONS in 1 Shot: All Concepts & PYQs Covered | JEE Main & Advanced

Good evening, party of children. Good evening. How are you, brother? Welcome back to the Manzil series. You have completed many chapters. Some chapters have been done in Physics. Some chapters have been done in Maths, and some chapters have been done in Chemistry as well. And I think whoever is revising seriously, all these chapters must be getting completed. The biggest reason for this is that along with theoretical discussions, we are also trying to cover all the PYQs related to those topics here. Because of this, the child only needs to revise a little bit of PYQs and a few things at home, and their chapter will be ready. So my suggestion is, brothers, everyone should follow this series very wisely and very seriously. You can do it according to whatever you need to do. You can do it according to yourself. You don't need to practice too much on topics that you find easy. But there are some chapters or topics that will require a little concentration. So practice questions on those topics, and the best way at this time is to solve the PYQs asked in JEE in the last four to five years. The reason is one. NTA is very predictable. There is a lot of truth in this. The reason for that is very clear. Many children say, "Sir, why do you say that?" It's possible something new might come. Look, novelty comes every year. It's not that novelty doesn't come at all. And novelty comes in things. Earlier, they used to ask about a person's osmotic pressure. Sometimes it happens that they ask about osmotic pressure by combining two solutes. So, you will see some novelty, but it will be such that you will understand by looking at the question. But something like, "Sir, he will do something very difficult." The chances of that are negligible because to make it difficult, he has another exam that is asked after clearing Mains, which you call JEE Advanced. Therefore, start preparing with great peace of mind, with your own satisfaction, by taking the name of the Almighty, and your PYQs will help a lot in this. Well done. So, I think many children have joined. Ah, many children have joined. Uh, alright, brother, tell me quickly, can you hear my voice? Can you see me? Can you see and hear me? If so, then give a thumbs up or make hearts or drop goats, whatever your heart desires. Let's start the work quickly. And then we will start today's class. First of all, with concentration terms, which are a major part of solutions, and after that, we will discuss vapor pressures of solutions and colligative properties. The chapter is not very big, so we won't take too much time because the questions will be endless. You can do as many questions as you want, and I have also brought many questions. But many of these questions will be given to you to do. You can do this work from its PDF. Clear? Many children can also take classes through Pi. Pi app is available on Android phones, you can use this app. You will find it there as well, and also, the good news is that the first test of Manzil is also coming up, and if you look closely at this test, you will only be able to take this test first when you are on this app, and you will also find the description of the batch below this YouTube lecture. You can take the batch from there and give the test from there, and the date of the test will be announced. I think you will get all the information about the first test date. Clear? Uh, the first test will be on 30th November. So, the first test will be on November 30th. So, those who are preparing, their purpose will be solved only when they give the test. So, definitely give one test. As far as the duration of this lecture is concerned, it's not a very long lecture, I think it should run for about 7 hours, then we'll see if it's a little more or less. As such, I cannot tell exactly, it depends on how involved you are. The more involved you are, the more you will feel like telling those things. Clear? Alright, so shall we start, brother? Many, yes, intentions are good. A child is asking, what are the intentions? The intentions are very good, friend. The intentions are very good. Will Manzil be sufficient? Well, now, now, asking questions like this doesn't make any sense, brother. You tell me, if I say Manzil will not be sufficient, then what will you do now? Alright, fine. If Manzil is not sufficient, then what will you do now? "Sir, I will study." Oh, then that's a very good option. Then you have to study, brother. So, you have to study. At least take an idea from this series about what you need to do. You have to study at this time. It doesn't matter whether you do Manzil or attend classes from the Manzil series or not. But if you are not studying at all, then selection will definitely not happen. Percentile will not come at all. Therefore, my suggestion is that for those children who are coming for revision or for those children who are thinking that now I have less time. Now I have to read this chapter once to see what the entire chapter is, and then practice questions on it. Then this Manzil will be most beneficial for them. Okay? Alright, so let's start, brother. Uh, let's start the work. Very good. Alright, sir, you start once. The first discussion we need to have is about concentration terms within solutions. So, first of all, I need to have an idea of what solutions are called. Brother, please tell me quickly. Can you hear my voice? Is it okay? Can you see me? And if everything is good, then quickly drop some goats and we'll start the class. Quickly, there's no time at all. Let's start quickly. Can you hear my voice and can you see me? Please tell me both these things quickly. Whether you understand or not, that's your problem. From our side, these things are clear. Alright, tell me quickly. Well done. Yes. An English line. Yes, an English line. Very good. The voice is coming, yes sir. Very good. So, it means everyone's voice is clear, and they can hear. Everyone is writing "All clear." Alright, very good. So, we will start. So, now we will start. Now, now, my suggestion is that we should start the chat only when we have some discussion. So, now, okay. Very good. Let's all prepare with full enthusiasm. So, let's start with enthusiasm. Let's try to understand solutions first. What are solutions actually? The duration, as I mentioned earlier, I think it should be around 7 hours. It can be less, it can be more. That depends because the chapter is simple. It's not very technical. So, practicing questions will be mainly important for us. Right? So, let's start. Shall we start, brother? Alright, so let's start. First, let's talk about solutions. What are these solutions? So, I think everyone will agree with this, and at this level, it doesn't seem wise to talk too much about this: something that is a homogeneous mixture of two or more non-reacting substances. That is, when you mix two or more non-reacting substances homogeneously, a system is formed which you call a solution. Some people always have a thought in their mind. Will a solution always be liquid? Will it be in liquid phase? Like, if you mix Rooh Afza with water, a liquid solution is formed. See, your thinking is not wrong. Because mainly, this is the first thing that comes to mind. Solution means something that is in liquid phase. Whereas this is not the case. A solution can be solid, a solution can be liquid, a solution can be gas. I will talk about this later. But actually, the definition does not contain solid, liquid, or gas. The definition only states that when two or more components mix with each other homogeneously, the system formed is called a solution. Now the question arises, sir, what is called homogeneous? So, I think it's very easy to talk about homogeneous. Homogeneous means uniform throughout, meaning the entire system should appear the same to you. That is, everything should be exactly the same, and we discussed this in the last class when we were talking about mixtures. Mixtures were homogeneous, and mixtures were heterogeneous. That is, a system in which components are dissolved homogeneously is known as a solution. Just like it appears here. Here, the solute is mixed completely uniformly within the solvent. So, this is homogeneous. But if you dissolve soil in water, or dissolve sand, or dissolve iron powder, then after some time, the soil will settle down. Sand will settle down. The upper part will be something else. The environment at the bottom will be something else. Sir, such a system will be considered a heterogeneous system, and heterogeneous systems are not solutions. That is, one thing is very clear about a solution, which is very clear, is that if you take a homogeneous mixture of two or more components, you call it a solution. Clear? Alright, sir, let's quickly move to the next point. The next point is, sir, how can you define solutions in terms of their number of components or constituents? So, it's very simple. All children will understand this: if two components are taken, meaning if my solution has two components. Tell me quickly, if there are two components in a solution, what will that solution be called? Sir, that solution will be called a binary solution. That solution is a binary solution. Similarly, if I have three components, then sir, it will be called a ternary component solution. If there are components, then you will call it a ternary solution. Similarly, if there are four components, then quaternary, and so on, and so on, and so on. That is, what it means is that solutions can also be defined in this respect, where how many components you bring will decide its name. So, if there are two components, call it binary. Actually, in our syllabus, we have binary solutions. So, generally, the discussion we need to have is related to this binary solution. But still, we should have an idea that when there are two components, there will be something and something else, and by mixing both, a homogeneous system will be formed. So, such a system will be called a homogeneous solution, which has two components, hence it will be named a binary solution. Clear? Understood? Okay? Alright, sir, let's talk further. The second important part is this. Now I am going to distinguish solutions based on the nature of the solute and the nature of the solvent. That is, sir, a solution can be solid, it can be liquid, it can be gaseous. But before that, first of all, I decide that if I am mixing two components, one is known as solute, and the other is known as solvent. This absolutely does not mean that sir, the solvent will always be liquid and the solute will always be a stone. As it comes to mind that solute means a solid thing and solvent means a liquid thing. So, by dissolving the solute in the solvent, a liquid solution is prepared. Now, solute and solvent can be anything. By mixing solute and solvent, if a homogeneous system is formed, you will call it a solution. Solute can be anything among solid, liquid, or gas. Solvent can be anything among solid, liquid, or gas. By mixing them, if a homogeneous system is formed, it will be called a solution, and that solution can also be anything among solid, liquid, or gas. Tell me quickly, is this clear? Is this clear to everyone? Because I am emphasizing this point a little because I have this doubt. I always had this doubt. Whenever I think of a solution, I think of a solution, meaning a liquid-like system in which a solid solute is dissolved in water. That is, what is the image of a solution in my mind? That the solute will always be like a stone, and the solvent will always be like a liquid, and by mixing them, a liquid-like system will be formed, which will be called a solution. But this is wrong, brother. A solution is a homogeneous system formed by mixing solute and solvent. Solute can be anything among solid, liquid, or gas. Solvent can be anything among solid, liquid, or gas. And the system formed by mixing them can also be anything among solid, liquid, or gas. Is it clear up to here? Well done. Absolutely correct. So, sir, please tell me once, when solute and solvent can be anything, how are solute and solvent distinguished? If I give you any solution and ask you, "Brother, tell me, which is the solute here? And which is the solvent?" How will you distinguish it? So, there are set rules for this. The most important rule, which I think is the most important rule, is that the phase of the solution is decided by the solvent. That is, the phase of the solvent and the phase of the solution will be the same. End of story. That is, what it means is, whatever the phase of the solvent is, the solution formed will also be of the same phase. If the solvent is liquid, then the solution will also be liquid. If the solvent is solid, then the solution will also be solid. If the solvent is gas, then the solution will also be gas. End of story. That is, what is the first point to distinguish between solute and solvent? The solvent is the entity that decides the phase or state of the solution. That is, the solvent is the one that decides the state or phase of the solution. Okay? Suppose, sir, this happens that the states of both entities are the same. Solid, solid, and the solution formed will also be solid. So, if the solute is also solid and the solvent is also solid, then how will you decide which is the solute and which is the solvent? Because, see, one thing is clear: if you dissolve sugar in water, you all know that a very tasty sherbet will be formed. But sir, the state of the sherbet is liquid. This means that if a liquid solution is formed by dissolving sugar and water, then the liquid phase among sugar and water is the solvent. Because if the phase of the solution is liquid, then the solvent must be the one that is in the liquid phase. That is, who is the solvent between sugar and water? Water. What is sugar? Solute. Okay? But sir, if you think that both were water, both were liquid, and by mixing both liquids, a liquid is formed, then whom would you call the solvent? Sir, this is also liquid. This is also liquid. Now, their phases are the same. Sir, in such a case, how will you decide who is the solvent? So, the second criterion has been made to decide this. The one that is in larger quantity will be the solvent, and the one that is in smaller quantity will be the solute. That is, the one with more amount is the solvent, and the one with less amount is the solute. Is it clear up to here? Has everyone understood this point? Because things are going to change gradually. That is, the one with the larger amount will be the solvent, and the one with the lesser amount will be our solute. Sir, it's also possible that the amounts of both are the same. What will you do now, sir? It's a big problem. Sir, the first thing, the deciding factor will be the phase or the state of the solution, which will be decided by the state of the solvent. That is, the solvent is the one that decides the state of the solution. Clear? If you can, the answer has come. But if you cannot, when can you not? Sir? When the phases of both entities are the same. Now, if both the solute and solvent components are of the same phase, then how will you decide which one is the solute and which one is the solvent? Then the criterion will be larger or lesser amount. Larger amount is solvent, lesser amount is solute. Sir, suppose both amounts are also the same. What will you do, sir? This is the last case, sir. If the amounts are also the same, then in such a case, the one with more moles is the solvent, and the one with fewer moles is the solute. The one with more moles will be the one with a lower molecular weight. Because if you take the same amount of both, then the one with the lower molecular weight will have more moles, and it will be considered the solvent. Tell me quickly, have you understood this point? Has this point been understood by everyone? Because a small objective question can be made on this in JEE and NEET papers. I have brought two-three diagrams according to my understanding. JEE or 2027 papers might have such a discussion with you. Therefore, you should understand this point. Clear? Well done. Alright, sir, let's quickly review. Quickly. Identify the solvent. Quickly tell me the answer, brother. Who is the solvent? And who is the solute? Sir, it's very clear, sir. You have added Rooh Afza to water. So, sir, this Rooh Afza solution has been prepared. Sir, sherbet has been prepared. The phase of the sherbet is liquid, sir. And in both, the whole world knows, sir, sugar is of solid phase, sir. This is solid. And this water is of liquid phase. And if water is of liquid phase, and along with that, the solution is also of liquid phase. So, there is no doubt, sir. The solvent is the one that decides the state or phase of the solution. If this solution is liquid, then sir, the one that is liquid among these two is our solvent. That is, I have no objection in saying that this is my solvent, and if this is the solvent, then sugar is my solute. Very good. Well done. All children are giving the correct answer. Very good. But sir, this is when you can decide very clearly. But it's also possible, sir, that the situation gets stuck. We said, how? Look here, sir. Sir, this is a solution, which is liquid. Very good, sir. This solution is liquid. So, sir, obviously the solvent will also be liquid. Oh, look here, liquid. Oh, but this is also liquid. And if both are liquid, then how will you decide? Sir, you are right. If both are liquid, then the situation will get complicated. And if both are liquid, then how will you decide? So, I just told you, the one that is in lesser amount is the solute, and the one that is in larger amount is the solvent. This means this is my solvent, and this is my solute. Is it okay up to here? Is this clear to everyone? Well done. That is, B is our solvent. A is our solute. But sir, if this happens that the amounts of both are also the same, sir. 10 grams of ethanol. 10 grams.

Sir, water. Now we will mix these two, sir. Ethanol mixes with water, sir. The whole world knows, sir. They enjoy it, sir. Ethanol is being mixed with water. But sir, in this case, the amounts of both are also the same, sir. The states of both are also the same. This is also liquid. This is also liquid. This is also liquid. And the amounts of both are also the same, sir. Now how will you decide? So when the amounts are also the same, the deciding factor is moles, sir. The moles of water are more because its molecular weight is less. Therefore, water became our solvent. And ethanol, whose molar mass is more, its moles are less, it became our solute. Clear? Is it clear? Well done. That means water is our solvent and ethanol is our solute. Okay, brother? Is it clear up to here? Did everyone understand this? Okay. Let's talk more. Let's come to the next point. That is, I have now decided what you are calling solute and what you are calling solvent. So sir, solute and solvent have been decided. We now come to the next point. Sir, I have got an idea about the solution. Okay? Let's talk further, sir. What is the next thing that comes up? The next thing that comes up is, for example, let's take this. The next thing that comes up is, sir, just as you were talking about defining the types of solutions in a new way. I want to discuss a small thing here in the same way, and it is important. It is important. What is inside it? Sir, they are saying that if you talk about gaseous solutions, then what is confirmed in this gaseous solution? Can you tell me by thinking about it? If the solution is gaseous, then one thing is certain. Whether I know anything else or not, I don't know. I know that sir, the solid solute can be solid, liquid, or gas, sir. And the solvent can also be solid, liquid, or gas, sir. But sir, if you have talked about a gaseous solution, then one thing is confirmed. This is certain. This is certain. What is certain? It is certain that the solvent will be gas. The solvent will be gas. Did you understand what I said? Did this point become clear to everyone? Because sir, if you have decided the phase of the solution or told the phase of the solution, then one thing is clear. Our solvent will be gas. Now you see anything, I don't care. But I am sure of one thing. The solvent will be gas everywhere, sir. And sir, the solute can be anything, sir. It can be solid, it can be liquid, and it can be gas. So if it is a solution of gas and gas. For example, sir, you mixed oxygen with nitrogen. Very good, sir. This also became a solution, sir. A solution of liquid and gas, meaning the solute is liquid and our solvent is gas. Sir, for example, you mixed chloroform with nitrogen gas. Solid is mixed with gas. The gas is our solvent and the solid is our solute. It is absolutely possible. If you talk about this, then sir, camphor was mixed with nitrogen. That is, these examples you are taking, these examples, in my opinion, we should remember them. JEE can make objectives on them because they are written exactly like this in NCERT. Therefore, my suggestion is that all of you should definitely remember these examples. Theoretically, if thought about, the main point coming in this is that our solvent is gas, and our solute can be anything from gas, liquid, and solid. Is it clear? Did you understand? Okay, this? Shall we proceed? So let's talk about the next point, sir. Next, if I talk about a liquid solution, then if you talk about a liquid solution, then sir, this is certain. What is certain this time, sir? This is certain. That if the solution is liquid, then the solvent will be liquid. The solvent will be liquid. Did you understand the point? If the solvent is liquid, then you, and you have to remember these examples. Which examples were taken? It is clearly visible here that sir, if the solvent is liquid everywhere. Look here, our solvent is liquid everywhere. So if the solvent is liquid everywhere, then in such a case, the solution will definitely be of liquid phase. Is it clear? So, for example, gas is being dissolved in liquid. So if you are dissolving gas in liquid, like oxygen dissolved in water. This solution that has been prepared is a homogeneous system in which oxygen is the solute and our solvent is liquid water. Similarly, liquid and liquid were mixed. As you did just now. Ethanol was dissolved in water. Sir, in this case, this is a solution that has been prepared by mixing liquid and liquid. Solid in liquid, this is very common, sir. Solid in liquid, like sugar dissolved in water, salt dissolved in water, glucose dissolved in water. Sir, this will be a solution in which liquid must be the solvent. The solute can be anything from these. Their examples can be seen. Next, if we talk, then sir, solid solution, and in my opinion, this is important. So everyone should pay close attention to the fact that we should know all the examples of solid solutions. So you all will definitely remember this. You must remember this. So if I talk very simply, then one thing is confirmed here too, that if we are talking about a solid solution, then it is certain that your solvent will definitely be solid. My solvent will be solid. This is confirmed. Do you understand this point? That is, it is confirmed that my solvent will definitely be solid. Now let's talk about their examples. If you look carefully, the solvent is solid, sir. And the solute can be anything, sir. The solute can be liquid, gas, or solid. So if I look at the solute carefully, if the solute is gas and it is being dissolved in a solid solvent. It has become very unique, sir. Gas is dissolved in solid. And this is a very common example. When you put hydrogen in palladium. Solution of hydrogen in palladium. A very good example. Everyone should try to remember this. If you are ever asked whether the mixture of hydrogen with palladium is a solution, yes, it is a solution. Why? Because hydrogen is homogeneously distributed within palladium. Secondly, what kind of solution is this? This is a solid solution. In this solid solution, which is the solute and which is the solvent? Here, palladium is the solvent and hydrogen gas is my solute. This is important. This can be asked in exams. It is given in NCERT. Therefore, it is important for boards and also important for us. Is it clear? So I should remember that if I am talking about a solid solution, then in that solid solution, if the gas is the solute and the solvent is solid, then a very good example of it is the dissolution of hydrogen gas in palladium. Secondly, sir, if you take the solute as liquid and the solvent as solid. A very good example of this is amalgam. Amalgam of mercury and sodium, you call it a solution that is a solid solution. That is, if this is a solid solution, then one thing is clear, that my sodium is the solvent. Sodium is my solvent. And mercury, which is liquid, is my solute. That is, amalgam is also a homogeneous system. A mixture that should come under the homogeneous category, and this is a solution known as a solid solution in which the solute is liquid mercury and the solid solvent is sodium. Clear. And the third case that arises is a solution of solid and solid, meaning solid is dissolved in solid. That is solid solid. And in my opinion, the whole world knows this, sir. There are alloys all over the world that are such homogeneous mixtures, sir. They are solid solid, sir. Solution, sir. Remember, copper was mixed with zinc. Copper was mixed with tin. Sir, all these people, impurities were added to gold. Sir, all these alloys that are being prepared, sir, they are all my solid solid solutions, sir. Is it clear? That is, the solute will also be solid and the solvent will also be solid. Is it clear? Tell me quickly, is everything clear up to here? Is everything clear up to here? Shall we proceed, brother? Tell me quickly. Well done. Very good. Brother, as I had told you before. Two-three spammers come to class. Right? But why do those spammers appear separately? They appear separately because their chat is visible. Oh brother, if these people are shown that no, no, there are also people here who are studying, then their chat can also be seen, right? There will be more people who are studying. So why do only they appear? You understand? Because they are okay, right? So anyway, whatever it is, when asked like this, is it clear to you, then make some noise so that the spammers get a little scared. Otherwise, they get blocked anyway. Well, so this point is understood. Is it clear up to here? Let's move on, sir. Now we come to the next point. The next point is concentration terms. That is, I have now decided one thing, what are solutions? What are solutions called? In how many ways were they defined? What are the different ways to define them? How are solute and solvent identified? And what can be the solutes and solvents in the different types of solutions, solid solutions, liquid solutions, gaseous solutions, and how are they identified, we have discussed this. Now we come to concentration terms. Look, I have written this here. Although it is not a very big deal as such. I have just written one thing that the terms we are going to discuss, which I know by the name of concentration terms. These will be the terms we have to discuss. The main concentration terms include molarity, molality, mole fraction, percentage concentration terms, parts concentration terms, and strength, or we will talk a little about formality. That is, in total, if I talk about concentration terms, I have to study these five-six concentration terms. Clear? And these concentration terms are asked a lot. These concentration terms are asked a lot. So if I talk about these concentration terms, the first concentration term we are going to define is molarity. Many children understand this, and many children have an idea of its definition. So, I will not waste much time in writing molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less, so the solvent will also be less and the solute will also be less. Here the solution is more, so the solvent will also be more and the solute will also be more. Sir, only this much difference will be there. But sir, one thing will be common, and that is important for us. If the solution has come out of the same tank, meaning if you have taken a part of any solution, then whether you take it less or more. One thing is confirmed. Its concentration is the same. That is, what it means is that if I take less solution from a large tank or more solution. The amounts of their solutes and solvents can be different. Sir, there will be more solute, somewhere there will be more solvent. Everything is fine, sir. I agree. But one thing will be common, and that is concentration. And I always have to take advantage of this. I will tell you how this can be taken advantage of. Is it clear? So, this means that if I prepare a solution by mixing solute and solvent, then the best thing that comes out of that solution is that no matter how much amount of that solution you take, its concentration will always be constant. That is, the concentration of this solution is the same as the concentration of solution number two. The same concentration as solution number three. And the same concentration as this tank. In terms of concentration, all these are the same. What is the only difference between them? Sir, there is a lot of water here. There is a lot of sugar here too. There is very little water here. There is very little sugar here too. But the concentration here and the concentration here are the same, sir. And that is why I have written one thing here. The concentrations of solutions coming out of the same tank are the same, and this is a very beautiful thing. That is, everyone will first remember this point that if solutions are taken out of the same tank, meaning if different solutions come out of the same tank, then the concentrations of those solutions will be the same. This is the most important thing. Is it clear? This is the most important thing for us. So now I will try to use these concentration terms. And I will define the first concentration term. And that is molarity. The first concentration term is molarity. Okay, this? So, sir, how will molarity be defined, sir? So this is a very simple definition and a very common definition. Many children understand this. So, I will not waste much time in writing the definitions of molarity or their definitions in detail because I have it written. I want to talk about the homogeneous nature first. This is very important for me because I will be using such sentences repeatedly here, which you will have to understand. That is, if we talk very clearly here. You have taken a tank, and in that tank, suppose you have dissolved the solute and prepared a solution. Okay? Now, the special thing about this solution is that no matter how much of this solution you take out. Whether you take this part, or this part, or this portion. That is, whether you take less solution from this tank or more solution. Where will the difference come? Sir, the difference will be that here the solution is less

There will be a benefit. And the children who have seen, the children who know will agree very well that sir, with that one line of English, we can finish the entire concentration terms. That is to say, if you are given the concentration value of molarity, 1.8, then remember how you explain that molarity. Remember this. That is, if I give the molarity value as 1.8 molar, how will this molarity be defined? 1.8 moles of KOH dissolved in 1 liter or 1000 ml solution. What will be the benefit of this? When you define it like this, what will be the benefit? The benefit will be that by writing 1.8 moles of KOH, you will know how many moles of solute there are. And when you write "dissolved in 1 liter solution," you will know what the volume is. Whereas the solution shown to you is kept hidden. You don't know how many moles of KOH are inside it, what the volume of the solute solution is. But you have defined your own solution, whose molarity is what? 1.8. You know everything about your own solution: that there will be 1.8 moles of KOH in my solution, and the volume of that solution will be considered 1 liter or 1000 ml. Is it clear? Did everyone understand up to here? The unit of molarity is written as moles per liter. That is, the most important points discussed here are in front of you: how molarity is explained? What is the formula for molarity? Secondly, since the term of volume comes in molarity, it is temperature-dependent. Thirdly, by multiplying molarity and volume, you can find the moles of solute. Fourthly, if you want to replace the molarity of a solution with your own solution. You want to define your own solution. Of the same molarity, how is this one line of English written to define it? You need to remember this. That is to say, if the molarity is 1.8, that means 1.8 moles of KOH dissolved in 1 liter solution. Clear? Did everyone understand up to here? Now, what is its application? This will be understood gradually. Did this point get understood up to here? Okay, this? Shall we move forward? Let's come to the next point, sir. What is the next point? The next point is very straightforward. This is a question asked in 2025, and it has been made a very good question. As I told you earlier, molarity is temperature-dependent. That is, as we have seen, molarity, if I look at it from my perspective, what was said about molarity? Molarity is equal to moles of solute. If I write it in my language, it will be moles of solute divided by what? Divided by divided by volume of solution. This is our formula. Volume of solution. That's fine, sir. In what unit should the volume of the solution be taken? Sir, it should be taken in liters. That is, this is the way to define molarity. Okay? From this, one thing is understood: sir, if the volume increases, the molarity should decrease. That's true, sir. If the volume increases, the molarity should decrease, and if the volume of the solution decreases, the molarity should increase. Is it okay up to here? Is this point clear to everyone? Sir, this is absolutely correct, and every child knows that if you increase the volume, because it is in the denominator, your molarity will decrease. And if you decrease the volume of the solution, sir, the molarity will increase. Sir, absolutely correct. Absolutely, absolutely correct. Sir, what does this have to do with temperature? It's very clear. The whole world knows. Normally, with an increase in temperature, the volume increases. That is, if I discuss generally, generally on increasing the temperature, generally speaking, on increasing the temperature, volume increases. Yes, that's right, sir. It seems quite logical that our volume will increase. Sir, with an increase in temperature, there will be expansion, and our volume will increase. This point seems quite logical to me. But sir, please understand this. With an increase in temperature, the volume increases, but with water, there are many problems. Sir, there are many problems with water. So I won't go into this explanation because these explanations are given to you in inorganic chemistry. But the beautiful thing about water is that when water goes from 0 to 4 degrees Celsius. That is, when water converts to water between 0 degrees Celsius and 4 degrees Celsius. The good thing is that in this process, its density increases, and after 4 degrees, its density decreases. That is, the maximum density of water is at 4 degrees Celsius. That is, when water goes beyond this, there is no issue at that time, sir. When it goes beyond this, if you talk about water, sir, in such a situation, its density decreases. That is, what are you trying to say, sir? What I am trying to say is that if the density increases from 0 to 4 degrees Celsius, it means, sir, the volume decreases. Sir, absolutely correct, sir. And if the density decreases, it means the volume increases. Yes, sir. So, it's a big hassle, sir. If you go from zero onwards, then in such a case, if you go from zero to four, your volume is decreasing for water, and above four, your volume is increasing. This is amazing, sir. If that's the case, then sir, the volume of that solution will also be less from zero to four, and because of this, its molarity will increase. But as soon as you go beyond four, sir, the volume of water will start increasing, due to which the molarity will start decreasing. Sir, this is a beautiful question, sir. The expectation was low, but JEE has made a beautiful question at the mains level. That is, if a very good thing is added here, this question is a very good question. It is clearly visible. Sir, its answer should come out as B. Why? Because sir, from zero to 4 degrees, look at 4 degrees. From zero to 4 degrees, molarity is increasing. Why? Because sir, density is increasing. With increasing density, volume is decreasing. And if the volume of the solution decreases, then sir, molarity will increase. That is, up to 4 degrees, it's fine, sir. But what's happening after 4 degrees, sir? After 4 degrees, sir, there's strange misbehavior, sir. After 4 degrees, the density of your water starts decreasing. And if the density of water decreases, its volume starts increasing. And if the volume starts increasing, the molarity starts getting suppressed gradually. Clear? Clear? Yes. A child is saying, sir, teach colligative properties directly. What is all this nonsense? That's true. My friend, when we study colligative properties, if you feel like it, you can come to class then. Join at that time. Leave now. This is all very nonsensical. These are questions for very small minds. They are not at your level. You have your own separate level. Wait for that level. Understand the point. Okay? So, when, uh, now, when a question of this level comes in your exam, then when you are in trouble, you will understand. Clear? So, everyone should understand this. A very good question was made in 2025, and I have great hope that you will see something similar. And it is being observed that the number of questions graphically is continuously increasing. JEE Mains level is starting to make more questions on graphs. So, everyone will keep this in mind. Very interesting, easy. Let's talk more, sir. Let's come to the next point. What is the next point? Sir, let's look at one or two more questions. What kind of questions has JEE asked? Look here, sir. Now, let's talk very directly. Sir, this is a question from some exam in 2024. It is being asked. It says that molarity 3 molar NaOH solution. I have a 3 molar NaOH solution. I want to make an NaOH solution whose molarity is three. Okay? I said, let's make it. If the molarity is three, then I am clear about one thing: sir, this three will be moles of solute, and the solute is NaOH. Moles of solute divided by volume of solution. Sir, this value of three should be equal to this, and this volume will be in liters, sir. Is this clear? Understood? So, if you want to make a three molar solution of NaOH, you will need moles of solute and volume of solution. Now, what is it asking? Which can be prepared from 84 grams of NaOH. We said, oh, this is very easy. Moles of NaOH will be 84 / 40. Remember? To find moles, if the weight of the sample is given, divide by the molar weight. Sir, the molecular weight of NaOH is 40. You divided this by 40, and below comes your volume. And that volume is to be calculated. But this volume will be in liters. Friends, you can calculate the volume from here. You will get the volume in liters, and you need the answer in liters as well. You might not know, that gentleman, sir, teach all those things. These are all very light matters. He might not know. 1 decimeter cube is equal to 1 liter. So, for those who don't know, don't fall for anyone's tricks. All these people who are acting like heroes, their time is about to come very soon. You work wisely. Get selected quietly. Go and study quietly. You should not be concerned with anyone else. These people who talk nonsense, "teach this, teach that," "teach what is not known." Their time is about to come. Because actually, they don't know what is going to be asked in the exam. Clear? So, everyone will solve this quickly. Whatever the answer comes out to be, but whatever the answer comes out to be, it will be in liters. You want to give it in liters. So, our answer will be in liters. Clear? Can you do this? Very good. Many children are solving it and telling the answer. Very good. Let's talk more, sir. Let's talk more, sir. Since you have done this much, do one more question. Let's do one more question quickly, sir. Here you go. Tell me quickly, sir. How to do it? The molarity of an aqueous solution containing. Here you go, sir. This time you want to know the molarity from me, so it means I will use the formula for molarity. If you want to know the molarity from me, which is denoted by capital M, I am writing its formula again. Moles of solute, and which is the solute? NaCl. Moles of solute divided by volume of solution. Clear? Volume of solution. In what unit? In liters. I am writing it repeatedly so that you can also remember it. Clear? Let's go, sir. Sir, now show me how to calculate molarity. How to calculate moles of solute, sir? 5.85 / 58.5. Sir, the molar mass of NaCl is 58.5, and the volume is 500 ml, sir. I know how to convert 500 ml to liters: 500 / 1000. Sir, this is your molarity. You can calculate it. This is one by .5 and that is 0.2 molar. Clear? So, sir, this is very easy. It can be done easily. Well done. Now, I am not talking to those one or two children who are saying yes or no, those who are of a different style. We are not talking to them. Brother, we are small people. Understand the point. We want to know if you can calculate the moles of solute or the volume of the solution or the molar mass of the solute if the question is to find molarity or if molarity is given. Yes or no? I haven't gone deep into molarity yet. Do you understand? The most important thing in this entire 45-minute, 50-minute discussion is the question from 2025, which was made regarding the density of water. Always remember that any kind of question can be asked. The density of water is maximum at 4 degrees Celsius. Between zero and four, its density increases, and after four, it decreases. That is, between zero and four, the volume of water is decreasing. But after four, the volume of water is increasing. That is, initially, molarity will increase, but then it will decrease. Well done. Many children are writing yes. Very good. Okay, this. Let's move forward, sir. Sir, since you have discussed this, let's discuss a little more. Are there questions that will be given to you to solve? Absolutely, as you said yes, your entire test will be taken here. You will have questions, you test, finish, move forward, talk. Let's come to the next point. The next point is that we see discussions related to this as well. Look, all the spammers are gone. Right? Now spammers are gone because they feel that the master is not listening to them. We are writing, end it, end it, and the master is busy ending it. We were trying to end the class. So, actually, I tell you this every time, and I am saying it again. Anywhere, whether it is a class or an exam, you will always find two types of people. One is those who have come to give the exam for fun, but they will scare you in every way. When you sit in the examination center, at that time, every other child besides you seems more intelligent than you. I don't know if you have ever felt this or not. If you have, then write yes. Sir, whenever I sit in an examination center, I don't know why, but every boy I see, and I am talking about those who are new to you. Have you ever taken an exam where everyone is new? Brother, you know the children from your school. Oh, this is a good-for-nothing. This one will seem a bit intelligent to me. But have you ever had an exam where you are sitting in a group of people you don't know and who don't know you? In such a situation, every child will seem more intelligent than you. So, in such a situation, sir, every child who seems more intelligent than you is just demotivating you, troubling you. Understand, you will find some people reading books, some people will be understanding something in their minds, revising something. You will feel, man, I haven't studied anything, man. Look at them. They are revising even now. They are revising something even now. They are murmuring, murmuring, discussing among themselves. Hey, what are you getting into, man? Nothing will happen to such people. Nothing will happen. I'll tell you the reason. The exam is very clear. This is the biggest reason. If there was any hassle in this exam, any chaos, I am not talking about JEE Mains. I am talking about both JEE Mains and JEE Advanced. These two exams are very clean exams. Even if I talk about NEET. This NEET exam or JEE exams are very clean exams. Unnecessarily, if you think something and want to do something wrong, create some chaos, nothing will happen from this. Nothing happens from this. Do you understand? The points are very clear. The child who studies these clear points and solves 10-10 questions will be able to do their paper. Nothing else needs to be done. Now, for example, about molarity, sir, I have learned two or four things. This is molarity. If a question related to this comes, I will be able to do it. I will practice four questions and throw it away. It's over. Sir, will I solve 50 questions? No need. Now let's talk about the second thing. Sir, can there be questions where when I bring two solutions and any solution and dilute it by adding solvent? I said, yes, I have done this many times. When making a sharbat solution of Rooh Afza at home, sometimes the sharbat becomes very sweet. So, in such a situation, my family members tell me, brother, this is too sweet. Add a little water to it. So, its sweetness decreases. Its sweetness decreases by adding water. That sweetness is molarity. That sweetness is concentration. That is, you are reducing the concentration of that Rooh Afza solution by adding water. But you are not changing one thing. You cannot change one thing, sir. There is another way to reduce its sweetness. Take out the Rooh Afza from it. Sir, I cannot do that, sir. Rooh Afza is dissolved, sir. Now I cannot take out Rooh Afza. Oh, why? Your glass is full, spill half the glass. Sir, that won't make a difference either. Even if half the glass is spilled, the remaining half glass will be as sweet as the whole glass, sir. This is the specialty of solutions, sir. Taste one spoon of Rooh Afza, taste one sip, or drink the whole glass, the sweetness feels the same, sir. The concentrations remain constant throughout because the system is homogeneous. So, in such a situation, if you want to reduce its sweetness, you have only one way, and that is to add water. You can reduce its sweetness by adding water to it. Is everyone understanding my point? What does this mean, sir? This means, sir, that adding water changes the concentration. But adding water does not change Rooh Afza. And here is the key concept that I need to use during dilution. That is, whenever any solution is diluted, the key concept used in it is this: Rooh Afza remains the same. That is, the moles of solute will not change. As much solute is here, that much solute will be here. You will all agree with this. Sir, to reduce the sweetness of the Rooh Afza solution, when I add water to it, sir, Rooh Afza does not decrease, sir. Whatever Rooh Afza was dissolved earlier, one spoon, it will remain one spoon later, sir. But with the increase of water, the concentration decreases. The sweetness decreases, sir. Clear? That is, whenever any solution is diluted, only one key concept is used at that time. The number of moles of solute remains constant. So, as many solutes are here, as much Rooh Afza is here, that much Rooh Afza is here. How were the moles of solute calculated? As I marked it as important earlier. Sir, to calculate the moles of solute, molarity and volume are cross-multiplied. That is, if I multiply the molarity here and the volume here, I will get the moles of Rooh Afza here. If I cross-multiply the molarity here and the volume here, I will get the moles of Rooh Afza from there. And the key concept says that the moles of Rooh Afza will remain equal. So, by equating with m1v1 m2v2, you can calculate the molarity of the new Rooh Afza solution. That is, one thing is.

It is clear that during dilution, molarity decreases because v2 is always greater than v1. This is because adding water increases the new volume. This means if v2 is greater than v1, then m2 will always come out to be smaller than m1. Is that clear? Yes, Varun Kumar has given an idea that if you want to reduce the sweetness of Rooh Afza, you can add a little salt to it. Absolutely, Varun, you can do this. You can absolutely do it. You can add something else to it. Do you understand what I'm saying? If you want to reduce its sweetness, instead of spending on salt, you might feel bad about adding water to it. You might feel bad. "Sir, what is this? Sir, why are you adding water? We will add salt." So you can add salt. Whatever you feel like. Is this clear? Is it clear? Is everyone understanding this point? Let's talk about the second thing. This means that for me, any questions about dilution, JEE has asked them, in fact. But I have understood the key concept behind them. And there is only one key concept. What is the key concept? During dilution, the moles of Rooh Afza remain the same. That's it. This is our key concept. Is it clear? Let's talk about the second thing. Sir, just as you talked about dilution. The second very important thing is how to calculate molarity when mixing two solutions? Sir, what is the key concept behind this? So let's think. One Rooh Afza solution is sweeter, and another Rooh Afza solution is less sweet. This means one sherbet is sweeter, and one sherbet is less sweet. If I mix these two, how will you determine the sweetness of the resulting sherbet? Now, now, forget about chemistry, sir. Use your own intelligence. Think and tell me what key concept should be used behind this? There is one Rooh Afza solution which is less sweet, and one is sweeter. We mix both. Sir, listen to one thing. From here and from here, when we mix both, sir, all the solute here, Rooh Afza, and the Rooh Afza here, sir. Both will combine to be equal to the Rooh Afza here. What does that mean? What is the key concept? Sir, the key concept is that when two solutions are mixed, the total moles of solute are equal to the sum of the individual total moles. And this is the key concept. Did everyone understand me? This means that the solute here and the solute here, both will combine and fall here. This means if this is an HCl solution, and this is also an HCl solution. Then this HCl solution that is prepared. The moles of HCl here will be equal to the moles of HCl here and the moles of HCl here. Is it clear? Did you understand? Is everyone understanding this point? This means if I try to calculate molarity during mixing, the way to calculate molarity is to add the moles of solute from both places. Those moles of solute will be equal to the moles of solute here. Now, tell me, how many moles of solute are here? m1v1. How many moles of solute are here? m2v2. Remember? Molarity multiplied by volume gives the moles of solute. And how many will be here, sir? There will be m net, whatever the net molarity will be, multiplied by the volume. And what will be the volume? v1 is coming from here. v2 is coming from here. So what will be the total volume? v1 + v2. This means the net moles of solute here are m net * v1 + v2. And the net moles here are m1v1 + m2v2. If I add these things, I will get m net from it. And that is m1v1 + m2v2 / v1 + v2. This means that whenever concentration needs to be calculated during mixing, it can be calculated from this concept. This means when two solutions of the same solute are mixed, the molarity of the resulting solution prepared from their mixing is calculated by m1v1 + m2v2 / v1 + v2. Quickly tell me, is this clear? Is this point clear? Is this clear? Quickly, don't get caught up in others. Don't worry about their comments. Concentrate on your comments. Yes, sir, I have understood that when similar solutions are mixed, m1v1 + m2v2 / v1 + v2 is used to calculate the resultant molarity. Very good. Okay, sir, let's talk a little more about this. Sir, for example, if a question like this comes up, and sir, I don't know if it has been asked in any exam. Look, there is some exam, and in that exam, it has asked that sir, there are two vessels. In one vessel, this NaOH is added, and in another vessel, this NaOH. If I mix both, what is the molarity of the resulting vessel? We said this is a very simple question. This is also NaOH. This is also NaOH. When you mix both, what does the key concept say? The key concept says that the moles of NaOH from both places will combine to be equal to the total moles of NaOH in the new solution. Is it clear? This means how much NaOH will come from here? Sir, how much NaOH will come from here? And anyway, you have just memorized the formula. What have you memorized? M net = m1v1, meaning moles of NaOH coming from one side + m2v2, meaning moles of NaOH coming from the other side, divided by, divided by what will come out, sir? Divided by the total volume, and what is the total volume? v1 + v2. Everything is given in the question. Sir, the value of m1 is two, the volume is 20. I am not taking this in liters because I will take milliliters below as well. If you want to take liters above, then take liters below too. It's the same thing. So this means 20 * 2 + here will come 400 * 0.5, and below will be the total volume. And what will be the total volume? v1 + v2, meaning 20 + 400, meaning 400 + 20. Sir, solve this. You will get the net molarity. And many children are also writing the answer. The answer is coming out to be 57. Okay, whatever it is, whatever comes out after solving, that is 57. So, whatever molarity comes out will be 57. So, solve this now. How much will this be? 40, and how much will come from here? 200. This means 24 / 42. If written more correctly, how much will this be? 6 / 13. This is 6 / 13. So the molarity will come out to be 6 / 13. Uh, point, uh, is it not 6 / 13? Uh, six, no. Uh, this will be how much? 12 / 21. So if you solve 12/21 a little more, it will be 4/7, right? 4 / 7. So 4 / 7 is the answer. So this will be 75, 35, then 577 = 49. So 57 molar. So if you want to write the answer, this is 57 * 10 raised to the power -2. Clear. Well done. 4 / 7. So, so now you understand. Now, for example, I wanted to learn a lot about molarity, I wanted to make a big fuss about it. But I think the good thing I learned about molarity is that molarity is temperature dependent. And it has asked this question many times. I mean, I can't tell you, at least 10 times JEE has asked this question: is molarity temperature dependent or not? I mean, in different forms, which of the four is temperature dependent? Is molarity temperature dependent? It has asked many questions about this in assertion-reason type questions. But this time it has made a good question. What is it? If water is our solvent, then the volume of the solution will be decided by water, and the volume of water changes with time and temperature. We said, okay, that's fine. What's new? What's new is that the volume of water decreases from 0 to 4° Celsius and then increases after 4°. So at the time when the volume of water decreases, its molarity increases. So this is a good thing that you should pay attention to. Okay? Alright, sir, let's talk more. And there will be many questions that will be given to you to solve. You can discuss these questions at your leisure. Let's move on to the next concentration term. And the next concentration term is molality. I said, sir, a child is asking, you didn't take the volume in liters. Sir, I told you, friend, look, understand. If you want to take the volume in liters, then take liters. For example, this 20, yes, 20. If you write 20 in liters, it will be 20 / 1000, and if you write 400 in liters, it will be 400 / 1000. So here too, it will be 400 / 1000, and 20 / 1000 will come, right? Above liters, then below liters too. Above milliliters, then below milliliters too. It cancels out. That's why I didn't unnecessarily create the hassle of 1000. Milliliters above, milliliters below, everything is set. Do you understand what I'm saying? Just don't make this mistake. Liters above, milliliters below, or milliliters above, liters below, the game will be over. Keep this in mind. Is it clear? Understood? Okay, let's move on to the next concentration term. And the next concentration term is molality. What does molality say? Molality, sir, is also a way to represent concentration, and it is a very straightforward way. If I want to tell you two or three things about it, then the first thing is that if you talk about the definition, the definition says the amount or moles of solute dissolved in 1 kg of solvent. This means if we only talk about the definition, the definition says moles of solute dissolved in 1 kg, or if you want to write it in grams, and 1000 grams of solvent, meaning however many moles are dissolved in 1 kg of solvent, that is molality. If you want to find its formula, then I can also find its formula. Sir, what is the formula? The formula is molality, which is denoted by small m, equal to moles of solute, and because it is dissolved in 1 kg of solvent. So this is divided by the weight of the solvent. Weight of the solvent. In what unit is it needed, brother? Sir, in kg. This means if you want to find molality, you have to remember this formula. Okay? This means this is a beautiful thing, that sir, if I want to find molality, just like you did some questions for molarity. How is molarity calculated? Similarly, if you talk about molality, then if you want to calculate molality, this is the formula for molality. This means what is needed? Bring me the moles of solute in any way, directly or indirectly, and I will calculate the molality. Also, tell me what is the weight of the solvent? Very important. Very important. Those students who will not even remember that in the definition of molarity, the numerator is moles of solute. Same, but the denominator is the volume of the solution. Here it is the weight of the solvent. Remember the difference between the two. Is it clear? Now, sir, one thing is clear, that if I look at this carefully, then sir, there is no term of volume here. And if there is no term of volume, then there is no doubt about it. Sir, this is temperature independent. Sir, this is temperature independent. This means I will not apply any intelligence here. This is temperature independent. Temperature independent. This means you were asking me two types of questions. First, sir, can you tell me how to find the molarity or molality of this solution? Then I will apply the formula. Second, sir, if I show you molality, that I have a solution with this molality, can you tell me how much solute and how much solvent is in that solution? No, sir, if you hide the solution, I cannot show it, I cannot tell it. But I should be able to define my own solution. Now I want to add something here, which is a very beautiful and important thing, that if, for example, I have any solution, suppose I have this solution about which it is being said that this solution is a solution in which solute has been dissolved, and about this solute, only one thing is said about this solution, that this is 1.2 molal, M O L L, which is called molality. This is 1.2 molal aqueous urea solution. Suppose he told me that I have a hidden solution whose molality is 1.2. So can you tell me how much urea and how much water is in that solution? So what will I answer him? That brother, if you haven't shown me the solution, how do I know if you are holding a lid behind, or if you are holding a glass behind, or if you have hung a bucket behind? I can't see anything. I don't know how much urea is in it, how much water is in it. If you are holding a bucket, then there will be more urea, and more water. If you are holding a lid, then there will be less urea and less water. I don't know what you are hiding behind. Is it clear? But one thing is clear. I will define my own solution. I will fix it. What you are hiding behind, I don't care. But I should be able to define my own solution. If I am given the molality of any solution, then I should be able to define my own solution. And the way to define my solution is 1.2 moles of urea, meaning solute, 1.2 moles of urea dissolved in, dissolved in 1 kg solvent, which is water, because I wrote aqueous. If I hadn't written aqueous, I would have just written solvent. So this means, sir, writing this gives me an advantage. What advantage does it give me? The advantage is that brother, if you have written like this, then your solution is well-defined, that in my solution, the moles of solute are this much. This means what became visible in my solution? Moles of solute. And along with that, what became visible? Weight of solvent. Weight of solvent. This means if someone asks me, brother, what is the weight of the solute and the weight of the solvent in your solution? Then you can only say, brother, look, he has hidden the solution, I don't know about that, but I have defined my own solution: if the molality is given for a urea solution or any solution, then the way to write it is this many moles of solute dissolved in 1 kg solvent. And this will be said in one line of English. This is one line of English. The student who remembers this will benefit greatly. But the one who doesn't remember, it's not that he won't be able to solve the problem. He will still solve the problem, but he will do it in his own way. Therefore, my suggestion is that you should definitely remember this. Just as you remembered the point about molarity. What was the point about molarity? The point about molarity was weight of or moles of solute in 1 liter solution. Similarly, what is the point about molality? This many moles of solute in 1 kg solvent. Is this clear? Yes, a child is asking, sir, why only 1.2 moles? Absolutely, instead of 1.2, it can be 2.4, it can be 2.9, it can be 1.8, something. But accordingly, the water will also change. If you take 1.2 moles of urea, then the water will be 1 kg. That's it. Do you understand what I'm saying? Brother, I have defined my solution. 1.2 moles of urea, 1 kg solvent. Now, if you think, he says, I have 2 kg of solvent, then you can say the urea will also be double. Do you understand what I'm saying? I can't see his solution, so I don't know how much urea and how much water there is. But I have learned to define my own solution: if a solution is 1.2 molal, then this is the way to define it. That's it. The benefit of this will be that at least I will know these two things about my solution. If I know about my solution, then perhaps I can answer some questions about his solution. I will talk about this now. This means that if you give me the molality of any solution, I should be able to relate that solution to my solution so that I at least know that if this were my solution, it would have 1.2 moles of urea and the weight of water would be 1 kg, 1000 grams. Is this clear? Has everyone understood this point now? Okay? Alright, sir. Now let's try to use them once. Let's try to use all these things once. How to use them? Let's think on our own. Look at this question. This has also been asked in some exam. Have we seen this question or not? Let everyone look at it once. Sir, what is the advantage and disadvantage of giving such a question? The advantage and disadvantage of giving such a question is only that the child might get scared, might panic, and no other logic makes sense. If you look with a little bit of intelligence, you can clearly see that at 10° Celsius, the density of a 5 molar solution of KCl, whose atomic mass is given as R 39, what is this atomic mass? Is X grams per ml, meaning the density is X grams per ml at what temperature? At 10° the density of the solution. The solution is cooled to -2° Celsius. The solution is cooled to -2° Celsius, and it is saying that the molality of the solution is unchanged. So I said, absolutely, you are right, friend. Why are you thinking? When we have already discussed that molality is temperature independent, so whether you cool it or heat it, molality will be unchanged. Is it clear? So the first statement, the assertion, is correct. What reason is it giving? The molality of a solution does not change with temperature as mass remains unaffected with temperature. You are also giving the correct reason. This means you have written the assertion correctly, and you have also written the reason correctly. Therefore, both assertion and reason are true, and the correct explanation of A. So the answer should be A. Logically, the answer should be A. Tell me, did everyone understand me? Well done. Very good. This means it is absolutely correct, sir. Now, in this question, many children might think, sir, what is all this given? Density is given as X. Molar mass, temperature. Oh, I don't care. We are talking about molality, and when we talk about molality, molality is temperature independent. It has no relation with temperature. Sir, the same thing is written in the reason, that we are talking about masses, and masses have no relation with temperature. So molality remains constant. That means the assertion is true, and the reason given is also correct. So the answer should be A. Clear? Understood? Okay, well done, very good. Okay, let's move on to the next statement. Now there will be many questions. Now let's talk about the second thing. Here you go. Now I am going to show you some questions that must have been asked at least 20 times in JEE. Look at this.

You talked about molarity. You and this is very important. Everyone will listen very carefully. Now everyone, very carefully. Explain the reason, Ankit. The reason is the same, man, that molality does not depend on temperature. Why? Because what is at the top in molality? Moles. Moles have nothing to do with temperature. What is at the bottom? Weight of solvent. Weight has nothing to do with temperature. This means, sir, that the top has nothing to do with temperature. The bottom also has nothing to do with temperature. So molality is temperature independent. Clear? Understood? Okay, sir, let's talk further. This question shown in front of you, JEE has asked this type or almost similar types of questions, I will show you if I have them all. JEE has asked this question at Mains and Advanced level at least 40-50 times. And you know what the best part is? It's still not stopping. You can see this is a question asked in the last exam, last year. This means either it's like this: Sir, it has stopped now. Sir, he asked until last time, so he will ask next time too. This means we are going to have the most important discussion. And this discussion is the conversion of molarity into molality. The interconversion of molarity and molality, we are talking a little bit about this, which JEE has used many times. That is, how molarity will be converted into molality or molality into molarity is very important for us. So those children who know, those children who know, it's fine, but those who don't know, they should definitely understand this. Now, please understand, if I am given the molarity of a solution and asked for molality, or if molarity is given and asked for molarity, then one thing is clear, sir, molarity is a concentration term that deals with volume. Do you agree with this? Deals in volume. And molality is a concentration term that deals with mass. So there is no doubt that we are talking about converting one concentration term into another concentration term, which is the interconversion of volume into mass or mass into volume. So there should be no doubt about this for any child. Sir, for that, I need to have an idea of the density. I will have to give you the density of the solution. That is, if you provide me with the density of the solution, then I can convert molarity to molality and molality to molarity. Clear? Did everyone understand this? Excellent. Many children are writing the answer. No, only one child is writing the answer and he is just spamming. Okay? You are right, friend. Absolutely right. Now, if we were rewarded, you wouldn't get it. So that's why you said it right. Just shut up. Okay? So, let's try to understand how to convert molarity to molality or molality to molarity. And there will be only one way to answer this. And that way is that you should know how to write that one line in English. If you look carefully, I am given a solution whose molarity is provided as three. A three molar NaCl solution, and what is asked to find? Tell the molality. Now you tell me, I won't waste much time. If I directly ask you what should be done to find the molality of any solution? What will you answer me? Sir, if you want to find the molality of any solution, you need to know two things. What are the two things you need to know, sir? You need to know two things. First thing is moles of solute. I need to know the moles of the solute. Remember the definition of molality, divided by the weight of the solvent. If I know these two things in kg. If I know these two things, then I can show you how to find the molality. Okay? Now, you tell me, the solution given to you is three molar. Does looking at a three molar solution tell you how many moles of solute there are and what is the weight of the solvent? Sir, how would I know, sir, you are hiding a three molar salt solution, sir. You don't tell me how many moles of salt you have and what is the volume of water? You don't show anything. In such a situation, sir, you have taught us to write one line in English. You know how to define your own solution. If you are given molarity, you know how to define molarity. Define that molarity, sir. That is, first of all, since molarity is given, define your solution by molarity, sir. Define your own solution. You have a three molar salt solution. Forget it, I'll bring my own three molar salt solution and calculate the molality of my solution. And that molality will be of your solution too. Why? Because we all came from the same tank. And those who come from the same tank have the same concentrations. That is, the molality that comes out of my solution will be the same molality as your solution. Because we are both coming from the same tank. Is this clear? This means that if the molarity is three molar, then first I will write the three molar NaCl solution in one line in English. And all the children will agree with this. Those who are listening will agree that the way to write three molar is 3 moles of salt in 1000 ml solution. Quickly recall, flip back your copy. How was molarity defined in one line in English just now? 3 moles of salt in 1000 ml of solution. What is the benefit of writing this? You don't know anything by looking here. But as soon as you define your solution, the benefit is that two things become very clear. One, I will see this. This is moles of solute. These moles of solute will be visible. See, you need moles of solute here. One task is done. How many moles of solute are there? Three. One tension is over. Now what is the second thing you are seeing, sir? The second thing I am seeing is the volume. Of what? Volume of solution. Talk very politely, brother. Volume of solution. Sir, I am seeing the volume of the solution. And I see the moles of solute in my solution. But sir, I need the weight of the solvent in the denominator, sir. I want the weight of the solvent, sir. How will I find the weight of the solvent in my solution? Let's use a little bit of intelligence, sir. Whose volume is this? This is the volume of the solution. Whose density is this? This is the density of the solution. If I multiply the volume of the solution by the density of the solution, I will get the weight of the solution. But sir, I don't need the weight of the solution. I need the weight of the solvent. Oh, so if you subtract the weight of the solute from the weight of the solution, you will get the weight of the solvent. Sir, how will you find the weight of the solute? Oh, if you are given the moles of the solute, can't you find the weight? That is, by subtracting the weight of the solute from the weight of the solution, you will get the weight of the solvent. Put that up there. Molality will come out quickly. I don't need to apply any formula. Tell me, did you understand? That is, what should be the correct way? First, what will I find? First, I will find the mass of the solution. Mass of solution. How much will it be, sir? Sir, the mass of the solution will come out. The volume of your solution is 1000 ml and the density is 1.25 grams per ml. Sir, ml will cancel ml, and the mass of the solution will be 1250 grams. Clear? But sir, I don't need the mass of the solution. I need the mass of the solvent. So let's find the mass of the solute. Mass of solute. Who is the solute, sir? Your solute is salt. How is mass calculated? Moles * molar mass. This will be the mass of the solute, sir. 3 * 58.5, how much will it be, man? Tell me by multiplying. 5 * 3 = 15, one. 8 * 3 = 24, 1, 25, 2. 15, 2, 17. That is 175.5 grams, this is the solute. Clear? Sir, this is the mass of the solution. This is the mass of the solute. By multiplying moles by molar mass. Sir, if I use both of these, won't I be able to find the mass of the solvent? Absolutely. Sir, how much will be the mass of the solvent, my friend? Sir, the mass of the solvent will be 1250 minus 175.5. What will this give, sir? Mass of solvent. Tell me quickly, what is this value? If you subtract 175.5 from 1250. How much is 1250 - 175.5, man? 1074.5. Sir, the mass is 1074.5. Whose mass is this? Sir, this is the mass of the solvent. The mass of the solvent is found. Everything is done. Everything is found. Now apply the molality formula directly, sir. Molality is equal to Molality is equal to moles of solute. How many are there? Is there anywhere? You defined your solution. Moles of solute were visible in it. Yes, sir, it's three. And what will come at the bottom, sir? The weight of the solvent will come at the bottom, sir. Let's put the weight of the solvent. How much is it? 1074.5. But this is in grams. You need to put the weight of the solvent in the formula. Sir, it has to be in kilograms. Sir, this means dividing by 1000, that 1000 will go up. Sir, it is clear that the answer should be less than three. Do you agree? The answer will be less than three. Because this value is greater than one. This is 1.07. If you divide by 1000, it is 1.074. So 3 divided by more than one. So the answer should be less than three. Clear? The answer will be less than three. Sir, I have seen the four options. In all these options, sir, look, this answer is wrong, sir. Three cannot be the answer. Clear? Sir, it won't be that small. Why won't it be that small? Oh sir, understand. You have to divide by 1.07, sir. The answer will be almost close to three, sir. The answer will be close to three. You see, 3 / 1.07. 3 / 1.07 is almost three. That is, it will be less than three, but it will come out to be almost three. So the nearest answer I see is the nearest answer, it's very clear. It won't be that small. Sir, it's almost close to three, that is 2.79. Clear? Yes, absolutely. Kshitij is saying, Kshitij is saying, sir, apply the direct formula. Whatever your heart desires today, Kshitij, you can do whatever you want, you can use the direct formula too. In my opinion, this is the most beautiful and easiest way. Clear? Tell me quickly, did everyone understand this? That is, I just want to say that and what I have shown you, I have been asked questions like this dozens of times, I will show you one after another, I won't solve them, but I will tell you that see, it's coming again, then it's coming like that, then it's doing the same thing, and this interconversion of molarity and molality is his favorite topic. Everyone agree with this. The interconversion of molarity and molality is the most favorite topic. In terms of interconversion of concentration terms. He asks the most questions. Clear? Okay? I'll show you more. I'll show you one more question so that you get more clarity. Look at this. I'm not doing it, but just showing you. Molality of 0.8 molar, meaning molarity is 0.8, density of solution is 1.06 grams per ml, and what is asked is molality. Is this the same question? Is this the same question? Sir, in 2025, you showed one question from one shift. I haven't even brought all the questions written down. I am showing one question from one shift. Sir, this question was asked just one year before. Sir, what was the need? When you have asked this question a year ago, why did you ask it again in 2025? This means, sir, you don't even know what you asked last year. That's why you will ask it this year too. Assume this. If even one question comes from concentration terms, it will be on the interconversion of molarity and molality or interconversion of concentration terms. And every child who knows how to write one line in English will get that question right. Understand this. Clear? Did everyone understand this? Did you understand this question? What to do? Sir, it's the same, sir. I'll just write one line in English, sir. The game will be over. Here you go, sir. I'll write it now. Here you go. See, 8 moles of H2SO4 in 1000 ml solution. The game is over, sir. Multiply this volume by the density, and you will get the mass of the solution. Subtract the mass of the solute from it. You will get the mass of the solvent. Put it directly in the formula. The answer will come. Clear? Tell me quickly. Did you understand this? Clear? Why won't option A be correct? Option A is because I think A was too small, man. 3 / 1.07 will be less than three. But it won't be that small that it becomes half. So it will be close to three, but less than three. The answer is B. Oh, you are a strange, confusing person. Calculate it, man. We were trying to explain to you with our intelligence so that you would think, wow, sir gave a great idea. We won't even have to calculate. How were we to know that you would get confused in this? Calculate it yourself by multiplying and dividing. Understand? Shall we move on? Okay, fine. Okay? So, sir, look, this is exactly the same. Okay, sir, let's do this, sir, let's look at one more step, sir. Sir, when you had asked in 2019, 20, 22, 24, you asked the same thing in 2017 too, sir. Let me show you this question again. Why? Because this time it's given in reverse. I'll do it. But I told you it's the same. 3 molal NaOH. Molality is three mol. What was the method I told you to define molality? Sir, define molality once. As soon as you define molality, you will know the answer. So, let's define molality once. How was molality defined? Sir, three molal means three moles of solute. Because this is molality, dissolved in 1 kg or 1000 grams of solvent. This is your method, sir. Remember the one line in English, sir. This is that one line in English, sir. As soon as you write this, all your tensions will be gone. If you look carefully, sir, these three moles of NaOH, this is your solution, sir. From here, what will be known, sir? Moles of solute will be known, sir. This is moles of solute. And what is this, sir? This is the weight of the solvent. This weight of the solvent is known. Now you tell me, what do you need to find, sir? Sir, I need to find molarity. So let's go to the corner and ask once, how is molarity calculated? What is needed for molarity? Sir, I need moles of solute. That is, NaOH, divided by the volume of the solution in liters. If I know this, then I can find molarity. As soon as you wrote that one line in English, one tension is over. Moles of NaOH are three. That is, the work above is done, it's three. Only the tension of the denominator remains, sir. How will the volume of the solution be found? Oh man, what is this? Oh sir, this is the weight of the solvent. Okay, from here what will come? Sir, this is the weight of the solvent. From here, the weight of the solute will come. This is the weight of the solvent. From here, the weight of the solute will come. If you add both, you will get the weight of the solution. And if you divide by the density, you will get the volume of the solution. The game is over. Tell me, did you understand? That is, for a child who is even a little bit intelligent, there is no hassle. There is no hassle. You can write in one line, sir. The weight of the solvent is how much? You have defined the weight of the solvent of your solution as 1000 grams. How much will be the weight of the solute? Sir, the solute is 3 moles. The molar mass of NaOH is 40. So 3 * 40 = 120 grams. That is, if I add both of these, I will get the weight of the solution. Absolutely correct, sir. You know the weight of the solution is made up of solute and solvent. So let's add the weight of both. 1000 + 120, that is 1120 grams. That is, the weight of the solution is found, sir. Done. But sir, I don't need the weight of the solution. I need the volume of the solution. Oh, so the density is also given. The volume is found. Sir, how much will be the volume of the solution? Volume of solution is equal to weight of solution, 1120 grams, divided by density, which is 1.11 grams per ml. How much will be the volume? 1120 / 1.11 ml. This is the volume of the solution. Look, it might seem difficult to you because I am doing it. But once you do it in your copy, you will understand everything. Clear? Understood, man? Clear? This means, sir, no, child, one child is saying, sir, quickly do the concentration terms. Look, what's the hurry with concentration terms? This whole chapter is ahead and it's fast. But this interconversion is very important. That's why I'm spending a little time on it. So, many children will find this easy if they do it once. Right? So, as you saw, to find the volume of the solution, the total mass of the solution, which came from solute plus solvent, was divided by the density. The volume is found. Now, calculate the molarity. Let's put it here. What will it be? What is the volume at the bottom? 1120. 1120 divided by 1.11. But in what unit is this? In ml. And in what unit do you need it? In liters. So when you divide this milliliter by 1000, that 1000 will go up. That's the answer. Now, if we think of a shortcut for this, think about what will come out. Let's see the shortcut. Sir, if you look carefully, this is 1.1120 and this is 1.11. Sir, this value that is coming out is slightly more than 1000. See, this is more than 1000. So, there is 1000 at the top and a value slightly larger than 1000 at the bottom. So the answer will be slightly less than three. It will be slightly less, sir, than three. This means, sir, this is wrong. This is wrong. This is wrong. Only one answer is correct. And that is A. Tell me, did you understand my point? But these are all children who give the exam thinking they need to score here. They are not giving the exam thinking that if they do something good, it will be fun. They are sitting to solve the questions thinking that I have to get this question right. So those who do the exam with this thought, they use all their thoughts and do all the work. They are foolish people who will sit to solve this. Oh, you idiot, you should understand that all the answers are greater than three. Only one answer is less than three. And looking here, it seems that the answer will be less than three. Because this term is less than one. Sir, this term, sorry, this term is greater than one. This is a number greater than 1000, sir. You see, 1120 / 1.11, this is a number greater than 1000. That is, there is 1000 at the top. There is a number greater than 1000 at the bottom. So the answer will be less than three, and only one option is less than three, sir. The

The answer is 2.97. This can be done even without calculation. Do you understand? You could have done this without calculation too. Did everyone understand? I haven't covered oleum yet. We do oleum within redox. The volume strength of hydrogen peroxide and the percentage labeling of oleum will be covered within redox. Don't ask again, or I'll hit you for no reason. Understand the point. Is it clear? Did you understand up to here? Okay? Let's move on, sir. Very good. Okay, this question has come up. Okay, and let's talk more. Sir, since you asked so much. This is probably the same question, right? The one asked in 204. Yes, this is the same. Alright, sir. Since you have asked so much, why did you ask this question, sir? When are you asking this? Sir, there was a gap of one year. Look at this. Molarity is given, density is given, molality needs to be calculated. Same question, will you do it? Tell me quickly, can you do it? Tell me quickly, can you do this? Yes or no? Okay. Same question, sir. It's a three molar solution, sir. To calculate molality, we need to know the moles of solute. We need to know the weight of the solvent. Sir, you haven't told us anything. No problem. I know how to define my solution, sir. As soon as I see three molar, a line of English comes to my mind, brother. 3 moles of which solution? NaCl in 1000 ml solution. Sir, I know how to write a line of English, sir. How much benefit has this one line of English given, sir? This one line of English. Whoever has learned it will be happy. Understand the point? Is it clear? Did everyone understand? So, this is the same question that he has been asking us continuously. Look at this, I'll show you more. All these lines are exactly the same. All these lines are the same. I haven't written all of them, you understand. Look at this. In 2024, they said, "Let's ask one more question." From that line, look at what they are saying. Tell me quickly, how many people can do it? Yes or no. Give me an answer in yes or no. Finish the discussion. Can you do the question or not? Density of x molar, meaning what do we need to find, sir? x molar means this time I need to find molarity. I will have to find the value of x, and what is x? Molarity. Molarity needs to be found. Is it clear? So, sir, molality will be given. Let's see, sir. Look at this, sir. Molality is given. Look at this. Molality is given. So, sir, density should also be given for the solution. Density is also given. Here you go. Sir, density is also given, molality is given, molarity needs to be found. It's the same drama, sir. Write one line of English, sir, and the work will be done. And since molality is given this time, how will the line of English be written? 3 moles of NaOH dissolved in 1 kg or 1000 grams of solvent. What's the benefit, sir? The benefit is that, sir, first of all, I can see the moles of solute. Here are the moles of solute, and from here I can see the weight of the solvent. What's the benefit, sir? The benefit is that to find molarity, I need moles of solute. They will be three. And when the volume of the solution is needed, sir, I will use it from here. Sir, this is the weight of the solvent. From here, the weight of the solution will come. Sorry, the weight of the solute will come. We will add both, the weight of the solution will come, and we will divide by the density of the solution. The answer will come. Tell me, did you understand my point? Did everyone understand this? Is it clear, sir? You can do it in one go, sir. I will do it in one go. This time it seems the exact answer will be three. How? Let's see by doing it. Sir, this will come. I am doing it directly. Let's see if you can understand or not. Molarity is equal to moles of solute divided by volume of solution. Wait a second. 1000 + 120, 1120 divided by 1.120 * 1000. Oh, you are such a foolish person. It's coming out to be exactly 3 molar. Exactly 3 molar. B. Clear. Oh, this term is the same this time, isn't it? What kind of person are you? Are you completely foolish? 1120 / 1.120. This will be 1000. 1120 / 1.120. This will be 1000. Will this 1000 cancel with the 1000 above? What will come? Three. Finished. Clear. Did you understand? This time the exact answer is three, but what I want to tell you is that this is not about the answer. The point is that how many times will you ask questions of this type? They are all the same questions. So, we have understood one thing: if I am asked questions related to calculating molarity from concentration terms, or interconverting molarity and molality, or if I have understood everything I have taught so far, then quickly write yes and confirm, sir, I will not ask any more questions about this. If there is any question related to molarity, molality interconversion, or anything related to it, I will solve it. Do you have that much confidence? Do you have that much confidence? Excellent, very good. Okay, sir. And let's talk more, sir. Now let's move on to the third concentration term, quickly, mole fraction. Sir, forget it, sir. We have been hearing this since childhood. The matter becomes very clear from the name "fraction." Sir, if you talk about mole fraction, it is very clear that if there is a solution in which there are n1 moles of solute and n2 moles of solvent, then if I want to find the mole fraction of the solute, it will be calculated as moles of solute divided by moles of solute plus moles of solvent. And if you want to find the mole fraction of the solvent, it will be calculated as moles of solvent upon moles of solute plus solvent. I think everyone will agree with this, and everyone will also understand that if the mole fractions of solute and solvent are added, it becomes one. And obviously, sir, if you add the fractions of all the people, it will be one. So, there is no hassle with mole fraction, sir. Bring the moles, take the fraction. But, sir, it is not necessary that moles are given directly. Maybe weight is given. Oh, sir, forget all this. If weight is given, I know how to find moles, sir. I have ingrained the Y-map into my blood, sir. If weight is given, I will find moles by dividing by the molar mass. And when I know the moles of solute and solvent, then whichever mole fraction you ask for, I will calculate its mole fraction. Is it clear? Did everyone understand? Sir, this means it is not a big deal, sir. Tell me something good, sir. Listen very carefully. I am going to tell you something very good. Let's say, just saying. Let's say I have a solution. I am going to tell you a good thing. Okay? Which you can call a beautiful thing. This is a beautiful thing. What is the beautiful thing? He is saying that, man, let's say I have a solution. A solution which has a mole fraction of anything, let's take urea. Mole fraction of urea, or let's not write it like this. Let's write it like this. An aqueous solution of urea in which the mole fraction of urea is 1/9, let's say this is the question. Now, it's not a question, it's just a part of a question: brother, I have a urea solution. In that urea solution, the mole fraction of urea is 1/9. Now, do you know what the problem is? Do you know what the problem is? The problem is that if a solution is shown to you. I have hidden a urea solution like this and I have told you, brother, tell me, I have a urea solution in which the mole fraction of urea is 1/9. So, have I shown you how much urea and how much water is there? Sir, I can't see anything. You have just hidden the urea solution behind. How do I know how much urea and how much water there is? So, you should know how to define your solution. Just as you have learned to define molarity in a line of English, just as you have learned to define molality, learn to define your solution. Define your urea solution in which the mole fraction of urea is 1/9. And this is again a beautiful thing that is going to come before you. And that is, if the mole fraction of urea is 1/9, then write it as 1 / 1 + 8. And as soon as you write it as 1 / 1 + 8, what will you understand the best? That sir, by writing it like this, I will understand one thing: because this is the mole fraction of urea, whose moles will be on top? Urea. And whose moles will be at the bottom? Urea plus water. Sir, the good thing is that by writing it like this, I will understand one thing: that in my solution, the moles of urea are one, and in my solution, the moles of water are eight. This is very important information that you can use. But you understand, sir, is it necessary that the solution he hid, whose mole fraction is 1/9, is it necessary that it has one mole of urea? If he shows you the solution, "Look, there are two moles of urea. You said one mole. I have two." Then you will immediately retort, "Oh, then your moles of water will also be not eight, but sixteen." Understand the point. Your fraction will also be 1/9. My fraction will also be 1/9. But I have learned to define my solution. I don't care what you are holding behind. If you are holding a bucket, it will have more urea and more water. If you are holding a cap, it will have less urea and less water. But sir, I have learned to define my solution. If I have to define my solution, how to define it? In terms of molarity, in terms of molality, and in terms of mole fraction. And this is the one line of English. That is, whenever you are given a mole fraction, you will always break it down in this way, and as soon as you break it down, it will seem very easy to you because by doing so, you will also see the moles of urea, i.e., the solute, and the moles of solvent. This is inside your solution. You are defining your solution. If you think about it, if you have defined your solution, then all the answers you are going to give for your solution will also be correct for the solution he is hiding behind. Why? Because that solution and your solution came from the same tank. Because the mole fraction of that solution is also 1/9, and in your solution, the mole fraction of urea is also 1/9. Is everyone understanding my point? Does everyone understand this? I will apply it now. But it's very interesting. Very interesting. Now some people say, sir, if it is 1/9, then we will write it like this. But what if it was something else instead of 1/9? For example, let's just write it arbitrarily: how will you define your solution? So, if I am going to define my solution, like this, let's say the mole fraction of urea is 2/9. What will you do now? If the mole fraction of urea is 13/17, then what will you do? So, it's very simple. I will speak very simply. If it is 2/9, then it will be 2 / 2 + 7. End of discussion. We won't think too much. And if it is 13/17, it will be 13 / 13 + 4. Understand my point? 13/3 + What's the benefit of this? The benefit is that, sir, at least you know about your solution. 2 moles of urea, 7 moles of water. 13 moles of urea, 4 moles of water. That is, you know how to define your solution. I will say only one thing that everyone should understand. If I ask you, I need an answer in yes or no, brother. Okay? Now, whoever is talking nonsense here and there should be completely quiet because we will not refuse. Whoever is chatting nonsense. Hi, so-and-so, etc. Understand, Pritam Gupta, whoever it is. Right? But I am asking the students who are studying for an answer. If I tell you that in this question, the mole fraction of urea is given as 2/9. Does this mean that there will be two moles of urea and seven moles of water? Does this statement seem correct to you? That if the mole fraction of urea is 2/9, that means moles of urea will be two and moles of water will be seven. Is this statement correct? If it is 2/9, the answer will be 2 and seven. Is this correct? Sir, this is not correct. It is not yes. Understand the point. This is your solution in which urea is two and water is seven. It cannot be like this. Think about it yourself. Is this wrong? Tell me yourself. 4 / 4 + 14. Is this value not 2/9? Is this value not 2/9? Yes, sir. Is this value not 2/9? Take anything. 6 / 6 + 21. Is this value not 2/9? Sir, this is also 2/9. What I want to tell you is that there are many values equal to 2/9. That is, in this case, sir, the moles of urea are changing. The moles of water are also changing. Because these are all those solutions that have come out of the same tank where the mole fraction of urea is 2/9. But sir, I have defined my solution. I have defined my solution: if it is 2/9, then it will be 2 / 2 + 7. At least I am clear about my solution: if there are two moles of urea in my solution, then there are seven moles of water. Now, if there are four moles of urea in the solution you hid behind, then there will be fourteen moles of water. If you have six moles of urea, then there will be twenty-one moles of water. Sir, that will keep changing, sir. The answer will come out the same. Why? Because we all came out of the same tank, sir. All our concentrations will come out similar. Define my solution. Calculate the answer from my solution, and all those answers will be correct for all of you. Why? Because you are all coming out of the same tank. Is everyone understanding my point? A child is asking when vapor pressure will start. Oh, vapor pressure will also start soon, man. Right? We are also working with courage, you also work with courage. I said this in the last class, and I am saying it again. If you don't have the courage at all, then there is no need to attend the class. This will be a recorded system. When you open YouTube, when you listen to songs on YouTube. Understand? At that time, if your heart desires, you can also take a look here. Spend your time for two, four, five, ten minutes. Understand? But we also need courage. Because we also know that we have to discuss the entire solutions after these concentration terms. So, we also need courage for that. You understand? Seeing your cheap comments like this breaks our courage. Like one child is writing, "End it, sir." Man, I have said before that this is in the hands of the Almighty. How can we end you? You have to live as long as God has given you life. You understand, nothing will happen by our doing. We can't do anything. Whatever God has written in destiny, that has been written. You understand the point. So, the end is not in our hands. Your end is written by God. It will happen when it is supposed to happen, friend. We won't be able to end you. Understand the point. How can we end it? Understand the point. Anyway, so you understood this point. Now let's try to use it. Okay? Let's try to use it. Look at this now, what are you studying, and even today it is still relevant. What will we discuss, and what does he ask? He is asking, if there are moles NA, NB, NC for three people, then what will be the mole fraction of C? Tell me this question. Oh, sir, moles of C upon total moles. Sir, what is there to think about? You understand my point? That is, what I mean to say is that, sir, he is also asking this question. That is, think about the exam you are afraid of, but okay, sir, it won't be such an easy question every time. I had to learn something else, so I am trying to learn that. Alright, sir, let's talk more. Now, try to understand a little. It's very interesting. Let's say, like this one. Now, everyone will listen very carefully and try to do it. How? He is saying, ah, this is not the molarity one. Okay. Molality of an aqueous solution. This was asked in 2024. You see, meaning in 2024, 23, 22, 19, 20, 21, he is asking the same kind of questions every year. The same concentrations. Think, what question is he trying to ask? He is saying that I have a solution whose molality is given. Can you tell me what is the mole fraction of that solute in it? What is the mole fraction of that urea? So, I, meaning you, what are you trying to do? You are trying to do: molality is given. What you are trying to do is this. Molality is given, and you want to go to mole fraction. You want to go to mole fraction. Or let's do the reverse. Mole fraction is given, and you want to come to molality. Now, tell me, will density be needed for this interconversion? Will density be needed for this interconversion? Sir, density will absolutely not be needed for this interconversion. Why will it not be needed? Sir, it will not be needed because this concentration term, we have already discussed it. It deals with mass, or mole fraction deals with moles. That is, this also deals with mass. Deals with mass. That is, both these concentration terms are the same type of concentration terms. Therefore, I do not need density. I do not need the density of the solution in any way. Now, how will you do the question, sir? Look at this, molality is given, and I need to find mole fraction. What method did you tell me, sir? Sir, the molality that is given to you, do you have any idea when calculating mole fraction? If you want to find the mole fraction of urea in this question, what do you need to know? Sir, whenever you want to find the mole fraction of urea, you need to know the moles of urea, and along with that, you need to know the total moles. Now, who will come in the total? Sir, it's an aqueous solution, so moles of urea + moles of water. If I know all these moles, then I can find the mole fraction of urea. Are all these moles given in the question? Sir, only molality is given. A solution is hidden from me, and I am told to find its mole fraction, calculate this and that. Sir, I cannot see the moles. How will I find the mole fraction? But you have taught me to write a line of English, sir. If molality is given to me, then I

I can understand everything by writing this molality in one line of English. Let me show you how. 4.44 molal, tell me quickly. How would you write 4.44 molal, sir? 4.44 molal means 4.44 moles of urea in 1000 grams of water. Did you understand? Sir, this is one line of English, sir. This is the line you just taught, sir. This is one line of English. If you learn it, it will be fun. Is it clear? What does it mean, sir? It means, sir, you gave the molality of urea, which I wrote in one line of English. As soon as you write it in one line of English, what will be the benefit, sir? The benefit will be that if you look carefully, the moles of urea will be visible from here. This is moles of urea. Is it clear? And I don't know if you can recognize it or not. This is the weight of water. So, the moles of water will also be visible from here. Can you find the moles of water from the weight of water? Sir, 1000/18, sir, I can also see the moles of water. 55.55. That is, sir, as soon as I write this line, think, I can see the moles of urea and the moles of water. Sir, what I couldn't see, I can see with this line, sir. I can see everything. Here is the answer, sir. The moles of urea are 4.44 divided by 4.44 + 55.55, sir. This is the final answer. That's it, sir. That is, you add these two together, sir. Whatever comes out after adding, sir, that will be the mole fraction of urea, sir. From here you can find the mole fraction of urea. It's very simple, sir. Very simple. Is it clear? Did everyone understand this? Did everyone understand this? The children are giving the answer. 74, I don't know the answer. Yes, it is given. So 74, meaning 74.074074, this is the mole fraction of urea. Right? This is what will come out. Is it clear? Tell me quickly. Did you understand? So, think about how much benefit there is from writing this line. Otherwise, what will happen, sir? Here, sir, looking at this molality, it is not clear from anywhere how many moles of urea and how many moles of water there are. And until the moles of urea and water are known, the mole fraction will not be obtained. But as soon as you break it down into one line, you will see the moles of urea and the moles of water. Oh, if you can see the weight of water, you will be able to see the moles, right? That is, the moles of water are also known. The moles of urea are also known. Directly put it in the numerator. Done. Clear? Tell me quickly, did you understand this? Did this make sense? Now it says calculate once. Oh, please calculate a little yourself. Don't make us calculate all this now. In some places, you have to use a little bit of your brain. If you add 4.44, it will come out to be something. Understand? So use your own little bit of intelligence. Right? You have to do some calculation somewhere. Is it clear? Let's talk more, sir. Now let's come to the next concentration terms. There will be many. There are questions that will be given to you to do. Try them. Let's come to the next concentration term. Our next concentration term is percentage concentration term. Percentage concentration terms are those concentration terms that are used in modern times. That is, the era of molarity, molality is gone now. Now the concentration terms are defined in terms of percentage. So, the percentage concentration terms we need to learn are mainly of three types. One is percentage weight by weight. If I talk about percentage weight by weight, then what will be the percentage weight by weight concentration term? In which it will be written, weight of, and you understand, weight of solute by weight percentage. How is percentage calculated? My weight upon total weight * 100. So, if you are showing percentage weight by weight, then the weight of the solute, whatever unit it is taken in, will generally be in grams. Weight of solute in grams divided by total weight, whose? Who will come in total? Weight of solution in grams * 100. So, this is percentage weight by weight. That is, if I want to find the percentage weight by weight of any solution, I will have to divide the weight of the solute by the weight of the solution. Just like percentage is calculated. Weight of solute divided by weight of solution * 100. Clear? Sir, this is very straightforward. If the weight of the solvent is known, then I will be able to calculate the percentage. Okay? It's a very straightforward question. We learned to calculate these percentages in fourth grade. What is more important than this? What is more important is one line of English. Understand carefully. If I tell you that I have a 10% weight by weight aqueous NaCl solution. That is, I have a solution. I hid this solution. I have a salt solution. 10% weight by weight. Can you tell me how much salt is there? So what will I answer? How do I know you hid the solution? How do I know if you are holding a bucket or a pot? If it's a bucket, there will be more salt, more water. If it's a pot, then there will be less salt, less water. I don't know how much salt and water you have. But I can do one thing. Hide whatever you want to hide. I will define my own solution, which will be 10%. How? Let's learn that. That is, if it is 10% weight by weight, then what is the way to define it? If it is 10%, how will 10 come? 10 will come from 10 divided by 100, and 100 will cancel out. 10 will come. That is, 10 grams of solute. Who is the solute? Salt. 10 grams of salt in 100 grams of solution. This is one line of English. Understand. And you can't even imagine how much benefit there is from this. This is one line of English. How much benefit is there? Tell me. Sir, I understood, sir. As soon as I write this one line, look what I can see. The weight of the solute is visible. Weight of solute. Tell me quickly. If the weight of the solute is known, then the moles will be known. That is, indirectly, the moles of the solute are known. And 100 grams is the weight of what? Sir, this is the weight of the solution. The weight of the solution is known. The weight of the solute is known. If you subtract both, then by subtracting both, the weight of the solvent will be known. That is, indirectly, what all did I get to know, sir? I know the weight of the solute. From that, the moles of the solute will also be known. I know the weight of the solvent. Because by subtracting the weight of the solute from the weight of the solution, I can find the weight of the solvent. Sir, I know the weight of the solute. I know the weight of the solvent. From the weight of the solute, the moles of the solute will come. From the weight of the solvent, the moles of the solvent will come. Sir, I know the mole fraction, sir. I know the mole fraction, sir. I know the mole fraction of salt in this solution, sir. From here, the moles of salt will come. From here, the moles of water will come, sir. I will know the mole fraction of salt. Sir, I know the molality of this salt solution. How, sir? In molality, you have to put the moles of salt in the numerator. Sir, how many moles of salt will be in 10 grams? I know how to calculate it. Divided by the weight of the solvent has to be put, sir. And I will find the weight of the solvent by subtracting. Sir, the moles of the solute will come from here. The weight of the solvent will come from here. I know how to calculate molality, sir. That is, just write one line. You will know the mole fraction. You will know the molality. And if you accidentally give the density of the solution, then you will also know the molarity. Tell me quickly. Did this make sense? Did this make sense to everyone? Tell me quickly, brother. It's very interesting. Tell me quickly. Did this make sense? Did this make sense to everyone? Are you understanding? That is, just write one line. You have those formulas memorized. What is molarity? What is molality? It's absolutely clear. As soon as you write that line, everything will appear to you on its own. This weight is here. This weight is here. We will subtract. Solvent is here. Now tell me, what do you want to find? Let's find the moles. We will find the moles. What needs to be put in the formula? We will put this. You will know everything on your own. As soon as you write this line. Clear? So this is percentage weight by weight. The second concentration term, first let's write all the concentration terms once. The second concentration term is percentage weight by volume. The second concentration term is percentage weight / volume. Percentage weight by volume. How will it be written, sir? It's clear. How will it be written? Sir, it's the same. Now weight, as it was written before. Weight of, above will be the weight of the solute. Weight of solute in grams. Below will be the volume, this time of the solution. Volume of solution in ml, let's take it. * 100. Sir, this will be your percentage weight by volume. Give me the weight of the solute and the volume of the solution. I can give you the percentage weight by volume. Ayush Pandey is asking who is going for a trip? Ayush, when the exams are over, there will be nothing but trips, because there will be no work, so try to do a job where you get to travel a lot. Are you understanding? So in such a case, the best job is that of a driver. You can become a truck driver. A truck driver is sometimes here, sometimes there. So if you are not focused on studies, are you understanding? Then do some work like this. But if you like to travel, you can do these things. Are you understanding? Many other things can be done for traveling. So think about this from now on, that if you have a habit of traveling, what can be done? You are a strange, confused person, aren't you? Who is going for a trip? That is, everyone is free, and those who go for a trip, are you understanding, what kind of people will they be? So all of you get together and form your own group. You guys buy a truck and drive it at night, and we drive during the day, understand? Anyway, weight of solute in grams divided by volume of solution in ml * 100. Okay? Sir, this is very clear. If I am given the weight and volume, I can calculate the percentage weight by volume. I learned this in childhood, sir. I will put the volume value and get the answer. Okay? What is more important is that I know how to define this concentration term myself. So, if I am ever told that I have, let's say, a 12% weight by volume aqueous urea solution. Let's assume this. So how will you define it? Brother, I have a solution. 12% urea, I hid it, sir. Tell me, how much urea is there? Oh, I said, are you a foolish person? I can't see your container. How do I know how much urea there is? How much water? I only know that it is 12% weight by volume urea. But I define my own solution. I will define my own solution here. Yes, a child has said this, so I will write this too. I forgot to mention that this is temperature dependent. Sorry, this one is temperature independent. This is temperature independent. Why? Because, sir, everything is about weight-weight. And weight-weight things have nothing to do with temperature. But this term, because volume is involved. So this is temperature dependent. So this is temperature dependent. You understand, right? Okay? Anyway. So if it is 12% weight by volume, then how to do 12% weight by volume? So, I will try to define it in my own line. What does one line of English say? So if you are defining 12% weight by volume. So this is 12 grams, weight is above. 12 grams of urea that is solute dissolved in, below is volume of, whose? Total dissolved in 100 ml solution. That is, 12 above, 100 below, 100 will cancel out, sir. The weight of the solute itself will become our percentage weight by volume. That is, 12 grams of urea is dissolved in 100 ml of solution, sir. What is the benefit of this, sir? This is one line of English, sir. This is one line of English. And what is the benefit, sir? As soon as I write this, I can see everything, sir. As soon as I write this, I can see everything. If you look carefully, 12 grams of urea means I got the weight of the solute. Is it clear? I got the weight of the solute. And 100 ml solution means I got the volume of the solution. What is the benefit, sir? The benefit is, sir, this is the weight of the solute. This is the volume. Don't you think from the weight of the solute you can find the moles of the solute? By dividing by the molar mass of urea. And this is the volume of the solution. Sir, you can find the molarity. Directly, molarity is equal to moles of urea divided by volume of solution in liters. Sir, you will calculate the moles. You will take the volume in liters. You will get the molarity directly. That is, if percentage weight by volume is given, you can calculate molarity in one second. And these interconversion questions can be asked in the exam. If even one child learns to write this one line of English, all their tension will be gone. Clear? Did everyone understand? Molarity will be calculated. That's absolutely correct, sir. Now you can calculate molarity because as soon as you write this, moles will come from the weight of the solute, and by dividing the moles by the volume, whose volume? The volume of the solution. In what unit? In liters. You will calculate molarity. Clear? Okay? Let's check once and write the third concentration term, and then let's try to do one or two more questions. Sir, the third concentration term is percentage volume by volume. The third concentration percentage concentration term is percentage volume by volume. This concentration term will be used when the solute is also a liquid volume. Because above is volume, below is volume. So now what will you write? Volume of solute. So obviously, this time the solute must also be a liquid. Volume of solute divided by volume of solution, volume of solution * 100. That is, when the solute is also a liquid, you can use the percentage volume by volume concentration term. That is, you can mention here. Here solute is also liquid. So, in such a case, you can also use this concentration term. Above will be the volume of the solute, below will be the volume of the solution. Multiply by 100. Clear? So, we can define concentration terms in terms of percentage in these three ways. And by learning the way to write them, we can do it easily. Now we can do this for gases too. The only difference will be that the volume of the gases will have to be found, and you should know the volume of the solution below. So this information will be given in the question that the dissolution of gas does not affect the volume of the solvent. Or how much effect it has. Because you need the volume of the solution. And in the volume of the solution, you will have to take the volume of the gas plus the liquid. So, did the dissolution of gas affect the volume? It will have to be mentioned in the question. Then we will do the question. Clear? Did you understand? Let's take an example, and it will become clearer. This was asked in some exam. How straightforward is the question. This was asked in 2023. Absolutely straightforward. That is, I am not doing it on my own. You can see for yourself. And solve this question yourself. A solution is prepared by adding 2 grams of x of 1 mole of water. That is, 2 grams of x were dissolved in 1 mole of water. Mass percentage. Now, is this even a question? You learned this in sixth grade at school, that the mass of one person is given. The mass of another person is given. Calculate the mass percentage. That is, a solution of is prepared by adding 2 grams. That is, if you want to find the mass percentage. Percentage weight by weight. Then weight of x divided by total weight. Keep this in mind, brother. Weight of x / total weight of solution. And what will come in total weight, sir? One will be the weight of 1 mole of water, 18 grams, and the weight of 2 grams of x. Are you understanding? By adding these two, you will get the weight of the solution. Clear? So, weight of solute divided by weight of solution * 100. Sir, by solving this, you can find your answer. So, this is 10% / weight. Clear? It's a very straightforward question. Let's move forward quickly and try to do more questions. It's absolutely straightforward, sir. Where it's a little bit, look here, sir. Asked again in 2024. I can't tell you how important this topic is. If there are, say, 10 questions in physical chemistry, or nine questions, then out of those nine, you can find one or two questions on mole concept, of which one is always on concentration terms. Do you understand? A solution is prepared by adding one mole of ethyl alcohol and nine moles of water. That is, one thing is clear. One mole is your ethyl alcohol and nine moles is your water. Okay, fine, sir. By mixing these two, we will make a solution. What do you want to know? The mass percentage of the solute. My goodness. You want to find the mass percentage of the solute. Sir, is this even a question? Do you have to do anything in this too? To find the mass percentage of the solute, how will you find the weight percentage of ethyl alcohol? Weight of ethyl alcohol divided by total weight, will everyone do it? Total weight * 100. Sir, you can easily calculate the percentage. You can find the weight of ethyl alcohol. You know how to find the total weight. This task is very easy. Everything is given in the question. The molar mass of ethyl alcohol is 46. Sir, there is one mole of ethyl alcohol. So this is 46 divided by what will come in total weight, sir? 46 + weight of nine moles of water. What will be the weight of nine moles of water? 180 minus 18, that is 162. So this is 46 + 162 * 100. Sir, this will be the weight percentage of ethyl alcohol. Clear? Did you understand, brother? Can you do it? Well done. Very good. And let's talk. Sir, all these questions are asked one after another. Look here, sir. What is it trying to make you do? Concentrated nitric acid is labeled as 75% by mass. Very good. That is, you have nitric acid hidden like this. Hidden nitric acid. And this is 2025, meaning my own observation and my own experience. Right? Otherwise, it's your choice. Do whatever you want. But my own experience says that if I observe the past years, I am starting to see good level questions on concentration terms because in 2025 I have observed that the 2025 questions on mole concept concentration terms are better. So whoever revises will definitely solve the 2025 questions. I have also taken almost all the 2025 questions. I have taken quite a few questions. But still, in every subject, in every chapter, definitely solve the 2025 questions.

Because I feel that in 2025, the physical chemistry portion of chemistry, which has been ongoing since the beginning, and which students feel is what is asked, has had slight variations introduced. There have been small, good additions, and this question is not new. However, it has also asked easier questions than this. Did you see nc / na + nb + nc? It has asked that too. But by asking this, it feels like this is better. This means that similar questions might come in your exam as well. If you go prepared beforehand, you will find the questions easier. Now, let's look at this question and try to solve it. You can all do it very quickly. Let's try to solve it once. There is concentrated nitric acid which has 75% by mass written on it. Sir, it is written 75% by mass. So, what is that nitric acid? Can you see it? It says it cannot be seen. It is only telling me that I have a nitric acid solution which is 75% by mass. So I said, okay, let's look at the question. The volume in ml of the solution which contains 30 grams of nitric acid is, meaning if I have a solution which is 30 grams. A solution of 30 grams of nitric acid. So, what this means is, the volume in ml of the solution which contains 30 grams of nitric acid. So now, think for yourself, if there are 30 grams of nitric acid, which is 75% of the total mass. So, if I just do this, let the total mass of the solution = m grams. Then 75% of m should be the weight of nitric acid, which is given as 30. From this, you will get the value of m, meaning the mass of that solution, which is 30 * 100 / 75. And I think if you solve this, it will come out to be 40. Meaning, your solution is 40 grams. It is clear, it is a 40-gram solution with a density of 1.25. So, what will be its volume? Here you go, sir, the question is finished. Volume is equal to mass divided by density, that is 1.25. So, you can do this by calculating 40 / 1.25. So, I think everyone will understand this that if you solve 40 / 1.25, what will come out? 40 / 1.25, obviously sir, it will be less than 40. So the answer should be 32. Is it clear? Did you understand C, brother? A student is saying, sir, this came in my shift. Look, it's a straightforward question, but it requires a bit of thinking. Meaning, a student might think, sir, how to do this? I don't understand how 30 grams of nitric acid will be in how much solution? Oh brother, assume your solution is m. It has 75% nitric acid. So, this means 75% of m will be the weight of nitric acid. From that, the mass of the solution will be obtained. And as soon as the mass of the solution is obtained, by dividing it by its density, you can calculate the volume of the solution. So, sir, the volume will be 40 / 1.25, and that is 32. Is it clear? Let's talk more, sir. All the questions will be similar. You can solve them very easily amongst yourselves. This can be done very easily. Look at this. This was asked in the 2024 shift. See what they are trying to say. The molarity of 1 liter orthophosphoric acid having 70% purity by weight is. I need the molarity, sir. Now, if I know about molarity, I can only write one thing about molarity. Molarity is equal to moles of solute. Moles of solute divided by volume of solution. I don't know anything else. Volume of solution. Sir, this is the way to calculate molarity. Now, you see, sir. If it is given to you, then solve it. Sir, one thing is clear. Solution is 1 liter, sir. The denominator is clear, sir. The denominator is one. Sir. I don't need to do anything else. Sir, just teach me how to find the moles of solute, sir. Now, use a little intelligence. If the solution is 1 liter, and its density is given, and the H3PO4 in it has 70% purity. Then how will molarity be calculated? Use your intelligence. Meaning, what does it mean, sir? It means, sir, if I can find the moles of the solute and the volume of the solution, then I can calculate the molarity. I just need to concentrate on the moles of the solute, how to find the moles of the solute. So, now, think for yourself a little, that sir, the molarity of 1 liter orthophosphoric acid in which 70% purity by weight is our sulfuric acid, sorry, orthophosphoric acid. Its molar mass is given as 98. The density of the solution is given as 1.54. You ultimately have to calculate the molarity. Can you do it, brother? Tell me quickly, can you do this? The answer is 11. Try to solve it. Try it yourself once. The answer is given as 11. Try to solve it quickly. How will you do it? How will you find the moles of the solute? Let's just see. I think if you want to find the molarity of 1 liter solution, whose density is given. Then, sir, first of all, the weight of the solution will be calculated. The weight of the solution will be 1, sorry, 1 liter, meaning 1000 ml. 1 liter means 1000 ml * 1.54 grams per ml. So, the weight of the solution is 1540 grams. Now, if the weight of the solution is known, how to find how much H3PO4 is in it, sir? H3PO4 is 70%, sir. It is 70% by weight, sir. So, this means, sir, if you take 70% of this, you will get the weight of H3PO4. So, meaning, if I calculate the weight of H3PO4, the weight of H3PO4 will be 70% of 1540. This will be the weight of H3PO4. And if the weight of H3PO4 is known, how to find its moles, sir? From weight, moles can also be found. 1540 * 70 / 100 / molar mass of H3PO4, which is given as 98. So, this will be the moles of solute, sir. These are the moles of solute, sir. The numerator's work is done, sir. Meaning, moles of solute are 1540 * 70 divided by 100 * 98 divided by the volume of the solution, which you have already taken as 1 liter. Sir, you just need to solve this. Let's try to solve this roughly once. Sir, let's also take this 98 as 100, right? So, it becomes 100. Meaning, what will come on top will be 15 * how much? 1.5 * 7, meaning 10 point something. You understand, whatever they have written, 11, this answer will be 11. Let's multiply it once, brother. Let's multiply it once. 1540 * 70 / 9800. Sir, this is exactly 11, sir. Exactly 11. So, the answer is 11. Meaning, the molarity is coming out to be exactly 11. Meaning, there is nothing to do, sir. We started the question from here. From where? We assumed that the solution is 1 liter. That is given. Density is given. Meaning, you have the mass of the solution. It has 70% solute. So, by taking 70% of the solute, we got the moles of the solute, and we directly put the volume into molarity. It came out to be 11. Is it clear? Let's talk more, sir. All of them are similar, sir. All of them are similar. If you try to do them, you will find them all similar. Look at this. What to do, sir? Look, let's use a little intelligence. It is talking about percentage weight by weight. It says I have an HCl solution which is 29.2, and its density is given. It is asking me, can you tell how much volume of this solution should be taken to prepare 200 ml of 0.4 molar HCl? Meaning, first of all, tell me, what is the molarity of this solution? And how much volume of this solution should I take to prepare 200 ml of 0.4 molar HCl? Now, this is a good question, and obviously, it is a JEE Advanced question. Why is it good? Let's think about it a little. First of all, how much volume of this solution should be taken? Meaning, which solution? That solution which is 29.2% weight by weight. How much volume of it should I take? So, one thing is clear. Whatever volume of this solution you take. Suppose I take this much volume of this solution. This solution. Okay? So, you are going to convert it into this solution. Into which solution? A solution that is 200 ml of 0.4 molar HCl solution. So, tell me, isn't this a question like, if you are going to convert it into this, it means you will add water to it. So, by adding water, the moles of solute here will be the same as the moles of solute here. Remember, the amount of solute remains fixed. This means, sir, one thing is clear, it is very easy. Now, it is very straightforward that the moles of HCl here are equal to the moles of HCl here. Meaning, the moles of HCl are equal in both places. Meaning, if I can somehow find the molarity here, then by taking its volume V, I will find the moles of solute. Here, I will find the moles of solute, and equate both of them. And this will be a good question. So, first of all, what should come is, sir, do I know how to calculate molarity from percentage weight by weight? I am talking about that solution from which I have to prepare this solution by adding water. Do you understand? So, how will the molarity of this original solution be calculated? First of all, I should know that. So, if I talk about the molarity of the original solution, what should be done to calculate the molarity of the original solution? Sir, first of all, what is given to you? I am given percentage weight by weight. And that is 29.2% weight by weight. Remember a line from English. Yes, sir, you just told me how to write 29.2? 29.2 grams of HCl in 100 grams of solution. Sir, this is a line from English, sir. How beneficial it is, sir. Seeing this, I started seeing molarity. How? Sir, from here, the moles of HCl will be obtained, and by dividing the volume of 100 grams of solution by density, the volume of the solution will be obtained. Sir, let's calculate molarity directly. Meaning, the molarity of my stock solution, the main solution, will be moles of HCl, that is 29.2 / 36.5. These are the moles of HCl. Divided by the volume of the solution. It is a 100-gram solution. The density is 1.25. So, what will be the volume? 100 / 1.25. But this will be in milliliters. To convert to liters, we will divide by 1000, and that 1000 will come on top. Sir, this is the molarity. Will someone quickly calculate and tell me what this answer will be? What is this molarity coming out to be? Calculate quickly. Meaning, if I am given percentage weight by weight and density, can I find molarity? And this is a mains level question. It is a mains level question to this extent that if percentage weight by weight is given and density is given, we can calculate the molarity. Because as soon as you write it in one line of English, you will see the moles of solute and the volume of the solution. You can calculate molarity. Tell me quickly, what will this molarity come out to be? Can anyone calculate? Calculate correctly, brother. A student is saying, sir, it is 10. Let's take this as 10 molar, sir. This is coming out to be 10 molar. Meaning, that solution, the original solution, is 10 molar. Now, it is asking, how much volume of that 10 molar solution should I take so that by adding water to it, this can be prepared? This means, sir, whatever moles of HCl are in this 10 molar solution, we will have to take some volume of the 10 molar solution. Whatever moles of HCl are in it will be equal to the moles of HCl here. Is it clear? Do you understand? Okay? So, let's calculate and see. If, suppose, this is a 10 molar solution and we take its volume as V ml. This is 10 molar, and from this, I want to prepare this, which is how many ml? Which is 200 ml of 0.4 molar HCl. Meaning, this is 200 ml of 0.4 molar. What is the concept, sir? Tell me. What concept works when diluting? Sir, only one concept works when diluting: however much solute is here, that much solute is there. And the way to find the solute is m1v1. So, 10 * v = 0.4 * 200. So, v = 0.4 * 200 / 10. Sir, this is 8 ml. Sir, this was a question asked in JEE. A student who is even a little intelligent will get this question right because here they had to use their intelligence to understand that sir, if I am given percentage weight by weight, then with the help of density, I can find the molarity of the original solution, but how to prepare that solution from it? So, if we take volume v of the solution you found, which is 10 molar, then whatever moles of HCl are here, molarity into volume. Remember, what concept was used for dilution? m1v1 = m2v2. And you have to find v1. So, the answer is m2v2 / m1. You have already calculated m1. You can see this, you have to find v. m2 and v2 are given in the question. This means, sir, now you can find the volume of the original solution. And the volume of the original solution is, the volume of the original solution is 8 ml. Meaning, the solution taken was 8 ml. Is it clear? Do you understand? Let's talk more, sir. The next discussion we need to have is. There will be many questions given to you to solve, and they will all be almost similar. All these questions will be of the same type, where we will have to find concentrations or interconvert concentrations. The next term is almost the last term of concentration terms, and that is parts concentration terms. What is this parts concentration term? Generally, it is said that parts concentration terms, listen very carefully, brother. See, it's like this, we are also trying very hard to cover everything once and give you some questions to solve so that you can strengthen yourself with those questions. Is it clear? So, once everything is understood here, solving questions will become easy for all of you. Parts concentration term means concentration terms that are defined in parts. Meaning, they say, look, parts concentration terms like parts per million or parts per billion. So, I said, brother, what does per million mean? What is the problem with per liter? We have heard per liter, we have heard per gram, we have heard per 100 grams. This per, do you understand? Per million. What is the need for this? So, generally, these concentration terms are used when the solute dissolves very little in the solvent. Meaning, the solvent is a lot, and the solute dissolves very little. So, in such cases, you have to use a concentration term, parts per million or parts per billion. So, I said, okay, how is it defined? So, the definition is very clear. Per million means in 10 raised to the power of six. Meaning, weight of solute upon weight of solution * 10 raised to the power of six. Is it clear? Weight of solution can also be written here, and in some places, weight of solvent is also written. And I think everyone will understand this themselves that because the solute is very little, the weight of the solvent and the weight of the solution are almost equal. So, weight of solute upon weight of solvent, or weight of solute upon weight of solution into 10 to the power of six is parts per million. Is it clear? Did everyone understand this? This is parts per million. In exactly the same way, parts per billion is also defined. Parts per billion means, sir, it will be used where the solute is even less, because you have multiplied by 10 to the power of 9 to make this value a little larger. Is everyone understanding my point? What did we do before? We multiplied by 100. So, what was the answer? It was percentage. Sir, but by multiplying by 100, the answer here will be negligible. The weight of the solute is so little that even if you multiply by 100, the answer will be 0.0. That's why I multiplied by 10 to the power of 9. When the solute is very little, I use parts per million or parts per billion instead of percentage concentration terms. Meaning, weight of solute upon weight of solution, or instead of weight of solution, what can be written? Weight of solvent. Why? Because, sir, the solute is so little that whether you take its weight or the weight of the solution. Both things are similar. Take the weight of the solvent or the weight of the solution. Both things are similar. Is it clear? So, whether you talk about parts per million, or parts per billion. Both things are the same. These are also concentration terms. It is a concentration term that is asked from us. So, let me show you. As far as the important thing is concerned, it will be used as I said just now. This is the concentration term. It is defined when the solute is very little. Having very less solute. If there is very little solute, then you will use this concentration term. Mass of solution and mass of solvent will be approximately equal. Sir, temperature will not have much effect on this. Why? Because, sir, it's all about mass, mass. There is no term of volume. So, this is temperature independent. And as far as the unit is concerned, sir, it is written in the form of ppm or ppb. Parts per million or parts per billion. Is it clear? Tell me quickly. Is it okay up to here? Is it okay? Let's talk more, sir. Sir, let's think of something on our own, let's use our brains. Like, for example, uh, okay, this is also a question that has opened up, so let's see what they are trying to say. They are saying, tell me quickly. The number of units which are used to express the concentration. What are those units that define concentration? Tell me quickly. Does mass percentage define concentration? Yes, sir. Does mole define concentration? No, no, sir. Mole has nothing to do with concentration. Is mole fraction used for concentration? Yes, sir. Is molarity used? Absolutely, sir. PPM, absolutely. Molality, absolutely, sir. How many are these four or five people? These five people are those who define concentration terms. Sir, mole has nothing to do with it. Is it clear? Is it clear? Do you understand? Okay. Very good, sir. Let's talk more. Let's think about it. For example, look at this. Understand it yourself. All these questions are similar. Meaning, if you do them, you will understand them all as similar. For example, look at this, what are they saying? Fortification of food. This is asked in 2025. As I have told you, I like the way questions are asked in 2025. Simply because it seems like there is something new in the way they are asked. If you look at this question this time as well, it's not like something very difficult or amazing is going to happen. But the way the question is asked is good. Fortification of food with R is done.

Using FeSO4.7H2O, okay. You have provided some information. The mass in grams of FeSO4.7H2O required to achieve 12 ppm of iron in 150 kg of wheat. To achieve 12 ppm of iron in 150 kg of wheat. Do you understand? So, can you tell me? What mass in grams of FeSO4.7H2O should be taken? Think, use your brain. Use your mind. That is, they are saying that iron is being used for the fortification of food. And where will that iron come from? Sir, that iron will come from FeSO4.7H2O. Okay? Now, what they are asking is, what mass in grams of FeSO4.7H2O should be taken? So that I can get 12 ppm iron. You understand yourself, how will you define 12 ppm of iron? What does 12 ppm of iron mean? In 150 kg of wheat. Sir, this means that if I take the weight of iron divided by the total weight and multiply by 10 raised to the power of six, it should be 12, sir. Do you understand the point? That is, weight of iron upon total weight into 10 raised to the power of 6 will be 12 ppm, this is what it means, sir. You have given the total weight, sir. From this, the weight of iron can be found. Weight of iron is equal to 12 * total weight, which is? 150 kg, meaning 150 * 10 power 3 grams. The total weight is 150 kg. So, 150 * 10 power 3 grams divided by what will come, sir? Divided by the total weight, weight of iron. The total weight has come, and below it is 10 raised to the power of six. This is the weight of iron, sir. Is it clear? Understood, sir. But I don't need the weight of iron, sir. I need the weight of FeSO4.7H2O, sir. I need its weight because the iron will come from here, sir. So, if you know the weight of iron. If you know the weight of iron, it means you know the moles of iron. The moles of iron will come from here. So, as many moles of this are there, that many moles of iron will also be there. So, it means if you know the moles of iron, you know the moles of FeSO4.7H2O. By multiplying it by the molar mass of FeSO4.7H2O, you can calculate the weight of FeSO4.7H2O. The question is good, man. That is, first you used ppm. From the use of ppm, what did you find out? Sir, first, from the use of ppm, I found out the weight of iron, which is visible in 150 kg of wheat. Sir, 12 ppm iron in 150 kg of wheat means there should be this much grams of iron. Okay? From this iron, I calculated the moles of iron. Let's see, how many moles of iron are there? Moles of iron. Sir, moles of iron are 12 * 150 / 10 power 3. These are the moles of iron. Is it clear, sir? These are the moles of iron. And as many moles of iron as there are, that many moles of FeSO4.7H2O will also be there. Why? Because sir, you will get one iron only when you get one FeSO4. This means if you want this many moles of iron, then these will be your moles of FeSO4.7H2O. And when you know its moles, you will know its weight. So, let's calculate the weight. Weight of FeSO4.7H2O is equal to how much, sir? Moles * molar mass, meaning 12 * 150 divided by 10 to the power of 3 * can anyone tell what the molar mass of FeSO4 will be? Sir, FeSO4 will be 56 + 32, O4 is 64, and 7H2O means 18 * 7. 8 * 7 = 56. 7 * 1 = 7, 5, 2. Sir, this is the total weight of FeSO4. Just add it up quickly and tell me what the total weight is? 56 + 32 + 64 + 126 = 278. Sir, this is the total weight, 278. That is, you multiplied by 278. Let's solve this. So, how much will this be? Now this will be 12 * 150 * 278 / 1000. Approximately 500. Let's see it once, understand it yourself, what are they trying to do? If only the weight of iron FeSO4 is to be calculated, then the weight of FeSO4 can be calculated like this, directly multiplied by the moles that are coming. Have I made a mistake somewhere here? Is there a mistake here? Oh, there's a mistake here. Weight of iron, something is wrong. 10 raised to the power of 3 moles of iron. One second, let's look at the question again. Is the formation correct or not? Let's check it quickly. Is there some calculation error here, man? Let's check once. Oh, this is the weight for moles. I made a mistake. I didn't divide by 56. Here it should be divided by 56. So, the term 56 should also come in the answer, right? Am I doing it correctly? If my weight is so much, then for moles, I should divide by 56. So, according to me, the answer will be divided by 56. What else will happen? Divide the answer by 56. Let's do it like this. So, if the answer I am getting is divided by 56. 8.93. 8.93 grams. Now it's correct. So, the nearest integer will be nine. Now, understand this. The question asked, the answer is nine. Is it correct? I didn't pay attention. This is moles, this is weight. So, to find moles after weight, you have to divide by the molar mass of iron. So, I didn't divide by 56. But anyway, now, understand this. Doesn't this question seem like how will they do it? That is, how good is the link that first you asked to find the weight from parts per million, which you have asked before. This is a direct formula, sir. Weight of iron upon total weight * 10 raised to the power of 6 = ppm. Sir, from this, the weight of iron will come. The portion after that is good, sir. From that, I have to find its moles, sir. So, first, from the weight of iron, the moles of iron came, and as many moles of iron as there are, that many moles of FeSO4.7H2O will also be there because one mole of FeSO4 gives one mole of iron. This means, sir, from this, I know this many moles of FeSO4.7H2O, and if you want its mass, you can calculate the weight of FeSO4.7H2O by multiplying it by its molar mass. That is, if you use 8.93 grams of FeSO4.7H2O, you will get 12 ppm iron in 150 grams of wheat. Clear? Tell me quickly. Did you enjoy the question? Is it clear? Did everyone understand? And you are seeing the level, this seems like a good question for 2025, man. I like this question because it will be difficult for the child to link from here that sir, the weight of iron has come. Now what to do? Many children will write this itself as the answer, that whatever weight is coming out, that will be the answer. 12 * 150, meaning 180 / how much? 1.8. 1.8 grams is the answer. Whereas this is wrong. This is wrong. 1.8 is not the answer. Because this is the weight of iron. We need the weight of this salt. To find the weight of this salt, as many moles of iron are here, that many moles of FeSO4 will also be there. Only then will the answer come out. Is it clear? Did everyone understand, man? No, man, don't talk about breaks. First, we will finish the concentration terms. We will start the vapor pressure of solutions. Then we will think about breaks. We are not talking about breaks or anything now. Okay, let's talk more. So, you have to solve this a bit more according to your own understanding, right? Solve this further. Now, let's talk about the next concentration term. Strength is a very simple concentration term. A very simple concentration term. What is it? Strength. Although I have seen that JEE has asked very few questions related to strength. Therefore, I will not hesitate at all while writing this that this can become a very important part of concentration terms for JEE. That is, in JEE 2026, it is highly expected that they will talk about concentration terms related to strength. So, we just need to know about strength in concentration terms. So, if I talk about strength, then strength means the amount of solute dissolved in 1 liter of solution. Oh sir, this is also molarity. Amount of solute dissolved. But this amount is taken in grams. Do you understand? There, that amount is taken in moles. This amount is our weight. That is, if you want to define strength, then weight of solute divided by volume of solution. What was there in molarity? Moles of solute divided by volume of solution. Is everyone understanding me? That is, strength and molarity are interconverted. Why? Because sir, they are interconverted because if you convert the weight of solute into moles here, you will know the molarity. And as far as the unit is concerned, you can see it. Above is grams, below is liters. So, generally, the unit is defined as grams per liter. And it must have temperature dependence. Because sir, the volume is at the bottom. Now, see, the same thing is coming again. The question that was asked last year regarding molarity, that temperature change one, the same question can be asked regarding strength. Same. And here too, the answer will be the same. Why? Because sir, as far as volume is concerned, if you are moving from 0 degrees, then in the case of 0 to 4 degrees, your volume or strength will decrease. Sorry, it will increase because the volume is decreasing. And sir, after that, your strength will keep decreasing. Just like molarity. Understand? So, it is possible that this year they might ask us a question related to strength and temperature. But definitely keep in mind that the question asked related to strength and temperature, the question asked related to strength and temperature will start from 0 degrees. That is, 0, 1, 2, 3, 4, 5, 6, and so on. So, in such a case, sir, from zero to four, the strength is increasing. But then your strength will start falling. The maximum strength will be seen at 4 degrees. Tell me, is everyone understanding me? So, it is possible that in our next exam, they will talk about strength and temperature. Okay? So, everyone will pay attention to this. What is the second thing? Sir, strength can also be defined in one line in English. When you yourself say that weight upon solute, weight of solute upon volume of solution is strength. So, you can write one line in English. Suppose if you are told that the strength of the solution is 'a' grams per liter. How will you define this? So, you can define your one line. 'a' grams of solute in 1 liter of solution. You can define your one line. What is the benefit of this? The benefit will be that you will see the mass of the solute. From here, you will get the weight of the solute. And from the weight of the solute, you will know the moles. And by writing this, you have known the volume of the solution. Volume of solution. So, from here, moles will come. This is the volume, so you can directly calculate what? Molarity. That is, what can be directly calculated from strength? Molarity. Are you understanding me? JEE has also asked a question related to this once. I will show you. Related to strength, look here. No, look here, this question is very straightforward and a very beautiful question, a very lovely question. Those students who have studied strength very little, because they generally think about molarity, molarity, mole fraction, percentage concentration terms, at most ppm, ppp, that's it. But strength is a neglected, untouched concentration term on which they have asked few questions. They might ask you questions related to strength in the coming years. As they asked here. Look what it is saying. It is saying that the strength is given to you in blood. The concentration of glucose is given in this form. Now, tell me, what do you see from this? Gram per liter. Sir, gram per liter is the concentration. So, that means this is what? Sir, this is strength, sir. If it is gram per liter, then this is the given strength. Now, how will you do the question, sir? Sir, strength is given, molarity is asked. So, it means, sir, I will write one line in English. 72 grams of glucose in 1 liter of blood. That's it, sir. There will be 0.72 grams of glucose in 1 liter of blood. Now, what do you need to find? Sir, I need molarity. So, how will molarity come? Molarity is equal to moles of glucose. How will they be calculated? 72 / molar mass of glucose divided by sir, the volume of blood at the bottom, which is assumed to be 1 liter. Sir, this is the molarity of the solution. That is, you can calculate the molarity of that blood from here. As soon as you write one line, you will understand. Are you understanding me? And I think everyone will agree, sir, this will be 0.004 something, right? This is 0.004 molar. So, it will be 4 * 10 raised to the power of -3. Clear? There was nothing. What was needed, sir? Just write that one line in English, and it will be fun. Sir, this line you have written. From this, I understood the whole system. One line in English. From this, I understood the whole system that as soon as I write this line, I see the weight of glucose and the volume of the solution. I need molarity. What is needed in molarity? Moles. If the weight is visible, moles will come. And the volume is already given as one. Sir, put it directly into the formula. Molarity will come out. That is, questions linking strength and molarity can be asked. Second thing, sir, if the density of blood is given in this question, then any concentration term can be asked. Sir, as soon as density is given, you assumed volume as 1 liter, density is given, so you will get the mass of blood. Sir, subtract the mass of glucose from the mass of blood, then the mass of the solvent. Are you understanding me? The whole picture will become clear, sir. If you want to convert any concentration term into any concentration term, then just provide me with the density of the solution, and I can interconvert because I know how to write that one line, sir. As soon as I write one line, I will start thinking about what I need to do to find what I need. So, as soon as you write one line, half the problem is solved at a glance, and the remaining problem can be solved by using density or something, adding and subtracting masses, and directly putting it into the formula. So, those children who want to understand these concentration terms can understand them in a very simple way. The last concentration term that I will discuss here is formality, which I should not discuss, because no question is asked on formality in JEE. There is a reason for it. I will write just one line, and you will understand it yourself. Molarity is actually formality. That's it. That is, whatever molarity is, that is formality. The only difference is that the word formality is used for ionic solutes. For solutes that are ionic compounds, NaCl, CaCl2, MgCl2, which are ionic compounds, you can use formality instead of molarity. Otherwise, molarity and formality are both the same. The formula used for molarity is the same formula used for formality. What came at the top for molarity, sir? Moles of solute. What will we write here, sir? Moles of or number of gram formula mass. This gram formula mass is actually moles. How it will be calculated, look. Mass upon formula mass. The only difference is, sir, because formula units are defined for ionic compounds. So, just as we write moles above, we write gram formula mass here. And to find gram formula mass, we divide the given mass by the formula mass. That is, these are actually moles. Look carefully, these are moles, and formula mass is molar mass. Exactly the same. That is, what I mean to say is, sir, you do not need to study formality separately. If you are using it for ionic solutes, then consider formality and molarity similar for ionic solutes. You don't need to do anything new or different. Is it clear? Understood this? That is, if someone, you also did a question. I remember 9.85 or 5.85, which we did at the beginning. If you look carefully, there was a question with 5.85. It came at the very beginning. You can consider this as formality. Here it is. This is exactly what we asked. In this, "The molarity". I can also write formality here instead of molarity. Why? Because the ionic solute is NaCl, sir. NaCl is ionic. So, if you ask formality in this question, the answer will be the same. The only difference will be. Instead of M, it will be F. That's it. That is, the answer should be 0.2F. Done. Just do this. Are you understanding me? So, what I want to say is that just as molarity is calculated, formality is also calculated. It has never been asked in JEE, but still, we should know. Formality is defined for ionic solutes instead of molarity. Now, the last one remaining is normality. Normality will be taught in redox because the concept of equivalents is used in normality. And that concept of equivalents is done when we do redox. Therefore, normality is the last concentration term that we will cover in the redox chapter in the next lecture. So, all our concentration terms have been discussed. We should know the definition of all concentration terms. We should know how to write all concentration terms in English, and we should understand them from the heart. After that, there will be no question related to concentration terms that you cannot do. Tell me quickly, are all these discussions about concentration terms clear to you? Absolutely, this lecture that we invested 3 hours in, are the concentration terms now completely clear to you? Tell me quickly, man. Is this clear? Excellent. So, what we were discussing was about concentration terms. Although all those things will continue to be used here as well. But now, let's start discussing something else. Just as we discussed these properties or these points of solutions, how their concentrations are defined, how those concentrations are linked together. Now, let's discuss a bit further that solutions have some other properties. Like what is their vapor pressure? How are the boiling points of those solutions calculated? How is their freezing point calculated? How is the osmotic pressure of solutions calculated? So, let's discuss some more properties. First, we will discuss the pure liquid, what does the vapor pressure of a pure liquid mean? Let's discuss this a bit first. It's an easy discussion. First, let's discuss this point: if I talk about the vapor pressure of a pure liquid, what does it mean? So, look, it's very easy. Very simple. The liquid you have, this is pure liquid. I am not talking about solutions, man.

We are currently discussing the vapor pressure of pure liquids. Regarding pure liquids, it is said that in a pure liquid, some particles are inside, and some particles are on the surface. The particles inside are called bulk particles, and the particles on the surface are called surface particles. There is a significant difference between these two types of particles.

The particles found in the bulk are stable, meaning the forces acting on them from all sides are equal. The forces from here, the forces from there, the attraction from here, the attraction from there – all these forces are equal to each other. That is, particles within the bulk are of lower energy, stable, and in equilibrium because all the forces acting on them are balanced. However, the particle on the surface, understand this, the particle on the surface is unstable. It is not in equilibrium; it is of high energy. Do you understand? This means that the particles on the surface are unstable because all the forces acting on them are not balanced. Their energy is higher, and therefore, they can leave the surface.

This logic suggests that whenever a liquid is taken in a closed container, the molecules on its surface continuously leave the surface and escape, and they also condense back. Do you understand what I am saying? This means that the particles on the surface have very high energy and are unstable. So, they keep leaving the surface. Because of this, a portion of vapors starts accumulating above the liquid. And this portion of vapors, at one point, starts exerting a pressure, which is called the vapor pressure of that liquid.

So, everyone try to understand this: if I am talking about the vapor pressure of a liquid, it means that the particles on the surface of the liquid are unstable. They have high energy. They are not in equilibrium. They leave the surface. They go up and then condense. This process of evaporation and condensation continues.

To begin with, the rate of evaporation is very high. The rate of condensation is zero. Why? Because if no one is up there, what will condense? Right? As people start accumulating above, the rate of settling from above, which you call condensation, starts increasing. So, initially, the rate of evaporation is high, and the rate of condensation is low. Gradually, the rate of evaporation decreases, and the rate of condensation increases. A point comes when the rate of evaporation and the rate of condensation become equal. At that point, these vapors, the vapors forming above the liquid surface, and the liquid attain an equilibrium.

So, everyone will understand this. Because this is the most important point regarding vapor pressure. When do you define vapor pressure? We define vapor pressure when equilibrium is established between the liquid and the vapor. At that time, the pressure exerted by the vapors in all directions, or on the surface of the liquid, is called the vapor pressure of that liquid at that particular temperature. So, everyone keep this in mind, and this is the definition I wanted to convey.

"The pressure exerted by the vapors which are in equilibrium with the liquid is called the vapor pressure of that liquid at a particular temperature." Did everyone understand this point? This means if you take a pure liquid, after some time, the pure liquid attains equilibrium with the vapors above it. And at that equilibrium, whatever the pressure of the vapors is, that is called the vapor pressure of that liquid at that particular temperature. Does this make one thing clear? That vapor pressure will be defined only when the liquid and vapor form an equilibrium. Is this point clear? Did everyone understand this point? So, one thing is clear: an equilibrium between the liquid and vapor will form. At that time, whatever the pressure of the vapors will be, it will be called vapor pressure. If equilibrium is not formed, then you will not call the pressure of the vapors, vapor pressure.

So, when is vapor pressure defined? Vapor pressure is defined when the liquid and vapor come to equilibrium at a particular temperature. At that time, whatever the pressure of the vapors is, it is called the vapor pressure of that liquid at that temperature. Is everything clear up to here? Did everyone understand this point? Okay, this is it.

Now, sir, there is a very beautiful aspect to this. What is it? The beautiful aspect is that, sir, if you look carefully, you are saying that the liquid and vapor are in equilibrium. Yes, absolutely, that's what I'm saying. The liquid and vapor must come into equilibrium. So, sir, do you understand that this equilibrium will have its own equilibrium constant, whose value will be equal to the pressure of the vapors? Sir, when equilibrium is reached, whatever the pressure of the vapors will be, sir, it will be equal to KP, because liquid is not included in the expression for KP.

What does this mean, sir? It is clear that the vapor pressure is indirectly equal to what? Equal to KP. And do you know what the good thing is? KP is only temperature-dependent. KP depends only on temperature. And if KP depends only on temperature, then the vapor pressure of a liquid depends only on temperature. It depends only on temperature. Did everyone understand what I said? This is very important information. Many children do not understand why the vapor pressure of a liquid depends only on temperature. This is because the vapor pressure of the liquid is equal to KP. If I call the equilibrium constant of this equilibrium KP, how is it defined? Do you remember KP? KP means writing only the pressure. So, whatever the pressure of the vapors will be, and the pressure of the liquid is not there. This means, sir, whatever KP will be, it will be equal to the pressure of the vapors only, and KP depends on temperature. Therefore, the pressure of the vapors will also be temperature-dependent at equilibrium. If the temperature is constant, then the vapor pressure of that liquid is fixed. End of story.

This means the liquid is fixed. If equilibrium is established, then the vapor pressure is fixed. Why? Because vapor pressure depends only on what? Vapor pressure depends only on the temperature of the liquid. If the temperature is constant, then the vapor pressure is constant. Tell me, is this point clear to everyone? Tell me, is this point clear to everyone? So, what we discussed in the last 10 minutes was that the vapor pressure of a liquid depends only on temperature. If the temperature changes, the vapor pressure of the liquid will change. If the temperature does not change, the vapor pressure of the liquid will not change. Why? Because the vapor pressure of the liquid is equal to KP. Is everything clear up to here?

Okay, now let's talk about something else. What is the second point? What is the second important piece of information? The second important piece of information is that, sir, I have heard that if at temperature T1, the value of K is KPT1, and at temperature T2, the value of the equilibrium constant is KPT2, then I was taught an expression in chemical equilibrium: log of KPT2 / KPT1 = deltaH / 2.303r * (1/t1 - 1/t2). Sir, this expression was taught to link the values of K at two different temperatures. But you just said that KP is equal to vapor pressure. So, this means that the vapor pressure at temperature T2 and the vapor pressure at temperature T1 will be linked by this equation. Sir, this is amazing!

So, log (vapor pressure at T2 temperature / vapor pressure at T1 temperature) = deltaH / 2.303r * (1/T1 - 1/T2). So, if someone ever tries to ask you a question like, "Can you tell me the vapor pressure at two different temperatures?" No, this is a wrong question. A child is trying to know from me, "What is KP?" KP is the equilibrium constant, which is written in terms of pressure. And only gases have pressure. So, I only wrote the pressure of what? Of the vapors. This means, sir, if you are defining KP here, then KP = pressure of vapors only, and KP depends on temperature. Therefore, the pressure of vapors also depends only on temperature. The first point is done.

Okay, if it depends on temperature, then how does it depend? KP depends on temperature in this way. So, because KP is equal to pressure, you can write vapor pressure at T2 instead of KP T2, and vapor pressure at T1 instead of KP T1. From here, you can also link the vapor pressure at temperature T1 with the vapor pressure at temperature T2.

Okay, now I come to the Mains level. What is the level? The Mains level is that from here, I understand that vapor pressure depends only on temperature, exponentially. Exponentially, meaning vapor pressure depends on temperature. You have understood this. How does it depend, sir? It depends exponentially. You see this logarithmic expression. This means the relationship of vapor pressure with temperature is an exponential relationship. What does this tell us, sir? If you change the temperature, the vapor pressure will increase, sir. If the temperature increases, the vapor pressure will increase, and it will increase so much that you cannot even imagine. This means an exponential change. What does exponential change mean? A big change. A big change. So, one thing is clear. If the temperature changes, the vapor pressure will change. And you can use your own logic, sir. Increasing the temperature will cause more liquid to evaporate. And if more liquid evaporates, then sir, the vapor pressure will be higher, and it will be much higher because vapor pressure depends exponentially on temperature. Is everyone understanding what I'm saying?

I will tell you a myth here. Many people think that vapor pressure depends on temperature in this way: "Vapor pressure increases on increasing temperature." True or false? Sir, everyone knows that if you increase the temperature, more vapor will form, and if more vapor forms, the vapor pressure will increase. Absolutely correct. This statement is correct. "Vapor pressure depends linearly on temperature." This is wrong, sir. This statement is wrong because vapor pressure does not depend linearly. It depends exponentially. Exponentially. This means vapor pressure depends on temperature exponentially. What does linear mean, sir? Sir, linear means if the temperature increases, the vapor pressure will increase. This is vapor pressure, and this is temperature. This is linear variation. But actually, it is not a linear variation, sir. It is an exponential variation. And only a child who knows this will be able to answer this question correctly in JEE.

For example, here too. Some children say, "Sir, pressure is obviously directly proportional to temperature." If you increase the temperature of any gas, the pressure will increase. Absolutely correct. But according to them, if you double the temperature, the pressure will double. Sir, I agree that pressure increases with increasing temperature, and vapor pressure also increases. But sir, you cannot calculate vapor pressure from this expression, sir. If you want to calculate vapor pressure, you can calculate it from the exponential relationship. The relationship of pressure with temperature is such that if temperature increases, pressure increases. But you cannot calculate pressure this way for vapor pressure because vapor pressure does not depend linearly on temperature. First point.

Second point. This simple diagram I have drawn is only to explain why vapor pressure increases on increasing temperature. Everyone knows, sir, if you increase the temperature, first of all, the velocity of people, the molecules, will increase, so people will leave the surface more and more. So, initially, if only this fraction of people had energy greater than E (meaning the energy required to leave the surface), then when you increase the temperature, the fraction that comes out increases, sir. This is the fraction of people who will leave the surface and run away. And if you increase the temperature, this fraction increases further. I am not trying to teach you this graph here, nor am I trying to make you memorize it. I just want to convey that I, or books, have this explanation for why vapor pressure increases on increasing temperature. The explanation is that on increasing the temperature, many people start leaving the surface, due to which the vapor pressure increases. Is it clear? But the important thing is that its dependence on temperature is not linear dependence. Its dependence on temperature is exponential dependence. Did everyone understand what I said? Is everyone understanding this point? Is this logic understandable that if you increase the temperature, more molecules will start leaving the surface because the velocity of the molecules will increase? If the velocity of the molecules increases, then the number of people crossing a particular energy and escaping will increase. Is it clear? So, if the fraction of people escaping is increasing, it means more people are accumulating, and if more people accumulate, then the vapor pressure will also increase. But sir, will it increase linearly? No, it will increase exponentially. This is the reason I am telling you this. And if this question is asked in JEE 2026, you will understand that many fools will get this question wrong because they only know that pressure is = nrt / v, doubling the temperature doubles the pressure. In any case, yes, a learned person will not tick this answer. Why? Sir, the temperature is increasing, and the vapor pressure is constant. What nonsense is this? This is wrong, sir. The temperature is increasing, the vapor pressure is increasing. This is correct. Why? Sir, the temperature is increasing, and the vapor pressure is increasing. But what is this dependence, sir? This is linear dependence, sir. This is linear dependence. And sir, this is completely wrong. The temperature is increasing, and the vapor pressure is decreasing. This cannot happen. Sir, only this is correct because with increasing temperature, vapor pressure increases exponentially. This is exponential increase. And if this is an exponential increase, then sir, this answer will be correct. Did everyone understand what I said? Did everyone understand this point?

So, what I wanted to tell you is that first, there should be clarity on what vapor pressure is. Second, clarity is needed that equilibrium is necessary when defining vapor pressure, and if there is equilibrium, then vapor pressure is equal to KP, and KP depends on temperature. This means vapor pressure also depends on temperature. KP depends exponentially on temperature. Therefore, vapor pressure also depends exponentially on temperature. Increasing the temperature increases the vapor pressure very rapidly. The reason for this is that many people start leaving the surface, which causes the vapor pressure to increase. And along with this, we must remember this graph. Is everything okay up to here? Is the point up to here clear? Okay, this point? Okay.

Let's talk further, sir. Let's come to the next point. The next point that is emerging is what I just said. "Vapor pressure of a pure liquid is only temperature dependent, irrespective of the amount of the liquid and shape of the container. Vapor pressure is constant at a particular temperature." If the temperature is constant, then no matter what the container is, no matter what the amount of liquid is taken, if equilibrium is formed, then the vapor pressure is fixed. Why? Because if equilibrium is formed, the vapor pressure will be equal to KP. And KP will depend only on what? Temperature. So, if the temperature is constant, then KP is fixed. KP is fixed, so vapor pressure is fixed. This means it doesn't matter to me whether more water is kept or less water is kept. If equilibrium is established and the temperature is common, then the vapor pressure is common. End of story.

So, vapor pressure depends only on what? On temperature. The vapor pressure of any pure liquid is only temperature-dependent. You can only change the vapor pressure by changing the temperature. Okay? Third point, sir. Third point is, take at least enough liquid so that equilibrium can be formed. It should not happen that the liquid evaporates completely before reaching that pressure. This means, to reach KP, you need to take a sufficient amount of liquid. If you take very little water, all the liquid will evaporate. Sir, equilibrium will not be established, and then you will not talk about vapor pressure. This means, take at least enough amount of a liquid so that equilibrium can be formed. After that, do whatever you want. Whether you take more liquid, whether you take a larger container, whether you take a smaller container. It makes no difference to me. If the temperature is constant, the vapor pressure is constant.

Next point: Vapor pressure depends exponentially on temperature and can be calculated using this expression. Clear? Quickly tell me, did you understand up to here? Chaitanya, exponential means a very big change. Sometimes you hear it said about someone, "They are experiencing exponential growth." Exponential growth means growing very rapidly. So, what is meant is that the same thing is said about vapor pressure because vapor pressure is KP, and KP is exponentially temperature-dependent, so vapor pressure also depends exponentially. This means if the temperature increases, the vapor pressure will increase, but it will increase very rapidly. It will not increase linearly. It will increase very rapidly. Did everyone understand what I said? Okay? And if you have understood this, then here is a question that will be asked in JEE 2026, and most children will get it wrong. Many children will get this question wrong. Just think about it. Here the temperature is 300 K, and the pressure of vapors is 1.2. Here the temperature is 400 K, so what will be the pressure of vapors? Sir, one thing is clear. The answer that comes will be greater than 1.2. Do you agree or not? It should be greater than 1.2 atm. Why? Because sir, the temperature is increasing. If the temperature increases, the vapor pressure will increase. Clear? So, this means the answer cannot be 1.1. The answer cannot be 1.2. Now, either the answer is 1.6 or the answer is 1.8. Sir, how will I decide, sir? Will the answer be 1.6 or 1. Both values are greater than 1.2.

Now let's think, and let's think very beautifully. No child can answer this question because they cannot think that much. And this question will be asked in 2026. So, very few children will be able to do this question. Many children understand that the answer can never be C and D, but the answer could be 1.6 or 1.8. You have to decide which of these two should be the answer. Now let's think. Tell me, if I say that P is directly proportional to T, meaning if temperature increases, pressure increases. Okay? If it were linearly dependent, would you understand that the value of P1 / T1 would be equal to P2 / T2? This means P / T should be constant. P is directly proportional to T means P / T is constant. And if P / T is constant, it means P1 / T1 = P2 / T2. So, if I find P2 from here, tell me, what will be the value of P2? Here.

If you calculate P2, it comes out as P12 / t1. What is P1? 1.2. The value of t2 is 400 and what is the value of t1? 300. Sir, if I solve this, what value will come out, sir? It will be 1.6 atm. This means P2 will be 1.6 only when pressure has a linear relationship with temperature. That is, if P is directly proportional to T linearly, then the new pressure will be 1.6. But you said it increases exponentially. This means, sir, 1.6 is also not correct. The answer should be 1.8. Tell me, did you understand my point? Quickly tell me how many people understood this, and everyone should also understand this. We are discussing this at a very different, good level. We are trying to understand a very small thing a lot. Because what is expected is visible to me, and whoever is intelligent will understand that sir, we remembered that vapor pressure means the pressure exerted by the vapor when equilibrium is formed between liquid and vapor. But all these things about it, that vapor pressure depends on temperature. How it depends. How much does vapor pressure increase when temperature increases? All these things, sir, I am understanding now. Quickly tell me, is this clear? Yes, it is possible that a child might ask, sir, how will 1.8 come? Look, this is a wrong question. This question is wrong because now I don't know how 1.8 is calculated. That will be calculated with the help of KP. We need to know the KP at 400 Kelvin. And the formula to calculate that KP, which you just wrote, log KP2 / KP, meaning here the vapor pressure and here the vapor pressure, and using these two temperatures, you can calculate the vapor pressure. If I know the delta H value, meaning the delta H of vaporization from liquid, if that is known. But he hasn't given that much information. So in such a situation, sir, there is only one way. The first and fourth options are incorrect anyway. 1.6 could have come. But that would have happened if there was a linear relation. So it means the answer will be greater than 1.6, and only one option remains. We will tick option C. Tell me, did you understand my point? Is everyone understanding this point? This is important. So everyone should definitely understand this, brother, and this is important. Let's talk further, sir. So this means, okay, that vapor pressure, if you are talking about a particular liquid, then the vapor pressure of a particular liquid is temperature-dependent. Because vapor pressure is equal to KP, and KP depends on temperature. To calculate vapor pressure at different temperatures, we can use that logarithmic expression. Okay? But it can become an advanced level question. At the mains level, it is as important for us to use that logarithmic expression as it is to know that vapor pressure depends exponentially on temperature. That is, if it increases, it will increase like this. Is it clear up to here? Okay, sir. Now let's come to the second part. Sir, just as you are talking about one liquid, similarly, if I talk about the vapor pressures of two different liquids, taking the same temperature. I said, what do you mean, sir? You are saying there are two different liquids, sir. You just said that if only one liquid is taken, its vapor pressure will depend only on what? Temperature. If the temperature increases, the vapor pressure will increase. Do you understand? But sir, if I take two different types of liquids and take the same temperature for both, will their vapor pressures be the same, sir? Because you were saying that vapor pressure depends only on temperature. No, no. The vapor pressure of any one liquid depends on its temperature. But if you take two liquids, they are two different liquids. The equilibrium values of both those liquids will be different, so their vapor pressures will also be different. Absolutely correct. So, sir, what will they depend on, sir? How do we decide how to compare the vapor pressures of two different liquids? So, look, you can use your own intelligence, and all the children will understand. More the force of attraction between molecules of liquid, lesser will be the tendency of the molecules to leave the surface, lesser will be the vapor pressure. Tell me, did you understand the logic, sir? If you take two different liquids, and in those two different liquids, the liquid with more molecular interactions will make it difficult for the molecules to leave the surface and go up, sir. Because the molecules hold each other. In such a case, the liquid with more molecular interactions will be difficult to convert into vapor. Its vapor pressure will be considered less. And the liquid with less intermolecular forces of attraction, it will be easier for their molecules to go into vapor. Its vapor pressure will be higher. That is, if you talk about two different liquids, temperature is one factor, sir. With increasing temperature, vapor pressure increases, sir. That's a separate matter. But even if the temperature is common, the vapor pressures of two liquids will depend on their forces of attraction. And there is no doubt, sir, that if you try to write this in one line, I can write it in one line. Vapor pressure is inversely proportional to the force of or intermolecular force of attraction. Intermolecular force. Do you agree with this? The more the inverse, understand, one upon, understand, one upon intermolecular force of attraction factor, the higher it is, the lower the vapor pressure will be considered. So vapor pressure is inversely proportional to intermolecular force of attraction factor. Is it clear up to here? Did everyone understand this? Okay? If we talk about what is important for us, in inorganic chemistry, you study many forces like London forces, dipole-dipole interactions, induced dipole interactions. If I talk about what is important for us, then these three forces are most important for me that I need to remember, which are related to this chapter. If hydrogen bonding is involved between molecules, then it will be considered the strongest interaction. Although the strongest interaction is ion-ion interactions. But we are talking about our liquids now. There are no ions in liquids. So this means, sir, if we talk at our level, if there is hydrogen bonding between molecules in a liquid, it will be considered the strongest. After that, dipole-dipole interaction, which is weaker. That is, if a molecule is polar. For example, let's talk. Hydrogen bonding means that if, suppose, I tell you that I have H2O. I have H2O. Suppose I have CH3COCH3, let's assume, and suppose I have CS2. These are three liquids I have. He wants to know from me. These three liquids are taken at temperature T. All three are at temperature T. Okay? Now tell me, how will you decide the vapor pressure of all three? So some fools think that since the temperature of all three is the same, the vapor pressure will be the same. Sir told that same temperature, same vapor pressure. Oh brother, I was talking about a single liquid. The vapor pressure of any single liquid remains the same if the temperature is the same, whether there is less liquid or more liquid, it doesn't matter to me. Clear? But here are three different liquids. And the vapor pressure of three different liquids will be decided by their intermolecular interactions. Now, if I look closely at H2O, you have read many times in organic and inorganic chemistry. Water molecules have a special characteristic that they are hydrogen-bonded to each other. That is, what kind of forces of attraction are seen in water molecules? In water molecules, HBA interactions are seen, which are called hydrogen bonding. Okay. What about acetone? I said, look, if I look closely at acetone, acetone is a polar molecule. If you look closely, there will be a delta negative charge on oxygen. There will be a delta positive charge on carbon. Exactly in the same way, if I take another molecule of acetone, I think everyone will understand this. This is delta negative and this is delta positive. So everyone agrees that sir, acetone has partial positive and partial negative charges. So, sir, this is a polar molecule, and the interactions between any polar molecules are known as dipole-dipole interactions. Sir, this is a dipole plus minus plus minus. So dipoles will interact with each other, but dipole-dipole interaction is weaker than hydrogen bonding. That is, acetone molecules, because acetone is a polar molecule, will show dipole-dipole interactions with each other, but it will be considered weaker with respect to hydrogen bonds. Clear, sir? Now let's come to CS2. Sir, if I look closely at CS2, CS2 is linear, sir. If you look closely, CS2 has a linear structure and a linear structure is non-polar, sir. This is a non-polar molecule. And in non-polar molecules, sir, only one thing works. And that is, due to their bulk, due to their mass, whatever attractions are between the molecules, and that attraction is given the name of van der Waals interactions. We are not talking about inorganic chemistry. We are just trying to explain that non-polar molecules can have van der Waals interactions, polar molecules can have dipole-dipole interactions, and water has hydrogen bonding. Therefore, the vapor pressure of water, vapor pressure of H2O, will be the least, vapor pressure of acetone, and the highest vapor pressure will be seen for CS2. Tell me, did everyone understand my point? Is this clear to everyone? Is this point understandable? That is, sir, okay. Now, if the temperature is common, then the vapor pressures of different liquids will depend on molecular interactions, sir. And if you have more molecular interactions, then sir, the molecules will remain bound, they will not convert into vapor. And if they are not converting into vapor, then the vapor pressure is wasted, sir. So, what is important for us in this chapter, if I talk about it, then it is most important for me to concentrate on three types of forces. Hydrogen bonding, dipole-dipole interactions, and van der Waals interactions. And their sequence is also this. Hydrogen bonding is the strongest. Dipole-dipole is weaker than this. And the worst force is van der Waals forces. Is this point clear? Tell me quickly. Is the point up to here clear? Okay? Shall we move forward? Okay, sir. Very good. So I also understood this point, how to compare the vapor pressures of two different liquids. Okay, sir. Now let's quickly talk about this as well. What do you want to get done with this? I have been told that we made a beautiful question in 2020. It was beautiful as a question, but they made the question only so that the child would think that such things are not taught to us. But whoever is intelligent understands everything. All the things I have told you should be clear to you. Sir, it is clearly visible here that the link of vapor pressure is being asked with temperature. What I see is that if you draw a line of fixed vapor pressure. This is a fixed vapor pressure, sir. So, for whose person is the fixed vapor pressure reaching at the lowest temperature? Check and tell me, sir. The lowest temperature is 293, sir. That is, x is at the lowest temperature, and its vapor pressure is three, what is it? 800 mmHg, sir. To get this same 800, y has to be heated more, sir. And to get this same 800, Z has to be heated even more. That is, Z has to be heated the most so that its vapor pressure can reach 800. What does this mean, sir? It means Z doesn't want to evaporate, sir. Z's molecules are bound, sir. They don't want to evaporate. Only when you heat it will they start evaporating. That means Z has the most interactions. And the least interactions are in X's molecules. Tell me, are you understanding my point? This means if you want to know from me that X has higher intermolecular, absolutely wrong, sir. X cannot have higher intermolecular interaction, sir. Z has lower, impossible, sir. Z is showing maximum interaction, sir. X will have the least interaction, sir. Less than Y and less than Z. That is, among all these, the correct answer should be B, meaning A answer, in which it is said that our X shows the least interaction because its molecules are evaporating at the lowest temperature and achieving a particular vapor pressure. Clear. Harshit Chauhan is saying, sir, I didn't understand. Harshit, try to understand, brother. If it were chemistry, I would agree that there is something to understand. Oh brother, when you understand, there is a liquid, it has to evaporate, it has to convert into vapor, so if the liquid molecules are bound, how will they convert into vapor? This means the more bound the molecules are, the lower the vapor pressure will be. Clear. Here, if you look closely, a particular vapor pressure of 800 is coming for Z at this temperature, 333 temperature. That is, you have to keep the highest temperature to reach Z to 800. And here at 293, X reaches 800. That is, sir, at low temperature, it is 800, and at high temperature, it reaches 800. So it means, sir, Z has very high molecular interactions. Z has high molecular interactions, because of which you are heating it more so that they evaporate and create a pressure of 800. Now do you understand my point? Did everyone understand? Okay, sir. Very good. Very good, sir. Let's talk about the next one. Here you go, sir. Let's finish with one more quick nonsense. Compare the vapor pressure of chloroform and H2O. Sir, the world knows that chloroform is a polar molecule, sir. This is a polar molecule. And if it is a polar molecule, then dipole-dipole interactions are seen in it. And as far as water is concerned, the world knows. Water has hydrogen bonding. This means water's interactions are strong. So the vapor pressure of water will be less. Vapor pressure of water is less than vapor pressure of chloroform at the same temperature. If you increase the temperature of water, its vapor pressure can be higher than chloroform. But keep chloroform lower. Understand the point? If the temperatures of both are the same, then the vapor pressure of water will always be less. But if it happens that chloroform says, to hell with you. Now I am increasing the temperature of water. So if I am increasing the temperature of water, its vapor pressure will increase. It might exceed chloroform. That is, the vapor pressure of water at a higher temperature can be equal to the vapor pressure of chloroform at a lower temperature. Did everyone understand my point? That is, it was very easy for chloroform and this. Okay, up to here. That is, what needed to be discussed is this. What is a pure liquid? What is the vapor pressure of a pure liquid? Why does it depend on temperature? How does it depend? How are the vapor pressures of two different liquids compared? On what factors do they depend? All these things have been discussed. Now let's come to adding a solute to a liquid to make a solution. That is, now I will talk about the vapor pressure of solutions. Quickly tell me, is it clear up to here for everyone? Look, because I have to do many things, and if I want, you can do all these things yourself. You are also understanding. You have also seen many one-shots. If we don't do so many things, we can cover these things very quickly. But because I want to explain everything, I am going a bit fast, and those who stay will understand everything in the end. But they will have to listen very alertly. If you are not alert, you will miss out. So be very alert because whatever you do in chatting, nonsense, and you are like this, I am like that, you are like that, then you understand, nothing will happen. But those who concentrate completely will understand everything because I am trying to explain. Is it clear? Is it clear up to here for everyone? Okay, sir. Now let's come to solutions. This was the story of pure liquid. Now comes the story of solution. Okay, sir. Let's talk about solutions. What do we need to talk about in solutions? Sir, for vapor pressure for solutions, first make a solution. Make it in such a way that you are dissolving a solute in a solvent that is non-volatile. So I said, brother, explain the meaning of volatile and non-volatile now so that there is no difficulty later. So look, it's very simple English. Volatile means that which evaporates. That which evaporates. And non-volatile means that which does not evaporate. Non-volatile means that which does not evaporate. So that which does not evaporate should have nothing to do with vapor pressure. Because vapor pressure is decided by vapors, and if that person is not even there in the vapors, then we have nothing to do with it. The point is correct. So now he wants to know from us, brother, sir, tell me, if I take a pure liquid and also add a solute to the pure liquid that does not evaporate, what will be the effect on vapor pressure? So you are a strange confused person. There is a pure liquid, like water, and you have added sugar to the water. Now you are asking, is the vapor pressure higher here or here? So I will first ask, tell me, what is the temperature at both places? He said the same. So I said, then the matter is over. Who evaporates here? Water evaporates. And who evaporates here? Water evaporates. Because you added non-volatile sugar. So whatever evaporates will be water. So, sir, in both cases, since only water has to evaporate, won't the vapor pressure be the same, sir? What is there to think about? No, it's not like that. Let's use a little intelligence, sir. The vapor pressure will not be the same, sir. Whenever you make a solution by adding a non-volatile solute to a volatile solvent, your vapor pressure decreases, sir. Vapor pressure decreases. I said, what do you mean? I mean, sir, what I mean is that you observe this case and observe this case, and you will clearly see that only water is here. So if I enlarge this surface and look, you will only see water molecules. Clear? Here, along with water, there is also sugar on the surface. Brother, when you dissolve sugar, sugar will also come to the surface along with water, and water will also come. But who will evaporate? Sir, water will evaporate. So the water has decreased, hasn't it? Oh brother, since some sugar has taken the place of water on the surface, the water molecules have decreased, haven't they? And if the water molecules have decreased.

So, we will fly less, vapor pressure will also be less. Absolutely correct. This means one thing is clear, sir. If you ever dissolve a non-volatile solute in a volatile solvent, the vapor pressure of the solution will decrease compared to the pure liquid, sir. The vapor pressure of the solution is always less than the vapor pressure of the pure solvent. And two proper explanations can be given for this. The first is due to the decrease in the number of solvent particles at the surface. You see here on the surface, look, instead of the blue particles, red ones have also appeared, which means the blue ones have decreased, and who evaporates? The blue one. And if the blue one has decreased, the vapor pressure will also decrease. This is the first reason. What is the second reason given? The second reason is, earlier when water evaporated, what stopped it from evaporating, sir? Water pulled water, sir. And here, when water evaporates, when it tries to go out, what will stop it, sir? Water will stop it, and sugar will also stop it, sir. Meaning, it means that due to the interaction of the solute with the solvent, due to solute-solvent interaction, meaning here, when water tries to go out, sugar inside will also pull it, and water will also pull it. And this extra solute-solvent interaction will decrease the vapor pressure. Meaning, if you are educated, you will remember these two things first. And these are things we have been discussing with students for years. And the interesting thing is that this year, in the years before this, JEE has also made a question on this. People think, why discuss such small things? But the question is being asked, a question is coming in the JEE Mains paper. So, it means all these things are important for us. Meaning, when you dissolve the solute in the solvent, the evaporation of the solvent from the surface becomes difficult. For two reasons: one, the solvent particles on the surface decrease because the solute takes their place. And at the same time, while evaporating, the solute also pulls them. Due to which, it becomes difficult for the solvent to escape. So, because of these two reasons, the vapor pressure of the solution is less than the vapor pressure of the pure liquid. Is this clear? Tell me quickly by writing yes or no. Is this point clear to everyone? By writing yes or no? Tell me quickly. Is this point clear? Is it clear? See, only those who are studying and not just talking about what will happen on the 28th, what to do next, how will we meet, when will we go ahead, will understand. Because these are not the normal discussions, friends, that you will find in books. These are the discussions where you will understand that oh, these kinds of things could also be understood. They were not just to be memorized. They were not to be memorized. They could be understood. Okay.

Sir, now look, we will talk about what they have said, based on these points. From these points, one more thing has emerged. This theoretical discussion we just had, this point that has come to you, why the vapor pressure decreases? So, sir, the reason is in front of us, sir, due to solute-solvent interaction and due to the presence of solute particles per unit surface area, the decrease in solvent, sir, this reduces the vapor pressure. This point is further strengthened by Raoult's Law. Mr. Raoult says that whenever you calculate vapor pressure, the partial vapor pressure of each component in a solution is proportional to the mole fraction in the solution. We will explain what this means. The volatile component, you understand my point, the volatile component, the volatile component is the one that evaporates. So, he is saying that if you talk according to this law, then the partial pressure of any component above is directly proportional to the mole fraction of that component. So, I said, look, what I understand so far is that in the solution you have taken, only the solvent is volatile. So, it means that whatever the vapor pressure will be, PS, whatever the vapor pressure of the solution will be, it will be directly proportional to the mole fraction of the solvent because who is the evaporating entity? The solvent. Meaning, PS is directly proportional to the mole fraction of the solvent. Meaning, it means that for whichever component you want to find the vapor pressure, meaning with the help of which component you want to find the pressure of the vapors, multiply the vapor pressure of that component in its pure state by its mole fraction. I am getting straight to the point. Meaning, if you talk directly, then the value of PS is equal to P not * mole fraction of solvent. This is Raoult's Law. Meaning, Mr. Raoult says that if you want to find the vapor pressure due to the solvent, then multiply the mole fraction of the solvent by the vapor pressure of the solvent in its pure state and find it. If the solute were also volatile, then you would multiply the mole fraction of the solute by the vapor pressure of the solute in its pure state and find it. Meaning, Raoult's Law says that for whoever is volatile, to find the vapor pressure due to them, multiply their vapor pressure in the pure state by their mole fraction and find their share. I will explain this further. Here, try to understand the point. Let's take it like this. This is your pure liquid. Suppose this is your pure liquid. And this other entity is your solution. Okay? Suppose let's take it like this. This is solvent. And this is solution. Okay? The solvent is such that its vapor pressure in the pure state is P not. The solvent, as we discussed earlier, the pure liquid has its own vapor pressure. Suppose P not. And the vapor pressure of the solution is PS. Now tell me, who will decide the vapor pressure of the solution? Sir, in this case, in the case you just did, the vapor pressure of the solution will be decided only by the solvent because the solute is non-volatile. So, Raoult's statement is that whatever the vapor pressure will be, it will be calculated by multiplying the vapor pressure of the volatile component in its pure state, which is the volatile solvent. So, the vapor pressure of the solvent in its pure state. What is the vapor pressure in the pure state? P not, by multiplying it by the mole fraction of that solvent. Meaning, Raoult's Law states that for whichever component the vapor pressure is coming from, multiply the vapor pressure of that component in its pure state by the mole fraction of that component. You will get the vapor pressure formed by that component. Meaning, according to Raoult's Law, PS = P not * mole fraction of solvent. If we write this a little more carefully, it will become PS = P not * (1 - mole fraction of solute). If we write it more formally, then this is P not - PS / P not = mole fraction of solute. Which I can write as n solute / (n solute + n solvent). If this is our formula, meaning P not - PS / P not = mole fraction of solute. Meaning, if I ever need to link P not, PS, and mole fraction of solute, I can relate them with this equation. Now I will write this equation more broadly. Please understand, because many questions are formed, so there should be complete clarity. P not - PS / P not = mole fraction of solute. Mole fraction of solute can be written as n solute / (n solute + n solvent). Now, if I add a point here, for dilute solutions, for dilute solutions, n solute is very less than n solvent. Do you agree with this? Then in such a case, the value of P not - PS / P not can be calculated from n solute / n solvent. But this formula can only come if they mention in the question that the solute can be neglected with respect to the solvent. So, if you neglect the solute with respect to the solvent, then the value of P not - PS / P not can be calculated from n solute / n solvent. But in my opinion, I would suggest this. In my opinion, this is the formula. You should always use this formula. If they say in the question that you can neglect the solute, then you can use this formula. Otherwise, you have to start the question from here. But I have another formula too, which I can remember. That is P not - PS / PS = n solute / n solvent. And there is no approximation in this, whatever happens, this formula is also absolutely correct. Meaning, my suggestion is that first of all, for these types of questions where a non-volatile solute is dissolved in a volatile solvent, you will use this formula, and you will also remember this formula because this formula seems easier. If you look carefully, solving things here is easier compared to solving things from here. Everything is the same. Meaning, all the data is the same. But what is the difference, sir? Here there is a plus sign at the bottom. If you cross-multiply and solve, it will take time. Therefore, I have both relations. P not - PS / PS = n solute / (n solute + n solvent). Second, P not - PS / PS = n solute / n solvent. And here I have not taken any approximation. Here it is PS. In the case of approximation, P not was coming here. You see. Meaning, this expression, this formula, is an approximation. We will think about it when the question asks, which it does not. Meaning, this is an approximation. This is not correct. The real formula is this. And from this formula, I have derived this formula. And there is no approximation in this either. Meaning, if P not and PS are given in the question, then you can extract information about solute and solvent using this formula. Meaning, whenever a non-volatile solute is dissolved in a volatile solvent, I have this expression that solves all my numerical problems. Either this or this. Sir, this is the expression with which I can solve all my questions. Why? Why? Because I know one thing: when a non-volatile solute is added to a volatile solvent, the vapor pressure of the resulting solution is less than the vapor pressure of the solvent. The amount of solvent that used to evaporate alone will not evaporate as much now because the solute prevents it from evaporating. Meaning, the vapor pressure of solutions will always be less than the vapor pressure of the solvent, if our solute is non-volatile. Meaning, what was the first case I learned? My first case is if your solute is non-volatile, then the total vapor pressure of the solution is less than P not, and the value is PS = where did this formula start from? PS = P not * mole fraction of solvent. From this point. Then what did you do, sir? I wrote mole fraction of solvent as 1 - mole fraction of solute, and this formula was derived. And from this, that is, I need to remember all these three things. If the question asks me in any form about these types of cases. What kind of cases? Sir, cases where a non-volatile solute has been added. So, I will go with these three formulas memorized. I can find my answer using any of these formulas. Clear? Is the point understood up to here? Is it clear? For example, I will take an example. I will take an example. You will understand from it. Look at this. Look at this. The theoretical discussion I was just having, this is a question asked in 2020. I am not asking this on my own. This is a question that was asked. An open beaker of water in equilibrium with its water vapors in a sealed container. If I add some glucose, what will happen, tell me? Glucose is an entity that does not evaporate itself. That is non-volatile. Meaning, you have taken what kind of case? Non-volatile solute + volatile solvent. Do you agree? This is the case. He is asking what will happen if sugar is added? What will happen if glucose is added? Think and tell me. Sir, if you have added glucose, then you told me that the solution increases. Who? Our water molecules. What is the question? Water molecules leave the solution and increase. What? The water molecules will leave more. Sir, what are you saying? Sir, the water molecules will leave less. Leaves the vapor increases. Sir, the vapors will not increase. Leaves the vapor decreases. Sir, the rate at which water molecules leave. What is to be found? When a few grams of glucose are added to a beaker of water, the rate at which water molecules leave the solution. Oh, it's talking about the rate. The rate at which water molecules leave the solution. Will it increase? No, sir, it will decrease. Leaves the vapor increases. The vapor leaves and increases. Does the rate at which they fall down increase? No. Leaves the vapor. Vapor decreases. No, sir. The rate that comes will only be the rate of leaving the solution. It will decrease, sir. The rate of leaving the solution will decrease. Why? Because, sir, glucose will stop the water, sir. Glucose will also come to the surface. Therefore, it will be difficult for water to escape or for the solution to leave. Leaves the solution, meaning the rate at which water molecules leave the solution will decrease, sir. So the correct answer should be D. Tell me, did you understand my point? Tell me quickly, is this point understood? Meaning, it's a bit confusing statement, but if you read it calmly, you will understand. The rate at which water molecules leave the solution decreases because of those two reasons. Remember? Solvent decreases per unit surface area. And solute-solvent interaction prevents the solvent from evaporating. Due to which, it becomes difficult for your molecules to leave the surface. Is it clear?

Sir, let's talk more. And look, these are lines, meaning I am not doing this on my own. Look at them. These are the questions that are asked to us. What are the lines of questions saying? What weight of glucose must be dissolved in 100 grams of water? Okay? To lower the vapor pressure by 2. Meaning, the vapor pressure of pure water was, sir? Sir, the vapor pressure of water was 54.2. Now you have dissolved glucose in it, so the vapor pressure has decreased by. Okay, sir, I understand. Meaning, what is given, sir? I am given P not of water. Pure water is how much? 54.2. PS is given. PS is how much? 2 less than 54.2. That is 54. So, P not is given, PS is given. Okay, and what else is given? And the weight of water is given as 100 grams. Meaning, the moles of water are also given to us. And we need to find the moles of glucose. Oh, sir, this is the same relation. Use any relation, sir. You know a world of relations. P not - PS = moles of glucose. Remember the formula, divided by moles of water. P not is given. PS is given. You need to find the moles of glucose. Moles of water are known. 100 grams of water means 100 / 18, sir. This is 5.5. Meaning, it means that if I use the direct formula, then the value of P not - PS will be the change, which is equal to 2. You are already saying the value of PS is 54. This is equal to the moles of glucose you need to find, and you know the moles of water. Sir, by solving this, you will know the moles of glucose. And if you want to find the weight of glucose, then multiply the moles of glucose by 180. Is it clear? The formula is absolutely correct. This is what you don't know. This is the advantage. Read it carefully once, and watch this lecture again. All your pains will be gone. This is what you don't understand. You people think that sir, only one formula is given. We are given P not - PS / P not = n solute / n solvent. And sir, we are told this. Write this as n solute / n solvent. Oh brother, you can't write it like that on your own. If the question tells you that the solute is very less than the solvent, then you can do this. Meaning, your formula is this, which I just told you, the second formula. This is correct. But if you want to say, no sir, I want to take it in this form, then instead of this formula, you should remember this formula, which I just derived. P not - PS / PS = n solute / n solvent. This is not derived from any approximation. This is the exact formula. And this is the most important formula because it requires the least calculation. You see how easy the calculation will be here. Look. How much is the calculation, sir? You are given P not. PS is given. You need to find n solute, and n solvent is given. Sir, n solute will come directly. And from n solute, if you want the weight, then multiply by the molar mass of glucose. You will get the answer in grams. Sir, this will be 3.69. The question is finished. Nothing to do. Is everyone understanding my point? Tell me quickly. Is this clear? Okay? For example, I will take more examples and show you. All these are from the lines, meaning I am not doing this on my own. All these are asked from the lines. Look at this. Look, what is it saying? When a certain amount of solid A is dissolved in 100 grams of water. Meaning, the moles of water are given to us. Moles of water will be 100 divided by 18, that is 5.55. Okay. Make a dilute solution. The vapor pressure of the solution is reduced to one half of that of pure water. Meaning, if I take the vapor pressure of pure water as P not. Suppose we take the vapor pressure of pure water. If I take this as P not, then the vapor pressure of the solution, what will this be, sir? He is saying that our solution's vapor pressure becomes one half. Reduced to 1/2. Meaning, our solution's vapor pressure is P not / 2. Is it clear? This is P not. This is P not / 2. These are the moles of solute, sir. You see for yourself. What does he want? He wants you to tell him how many moles of solute there are. Look at the moles of solute. Which formula will you use, sir? Sir, we have been told P not - PS. Oh, you are saying this, you simpletons, understand the point. When he is not saying anything, there is only one way to make it easy, sir. P not - PS / P not = n solute / n solvent. Finished. P not - PS. What will be the value of P not - PS? P not - PS means the change. So, earlier it was P not, then it became P not / 2, so the change will be P not / 2. Initially it is P not. Sorry, this is PS. This will be P not / 2 and PS.

What is the value of the solution's P naught / 2? Wow, the moles of solute came up, the moles of solvent came down. How many are there? See? This became one directly. This got cancelled directly. This is one. So the value of n solute came out directly. How much did it come? Sir, it was understood from here that 5.55 moles of solute will have to be taken, sir. So, the answer is 5.55. Talking about the nearest integer. So the answer is six. Clear? Understood? That is, I will say one thing again. This is my first category, what is the first category, sir? The first category talks about this. The first category says that if you dissolve a non-volatile solute in a volatile solvent, the vapor pressure decreases. Which is called Ps. P naught is of pure solvent. The relation of P naught and Ps with moles is P naught equal to, sorry. Now Ps = P naught * mole fraction of solvent. First formula. I am writing it again at the very end. I am finishing this case. First formula Ps = Everything starts from here. This is Raoult's Law, mole fraction of solvent. When I write this mole fraction of solvent as 1 - mole fraction of solute, my second formula is ready. P naught - Ps / P naught is equal to mole fraction of solute. And what is mole fraction of solute written as? n solute / n solute + n solvent. Third formula, if I don't do any cheating, I know very clearly. This is P naught - Ps / Ps = n solute / n solvent. I have not used any approximation in any of the formulas. These three are absolutely correct. Most children are told to write this formula as n solute / n solvent. Oh brother, how can we write it like that? If the question says so or if you feel that the moles of solute are given very less, then you can write solute + solvent as solvent in approximation. Otherwise, you cannot cheat. So these are the exact formulas. And why do you want to write n solute by n solvent anyway? Sir, it makes the calculation a little easier. Oh, then it's better to do this. Use this. There is no approximation in this either. Sir, this is the exact formula that is derived from here. You can derive it at home if you want. If you write it in reverse, you will understand it yourself. Understanding the बात को, writing it as 1 - mole fraction of solvent. So you can derive this formula yourself. But I say, leave it. You remember these three things for this first case. Clear? Tell me quickly if everything is clear up to here? Pushpendra is saying something about girls, he has a lot of idea. Come on Pushpendra, stop it. Clear, brother? Is it okay up to here? Okay? This was our first case. Now let's come to the second case. Now I am going to take the second case. I will make a solution again. I will make a solution again. But this time I will make a solution in which both the solute and the solvent will be volatile. Tell me, what is the difference from the first case? Write quickly, what is the difference? Let's see who is sleeping and who is awake. What is the difference from the first case? What is the difference in this case? What is the difference between the first case and this case? Tell me quickly once. What is the difference between the first case and this case? In the first case, the solute was non-volatile. This time the solute is volatile. That's the only difference, sir. In such a situation, you are absolutely right. Well done. Those who are listening are giving answers. Very good. Brother, I have already said about the dinner break. How can I tell you? You are not understanding. Don't break my spirit, brother. I know the destination is something that is difficult for you too, and difficult for us too, in the sense that we have to take classes continuously. Right? So this is not an easy task. So in such a situation, please understand a little. Take something to eat and drink nearby. You can take it, right? Take something nearby, eat something, understand something. Take biscuits, take namkeen. Study a little, understand a little. Manage a little, understand. Because there is a plan, brother. Now by taking a break, you are understanding the बात को. A person becomes sluggish. After that, we won't be able to do it. So, we have a target, we want to complete the major portions in any way. After that, we just have to apply the formulas of colligative properties and get the answers. Then it won't be that difficult for us. That's why I want you to act a little wisely. Don't talk about breaks yourself. Take a break yourself. How many children are watching, brother? Understanding the बात को? Those who don't want to study. You see how many children there are, what is the benefit of these classes? So at least let those who are watching do it. Whoever wants to take a break, take a break themselves. Don't tell us. What does a break mean by my saying it, brother? You just turn off the TV and leave. That's the break, brother. Don't tell me unnecessarily about breaks. Is everyone understanding me? Okay? So, here they want to say that brother, there are two solutions and two liquids. We will mix both of them. Now you understand the बात को. If the solute is also volatile, meaning the solute also evaporates. Now if the solute also evaporates, it means the solute will also be a liquid. So generally, when the solute is a liquid and it is added to a liquid solvent, this case arises because liquids have their own vapor pressures. This means liquids evaporate, that's a different matter. Some evaporate more, some evaporate less. Due to force of attraction. Remember? But sir, when two liquids are mixed, both are volatile, then a new case will arise. In such a situation, how to find the vapor pressure? So, it's very clear, sir. Does this liquid A evaporate? Yes, sir. It is volatile, sir. If it is volatile, then it will have a vapor pressure at a particular temperature. Sir, it will definitely have it, sir. PA naught of pure state at a particular temperature. Any liquid has its own vapor pressure, sir. Absolutely right. Sir, does B also evaporate? Yes, B also evaporates. So, sir, B will also have its own vapor pressure. Of pure state, it will definitely have PB naught. Now, if you mix A and B, then this will be our solution. Due to this solution, vapors will form above. Will anyone think and tell me who will be in the vapors? Can anyone think who will be in the vapors? Sir, both will be in the vapors, sir. A will be in the vapors, B will be in the vapors. Do you agree with this, why? Because both are volatile. And if both are volatile, then A will evaporate and B will evaporate. And because of this, the pressure of the vapor will be known as total vapor pressure PT here. Is it okay up to here? Now the question is, sir, how do I find this PT? Sir, in the previous case, you taught how to find PS. What was that, sir? Multiply P naught by the mole fraction of the solvent. Sir, multiply the mole fraction of the one that evaporates by its vapor pressure in the pure state. This was Raoult's Law. Remember this? Are you understanding all this? When I used to study, I didn't understand where these formulas were coming from. After teaching for so many years, I am now understanding all these things, how beautiful a law Raoult gave. He said that the pressure due to whoever evaporates will be found by multiplying the vapor pressure of that person in the pure state by the mole fraction of that person. This is Raoult's Law. So I said this is easy. If you want to find PT, then PT has the contribution of two people. There will be vapor pressure due to A. There will be vapor pressure due to B. And Raoult says that if a component is volatile, then the vapor pressure due to A will be found by multiplying its vapor pressure in the pure state by its mole fraction. Understand the बात को? This is Raoult's Law. Raoult says that if you want to find the vapor pressure due to A, you want to calculate the partial vapor pressure of A, then it will be found by multiplying the vapor pressure of A in the pure state by the mole fraction of A in the liquid phase here, whatever the mole fraction of A is, mole fraction of A, XA, whatever you want to say, XA, XB, these are the mole fractions of A and B in the liquid phase. When you mix these two, their mole fractions will come out to be something. So if their mole fractions in the liquid phase are multiplied by their vapor pressure in the pure state, then their contribution above will be found. Their contribution above will be found. Clear? Is it okay up to here? Okay, sir. Now comes B. Is there vapor pressure due to B as well? Yes, sir, there is vapor pressure due to B as well. How much is due to B? Sir, it is found by multiplying the vapor pressure of B in the pure state by the mole fraction of B. Are you understanding? When I used to study, I used to think this formula came from nowhere. I understood later that this is Raoult's Law. If a third component is also taken, then it will be Pc naught * Xc. Because Raoult says that the vapor pressure formed due to the volatile components is found by multiplying their vapor pressure in the pure state by their mole fraction. Clear? Has everyone understood? Aman Sharma is saying speed up, sir. Speed up. What a problem, brother. Aman, if we speed up, the lecture will end soon. Right? You agree? So it will be easy for me too. It will be easy for me. But if I am not able to do it, I want my own ease. I want the lecture to end soon. The hassle to end. Understanding the बात को? But still, I am not able to do it. This means, this means that what is necessary is happening. I also want to finish in half an hour. Go home and sleep comfortably. Don't you think this is easy for me? But still, it's not happening. Why? Because, sir, you are thinking about us. No, friend, absolutely not. I am just fulfilling a responsibility to cover everything for you. I will move on. Whoever wants to do it, let them do it. Whoever doesn't want to do it, let them not do it. This is my duty. Are you understanding me? It's not like some special relationship, understanding the बात को? I want you to get selected. If you don't get selected, I will die. There is no such intention. No such plan. It's just a job that I want to do honestly. Whoever accepts it among you will benefit. Whoever doesn't will not benefit, and I won't know who benefited and who didn't. So, I myself want to speed up, but for some reason, it's not happening, right? Are you understanding? Maybe you know it, but not everyone knows it. So I want to explain it a little elaborately. Okay? And secondly, if you know it. Then what are you doing? You are wasting your time, brother. Anyway, so the value of PT will be the pressure coming due to A and the pressure coming due to B. And the pressure due to A will be found by multiplying its vapor pressure in the pure state by its mole fraction in the liquid phase, and the vapor pressure of B in the pure state by its mole fraction in the liquid phase. Is it okay up to here? This is the value of PT. Hundreds of questions have been asked on this, not one, not two, hundreds of questions. That is, just as I made you remember those three formulas there, in the same way, I am making you remember this first formula here. Very important. Is it okay up to here? Second thing. The second thing is that, sir, okay. To find the total vapor pressure, this action will be taken. Okay, I am also mentioning all the things here, otherwise, children won't be able to do it. There is a lot of confusion between XA and XB. So I write clearly. X means, sorry, mole fraction in liquid phase. Mole fraction of A in liquid phase. Similarly, what will XB be? XB is the mole fraction of B. Mole fraction of B in liquid phase. Understanding the बात को? That is, XA and XB are the mole fractions of A and B inside the liquid phase. When you mix these two, they will have their own mole fractions, which you will put here. P naught will be given in the question. Quickly, PT will come. It's over. How many questions have been formed, sir? You understand? Instead of XA, calculate moles. Instead of moles, calculate its total moles. Calculate P naught, calculate PT. Brother, you have asked hundreds of questions, sir. You have made hundreds of questions on the same formula. Now let's come to the second thing. What is the second thing? The second thing is that, sir, okay, liquid will evaporate from here, so vapors will form here. Who will be in the vapors, sir? Oh brother, A will be in the vapors, and B will be in the vapors. Sir, both are evaporating, so both will be in the vapors. Do you know what's good, sir? If you want to find the mole fraction of A and B in the vapors, or the composition in the vapor phase, how to find it, sir? This is important, understanding the बात को. That is, it means that the mole fractions of the liquid phase are understood by us. For example, let's take a question now. This is a question asked in 2025. You look at it yourself and tell me if you can do it. Okay, sir, let me also look at it once. Let's look at it once. Let's try to do it. A solution made by mixing one mole of volatile, who are given? Liquid A, meaning, moles of A are one. Moles of B are three. Vapor pressure of pure A is 200. That is, the value of PA naught is 200. And the vapor pressure of the solution is 500. That is, the value of PT is 500. So, will you find the vapor pressure of B? What, sir? What nonsense, sir? First of all, tell me, who is more volatile, sir? Does A evaporate more or does B evaporate more? Oh sir, let's check. The vapor pressure of A at a particular temperature is 200. First, let's find the vapor pressure of B. The one whose vapor pressure is higher will be more volatile. Okay? So, let's find B, sir. How to find it? Sir, there is only one formula. PT = PA naught * XA + PB naught * XB. Sir, the value of PT is given as 500. PA naught is 200. And the mole fraction of A is 1/3 + 1, meaning 1/4. + PB naught * 3/4. You can find PB naught from here yourself, and it will be 600, sir. Sir. That is, A shows a vapor pressure of 200. B shows 600, meaning B's vapor pressure is higher. Sir, B is more volatile, sir. B is more volatile. So, first of all, this is wrong. This is wrong. Now, between these two, sir, the vapor pressure of B in the pure state is 600. The answer is C. Clear? Understood? Understood? B is more volatile because B's vapor pressure is higher. PB naught is greater than PA naught. So B is more volatile. B evaporates more. Clear? Understood? Okay, sir. Now let's come to the important point. Hundreds of questions have been asked on this topic as well. How to calculate the mole fraction of A and B in the vapor phase? Sir, the mole fraction of A and B in the liquid phase was XA and XB. You can calculate PA naught values, PT, etc. Sir, but when they evaporate, vapors form above. So, sir, there will also be some mole fraction of A and B in the vapors, right? Brother, if it is XA and XB in the liquid, then it is not necessary that it will be equal to XA and XB in the vapors. Sir, the composition of the vapor will be something else. The composition of the liquid is something else? It can definitely be. Sir, tell me, how to find the composition of the vapor, sir? With the help of XA, XB, and P naught, how to find the composition of the vapor? So, it's very simple. Everyone will remember this that if I need the composition of the vapor phase of A. Y means vapor phase, X means liquid phase. Okay? So, if I need the mole fraction of A in the vapor phase, it will be found by dividing the partial pressure of A by the total pressure. And this is Dalton's Partial Pressure Law. Dalton's law states that in any gaseous mixture, the mole fraction of any gas can be found by dividing its partial pressure by the total pressure. As far as the contribution of A is concerned, Raoult has already explained it: pure state * mole fraction. And the value of PT, you have also calculated that. What was PT equal to? PA naught * XA + PB naught * XB. That is, if you want to find YA, you can find it from this equation. Rather, wait. I will tell you a more beautiful formula. If you want to find YB, it will be found from Dalton's Partial Pressure Law as PB / PT, and the value of PB will be PB naught * XB divided by the total pressure, and what is the total pressure? PA naught * XA + PB naught * XB. That is, if you want to find the mole fraction of A in the vapor phase, you use this equation. If I divide these two equations. I want to simplify things further. If I divide these two equations, you will see that an equation will be formed: YA / YB = PA naught / PB naught * XA / XB. See? This is the equation being formed. YA / YB. When you divide both, the denominator will cancel out. This expression has come. Now see what I am doing. I am leaving YA as YA. And I am writing YB as 1 - YA. This is okay, sir. The sum of mole fractions of A and B in the vapor phase will be one. So YA and 1 - YA = PA naught / PB naught. I am leaving XA as XA and writing XB as 1 - XA. My own suggestion is that you calculate YA and YB using this equation. It is easier. Instead of finding YA from this expression. Brother, see, everything is the same. PA naught is needed here too. Needed here too. PB naught is needed there too. Needed here too. XA is needed here too. Needed here too. All the data is the same. But if you use this equation instead of this one to find the answer, it will be easier. That is, I want you to remember this thirty-second formula now, on which hundreds of questions have been asked: whenever the mole fraction of the liquid phase is given,

So, the mole fraction of A in the vapor phase is calculated like this. Or, if the mole fraction of the vapor phase is given, then the mole fraction of the liquid phase is calculated like this. That is, what is this formula based on? This formula is based on bringing XA closer to YA or YA closer to XA. Understand the point. I am not using the word B. If XA comes, XB will also come. So I am talking about only one component. If you want to interrelate XA with YA and YA with XA, take the help of this equation. You will have fun. You cannot even imagine how much trouble will be solved. And very few students use this formula. Very few students know about this formula. They only know this one method. YA is calculated like this, YB is calculated like this, to hell with it. But I am suggesting you calculate Y. Calculate it this way, you will find it much easier. Is it clear? Did you understand? Did you understand up to here? That is, using the liquid phase, you can calculate the total pressure. Using the compositions of the liquid phase, that is, using XB, you can calculate the total vapor pressure. And using the total vapor pressure, or with the help of XA, XB, and P naught, you can also calculate the composition of the vapor phase. Is it clear? Where is the mistake? Some child is saying we did something wrong. No, you won't understand. If you have never studied, what will you understand? You won't understand this. Just write it as you are being told, and the derivation is in front of you. YB can be written as 1 - YA. If there has been any mistake in writing something here, correct it. Otherwise, everything is correct. Is it clear? Did you understand up to here? Okay, this? Now, as I tell you, you will enjoy it. For example, let's do something very straightforward, very straightforward, just like this, once. Sir, here, I don't know what the question is. I just brought it like this once. Let's see. Sir, total pressure of a mixture of non-reacting gases. This is completely nonsense. This should not be done at all. Sir, there are two gases. This has no relation to a liquid solution. The moles and weights of two gases are given, and their molar masses are given. That is, the moles of both gases are given, and the total pressure is given. We need the partial pressure of gas X. So, I just told you Dalton's law: if you want to find the partial pressure of any gas, multiply the total pressure by its mole fraction. We just talked about Dalton's partial pressure law. Partial pressure = Total pressure * Mole fraction. How did you calculate the mole fraction just now? Mole fraction = Partial pressure / PT. That's what we did. So, if you want to calculate the partial pressure, multiply the total pressure by the fraction of that gas, and you will know the partial pressure of that gas. So, everything is given in this question. The total pressure is given as 740, and you will calculate the mole fractions from here. 6 upon I won't calculate. 6 / 20 / 6 / 20 + 45 / 45. Sir, you solve this, and you will know the partial pressure of X. And this will be the answer. Finished. I mean, this is such a pathetic question. I mean, even such questions are being asked. You see. That is, you know the mole fraction of a gas, and you are given the total pressure. Dalton's partial pressure law states that the mole fraction of a gas, understand, there are two gases. The total pressure due to both is 100. If asked, how much is due to one? What fraction of that one is here? If I multiply it by 100, I will get my share. And if I multiply B's fraction by the total, I will get B's share. That's what we are doing here. If I multiply the mole fraction of X by the total pressure, I will get the share of X. What is the share of X in 740? The share of X in 740 is calculated like this. And similarly, the share of B has been calculated. Is everyone understanding me? Let's take more examples. Beautiful. The year these questions came. Very good. In 2025, and you know what's funny? This question came in 2025. The same question came before. What does this tell us? This tells us that it is not thinking. It is not thinking. It feels like this is the ultimate challenge. We will break people with these. And indeed, these are questions that some students find difficult. Because they don't think about all this. They are told to use this formula, use that formula. And they are shown 10 questions. It's fun. Now, look carefully here, how it should be done. Let's use a little intelligence. Sir, look, one thing is clear. The relations I need to find here are between XA, XB, and YA, YB. I understand one thing, sir. The game is something like this: the relation between Kai A and YA, Kai and Y, sir. The matter is going something like this, sir. Do you agree? The whole game is about Kai and Y. Sir, I was taught that sir, if YA / 1 - YA can also be written as YB, which you just learned. YA / 1 - YA, remember the relation? Which I said very few people use. Very few people know. YA / 1 - YA = PA not * XA / 1 - XA. Remember this formula? It was just told. Okay, sir. What is 1 - YA? Sir, 1 - YA is YB. So this is YA / YB = PA not / PB not * XA / XB. Is it okay up to here? Is it okay up to here? And sir, here you have given that the value of PA not is 350 and the value of PB not is 750. That is, the value of PA not is less than PB not. So, if PA not is less than PB not, it means this will be less than one. It means this value is less than this. The matter is over. That is, from this, it is understood that the value of YA / YB is less than Kai A / Kai B. Sir, look at this beautiful question. And a student who remembers this relation will be able to solve this question. Whoever remembers this relation will solve this question quickly. And whoever doesn't remember will have to do things lengthily. Is it clear? So, anyway. So, YA / 1 - YA = PA not / PB not * XA / 1 - XA. This is the way to find YA from X and X from YA. I have put YB in place of 1 - YA here, so my relation became this. In the question, PA not is given as smaller than PB not. So, it means PA not / PB not is less than one. It means the value of XA / XB is greater than YA / YB. So the answer should be C. And you will see that I have not brought this same question from my own mind. This same question is from 2000, when? That was from 25. This is from 2019. The same question was asked in 2019. And what will be the answer? XA / XB > YA / YB. That is, the answer will be B. XA / XB > YA / YB. Is it clear? Understand. Exactly the same question. Exactly the same. The only difference is? M and N are used instead of A and B. Tell me, did you understand my point? Is this clear? And let me show you more interesting things. There are so many questions filled with these lines, they have been asked in abundance. Pick any question. Let's see, sir. Let's see more. Here, sir. What are you trying to say? What to do? Sir, let's read one by one. The vapor pressure of pure benzene and methylbenzene. Okay, sir. That is, if you know methylbenzene, it is toluene. Benzene with methyl on it means toluene. So, if I talk about PB, it's benzene, whose value is given as 80, and if I talk about toluene, it's PT not, whose value is given as 24. Okay? Good. The mole fraction of methylbenzene in the vapor phase. See this, in the vapor phase. Of methylbenzene. That is, what is given, sir? This, sir, this is given. Okay, do we need to find this? YT, sir. We need YT, sir. Vapor phase Y, and for toluene, we need YT. Okay, sir. And what is said? It is said that the composition of the liquid phase is an equimolar mixture of two liquids. Equimolar means both have the same moles. And when both have the same moles, the mole fraction of benzene and the mole fraction of toluene will be the same. And that is half. When the moles are equal, the mole fraction is half. Those who don't know, learn this point now. What is there to learn? Just understand it yourself. If both have 10 moles each, what will be the fraction? 10 / 20, 10/20, that is 1/2. That is, Kai is known. YT needs to be found. P not is known. Which equation will we use, sir? Sir, there is only one equation that you told us, sir? YB / 1 - YB = PB not / PT not * XB / 1 - XB. Sir, this is for benzene. Sir, this is for benzene. If you want to find for toluene, you can find YT, sir. You can write the same expression for YT, sir. Calculate for benzene, then subtract from one, and YT will come. Do as you please. Finished. Understand the point? Did you understand? If you want to write YT, how will you write it? YT / 1 - YT = PT not / PB not * XT / 1 - XT. You can find YT from that. Everything is given in the question. Let me calculate it once. First, I will calculate the mole fraction of benzene in the vapor phase. YB / How easy it becomes with this formula. See. Equal to PB not / PT not. Pb not means benzene's 80, and PT is 24. And what was X? XB / 1 - XB. X is also 1/2, and 1 - XB is 1 - 1/2, which is also half. This is one. Sir, directly calculate, what will be the value of YB? So this is 24 YB, which is equal to 80 - 80 YB. So YB = 80 / 104. This is your YB. You have calculated it. From here, YB will come out. How much will YB be? This is correct. This is for benzene, brother. This will come out for benzene. So, how much will ours for toluene be? YT = 1 - 80 / 104. So this is 24 / 104. So it looks like this is almost 0.23. And what will be the answer? 0.23 means 23 * 10 power -2. Finished. So, for those who have understood how to get from X to Y and from Y to X, all questions are easy for them. You can take any question from the line. These are questions asked in a line. I am not doing one or two. These are questions asked in a line. Look at this. All of them are the same. I will show you more. Look at this. Asked in JEE Advanced. What are they trying to know? They are saying that there are two liquids, and they are talking about their compositions. Two different solutions have been made of A and B. One solution has a mole fraction of A as 0.25. And its total pressure is 3. And another solution is such that the mole fraction of A is 0.5, and the total pressure of that solution is 0.4. Tell me, what are PA not and PB not? Look at how pathetic the question is. You see? That is, there is one solution whose vapor pressure is 0.3, and PA not of A in its pure state, and mole fraction of A is 0.25. For B, it will be PB not, and the mole fraction of B will be 1 - 0.25, that is 0.75. This is the first equation. The second equation says that the total vapor pressure will be 0.4. This will happen when the fraction of A is 0.5. So, if A is 0.5 in the second solution, then it will be 0.5 + PB not * 0.5. Sir, will PA not and PB not not be found using these two equations? Tell me, what a pathetic question. It will be solved in one second, and it is asked at JEE Advanced level. That is, there is only one equation on which questions are continuously being formed. So, I will say again, whenever a question about a volatile system is formed, where both the solute and the solvent are volatile, you only need to pay attention to one thing. The question will be about total vapor pressure, or about liquid composition and vapor composition. Is this clear? Let's see more. Look at this. It's the same person. I am telling him. Tell him to go. Is this clear? Is it okay up to here? Okay, sir. Let's look at this question too. What are they trying to say here? Same. Absolutely nothing new. You will understand everything if you look at it yourself. Absolutely the same. What to do? The vapor pressure of two volatile liquids A and B are 50 and 100. Okay? Or the vapor pressures of two volatile liquids. That is, PA not is given. What is it? 50. And PB not is given as 100. Very good. And what else is said? If the liquid mixture contains 3 mole fraction of A. Liquid mixture. This means what is given, sir? This is given. XA = 0.3. Clear? Then the mole fraction of B in the vapor phase. We need the mole fraction of B in the vapor phase. So, what relation did I remember just now? I remembered the relation YA / 1 - YA = PA not / PB not * XA / 1 - XA. Remember this? That is, if you want the composition of A in the vapor phase, it will be calculated like this. And if you want for B, how will it be calculated, sir? If you want for B, then put 1 - YB in place of YA and YB in place of 1 - YA = PA not / PB not. Put 1 - XB in place of X and XB in place of 1 - X. Both relations are the same. You see, both relations are the same. I just put 1 - YB in place of Y. Okay? So, YB came in place of 1 - Y. So you can use this relation. Now, let's use it directly. 1 - YB / YB is equal to what is PA not / PB not? Sir, the value of PA not / PB not is given as 50 / 100. XA. What will 1 - XB be? Sir, if the value of XA is 0.3, then the value of XB will be 0.7. So 1 - XB will be 0.3, and XB will be 0.7. Sir, now look carefully. From here, you can solve for YB. So, if you solve for YB, it will be 14 / 17. That is, the mole fraction of B is 14/17. That is, X/17 means the value of X is 14. Same formulas. Questions have been asked in abundance on the same formulas. Questions have been asked in a line. If you look carefully, all these questions are made on these cases, in a line. All questions are exactly in a line. Look at this. A gaseous mixture of two substances A and B under a total pressure of 0.8 ATM is in equilibrium with an. That is, the total vapor pressure is given as PT = 0.8 ATM. Okay? And this vapor is in equilibrium with the liquid. What kind of equilibrium? The mole fraction of A is 0.5 in the vapor phase. That is, the mole fraction of A in the vapor phase is 0.5. That is, YA = 0.5. Okay. And what else is given? And 0.2 in the liquid phase. What is this, sir? This is given for A in the liquid phase. That is, XA = 0.2. What needs to be found? The vapor pressure of pure liquid A. Pure vapor pressure in the pure state. So, sir, it's a very simple matter. You are given the total vapor pressure as 8. Is it clear? And in that case, the value of X is 0.2. So, can I write 0.8 = PA not * 0.2 + PB not * 0.8? Tell me, did you understand this point? Sir, the same total, the first formula, PT = PA not * XA + PB not * XB. This is that same formula. Okay, sir. One point is finished. This is the relation between PA not and PB not. Now, let's come to the second point. Sir, the value of YA is also given. XA is given. So, why not make an equation by linking YA and XA? Let's make it. What will be the equation, sir? The same equation you had. YA / 1 - YA = PA not / PB not * XA / 1 - XA. Very good, sir. Okay, sir. Let's use this equation too. The value of YA is 0.5. So this is 0.5 / 1 - 0.5 = PA not / PB not. The value of XA is 0.2, and the value of 1 - X will be 0.8. From here, a relation between PA not and PB not is coming. Is it clear? Let's see how much it is, sir. PA not will be equal to what? This will be 1/4, and this will be one. So PA not = 4 PB not. Sir, if I put this relation of PA not here, you will find the value of PA not. Sir, from here you can calculate PA not. 0 point, whatever it is. Try putting PB not here. What will come? 0.8 = 0.8 = PA not * 0.2 + PB not. What can be put in place of PB not? In place of PB not, you can put PA not / 4 * 0.8. Tell me, what will come after solving? Sir, this will be 0.2, 0.2. So this will be 0.4. So that is 8. So the value of PA not directly came out to be 2 ATM. What to do, sir? The same two formulas. So, I am going to finalize again. One is this: when the case of two volatiles arises, PA not + PB not, this is the first relation. And the second is: if you are concerned with the composition of the vapor phase, then you should take the help of YA / 1 - YA = PA not / PB not * XA / 1 - XA. Sir, these are two relations. These two relations can solve all the questions that are asked about solutions prepared from a mixture of two volatile liquids. Is this clear? Tell me quickly. Is this point clear to everyone here? Tell me quickly, is this clear? Is this point clear to everyone? Excellent. Look, don't ask about the duration because now I will talk about ideal and non-ideal solutions, quickly. This is easy. We will try to cover it in half an hour. Azeotropes etc., all will be included. It will take a little time, and then we will have colligative properties. So, colligative properties will not take much time because they are directly based on formulas. So, we will first read all the colligative properties together and then practice some questions on them. Okay? So, now let's move on to the next part. Let's have a quick discussion about ideal and non-ideal solutions. It's a simple discussion. We won't try to go into too much detail. But one thing should be understood. What is an ideal solution? An ideal solution is a solution that follows Raoult's law at any composition. That is, if you make a solution by mixing two liquids, it will be ideal. This is a definition. I will try to give you a more proper refined definition as well. One definition that is written in books is that a solution that follows Raoult's law over the entire range of composition. That is, put any value of XA and XB, the value of PT will always be calculated from PA not * XA + PB not * XB. So that is Raoult's law. That is, you can calculate PT by putting any value of XA and XB using this expression. So this is an ideal solution. It is called an ideal solution. That is, for any composition of XA and XB. A solution that follows Raoult's law. That is, solutions which follow Raoult's law over the entire range of composition are called ideal solutions. Okay? I can think of an even better definition. And that better definition is that when you mix A and B together, what is formed after mixing? Sir, a solution is formed after mixing. In that solution, A interacts with B. That is, in one case, A was alone, B was alone. Then you mixed these two, so A and B were formed. Now, after A and B are formed, if I ask A, listen carefully. If I ask A, hey, how do you feel now? And if A's answer is, I feel the same as before. No difference. We said, hey, you were alone before. Now you are with B. Some difference must have occurred. It says, no, no difference. That is, it means that if AA interactions and BB interactions are similar to AB interactions. That is, if the interactions formed by mixing A and B are the same as the interactions of A and B, then the solution must be ideal, sir. That is, it means that when interactions of one type replace interactions of a similar type, the solution that is formed is an ideal solution. That is, A and A and B are alone. When you mix them, the interactions created by mixing them are the same as the interactions when they were alone. So, in such a case, A feels that whether it stays alone or with B, everything is the same. So, in such a case, the solution formed is an ideal solution. That is, what is the definition of an ideal solution? When AB interactions are similar to AA interactions and BB interactions. And if the interactions are the same, then these four things, this graph, this graph can be drawn very simply. If you plot the value of PA not, PT, and the values of PA and PB. So, if I take XA as 0 here, and XA as 1 here, then it is clearly understood that if XA is 0, then XB will be 1, and here if XA is 1, then XB will be 0. So, at XA = 0, the pressure will be only due to B, sir. So, how will the pressure of A be calculated, sir? The pressure of A is this. Understand. That is, here when the value of XA is one, there will be only the pressure of A, that is PA not. If XA is 1, it means B is not present. And if XA is alone, then what will be the total pressure? It will be equal to PA not. Similarly, if I talk about B, then the pressure coming out for B is this pressure. Understand. Why? Because when XB was 1, the total pressure was this. When XB was 1, the total pressure was this. This is PV not and this is P not. And the total pressure is the sum of these two. Sir, this situation that is being shown to you is an ideal situation. And in this ideal situation, PT will always be calculated from PA not + PB not. Always, sir. This is an ideal situation. This is an ideal situation that is being shown to us. Is it clear? That is, what I mean to say is that if I am talking about an ideal solution, then when X is zero, whatever pressure there is, it will be due to B, and the total pressure due to B is PB not. Similarly, when X becomes 1, XB will become 0. So, the total pressure will be PA not. So, at a different composition, the total pressure will be predicted by looking at this graph. Looking at this, it seems that I have assumed A to be more volatile. I have assumed A is more volatile. I have assumed this. That's why the vapor pressure of A is higher. So A is more volatile. I have assumed this. So, if A is more volatile, then your graph will look something like this for an ideal system. That is, what does it mean to talk about an ideal system? It means that if I take a particular composition, then at this composition, let's assume the value of XA is 0.2, and let's assume the value of XB is 0.8. Then the pressure of A at this composition, at this composition, the pressure of A will be from here. The pressure of B will be this, and the total pressure due to both will be this. Is everyone understanding me? That is, what I mean to say is that if I talk about this composition or any ideal system, then an ideal system is a system in which the vapor pressure of A changes in this way, the vapor pressure of B changes in this way, and the total pressure changes in this way. This is an ideal situation, sir. And what is good about an ideal situation? That when everything is the same. When the interactions are the same, then it can only be seen when your solutions are made of similar types of substances. For example, I will explain to you with just one example. The rest you have to remember. For example, let's talk about hexane and heptane. Okay? If you look at hexane carefully, hexane is like this. CH3 CH2 CH2 CH2 CH2 CH3. If you look carefully, the interaction between two molecules of hexane can only be Van der Waals interaction. Sir, only Van der Waals interaction can occur between hexane molecules. Why? Why can it occur? Because sir, it is non-polar, sir. Hexane is a non-polar molecule. And what happens in a non-polar molecule, sir? Only Van der Waals interaction. So, there is only which interaction between them? Van der Waals. Okay? Okay, sir. Now let's take heptane. Let's take heptane, sir. The shape of heptane, sir, is like this. CH3. One more carbon will be added. CH3 CH2 CH2 CH2 CH2 CH3. Sir, this is your heptane. So, the interaction in a heptane molecule, CH3 CH2 CH2 CH2 CH2 CH3. What is the interaction between them, sir? This is also non-polar. The interaction between them will also be Van der Waals, sir. This is also Van der Waals. So, if you mix these two, what will happen, please tell me? If you join these two, then the interaction between hexane and heptane will also be Van der Waals, won't it, sir? If you join these two, then what will happen, sir? When you join these two, the interaction between hexane and heptane will start. Sir, these are CH3 CH2 CH2 CH2 CH3 and heptane will be CH3 CH2 CH2 CH2 CH2 CH2 CH3. Sir, are these two not non-polar? And if they are non-polar, then what will be the interaction between them, sir? The interaction between them will also be Van der Waals, sir. That is, what it means is that if they were alone, there were Van der Waals interactions. Here too, there were Van der Waals interactions. When they mixed, there were still Van der Waals interactions, sir. That means similar types of interactions, similar types of interactions are replacing each other. That is, it was Van der Waals before. It is Van der Waals afterwards. Sir, ultimately, what is this solution going to be? Sir, this is going to be an ideal solution. Is it clear? Did everyone understand? That is, what it means is that this solution will be a Van der Waals solution, this will be an ideal solution because it is made of similar types of substances. Sir, when heptane was alone, it showed Van der Waals interactions. When hexane was alone, it also showed Van der Waals interactions. And when you mix these two, the interaction between them will also be Van der Waals because they are non-polar molecules. This means your solution will be ideal. That is, when are ideal solutions generally formed? When liquids of similar types mix. Hexane, heptane, benzene, toluene, ethyl bromide, ethyl iodide, chlorobenzene, bromobenzene. My suggestion is that you just memorize the examples I am writing, and keep in mind that if they ask why this happened, then you can say that interactions of a similar type replaced interactions of a similar type, hence Van der Waals interaction occurred. Is it clear? Okay. That's why our solution became ideal. Now, if I talk about non-ideal solutions. In fact, if I here

Let me add one small point: if I calculate the delta mixing for ideal solutions, calculate delta V mixing, calculate delta mixing, and calculate delta G mixing, what values do they come out to be? So, all students will agree that sir, when the interactions are similar, the interactions will break first, and then new interactions will form. That is, we were alone there, and then we met here. So, first, the individuals will have to be separated. A and A will have to be separated. B and B will have to be separated, and then A and B will have to be joined. Sir, because the interactions are similar, the energy spent in breaking will be released in forming. That is, ultimately, the use and liberation of energy in bond breaking and bond formation are the same, sir. This means that such processes will be such that delta H mixing will be zero. Tell me, do you understand what I'm saying? If all the interactions are similar, that means if the similar type of interactions, they are replacing the same kind of interaction. So, ultimately, bond dissociation and bond breaking, bond breaking and bond making will be exactly the same. Which means the net heat exchange will be considered zero. And because the interactions are similar, the change in volume will also be zero. 10 ml of mine and 10 ml of yours will combine to prepare 20 ml of solution, sir. Because all interactions are similar, sir. First, we were alone, now we are with you, but it's similar. It doesn't matter. This means, sir, 10 ml and 10 ml will combine to form a 20 ml solution. And this is ideal. That is, what does ideal mean? 10 ml + 10 ml combined to prepare a 20 ml solution. This is ideal. That is, what is the change in mixing? Sir, the change in volume is zero. It was 20 before. It is 20 afterwards. Sir, the change in volume mixing is zero. Let's talk about delta S mixing. My suggestion is that you memorize this fact without thinking: the entropy of mixing is always positive. Whenever mixing occurs, the entropy change will always be positive. Because mixing creates an asymmetric system. AB is asymmetric. AA is symmetric. That is, if you look, it's happening like this. A + B gives AB. So, if you look carefully, this is a symmetric system, AA. This is also a symmetric BB. But this is asymmetric. And an asymmetric system always forms a random system. Its entropy is always higher. This means, sir, if you want to find delta mixing, the entropy here is higher. The entropy here is lower. So, the change in entropy will be positive. And as far as delta G mixing is concerned, because mixing has occurred, delta G is negative. Because you might remember that if any process occurs, the free energy change is negative. So, this means if two substances are mixing, no matter what kind of solution is formed, mixing has occurred. If mixing has occurred, delta G will always be negative. And my suggestion is to remember this. No matter what kind of solution it is, this is always true. Because whatever the solution, if mixing occurs, entropy will definitely increase because asymmetry will arise, and mixing is happening. Therefore, delta G will always be negative. So, whether it is an ideal solution or a non-ideal solution, these two terms will always be fixed. That is, delta S mixing and delta G mixing. Clear? Is it okay up to here? Let's move to the next point, sir. The next point is, sir, what happens if I talk about non-ideal solutions? It's very clear, sir. Non-ideal solutions will be those solutions that do not follow Raoult's law over the entire range. That is, the value of PT will not always be equal to PA not XA + PB not XB. Sir, the matter is settled. That is, those solutions which do not follow Raoult's law over the entire range of composition. Sir, they are non-ideal solutions. If I talk more technically, what is the technical बात? The technical बात is that similar kinds of interactions, that is, now a particular kind of interactions, they are now being replaced, meaning the interactions that I am going to replace after mixing are different, sir. Earlier, you had hydrogen bonding. Now you don't have hydrogen bonding. So, this means the interactions before and the interactions after mixing are changing. And if the interactions are not the same, sir, those solutions are non-ideal solutions, sir. Such solutions will be categorized as non-ideal. Is it clear? Did everyone understand? That is, it is very simple, very easy. First, remember the legal definition. What is the legal definition? Solutions that do not follow Raoult's law over the entire range of composition. What is Raoult's law? PET = PA not XA + PB not XB. That is, those that always follow this are ideal solutions, and those that do not follow this are non-ideal solutions. Clear? Now, if you talk about non-ideal, there are two types: positively deviated and negatively deviated. What are positive deviations? Sir, when do positive deviations occur? Positive deviation means the vapor pressure is higher than what it should be according to Raoult's law. Positive deviation is occurring. Deviation means moving away from the ideal line. Deviating. But deviating upwards. That is, the vapor pressure is increasing. We said, what does it mean? It says that for such solutions, somehow, if such a situation appears that the value of PT is greater than PA not XA + PB not XB, then an ideal situation, an ideally positively deviated system is being prepared. We said, how can this be possible that the total vapor pressure comes out to be greater than the ideal situation? It says it can happen, and for that, the perfectly beautiful definition is that whenever stronger interactions are replaced by weaker interactions, whenever strong interactions are replaced by weaker interactions, a positively deviated system is generated. What does it mean, sir? I asked A, "Brother, tell me, how did you feel when you were alone, and how do you feel now that you have joined B?" If A replies, "Oh, I feel so free now. Earlier, there were A and A, so we were more bound. Now I have come with A and B, or now I have come with B, so I feel so free. Now I will fly more, due to which the vapor pressure will be higher." Sir, this will form a positively deviated system. And when will this happen? This will happen when the interactions within AB are weak, and the interactions of A and BB are strong. That is, when they are mixed, a weaker interaction is produced. That is, a weaker interaction has replaced a stronger interaction. So, whenever weaker interactions replace stronger interactions, sir, in that case, the value of PT will always be greater than PA not XA + PB not XB, and such solutions will be categorized as non-ideal positively deviated solutions. That is, when does this happen in positive deviation? When the interaction of AB, that is, the interaction formed by mixing A and B, is weaker than their individual interactions. If it becomes weaker than any of the individual interactions, you will see a positively deviated system. Any of the interactions, whether it is the interaction of AA or the interaction of BB. If the interaction of AB is weaker than even one of the interactions, you will see a positively deviated system. And I will definitely prove this to you somewhere. Is it clear? Okay, sir. As far as delta H and delta V are concerned, sir, now because A and B feel free. This means A and A were more strongly bound when they were alone. B and B were more strongly bound when they were alone. So, more energy will have to be given to break them. And when they join, it's a weak interaction, sir. So, less energy will be released. That is, more is given, less is released. That is, it is an endothermic process. And if it is an endothermic process, then it is positive, sir. That is, delta H mixing is positive. Then the same happened. Delta V mixing is also positive. Why? Because, sir, they will feel free, so combining 10 ml and 10 ml might result in 22 ml. Because they feel free now. Interactions are becoming weaker. Due to which the volume might increase. So, in such a case, delta V mixing will be positive. And delta S has already been discussed, sir. Whenever mixing occurs, delta is always positive. And because mixing is happening, delta G is always considered negative. Is this clear? Is it clear? AA interaction, look here, AB interaction is weak. That is, when A and B are mixed, weak interactions are formed. So, this means when will energy be released? Energy is released when bonds are formed. So, the weaker the bond formed, the less energy will be released. That is, less energy is released from their formation. And these are strong bonds. More will have to be given to break them. Brother, you have to break A and A, and B and B, only then will AB be formed. So, this means more has to be given to break them. Less is released during formation. So, this means more is given. Isn't it endothermic? So, this process is endothermic for us. That is, delta H mixing is positive. And what is being said for delta V? Sir, when two substances are mixing, the interactions are becoming weaker. So, it means it's like this: when 10 ml is added to 10 ml, because they are opening up, they might become 22 ml instead of 20 ml. They might become 24 ml. They might become 21 ml. So, the value of delta V will be positive. That is, if there is positive deviation, then delta H will also be positive. Delta V will also be positive. These two are always fixed, sir. They are always true. They will always remain the same, no matter what the solution, whether ideal or non-ideal. Clear? And in this, if you are asked to draw the graph, as we did before, it is perfectly correct, sir. It will be the same graph. If you talk about A, it used to form like this. If you talk about B, it used to form like this. Remember? In the ideal situation. And if you talk about the total, it used to form like this. Sir, this is the ideal situation, sir. But now the situation is not ideal, sir. Now the situation is not ideal, sir. Now it is non-ideal. A feels that now I will fly more. B feels that now I will fly more. So, this means A's situation is now this, sir. This is A's situation. B's situation is this, sir. And the total vapor pressure situation is this, sir. This is the actual situation, sir. Now everyone's vapor pressure is higher. That is, at the composition where you used to say that at this composition, my actual pressure of A should be this. This is PA not. This is PB not. That is, at the composition where the actual pressure of A should have been this. Do you understand this? This should have been this. Now that pressure is this. That is, A would have flown this much ideally, but now it is flying more. Why? Because it feels free now. Similarly, B's vapor pressure, which should have been this. Now actually this. Total pressure, which should have been this. Now it is this. That is, everything has increased. Sir, this is a positively deviated system, sir. This is a positively deviated system. Do you understand? That is, it is being said that when we mix two substances and prepare a positively deviated system, such a situation is observed. Second point, sir, if a positively deviated system is asked with an example, I will explain it with just one example. The rest, I want, in fact, I will tell you one or two more, but I want you to memorize them. Like, all these examples, you won't find them anywhere else. Memorize all these examples. Nothing will come from outside this. Okay? The first point is finished. But I am still trying to explain to you so that if it ever comes up, at least you can do it. At least you can do it. So, look, let me take ethanol and cyclohexane as an example. Let's do it here. Ethanol plus cyclohexane. I am just trying to explain. Ethanol plus cyclohexane. And I think everyone who is listening today will have their eyes opened. They will know that all these things are thought of like this. We have just memorized them. The matter is settled. Today you will understand that all this is logical. Every single thing is logical. Ethanol plus cyclohexane. Let's look at ethanol, sir. Sir, ethanol is this. CH3CH2OH. CH3CH2OH. If you remember, there is hydrogen bonding in ethanol. Sir, hydrogen bonding is observed in ethanol. I remember it very well, sir. There is hydrogen bonding in ethanol, sir. That is, the interactions between ethanol molecules are how, sir? They have hydrogen bonding. Okay, fine. Let's come to cyclohexane. This is cyclohexane. Let's assume cyclohexane is this. This is cyclohexane. And I think everyone will agree that cyclohexane is a non-polar molecule. There is no polarity between carbon and hydrogen. So, what kind of interactions will be between them? Sir, van der Waals. What are the interactions of non-polar molecules? Van der Waals. And hydrogen bonding in ethanol. Now, if I mix these two, what will happen? Just think, sir. Now, if you mix these two, something amazing will happen. What will happen, sir? The amazing thing will be that this cyclohexane, when you mix it with this, this cyclohexane will start to intrude between this hydrogen bonding. Sir, and it will weaken the hydrogen bonding of ethanol. Understood? That is, one thing is clear: cyclohexane reduces the extent of hydrogen bonding in ethanol. Now, if this happens, what will happen, sir? If this happens, sir, due to its intrusion, the hydrogen bonding is weakening. This means that by mixing these two, weaker interactions are coming. Earlier the interactions were strong. Now the interactions are weaker. So, that means weaker interaction is replacing weaker interaction is replacing stronger interaction. Stronger interaction, sir. This is positive deviation, sir. This is positive deviation. Tell me, did you understand my point? That is, I have explained this with one example. And many such examples are written here. My suggestion is, let's try another example. Sir, ethanol and acetone. Tell me, how will you prove that it is positive? Oh, what is in ethanol, sir? There is HB in ethanol, sir. Hydrogen bonding. And acetone, sir. Acetone is polar, sir. What is in polar, sir? There is dipole-dipole. If you mix these two, what will happen, sir? When you mix these two, sir, acetone will intrude between ethanol, sir, and by intruding between ethanol, acetone will try to weaken the HB. Electrochemistry will also happen soon, brother. First, let's do this, then we'll do redox, then we'll see which chapter to do. We will cover the entire syllabus very soon, very soon, okay? So, don't worry. Okay? So, this means, sir, ethanol and acetone have dipole-dipole interaction. When you mix these two, this dipole-dipole interaction will intrude into ethanol and weaken the hydrogen bonding. What kind of deviation will occur? Positive deviation will occur. So, I want you to memorize all these examples. Although everything is perfectly logical. Acetone + CH2. Can anyone tell me how it will be positive? Sir, acetone is dipole-dipole. And CH2 is van der Waals. Tell me, what will happen, sir? When you mix these two, this CH2 will weaken this dipole-dipole, sir. It will intrude between the dipole-dipole. Sir, it will intrude between acetone, due to which the dipole-dipole interactions will weaken. Due to which a positively deviated system will be prepared. This means, sir, explanations for all these examples can be given. But my suggestion is, memorize these nine examples silently. Finished. Clear? Let's talk more, sir. Exactly similar, like look at this. I am not doing this on my own. These questions are asked to us. Look at this question. I am not going into full detail, but I just want to ask you that if they ask me in this question, can you tell me which one shows positive deviation? If it is a single choice, because I haven't studied negative deviation yet. So, if it is a single choice, then I understand very clearly that acetone + CH2 shows positive deviation. Sir, the matter is settled. This means all the others are negatively deviated solutions. But this is positive deviation. We just studied it. I just took an example. Why? Because in acetone, there is dipole-dipole, and in CH2, there are van der Waals. This will intrude and weaken the dipole-dipole. Due to which you will see a positively deviated system. Clear? Did you understand? Let's talk more, sir. Now let's come to negative deviation. When will negative deviation occur? Exactly the opposite. Whenever weaker interactions are replaced by stronger interactions, sorry, when weaker interactions are replaced by stronger interactions, what kind of solution will be prepared? Negatively deviated solution. That is, earlier A is saying: "When I was alone, I felt free. Now that I have joined B, I feel bound." So, in such a case, the solution formed will be negatively deviated. And this will happen only when the AB interactions are stronger than both AA and BB. That is, if AB interactions are stronger than AA and BB, then it will become difficult for A to fly, difficult for B to fly, and the vapor pressure will drop. It is a negatively deviated system. Sir, this will be considered a negatively deviated system. Clear? This will be considered a negatively deviated system. Okay, is this understood? Let's talk more, sir. If I write the same thing for delta H mixing, etc., I don't think I need to say much more. Everyone will agree that sir, when writing delta H mixing, it will be negative this time. Delta V mixing will also be negative. These two are already fixed. If mixing occurs, delta H mixing will be positive. And because mixing is spontaneous, it will always be negative. That is, this will always be true, no matter what. Clear? Is it understood? As far as the graph is concerned, sir, the graph is also very straightforward. Sir, this time too, if you want, if you talk about the ideal situation, then sir, this is the situation. Look here, sir. This is the ideal situation. Look here, this is the ideal situation. This is the total pressure. But sir, now the situation is negatively deviated. Negatively means the vapor pressure is not coming out as much as it should, sir. Now it is coming less. So, what does this mean? Sir, this means that the curve that is forming now, sir, is forming like this. A's pressure is also coming less. B's pressure is also coming less than the ideal situation. And the total vapor pressure is also coming less than the ideal situation. Sir, this is a negatively deviated system, sir. That is, if you say that at a particular composition, if I talk about pressures, then the pressure that should ideally have been for A, sir, actually this is PB not. Let's consider this as A not. So, ideally, it should have been this. Now it is coming more. Understand? Earlier it was coming this much, now it is coming this much. Similarly, B's pressure should have been this. Now it is coming even less. Total should have been this, sir. Total is also coming less. That is, individual vapor pressures have also fallen, and total vapor pressure has also fallen. That is, this will only happen. This means that now what is the expression? PT is less than PA not XA + PB

This is not an ideal negatively deviated system, sir. It will be considered a non-ideal negatively deviated system. Is that clear? Okay? Good. Now, as far as examples are concerned, I have written a total of six examples here, and my suggestion is that you do not need to memorize anything beyond these six. Yes, it is true that you should have good clarity, or else you should know the logic. For instance, let me explain with an example. This first example is also given in NCERT and is explained very clearly. What happens when chloroform is mixed with acetone? So, let me show you. I will show you how to make chloroform. Chloroform is this. CH Cl3. This is chloroform. Now, tell me, can you see that chloroform is a polar molecule? Yes, sir, it is clearly visible. So, I believe everyone knows the interactions that occur within a polar molecule. Sir, if a molecule is polar, then there will be interactions between its polarities, which are called dipole-dipole interactions. That is, dipole-dipole interactions in chloroform. Okay? Good. Now, let's come to acetone. If you look at acetone carefully, you have now memorized that acetone is also a polar molecule. It is also polar, and the interactions within it are also dipole-dipole interactions. Absolutely correct, sir. Now, mix these two, sir, and it will be fun. Let's mix them. What will happen when you mix these two? Sir, when I mix these two, a stronger interaction will be generated between them, which will be called hydrogen bonding. How? Look here, sir. CH3 C = O CH3. Sir, you will see hydrogen bonding of a decent strength. Sir, this is chloroform. And this is hydrogen bonding, sir. So, what does it mean, sir? It means that initially, there was dipole-dipole interaction, but due to the mixing of both, HB came. And you know that HB is more dominating than dipole-dipole. So, that means this is a stronger interaction, and these are weaker interactions, and this stronger interaction is replacing these two weaker interactions, sir. Sir, this is a negatively deviated system, sir. This is a negatively deviated system, sir. Now, if someone says to evaporate from acetone, what will it say? Oh, we were alone before, we used to evaporate more. Now that we have come with this, we are more bound. We cannot evaporate now. If someone says, "Let's evaporate from chloroform," what will it say? We were alone, so there was dipole-dipole interaction. We used to evaporate more. Now, chloroform, having come with acetone, is bound by hydrogen bonding. Now we will not evaporate. That is, the vapor pressure that will come out will be less than the ideal situation. And this is a negatively deviated system. Clear? Tell me quickly, did you understand? See, those who are studying will understand these things a lot, and today they will understand that this is how these things are thought of. We never thought about it. And I am not taking all the examples. In fact, you can prove this with all the examples, and I can tell you more things here. But my suggestion is that you just learn these examples and nothing else. Just learn these examples. I can explain each one to show why they are showing negative deviation. But I don't want to go into that detail because perhaps it is not needed. In the exam, you will only be asked which ones are ideal and which ones are non-ideal. So, if you have memorized these examples, your work will be done. Clear? Did everyone understand? Okay? Let's talk further, sir. Now, let's take one more step, and look at this question. This is a question that has been asked. The question is, if miscible liquids are showing negative deviation, if you see negative deviation, what will happen? So, we said, look, if there is negative deviation, the vapor pressure will decrease. It will decrease. Do you agree? Vapor pressure will decrease. So, this means these ones are messed up. This one is messed up. Because vapor pressure will decrease. Here it is an increase. Now, both of these are decreases. Sir, a decrease in vapor pressure leads to an increase in boiling point. Why? Because boiling point means when vapor pressure becomes equal to atmospheric pressure. Boiling occurs when vapor pressure is equal to atmospheric pressure. So, if the vapor pressure has dropped, it will take longer to reach the atmosphere. That is, more heat will be required. That is, the boiling point will increase. That is, if vapor pressure is decreasing, then boiling point should decrease. That is, the correct answer should be D. Clear? That is, it is absolutely clear. Vapor pressure will decrease. Boiling point will increase. And I will understand this in colligative properties as well. Clear? Let's talk more, sir. Next, I want to have a small discussion. An ideal system is a system. Although it has no use, I want to explain it to you. Ideal solutions, when formed, can be separated by the distillation process. Separated means, for example, you mixed two substances, and an ideal solution of A and B was formed. Then those substances will convert into vapor. You condensed this vapor, let's say. Then this condensed vapor will also evaporate. Then new vapor will form. You condensed that too. Then vapor formed, you condensed that too. If you do this work many times, you will see that you can separate A and B from each other. You can separate A and B from each other. If an ideal solution of AB has formed, then you can separate that ideal solution from each other by fractional distillation or distillation process. Let me explain the process. The process is this. You mixed A and B. Okay? Let's assume A is more volatile. That is, A evaporates more. So, there will be more A in the vapor phase. Okay? Now, what are we saying? We took this vapor and condensed it here. Condensed means converted it into liquid. So, if this vapor has converted into liquid, then there are two A's here. I am just explaining. So, there will be two A's here as well. Whatever was in the vapor there has now converted into liquid, so there will be two A's here. Okay? Now, this A is more volatile. You said so. So, if there are two A's here, then more A's will come into the vapor, so there will be three A's. Now, those three have condensed here. Here there are four A's, those four have condensed here. Here there are five A's, those five have condensed here. There will come a time when you will see almost all A's in one container. That is, you are seeing the value of A increasing below: A, 2A, 3A, 4A, 5A. That is, the amount of A is continuously increasing. And there will come a time when you will see only A. And this is distillation. You have separated A from B, sir. That is, the distillation process is applicable to an ideal solution. You can separate an ideal solution into A and B by this method of distillation. That is, if you mix A and B to form an ideal solution, then A and B from that ideal solution can be separated again by this method. Clear? Is everyone understanding how it is happening? Sir, it is very easy. A and B formed A. More A formed. We are assuming here that A is more volatile. So, A will evaporate more. If B were more volatile, then B would form. So, A formed. Then we took this vapor and condensed it here. So, if there are two A's here, then there will be two A's here as well. Okay? Now, since it evaporates more, if there are two here, then there will be three in the vapor. Now, condense this again. So, if there are three here, then there will be four here. So, gradually, the amount of A will increase. This is known as the distillation process. I can also understand this from this graph. What is this graph? This is the line that defines the vapor pressure of the liquid state and the composition of the liquid, and from this composition, it calculates the vapor pressure. The line I have drawn below it calculates the vapor pressure from the composition of the vapor phase. That is, what it means is that if we talk about this particular composition, this is XA. Then, when the XA of a pure ideal solution is this, what is the total vapor pressure, sir? That total vapor pressure will be determined from here, sir. Look here, this is XA. You cut here and extend this line, sir. This is the total pressure, sir. This is PT. Okay? And if you calculate from YA, YB, will it be the same? Yes, sir. PT was calculated with the help of XA, XB. So, if you also calculate the total pressure with the help of YA, YB, it will be the same. So, how will the value of YA, YB be found? Sir, you have extended this line. It is cutting the vapor line. So, the composition of the vapor is obtained. This is the composition of the vapor. That is, what it means is that the composition of A. At that time, if it is X, then the composition of A in the vapor phase at that time is this. Understand the method. Came from X. Extended the line above XA, calculated the total pressure. Cut that total pressure with the vapor line and brought it down. So, with the help of XA, you got YA here. Okay? Now, what did we do? Tell me. Sir, you would condense this YA again by cooling it. So, when you condense this again, this YA will now become XA for the second liquid. Look here, what was YA here, now it is X. 2A, 1B, 2A, 1B. So, the composition of the vapor phase here is the composition of the liquid phase here. That is, X has become YA. From this Y, a new vapor phase will come, which will become its X. That is, what it means is that the YA that came from here became X for the second container. Now, if it has become X, then what will be the vapor pressure, sir? It will go up again, and this line will be cut above, sir. Look here, this is the vapor pressure. And if you want the composition of the vapor of this vapor pressure, then sir, it will come down. Then it will be cooled again. That is, what it means is that it is proceeding like this. It is going like this, like this, like this, like this, like this, like this, like this, like this, and at some point, you will get pure A. This is what I wanted to say, that if you talk about an ideal system, then for an ideal system, the distillation process is a good distillation process in which you can separate both components of that ideal solution from each other, and you can enrich your solution with the component that is more volatile, and you can increase it. And what is the method for that? The line for the liquid phase is this. The line for the composition of the vapor phase is this. You took XA, so XA will cut the upper line. It will tell you the total pressure. Okay? Now, this total pressure will also be due to YA. So, what will YA be? So, we cut the line of this total pressure with the lower line and brought it down. So, if XA is this much, then YA is this much. Okay? YA is known. Now, you will make this YA the XA of the second container. So, this XA will again cut the liquid line. What will be its pressure? This much. And what will be the vapor of this vapor pressure, this Y, how much will it be? This much. Brought it down. Then made it X again. That is, you kept moving forward, moving forward, moving forward, and ultimately you reached where? Ultimately, I reached the pure liquid, the pure component that I wanted to separate. But this action you are doing, you are doing for an ideal system. You cannot do such an action for a non-ideal system. Understand? Well. So, now, if we talk about the second thing, the second thing is that a big drawback within a non-ideal system is this. If I work for a non-ideal system, let's see how it will happen. This is A, this is B. Which one will evaporate more? A. So, two A's will come here. Just like we were doing. These two A's will come down. So, more A will evaporate. So, three A's will come here. Those three A's will condense here. So, three will come here. Now, it will become four. After becoming four, it should become five. Sir, it became four, so it is also four. What is this? And if it is four, then when you condense it, it will also be four. And if it is four, then it will also be four. When there were four here, and four formed here, then if there are four here, then four will form here as well. We said, what is this? How is it happening that after a certain composition, you are unable to purify it further? You are unable to separate A from B any further. Whereas in the previous situation, what was happening? Sir, in the previous situation, the situation was that you took a place, two came, two A's came, three A's came, four A's came, five came, six came, seven came, and it filled up. Sir, it filled up with A. Sir, this is the situation of an ideal situation, sir. It will not happen like this in a non-ideal situation, sir. In a non-ideal situation, it is a big problem. In a non-ideal situation, there will come a time when the composition of the vapor phase and the composition of the liquid phase will become the same, sir. Now, if you think about it, if this is also 4AB and this is also 4AB. Then when you condense it, it will also be 4AB, and if it is 4AB, then it will also be 4AB. Then you condense it, and it will be 4AB. So, you will not be able to separate A and B any further. This situation that has arisen is called an azeotrope. This is known as an azeotrope. That is, azeotropes are observed within a non-ideal system, whether it is positively deviated or negatively deviated. Azeotropes will be seen in non-ideal situations, and they are seen when either the azeotrope is called when the composition of the liquid phase and the vapor phase becomes the same. When the value of XA, XB of the liquid becomes equal to YA, YB, then you will not be able to separate those two liquids any further. And that system is known as an azeotropic system. Which starts boiling at a fixed temperature. Now you will not be able to separate it further. 4A, 4B, 4A, 4B, 4A, 4B, 4A, 4B. That is, what it means is, sir, here four A's, and above also four. Now in every container, you will see 4A and 1B, 4A and 1B, 4A and 1B. That means, sir, now this system has become like a pure liquid, sir. Pure liquid evaporates, vapor forms, then it condenses again, pure liquid, pure liquid, pure liquid, pure liquid. This means, sir, an azeotropic mixture behaves like a pure liquid and starts boiling at a constant temperature, sir. Sir, it is a system in which the liquid phase composition and vapor phase composition are similar. But this only happens when a strongly negatively deviated system or a strongly positively deviated system is in front of you. That is, if you talk about azeotropic mixtures, then an azeotropic mixture will be a mixture, a binary solution containing two volatile liquids in which both liquid and vapor have the same composition. Sir, if the composition of the liquid and vapor are the same, then sir, that system will be considered an azeotropic mixture. Sir, this will be considered our azeotropic mixture. For example, if we talk about it, there can be other definitions. For example, the composition of a liquid mixture at which distillation cannot separate the two liquids because the condensate has the same composition as that of the azeotropic mixture. That sir, now you will not be able to separate the two people any further under any circumstances. Because the composition of the person being prepared by condensation is the same as the composition of the liquid phase was before. That is, what is below is now above. Now you will not be able to separate the two liquids any further. These are called azeotropes. Such azeotropes that are formed from positively deviated systems are known as minimum boiling azeotropes. That is, what it means is, look, I will prove it to you here that you cannot separate. Look how. Suppose I take a particular composition. Let's take this composition. Okay? Now, what will be the composition of the vapor, sir? It will be this. Now, when you condense this again, the liquid will be this. Okay? You are moving along. Moving along. Moving along. Moving along. Moving along. Moving along. Just stop here, sir. You cannot purify any further from this portion. That is, if I take the system of water and ethanol, then you cannot separate water and ethanol beyond 95% ethanol and 5% water. Because now you have reached this composition. And this composition is our azeotropic composition. That is, now you cannot separate it any further. And these are the minimum boiling azeotropes observed within positively deviated systems. That is, when are minimum boiling azeotropes formed? When these azeotropes are formed by solutions having large positive deviations from Raoult's law. Solutions that show high large positive deviations from Raoult's law. Such solutions, our positively deviated system people, will form minimum boiling azeotropes. Why am I saying minimum? Because if there is positive deviation in vapor pressure, it means vapor pressure is high, and due to high vapor pressure, the boiling point decreases. So, who will form minimum boiling azeotropes? Positively deviated systems. And if we talk about the boiling point, then the boiling point will be observed to be lower than that of any solution. That is, for any of the two components, like water and ethanol. Then, from the boiling points of both, you will see a lower boiling point of this minimum boiling azeotrope. Clear? That is, azeotropic mixtures are very interesting. Children do not understand how an azeotrope is formed. See, if a negatively deviated system or a positively deviated system is taken, it can form an azeotrope. See, it is in front of you. Azeotrope means you cannot separate it any further. Why? Because the composition of the vapor phase and the composition of the liquid phase have become the same. That is, here XA

And X YA same. The rest is not there, sir. Here XA is this. YA is this. Understand the point? For example, if we talk about any point, sir, let's assume XA is this. Then tell me, what will YA be? So what will we do, sir? We will raise this line upwards. We will raise this line upwards and YA will be this, sir. Meaning, at the time when XA is this, at that time YA is this. They are not same. They are not the same, sir. But after reaching this point, sir, XA and YA will become the same, sir. And when XA and YA become the same, then you will not be able to separate these two any further. And such a system will be known by the name of azeotropic system. This is minimum boiling azeotrope. And similarly, this will be our maximum boiling azeotrope, which will be formed from negatively deviated systems. Meaning, these azeotropes are formed by the solutions which show negative deviation from Raoult's law, and the boiling point that will come out will be greater than the individual components. Because these are maximum boiling azeotropes. Is it clear? Did you understand this? It is very straightforward. Very easy. Is it clear? For example, let's talk. Look at this. What are they trying to say? They are saying, can you tell which of these will form minimum boiling azeotropes? Sir, minimum boiling azeotropes are formed by those which are positively deviated systems. Meaning, positively deviated systems form minimum boiling azeotropes. So, only those that show positive deviation will form our minimum boiling azeotrope. And if you have memorized it, you will know that positive deviation is not present in this. Not present. So, what will our negatively deviated system form? It will form a positive maximum boiling azeotrope. So, if you are being asked, who is the one that forms a minimum boiling azeotropic mixture, then the minimum boiling, minimum boiling point, minimum boiling azeotropic mixture will be formed by the one with positive deviation. And who does not form it? Meaning, among these, the one that shows negative deviation will be our answer. So, if you look at the first one carefully, it is HB in water. And this is our ketone type. It has DPDP. So, what will happen? You must have learned. HB will disturb DPDP. What will be formed? Positive deviation. If there is positive deviation, then a minimum boiling azeotropic mixture will be formed. So, this is correct. Let's take the third one. CH2 Van der Waals acetone DPDP, do you remember? What will happen, sir? It will enter inside. What will be formed? Positive deviation. This HB HB, this DPDP. What will happen, sir? It will enter this HB. What will be formed? Positive. So, which answer is correct then, sir? B. Phenol and aniline always show negative deviation. Due to the negative deviation of phenol and aniline, they form maximum boiling azeotropic mixtures. All these students can do this if they have memorized the examples. You are seeing how beautifully this question has been made in 2025. Those who went by rote memorization will not understand anything, and those who went by understanding will understand that sir, if you put DPDP into HB, then DPDP will weaken HB and create positive deviation. Sir, if you put Van der Waals into Van der Waals or DPDP, then Van der Waals will weaken DPDP and create positive deviation. If you put DPDP into HB, then DPDP will weaken HB and create positive deviation. Therefore, the answer should be B. Clear? Understood? And here you go, sir. Let's take another example. What is being asked, sir? Which of the following options is correct? Let's check. Sir, look, this is the method. First, let's check A, because A is both A3 and A2. So, by looking at A, two answers will be wrong. Let's see which one is correct. Let's check. A is a solution of chloroform and acetone. We just studied this. Chloroform starts forming hydrogen bonding with acetone. Meaning, strong interactions are created. Negative deviation occurs. And when negative deviation occurs, they form maximum boiling azeotropes. Remember? Meaning, it is clear that sir, if you take acetone, it will form a maximum boiling azeotrope. Meaning, if it is A3, then it will not be A2. Meaning, these two options are wrong. Let's cross them out. These two options are wrong. Okay? Now let's check among these. B is also different, C is also different. D is the same. So, let's check anything between B and C. Let's check C. Solution of benzene and toluene. When people are similar, an ideal solution is formed. And for an ideal solution, delta V mixing is zero. Meaning, sir, meaning what it means is, delta V mixing of benzene and toluene is zero. Meaning, C should be 4. So, if C should be 4, then the answer should be A. Understand the point? You can check very easily. Clear? Understood? Let's move on, sir. Now let's come to colligative properties. Let's go, sir. Now this is interesting, and numericals are asked on this. So, we just need to understand what colligative properties are. So, look, first of all, we need to know about colligative properties. What are colligative properties called? Properties that will depend only on the number of solute particles, not on their nature. Such properties are our colligative properties. Meaning, if the number of solute particles increases, that property will increase. If the number of solute particles decreases, that property will decrease. Such a property is called a colligative property. Meaning, that property of solutions which depends only on the number of solute. That is colligative. Clear? Now, there are two conditions for studying these things. First, that our solution should be dilute. First, this is absolutely clear. Solution should be a dilute solution. And secondly, we are talking about the first case. Non-volatile solute in volatile solvent. Meaning, if you use a non-volatile solute, meaning the solute should be non-volatile. Meaning, the first case we used to have. Meaning, what kind of solutions' colligative properties are we talking about? We are talking about the colligative properties of those solutions in which the solute is non-volatile and the solvent is volatile. We will talk about the colligative properties of that solution. Okay? Meaning, which property? Which property is it? A property that depends only on the number of solute particles. Okay? The very first property is relative lowering of vapor pressure. You have already studied this. We have already covered this. How, sir? Do you remember the first case, sir? Yes, sir, do you remember the value of Ps? Ps = P not * mole fraction of solvent. Yes, sir, I remember. I definitely remember. Ps = P not * mole fraction of solvent. That was the first case. This was the case for non-volatile solute. Sir, what is relative lowering? We said, look, you know that by adding solute, the vapor pressure of the solution decreases from the vapor pressure of the pure solvent. Yes, sir, you told me that. So, what is the lowering? Sir, the lowering is P not - Ps. Meaning, how much was it before? P not of the pure state, and after adding solute, it reduced to Ps. This is the lowering. What is the relative lowering? We said, sir, with respect to the initial, this is relative. What was the initial, sir? When you brought water, the initial is P not. Meaning, P not - PS / P not. This is relative lowering of vapor pressure. First thing, did you understand, man, what are you doing with duration, duration? We don't know how long the duration will be. It's just going on, when it finishes, it will be over. Okay? So, relative lowering of vapor pressure means P not - PS is the lowering, divided by the initial, it is relative lowering. Meaning, it is clear, sir, relative lowering is always P not - PS / P not. Clear? And sir, you have also memorized the formula for this. Do you remember, sir? We memorized it without cheating. n solute / n solute + n solvent. Absolutely, no cheating, sir. Absolutely honest. This is n solute + n solvent. If you say in the question that n solute is very less than solvent, then I can write it as n solute by n solvent. Otherwise, this is my relative lowering of vapor pressure. That's all. This is relative lowering of vapor pressure. So, whenever relative lowering of vapor pressure is asked in a question, you have to find the value of P not - PS / P not with the help of this expression. Understand the point? Did everyone understand? Yes, I know another formula. That formula is not for relative lowering. Now you tell me, if I write P not - PS / PS, if I write this, which I write as n solute / n solvent, do you remember? I emphasized this formula a lot just now. This is our formula. But tell me, is this relative lowering of vapor pressure? Is this, sir, relative lowering? No, sir, sir, P not - PS is lowering, but if you divide by PS, it is not relative lowering because relative is always calculated from the initial value, and the initial was the vapor pressure of the pure solvent, that is P not. So, relative lowering of vapor pressure will always be P not - PS / P not, and this equation, yes, I also know this equation. Meaning, if I am given P not and PS, then I can use this equation. I can use this one too. It is better to use this one because it is easier. But if the name relative lowering of vapor pressure is mentioned in the question, then you have no choice but to use this formula, because this is not relative lowering. I have told you many times. I am saying it again. This is not relative lowering of vapor pressure. This expression is not for relative lowering of vapor pressure. Relative lowering of vapor pressure is always P not - PS / P not, from which this formula is derived. Yes, if you are given P not and PS, then don't think too much. You have this option, you have this option too. Do as you please. And in such a case, in my opinion, it is wise to use this formula. It is better. It is easier. Clear? Okay, this? Let's go, sir. For example, let's talk. There are many questions. I mean, I will say the same thing again. I myself am surprised that you will find all similar questions if you pick them up and look. So, I will not waste much time. I will give you these questions to do yourself, and you will understand yourself that these two formulas of mine are finishing the entire chapter. When a non-volatile solute is added to a solvent. Okay, sir, this is the condition. Non-volatile solute. The vapor pressure of the solvent decreases by 10. Okay, vapor pressure of the solvent decreases by 10. So, this means that before it was P not, then it became Ps, and this difference is 10. Do you agree? Decreases by 10 means what? Decreases by 10 means it went from P not to Ps. What is the difference? 10. Okay, this. What is the second thing? The mole fraction of solute in the solution is 2. Mole fraction of solute is 2. So, the value of P not - PS is 10. And the expression we have is P not - PS / PS = / P not / P not = solute. Remember? So, this means, sir, we can see it is saying that the value of mole fraction of solute is given as 0.2, and P not - PS is 10, so I think P not can be calculated from this. So, the value of P not will be 10 / 2, right? Are we doing it correctly? So, this is 10 / 2, and this is 50. Meaning, the value of P not is 50 mm. 50 mm. Okay? Now, what is the second part? The second part is asking, what will be the mole fraction of the solvent? If the vapor pressure decreases to 20. So, we said, okay, now you have made a second case. So, meaning, if the decrease in vapor pressure is 20, then the value of P not - PS is now 20. But you have already calculated P not. Your P not is 50. So, we all know that the value of P not - PS / P not is mole fraction of solute. This formula. We can write mole fraction of solute as 1 - mole fraction of solvent. P not - PS is 20. The total vapor, the value of P not, you have already calculated as 50. And this is 1 - mole fraction of solvent. So, if you calculate the value of mole fraction of solvent from here, the value of mole fraction of solvent comes out to be 0.6. Okay? This is 4. So, if you subtract from 1, this is 0.6. A good question. It's a 2025 question. A good question. In the beginning, it seemed like why were these two things done? Meaning, once the decrease in vapor pressure is given as 10, and once the decrease is given as 20. So, it will strike you immediately that when it is given as 10, calculate P not from it. Because if P not - PS is 10, let P not be P not, and this expression is equal to mole fraction of solute. Remember, n solute / n solute + n solvent, and mole fraction of solute is given as 2. This is 10. This is P not, and this is 2. So, it means P not comes out to be 50. One task is done. Now, what is the question asking? If the decrease is 20, what will be the mole fraction of solute? So, you have applied the same formula again. You have already calculated P not. Now you calculate mole fraction of solute. By subtracting from 1, calculate mole fraction of solvent. Clear? Excellent question. Okay? Let's talk more. And you will see that all these are similar. Meaning, this line, look here. What are they trying to do here? Same. Exactly. They are asking, can you tell what will be the order of relative lowering of vapor pressure? So, we said, look, this is how it is. I know relative lowering of vapor pressure is P not - PS / P not, whose value is calculated from n solute / n solute + n solvent. Remember? And n solute involves the weight and molar mass of the solute. So, one thing is clear, the higher the molar mass, the lower this value will be, and the lower the relative lowering will be. Meaning, the solute with higher molar mass has lower relative lowering of vapor pressure. Meaning, if the molar mass of the solute is higher, then the relative lowering of vapor pressure will be lower. So, I see the highest molar mass in C. So, C's relative lowering should be the least. So, the answer will be A > B > C. Clear? Every positive deviation mixture will be a minimum boiling azeotrope. You are absolutely right, Yash. You are absolutely right. Every negatively deviated system, which is a highly negatively deviated system, always forms an azeotrope that is positively, a maximum boiling azeotrope, and positively deviated systems always form minimum boiling azeotropes. Clear? Let's move on, sir. Let's come to the next point. The next colligative property is boiling point. Elevation in boiling point. Boiling point elevation is also considered a colligative property. So, I said, meaning, a colligative property means if you increase the solute, the elevation of boiling point will increase. He said, yes, keep increasing the amount of solute. Add one spoon of sugar, add two spoons of sugar, add four spoons of sugar. So, as the sugar increases, the elevation of boiling point, the elevation in boiling point, will increase. The elevation of boiling point will keep increasing. So, elevation is a colligative property. So, I said, how will you prove this, man? So, look, the explanation is very straightforward and very easy. One explanation is very simple. Meaning, what is a simple explanation? We can say theoretically, which we can also write here, that as sugar is added, the vapor pressure decreases. Remember? Does everyone remember? With the addition of solute, the vapor pressure decreases. So, how much solute you add? Why? Because sir, you have already explained this equation: the value of Ps is P not * mole fraction of solvent. So, as you increase the solute, the solvent decreases, and as the solvent decreases, Ps also decreases. So, on increasing the solute, the mole fraction of solvent decreases, and with the decrease in mole fraction, Ps, the vapor pressure of the solution, also starts decreasing. Okay, this? Your vapor pressure starts decreasing. So, in such a case, sir, if the vapor pressure is decreasing, it will take time to boil. Why? Because you explained that the boiling point is the point where vapor pressure is equal to atmospheric pressure. Boiling starts when the vapor pressure becomes equal to the atmospheric pressure. So, if your vapor pressure is already low, then the atmospheric pressure is the same, right? The atmospheric pressure is fixed. Now your vapor pressure has decreased by adding sugar. So, it will take more time to reach 1 atm, to reach atmospheric pressure. You will have to apply more heat. Your boiling point will increase. Meaning, what it means is, by adding sugar or by increasing the moles of solute, the mole fraction of the solvent decreases, and the vapor pressure decreases. We know this. If the vapor pressure decreases, it will take time to reach atmospheric pressure, due to which the boiling point will elevate. One simple explanation is this. The second explanation is a graphical explanation. Very easy. Try to understand. Let's take this line of vapor pressure. This is the line of vapor pressure, which, let's assume, reaches 1 atm. Meaning, boiling will start when the vapor pressure reaches 1 atm. Okay? Now I have taken pure solvent. Think and tell me, if I increase the temperature of pure solvent, the vapor pressure of pure solvent will increase. So, let's assume, sir, this is your pure solvent. Let's assume this is your pure solvent. At this particular temperature, the vapor pressure of pure solvent is this. Okay? This is the temperature. This is the vapor pressure. Now I start increasing the temperature. Tell me, is it boiling now or not? Oh, sir, what are you talking about? The value of vapor pressure is below 1 atm. It will not boil, sir. Okay? Let's apply heat. Now I start increasing the temperature. Do you remember that vapor pressure increases exponentially with increasing temperature? Yes, sir. Look, it started increasing. And a time came when the vapor pressure cut the line of 1 atm. Meaning, now for this solvent, this is pure solvent. We are not adding sugar yet. We are still talking about pure solvent. Sir, pure solvent.

This place was cut at 1 atm. So, at what temperature was the 1 atm cut? Sir, that temperature is called the boiling point of this solvent. This is TB, why? Because at this temperature, the vapor pressure of this solvent is equal to 1 atm. Clear? Now, let's do one thing, sir. Let's add a spoonful of sugar to it. What will happen when you add a spoonful of sugar to it? When you add a spoonful of sugar to this solvent, at the temperature at which the solvent's vapor pressure was this, at the same temperature, the vapor pressure of that one-spoonful sugar solution will decrease because adding sugar lowers the vapor pressure. That is, now the vapor pressure will start from here at this temperature, from below, sir. The vapor pressure will decrease, sir. Now, if you apply heat to it, the vapor pressure will increase exponentially, sir. See, it's increasing and will cut 1 atm here, sir. And where it cuts 1 atm, the temperature there, sir, will be the boiling point of this solution's vapor pressure. This is TB dash. So, this is Solution One, meaning one spoonful of sugar was added. Sir, add another spoonful of sugar. When you add another spoonful of sugar, the vapor pressure will decrease further. And then it will increase with increasing temperature. Sir, it will cut 1 atm there. And where it cuts 1 atm, the boiling point will be TB double dash. Sir, this is TB double dash. What are we learning? Sir, what we are learning is that as the amount of sugar increases, the boiling point keeps increasing. That is, this elevation is increasing. First, this was for the pure solvent. Add one spoonful of sugar, how much did it elevate? This much. Add two spoonfuls of sugar, this much. Add three spoonfuls of sugar, this much. That is, the spoonfuls of sugar are increasing. And this gap keeps increasing. So, this gap is a colligative property, sir. It is directly linked with the number of sugar spoonfuls. Is it clear? Meaning, as the sugar increases, the boiling point will also increase. Because as the sugar increases, sir, it will take more time for the solution's vapor pressure to reach 1 atm. You will have to apply more heat. This is the graphical explanation, sir. Is it clear? Is everyone understanding this point? Okay? That is, the boiling point is that point where the pressure of the vapors becomes equal to the atmospheric pressure. And because of that, when both pressures become equal, bubbles start forming inside that liquid, and air bubbles start forming, which you call boiling. Clear? Understood up to here? Okay, sir. This means, sir, we have understood that boiling point elevation is a colligative property. Okay? Now, tell us how it is calculated. So, let's try to calculate it. What is the method to calculate it? Sir, a very straightforward method has been devised to calculate it, sir. If you have understood that boiling point elevation is our colligative property, it means it depends on the solute particles. So, then this delta TB, which we are calling boiling point elevation, is directly proportional to molality. Molality includes the moles of the solute. So, if the moles of the solute are more, the molality will be more. So, delta TB will also be more. This means delta TB is directly proportional to molality. If I keep the proportionality constant, it becomes KB. So, delta TB = KB * M. This KB is a constant, known as the ebullioscopic constant or molar elevation of boiling point constant. This is the molar elevation of boiling point constant. Clear? So, this is delta TB, which is directly proportional to the molality of the solution. If sugar increases, molality increases. Because of this, delta TB also increases. The beauty of KB is that KB depends only on the solvent. It has nothing to do with sugar or salt. That is, add whatever solute you want. It doesn't matter to me. If the solvent is fixed, then this KB is fixed. Do you understand? The value of KB, meaning if I write it separately, what is this whole story? The whole story is that delta TB is a colligative property which is directly proportional to the number of moles of the solute. The moles of the solute are linked with molality. Molality also contains moles of solute. So, it is said that this is directly proportional to molality. Okay, sir, whoever made it. And if I put an equality sign, then delta TB is equal to a constant * molality. Where KB is our KB, our ebullioscopic constant. This is the ebullioscopic constant. Or it is also called molar elevation. This is molar elevation. Molar elevation constant. But this KB is the property of the solvent only. Property of the solvent only. That is, if the solvent is the same, then it doesn't matter how much solute you add. Our KB will be fixed because KB is a property of our solvent. This is correct. It is possible that KB is given in the problem, which is usually the case in most problems. But if KB is not given in some places, you can calculate KB yourself. So, if I have to calculate KB myself, I need to know this much information. KB = MR TB² / deltaH vaporization * 1000. If delta H is taken in kilograms, then this 1000 will be removed accordingly. Okay? So, this is our relation, the method to find KB. What are the values in this KB? Now, I am telling you this because a question has been made on this in Mains. So, you should have an idea about what these values are. So, all the values here are very clear. M is the molar mass of the solvent. It has nothing to do with the solute's molar mass. Everything is of the solvent. Molar mass of the solvent. TB is the boiling point of the solvent. DeltaH vaporization is the heat of vaporization of the solvent. Everything is of the solvent. So, if I know all these values, I can find KB by putting them here. And by putting that KB here, I can find delta TB. Understood? That is, I have a very straightforward formula to find delta TB. And that is KB * M. Nothing else to do. KB * M, and delta TB comes out. Finished. Clear? Understood? That is, it is clear that adding sugar elevates the boiling point. The more sugar you add, meaning you understand what sugar means, the more solute. The more solute you add, the more the boiling point will elevate. And if the boiling point is elevating, then our colligative properties are changing accordingly. Understood up to here? So, this is boiling point elevation. This is boiling point elevation. Well, if you look closely at this formula, I don't know if you remember it or not. But if we change this formula slightly, it can also become MR TB / deltaS vaporization * 1000. I don't know if you will understand it or not. But the thing is, deltaH / T is equal to deltaS vaporization. So, deltaH / T, deltaH / TB, that is deltaS. So, one TB will convert into deltaS, and one TB will remain. So, this is again a formula that can come before us, which is very important. So, everyone try to remember this formula as well. I remember that on the JEE Mains level, a question has been asked on this formula once. So, what is important for us? The formula is important. The formula is important that deltaH = no, delta KB, calculate KB. KB = M RTB² divided by deltaH vaporization * 1000. Or it can also be remembered as MRTB divided by deltaS vaporization * 1000. So, my suggestion is that you remember both these formulas, and the most important thing is that KB is a property of the solvent only. Property of the solvent only. If the solvent is fixed, then the value of KB is fixed. Finished. Clear? S is entropy. DeltaS is entropy change. That is, during vaporization, when liquid goes into vapor, the entropy change is deltaS. Clear? Okay, sir, let's move to the next point. Now, next, if I talk about the question, you can see. This is in front of you. These are the questions asked. For a child who has clarity, all this is nothing. Look, what is it trying to say? It's a vapor pressure versus temperature curve. It's a question asked in 2023. Quickly, think and tell me, can you see what the boiling point of the solvent is? Sir, the boiling point of the solvent will be that point where the solvent's vapor pressure is equal to 1 atm. So, which is the solvent's line? This one or this one? This one. Where is it equal to 1 atm? Sir, here. Look here. Look here. Do you accept 1 atm? Is everyone understanding? That is, this is the point where the solvent's vapor pressure, increasing, increasing, increasing, cuts 1 atm. And this is 82. So, the temperature is 82° Celsius. Clear? Imagine if it asked, tell me what is the boiling point of the solution? Then the boiling point of the solution is where it cuts. That is 83. If it asks, tell me what is the boiling point elevation in the solvent solution? Then the difference between 83 and 82, that is 1°, is your boiling point elevation. Clear? Understood? Okay, sir, let's talk more. Look here. This is the same thing I was talking about. You need the difference between delta TB of A and B. That is, there is a non-volatile solute, which should be 1 gram. That is, the weight or moles of the solute are fixed. I am dissolving this in 100 grams of different solvents. That is, the solute is fixed, but the solvent is changing. But the moles of the solvent are fixed. That is, the amount is fixed. So, this means molality is fixed. Sir, the moles of the solute are fixed, and even if different solvents are taken, but their weight is fixed, then molality will be fixed. So, this means, who will decide delta TB, sir? Sir, the expression for delta TB, you just told me that delta TB is KB * M. So, if the molality is the same. Do you understand? 1 gram of non-volatile solute has been fixed. It has been added once to 100g of A and once to 100g of B. So, if the grams are fixed, then molality will be fixed, right? Because molality is moles of solute, which is fixed, divided by weight of solvent. That is fixed, right, 100. So, whether it is solvent A or solvent B. Its weight is fixed. This means molality is given as the same. So, this means the ratio of delta TB, delta TBA, how will it be calculated, sir? It will be calculated from the ratio of the ebullioscopic constants of those two solvents. Do you agree? That is, if the molalities are the same, then it is clearly visible that this m will cancel this m. Do you understand? The molarities are both the same. So, this m will cancel this m. So, this means the ratio of delta TB will be the ratio of KB. And the ratio of the ebullioscopic constants is 1:5. So, the ratio of TB will also be 1:5. Clear? Clear? Absolutely straightforward, nothing is there. Absolutely easy. Okay, sir, let's move to the next point. And the next point is depression in freezing point. Okay, sir, let's discuss this quickly as well. This is also a colligative property. And this is your third colligative property. This third colligative property. What is this third colligative property saying? It is saying that just as adding sugar elevates the boiling point, similarly, adding sugar depresses the freezing point, it decreases. That is, if water freezes at 0°, then after adding a spoonful of sugar, the solution formed will freeze at -1°, at a lower temperature. That is, the freezing point depresses. The boiling point elevates. This depression is a colligative property. Just as elevation was a colligative property there, similarly, the depression of freezing point here is a colligative property. So, I asked to write two-three points about freezing point. So, the first point is that freezing point is that point where the crystal of ice starts forming. Where ice starts forming is called the freezing point. As soon as the first crystal of ice comes out, that is the freezing point. Okay? And what happens at the freezing point? At the freezing point, the solid and our liquid phase are in a dynamic equilibrium. Freezing always happens of the solvent. When you freeze a sugar solution, only water freezes. Sugar never freezes. And this is important. JEE has asked a question on this at the Mains level. I will show you. Okay? That is, freezing will always be of the solvent. Not of the solute. When we freeze a sugar solution, it's not like sugar freezes and comes out again. Only water keeps freezing. So, it means who will always freeze? Water. And what is good is that the freezing point is that point where the vapor pressure of the liquid phase and the vapor pressure of the solid phase become equal. This is also very important. That is, freezing starts when the vapor pressure of the liquid phase and the vapor pressure of the solid phase are the same. So, he said, please explain what you mean by this. So, look, I am trying to explain this graphically. Let's try to understand it once. I am trying to draw a graph for depression in freezing point, just like I drew a graph for boiling point elevation. Let's try to understand it once. Sir, because and this is vapor pressure and this is temperature. This is our temperature. Okay, sir. Because this time you are talking about freezing, it means it will get cold. You are talking about cooling. You are talking about cooling. And when you are talking about cooling, the vapor pressure will decrease. So, this means this time you are at a higher temperature and you are trying to freeze it slowly. That is, suppose your temperature is high initially. Your vapor pressure, I will take this as pure solvent. Okay? Now I will cool it. So, when I cool it, its vapor pressure will decrease. Okay, sir? This vapor pressure will keep decreasing. It will keep decreasing. It will keep decreasing. A time will come when its vapor pressure and the vapor pressure of this solid will become equal. That is, meaning, this is the line of vapor pressure of solid. Sir, solid also has vapor pressure. Yes, you have seen that steam also comes out of ice. Solid also has vapor pressure. Sir, this is that ice. This is that solid which has vapor pressure, sir. Sir, this is pure solvent water, and what is that point at which the vapor pressure of ice and the vapor pressure of water are the same? Sir, that point is this point. This is the point where the vapor pressure of solid and liquid are the same. This is the freezing point TF. Clear, sir? Now, let's do one thing. Let's add a spoonful of sugar to it. Then let's think. When you add a spoonful of sugar, the vapor pressure that was this before will decrease. Now, cool it. What will happen when you cool it, sir? It will keep freezing. The vapor pressure will keep decreasing. And a point will come when it will cut the vapor pressure of ice. Because ice has to freeze. Do you understand? Whether you freeze a solution of the solvent, freeze the solvent, or freeze the solution. The solid phase that will form will be of ice. That is, this line will always remain fixed. That is, this solution will keep freezing, and at this point, it will reach the vapor pressure of the solid. That is, this is Solution One. This is the point where the vapor pressure of the solution and the vapor pressure of the solid phase are the same. But that temperature has decreased, sir. This is TF dash. See, it has depressed, sir. By adding one spoonful of sugar. Sir, add another spoonful of sugar. If you add another spoonful of sugar, the vapor pressure will decrease further. Now, freeze it more. It will touch the solid at a further point. Sir, now this freezing point will decrease further because the freezing point is that point at which the vapor pressure of the solution liquid and the vapor pressure of the solid are the same. Sir, these are the points where the vapor pressure of the solid and liquid are coming out to be the same, sir, look here. So, the temperature will become tf double dash. That is, sir, as the sugar is added, what is happening? The freezing point has moved from here to here, from here to here, and it will reach lower, lower, and lower. Sir, this difference, this difference is increasing, sir. That is, sir, the depression of freezing point is a colligative property. Because as the sugar is added, the freezing point keeps depressing further. And in this too, I will say only one point: if this is a colligative property, then delta TF is directly proportional to molality. If I put an equality sign, then delta TF = KF * molality. If we talk about KF, then this is our constant, known as the cryoscopic constant. Or you can also call it the molar depression of freezing point constant. KF value is given in the problem. If it is not given, then you can calculate it from MR TF² / deltaH fusion * 2000. And you can also consider this as MR TF / deltaS fusion * 1000, as was said earlier. Is one thing clear? KF is the property of the solvent only. If the solvent is the same, then the value of KF is fixed. Finished. Absolutely the same. Clear. Clear. Okay, so this is exactly the same as what you were talking about, exactly the same. As far as the question is concerned, look, whoever has an idea is understanding. These are the same things. But only by doing it in this detail can one solve all these questions, otherwise, what can one do? Look, what is it trying to say, sir? It is asking, tell me which of these graphs is correct. Now, there is no need to think. It is understood, sir. This one seems correct, sir. Look at it. Which graph defines the freezing point of the solvent, depression in freezing point of the solvent, sir? It is clearly understood, sir. This is pure solvent. This is your freezing point, tf, and when you take the solution, it will cut here. So, this is the depression, sir. This is the depression. This graph represents the depression in freezing point. It is very straightforward, sir. Clear? Okay, sir, look at this. What are you trying to say here? Here you are trying to say. What happens to the freezing point of benzene when a small quantity is added. Finished, sir. If you add any solute to benzene. Benzene is a solvent. If you add any solute to this solvent, then we just discussed that the freezing point will depress. So, this means the freezing point will definitely decrease. Sir, this is old news, sir. Clear? Understood? Very straightforward, and these are all asked questions. It's not like, sir, you are talking about new questions. These are all asked questions, and very straightforward questions have been made. Very straight, very straightforward. Clear? Okay, let's do one more question if there is one. Look at this. What is it saying?

We want to say. C6H6 is benzene. Its freezing point is 5.5. The temperature at which a solution of 10 grams of C4H10 in 200 grams of C6H6 freezes. So it's very easy, sir. That is, I need the value of delta, I need the value of delta TB. Sorry, I need the value of delta TF. So the value of delta TF is KF * M. The value of KF is given as 5.12. I say, learn this, brother. Learn the KF of benzene, it is 5.12. So KF * M. What is molality? Moles of solute, 10 grams of C4H10, meaning 10 grams means 10 / 58 moles. 10 / 58 molality. Moles of solute divided by weight of solvent. What will that be? 0.2. Is this in grams? So if you write it in kilograms, it will be 0.2 kg. So moles of solute divided by weight of solvent is the molality. So delta TF is this. Let's solve this. What will this come out to be? Sir, when you solve delta TF, what will it become after solving? Let's see. So if we solve delta TF, what is it coming out to be? 5.12 into what is this, brother? 10 / 58 / 2. Sir, this is coming out to be 4.4, sir. That means delta TF is 4.4. So if delta TF is 4.4 and the freezing point of benzene is 5.5, then what will be the new freezing point? What will be the new freezing point of the solution, sir? Because the freezing point is depressing. What was it? 5.5 and it depressed by 4.4. Do you understand? So if we subtract 4.4 from 5.5, then 1.1 will be the new freezing point. So if you want the answer in integers, then your answer will be one. Clear? Did everyone understand, brother? It's very easy. It's very straightforward. There is no hassle anywhere. Just apply the formula. Finish the work. Clear? Okay? The advantage of doing it in one stretch is that at least you get an idea of what this entire chapter is like. After that, you will find many such questions to practice. That is, in my opinion, you just practice the PDF that I will give you. You don't need to do anything else. Your chapter is ready. Okay? You don't need to do anything else. Yes, it is true that you should revise it theoretically once. Alright, sir. So, just as you have talked about freezing point depression, in the same way, its fourth colligative property emerges. And that is osmotic pressure. This is our last colligative property, which is known as osmotic pressure. Now, what is this? See, osmotic pressure is a later matter. First of all, osmosis should be understood. What is osmosis? So for osmosis, they say that if, for example, I have taken solvent on one side. For example, let this be my solvent on one side, and on the other side, I have taken this solution. So there is solvent on one side and solution on the other. So it has been observed that if you separate these two things with an artificial or any natural semipermeable membrane. What is special about a semipermeable membrane? Sir, this is the special thing that says that what does it say? It says that I will only allow solvent particles to pass through. That is, what is a semipermeable membrane doing? A semipermeable membrane is saying that it allows, allows only solvent to pass. It only allows solvent to pass. So if I separate solvent and solution with a semipermeable membrane. Now, if it is artificial, it is made of copper ferrocyanide. If it is natural, it is an animal bladder or anything. Do you understand? So any natural semipermeable membrane can be used. So, if this semipermeable membrane is separating solvent and solution, it has been observed that the flow of solvent, relatively, is seen from the high concentrated solvent side to the low concentrated solvent side. Or, in terms of concentrations, talking in terms of solution concentrations, it is seen from the low concentrated solution side to the high concentrated solution side. That is, there should be no confusion in this. I will not waste much time. I am writing directly. From where to where is the flow of solvent seen? The flow of solvent will be written like this. From high concentrated solvent to low concentrated solvent. To the low concentrated solvent. This is one way of saying it. Or from low concentrated solution to high concentrated solution. To the high concentrated solution. That is, both statements are the same. Because if the concentration of solvent is high, it means the concentration of the solution is low. If there is more solvent, there will be less solute. So it means it will be a low concentrated solution. So the flow of solvent is always from low concentration to high concentration in terms of solutions, and from high concentration to low concentration in terms of solvent. Both statements are correct. In the beginning, I used to get very confused. Some books say from low to high. Some say from high to low. What is correct? So actually, both low to high and high to low are correct. The only difference is. Low to high is in terms of solutions. High to low is in terms of solvent. Okay? So if this process is seen, then you will understand. This process is known as the process of osmosis. It is given the name of osmosis process. Clear? This process is called osmosis. Okay. Now comes the question of osmotic pressure. Sir, pressure is fine, sir. First of all, tell me why osmosis happened? Why is it happening that the solvent is running from here to there? It's very clear, sir. There is a very straightforward reason behind this. The vapor pressure of the solvent is P not, and the vapor pressure of the solution is PS. Remember? Which one is greater? So P not is greater. Sir, you have already told us that the vapor pressure of the solution is always less. That is, P not is greater than PS. And if P not is greater, then sir, it pushes, sir. It pushes more. Because of this, the relative flow of solvent from here to there is seen more. That is, what it means is, sir, okay, sir, whatever the reason, but one thing is clear, sir. The solvent will always run from a low concentrated solution to a high concentrated solution, or from a high concentrated solvent side to a low concentrated solvent side. We understand the reason. The value of P not is greater than PS. Because of this, the pressure of P not will be greater on this solvent side. Because of this, more solvent will go from here to there. Less will come from there to here. Is it clear? Okay, sir. Now you tell me, what is osmosis, I have understood that too. Why is osmosis happening? Okay, I have understood that too. Tell me more, what is osmotic pressure? So, if I want to define osmotic pressure, it is very simple for me. Okay, a good question has come to me. Look at this. This is a question asked in 2024. A very interesting question has been made. They are saying that if copper sulfate mixes with K2Cr2O7, then you will see green colored copper copper dichromate. You will see Cu2Cr2O7. If these two mix together, this will happen. Okay? So he said, okay. If I separate these two with a semipermeable membrane, then tell me, will the green color be seen on this side? Will the green color be seen on that side? Because by mixing these two, as in the equation, CuSO4 mixes with K2Cr2O7, you will get Cu2Cr2O7. Clear? So he said, when will this happen? So you tell me yourself. Sir, these two will never mix. Because they are solutes, sir. The flow will be of what, sir? The flow will only be of the solvent, sir. The solvent will move from right to left, from left to right, sir. CuSO4 and K2Cr7 will never mix. This means don't even talk about green color, sir. No green color will be formed. Green color is formed when these two solutes mix together. The semipermeable membrane will not allow them to mix, sir. Clear? Okay, sir. Okay, this is fine. There will be a flow of water. Sir, from where to where will the water go? Sir, the water will come from the low concentrated solution to the high concentrated solution. Sir, this is the high concentrated solution, and this is the low concentrated solution. This means, sir, if its concentration is low, then the solute, the solvent, will come out of here and enter into it. That is, water will start accumulating inside copper sulfate. And if water accumulates inside copper sulfate, then sir, the concentration of copper sulfate will decrease. That is, ultimately, sir, the molarity of copper sulfate is lowered. So the correct answer is D. What a beautiful question asked in 204. It was a very interesting question. Only a child who had the complete picture would be able to do this, that these two never mix. Why? Because they are solutes, and solutes can never mix. The semipermeable membrane will not allow this. One thing is finished. Second, sir, if the semipermeable membrane allows water, then will water go from right to left or come from left to right? So it is very clear. Water will go from left to right. Why? Why? Because the concentration of copper sulfate is high. The solvent always goes from a low concentrated solution to a high concentrated solution. So water will go towards copper sulfate, due to which the concentration of copper sulfate will decrease, meaning the molarity will lower. Clear? Understood? Anyway, let's talk about something else. Sir, now about the osmotic pressure you were talking about, let's talk about osmotic pressure too. Sir, since so much has been said, let's talk about osmotic pressure. Tell me, sir, where will which flow happen? Sir, this flow will happen. Which flow? This flow will happen, sir. Why this? Because from solvent to solute, water came out and came towards the solution. This is fine up to here, sir. What will happen from this? Here, understand very carefully. The water level will start rising here. This level will start increasing. Do you agree? This level will gradually start increasing. What will happen from this? Sir, when it comes this way, this level will rise. Now, when this level rises, this extra height of the solution will start exerting extra pressure. You know, extra height of water exerts extra pressure. It is hydrostatic pressure. Sir, this extra height of water will start exerting pressure this way. And when it starts exerting pressure this way, then this flow will start slowing down, and the flow from there to here will start increasing. A time will come, sir, when this height will reach this much. It will reach that point where the pressure from here to there and the pressure from there to here will become equal. That is, the flow from here to there that started increasing, and the flow of water from there to here that started decreasing, sir, will now become equal. Sir, you will see osmosis stopped. That is, very soon you will see that this extra height, this extra height will exert a pressure, which will be known as hg. This extra height itself is known as osmotic pressure. That is, when solvent comes out from the solvent side and enters the solution, then sir, the level of water on the solution side starts increasing. That increased height exerts an extra pressure, due to which osmosis starts stopping. And a time comes when that extra height exerts so much pressure that osmosis stops. The pressure of that height itself is known as osmotic pressure. This is one definition. What can be the second definition? The second definition is that if I do not let osmosis happen at all, that is, if I apply so much pressure on the high concentrated solution side beforehand that osmosis does not even start. Can that pressure also be called osmotic pressure? Both are definitions. You can do it as you wish. What is the first definition? Let osmosis happen. Osmosis is happening. The level on the solution side is continuously rising. A time will come when the level on the solution side will rise so much that now the flow of water from the right hand side to the left hand side and the flow of water from the left hand side to the right hand side will become equal. So you will not see osmosis happening. The pressure of that extra height, due to which osmosis is not seen happening. That extra hydrostatic pressure is known as osmotic pressure. First point is done. What is the second definition? If I do not let it reach this situation at all. If I say beforehand, for example, suppose the value of pi is coming as 1 atm, 1.2 atm. So what does that mean? It means that if I apply this much pressure here beforehand. If I apply 1.2 atm beforehand, then what will happen? Tell me. If I apply 1.4 atm beforehand, then osmosis will happen or not? Osmosis will not happen. Do you agree? Osmosis will not happen. But if I apply more than 1.4, then what will happen? Sir, up to 1.4, osmosis will not happen because both flows are equal. But if you apply more than 154, then sir, the flow of water from here to there will increase. Tell me, did everyone understand what I said? Sir, the flow of water from here will increase, sir. And when the flow of water from here increases, then sir, the opposite story will start, which should not have happened, sir. The flow should always have been from here to there if it happened on its own. Sir, due to your action, sir, the flow from solution to solvent has started. This process will be called reverse osmosis. Sir, this is reverse osmosis. Reverse osmosis. What is the definition? If I apply more pressure than osmotic pressure on the high concentrated solution side, then reverse osmosis starts. Sir, this is the phenomenon called reverse osmosis. Clear? Is everyone understanding? So if they ask us such a question, like the value of osmotic pressure is 1.4 atm. I applied more than 1.4 atm pressure on the side of the high concentrated solution. Tell me what will happen? Reverse osmosis. And if, for example, to fool us, they say that if the value of osmotic pressure is 1.4, and I applied more than 1.4 atm pressure on the side of the low concentrated solution, then also most children write reverse osmosis. Oh, then osmosis will become even faster. If you apply pressure on this side, it will run even faster. Do you understand what I am saying? So keep this in mind. On which side is pressure applied? Pressure is applied on the high concentrated solution side, then the matter of osmosis or reverse osmosis comes. If you apply pressure on the low concentrated solution side, then osmosis was already happening without doing anything. Applying pressure will only make it happen faster. Do you all understand what I am saying? So always keep this in mind that always on the high concentrated. I am repeating myself. I cannot write this because you have to do it yourself a little bit. So keep this in mind completely. This is the high concentrated solution side. The extra pressure on the high concentrated solution side that stops osmosis is called osmotic pressure. If more pressure than osmotic pressure is applied on the high concentrated solution side, then reverse osmosis starts. This is a unique phenomenon called reverse osmosis. Clear? If osmotic pressure is to be calculated, then osmotic pressure can be calculated from pi = CRT. Clear? Let's talk about something else. What are hyper, hypotonic, and isotonic solutions? This is very clear. Same osmotic pressure. Same osmotic pressure. Isotonic solution will be called isotonic solution. That is, what does it mean for isotonic? Pi1 = Pi2. If pi1 is equal to pi2, then this is osmotic pressure. Second, if the value of pi1 is greater than pi2, it means that the one whose value is greater is hypertonic. This is hyper, and the one whose value is less is hypotonic. That is, the solution whose osmotic pressure is less than a given solution is called hypotonic, and the other one will be known as hypertonic solution. Clear? Understood this? So this is very straightforward, sir. There is nothing new in this. Let's talk more. Any kind of other questions can be taken. For example, let's add one more thing to this. Sir, if we want to find the osmotic pressure of a solution containing two or more solutes, then remember the formula. If you know the moles of both solutes, then the total concentration due to both solutes will be N1 + N2CRT. That is,

N1 + N2 means the moles of the total solute will be taken as N1 + N2 or Na + NB. This means that the osmotic pressure that will be formed will be calculated from Na + NB RRT / V. That is, the new concentration, meaning, do you understand the point? That is, if there is more than one solute, what is the logic? The logic is that we will add the osmotic pressure formed due to both solutes. That is, the osmotic pressure of a solution having more than one solute is the sum of the partial osmotic pressures. That is, the osmotic pressure formed due to this one solute will be pi one. And how will the osmotic pressure formed due to one solute be calculated? The osmotic pressure due to one solute will be calculated. Concentration NA / V * RT. Do you understand concentration? Moles by volume. And what will be the partial osmotic pressure formed due to the other? It will be NB / V * RT. By adding these two, you can calculate the total osmotic pressure. That is Na + NB RT / V. So the total osmotic pressure is this. You will definitely remember this. If there is more than one solute, the total osmotic pressure will be calculated from Na + NBRT / V. What is the second method? What is the second question? The second question is, if two different solutions are mixed, how is the osmotic pressure calculated? So, when the osmotic pressures of two different solutions are mixed, the net osmotic pressure that comes out is calculated from π1v1 + π2v2 / v1 + v2. So, everyone will first keep in mind that if I need to find the concentrations of different solutions, and calculate the osmotic pressure from the mixing of different solutions, then you can do this work from π1 v1 + π2v2 / v1 + v2. Is it clear? Understood? So this was very simple. Meaning, do you understand? There is nothing very difficult here. It is a very straightforward story that is being told to you. Okay. Let's talk more. Now, as I have observed, these questions can be asked. For example, let's say this is the question. Now it is saying that although such questions have never been asked, still such questions can be asked. When it mixes solutions. So, here too, if I mix two solutions whose osmotic pressures are given. So, 1 liter of one person was taken. 3 liters of the other person were taken. So, this means if I want to find pi net, what will it be equal to? π1v1 + π2v2 / v1 + v2. So, what is the value of π1 given? 1.5. What volume was taken? 1 liter. What is the value of π2? 2.5. And what volume was taken? 3 liters. Divided by v1 + v2. What is v1 + v2? 1 + 3. So, if you solve this, it is 1.5 + 7.5 = 9/4, which is 2.25. That is, the osmotic pressure will come out to be 2.25 atm. This is happening because you have remembered this equation. So, you also keep this in mind. This question can be asked in the JEE paper that if two different or two or more solutions are mixed, then the osmotic pressure is always calculated from π1v1 + π2v2 + π3v3 / v1 + v2. Is it clear? Okay, now let's come to the next point. The next point is very interesting. If I analyze all these colligative properties that you have studied, then many of my answers are coming out wrong. I said, meaning, what are you saying, sir? If you want to find the boiling point elevation, what formula will you use? I said, what formula will I use, sir? Delta TB = KB * molality. So, when you calculate delta TB from it, that answer will be different from the observed answer. So, we said, how can this be, sir? If the formula is correct, then our answer and your answer should be the same. There is a reason for this, and it is very interesting. Everyone listen carefully once. Many solutes, after going into the solvent, either dissociate or start associating. We said, meaning, what are you saying? You took one mole of salt. You put it in 1 kg of water. So, you will take molality as one. Moles upon weight of solvent is one. 1 / 1. That is, you thought there is one mole of salt. 1 kg of water. So, you took molality as one and calculated the answer from one. But you did not think that when that salt went into water, it broke down into Na+ and Cl- and converted into two moles. One Na+ was formed and another Cl- was formed. That is, one mole converted into two moles. So, the observation of the answer will be due to two. Your answer is due to one. So, there will be a difference between our answer and yours. Do you understand what I am saying? That is, what I want to say is that I had not taken these things into account until now. Now I will solve all my questions by taking all these things into account. That is, due to association or dissociation of some solute particles in the solvent, the observed colligative property is different from the theoretical colligative property. And the ratio of this observed and theoretical colligative property is known as the van't Hoff factor. That is, if the observed colligative property is divided by the theoretical colligative property, then the van't Hoff factor is seen. Sir, this theoretical colligative property is the same, isn't it, sir? The one you were calculating until now. KBM, KFM, CRT. Yes, this is the same property. So, if I multiply by i, will I get the actual answer? Yes. This means, sir, the important thing that is understood is that the observed colligative property, the observed colligative property, which I need, which is the reality, observed colligative property is equal to van't Hoff factor * theoretical colligative property. Understand the point. That is, all the colligative properties you calculated were theoretical. The reality is of observation. How to get the observation? So, multiply all the colligative properties you have learned to calculate by i. Understand. That is, what do I mean? Sir, what I mean is that if you ever need to find delta T B of any solution, then you do i * KB * M. We said, what is I? He said, I is my van't Hoff factor. I said, how is this calculated? We will learn that soon. Is it clear? Sir, this pi app is having a different kind of chat. Go to sleep, sir, go to sleep. Where are you putting your mind? Go to sleep, go to sleep. That's enough. You can't study that much. That's enough, sir. Go to sleep. Don't get into trouble. All this happens. Do you understand? Leave it. Anyway, so delta T B is equal to I * KBM. Okay? Similarly, delta TF. Sir, for delta TF, it is I * KFM. Understand my point. Normally, the answer is KB * M. The formula is KB * M. But in that molality, moles of solute come, and after going into water or solvent, those moles of solute either increase or decrease. That van't Hoff factor part comes for those moles of solute. So, I have taken it out. That I KBM is the molality delta TV. i KFM is the delta TF. Pi = ICRT. Relative lowering of vapor pressure is moles of solute * I. Moles of solute. This I is with what? With moles of solute. If moles of solute are increasing, then the value of I is more. If moles of solute are decreasing, then the value of I is less. That is, this I is taken for moles of solute. So, relative lowering of vapor pressure is always equal to this. And if it is a dilute solution, then it will be neglected with respect to the solvent. So, what will your expression become? i times solute by solvent. Okay? And the most important thing, which children always get wrong, is this fifth one. I will not explain much, but still, I will say that the value of I is calculated from calculated molar mass upon observed molar mass. Sir, what value of I did you just say? Sir, you said I is observed colligative property upon theoretical colligative property. Okay? Tell me, molality comes in colligative property. Moles of solute come in molality. Molar mass comes at the bottom of moles of solute. To find moles, we divide by molar mass, right? That is, the ratio of observed colligative property and theoretical colligative property is actually the ratio of theoretical molar mass and observed molar mass. That is, while writing the expression for I, another formula must be remembered: if the calculated molecular weight is divided by the observed molecular weight of the solute, then the van't Hoff factor can also be calculated. This is very important. That is, you calculate I from observed colligative property upon theoretical colligative property. Along with that, there is another way to find I: calculated molar mass upon observed molar mass. This is just the opposite. Observed colligative upon theoretical colligative property. That is I. And calculated molecular weight upon observed molecular weight of solute is I. I will explain this now. Is it clear? Do you understand this point? Okay? So, this means, sir, if I know the value of I, then all the work I have done so far will give me the answers. Now I have no problem. And I will teach you how to find the value of I directly. I will not get stuck in calculations at all. If any solute is dissociating inside the solvent, then the value of I is calculated from 1 + N - 1 * alpha. Where alpha is the degree of dissociation and n is, in my own language, the number of parts it breaks into. That solute breaks into how many parts, that is n. Its degree of dissociation is alpha. Using these two, you can find its i. And after getting i, you can calculate the observed values, which are the real values. This is the case of dissociation. And I think everyone will agree. Sir, the value of i will always be greater than one, sir. In case of dissociation, i will always be greater than one. Why? Because, sir, the number of parts it breaks into, that is, it is confirmed, sir, if something breaks, it will break into more than one part. Do you understand what I am saying? So, the value of n will be greater than one. If the value of n is greater than one, then this term will always be positive, sir. That i is always greater than one. Okay? Secondly, it is also possible that, sir, our solutes are dissociating after going into water or solution. Sorry, they are associating. If the solute is put into the solvent and they start joining together. Two people start joining. Three people start joining. Dimers start forming, trimers start forming. This is possible. This is also possible. So, in such cases, the way to find the value of i is 1 - (1 - 1 / n) * beta. Here, what is beta? Beta is the degree of association. Degree of association. Whatever is its degree of association. And what is n? The number of people joining. The number of people joining. Meaning what? If a dimer is forming. Tell me quickly. If a dimer is forming, what will be the value of n? How many people join in a dimer? Two. So, the value of n is two. If a trimer is forming, then the value of n is three. Is it clear? So, the number of people joining together is n. Beta is the degree of association. If you put the value directly, then it is also clear, sir, at this time, i will always be less than one, sir. This time, the value of i will be less than one. Because you can see that the people who join, the value of n, will be greater than one. Two people will join, three people will join. So, this value will always be positive. And if this is positive, then subtracting from one will always be less than one, sir. This means, sir, it is confirmed that the value of i will be less than one in the case of association. The value of i will be greater than one in the case of dissociation. And I tell you, don't think at all. These two formulas that are placed in front of you, remember them with your eyes closed. Whatever question comes, everything will be solved quickly. Here, sir. Let's talk about questions asked in JEE. Here, sir. To say, when these questions were asked, people must have struggled. A beautiful question from 2025 is visible again. Sir, what are you trying to say? Sir, what I am trying to say is that the percentage dissociation of salt at a given temperature is, meaning, what do I need to find? I need to find the degree of dissociation. We will convert this into percentage. Do you understand? Degree of dissociation is needed. Alpha. Okay? Okay. What is given, sir? The value of i is given as two. According to me, when dissociation happens, the value of i is 1 + n - 1 * alpha. The formula is remembered. Okay? The value of i is given as two. = 1 + Into how many parts are you breaking? That is n in dissociation. Sir, how many parts will mx3 break into? Please tell me. Sir, mx3 will form one m and three x. Into how many parts did it break? Sir, four parts, 3x and one m. That is, into how many parts is it breaking? n = 4. So, this means 4 - 1 * alpha. Sir, let's calculate alpha from here. It will be 1/3, which is 0.33. So, if you want the percentage dissociation, then percentage dissociation is 33%. Is it clear? Understood? And let's see more. And there are plenty of them, sir. This is not just one, sir. Look, they lined them up. 2025. Look at this. What do you want to know, sir? A to B is 30% ionized, meaning alpha = 0.3. What does it mean? The value of van't Hoff factor, show us how to calculate it. Okay, sir. Value of i. What is n, sir? How many parts will A to B break into, sir? Two A's will form. One B will form. That is, what is the value of n, sir? The value of n is three. n = 3. This means, sir, let's put the value here. So, n = 3. So, i = 1 + n - 1 * alpha. Sir, this is your i. I think it is 1.6. This is 1.6. The question is finished. Questions are asked. I am not doing it on my own. It is asking those questions. It is the same story every time, sir. And let me show you more. Very beautiful, sir. 2024. I find this to be the best question. A very beautiful question. What needs to be done? Let's see. It is a very theoretical question. The solution from the following with the highest depression in freezing point. Highest depression in freezing point. Meaning, delta, meaning delta TB, sorry, delta TF = I * KF * M. This is it, I KFM. Okay? Delta TF. So, the highest delta TF will be decided by whom? Sir, it will be decided by I, whose value is the largest. Okay, sir. Sir, where will you see the largest I? So, 180 grams of glucose, acetic acid dissolved in water. When acetic acid is dissolved in water, it dissociates. It starts dissociating. Meaning, if you look at acetic acid carefully, in a way, how many moles of acetic acid were taken? Three moles. Three moles of this. The molar mass of acetic acid is 60. So, three moles of this were taken. Sir, when you put it in water, it will dissociate. We are being asked that the solution from the following with the highest depression in freezing point, meaning the depression in freezing point should be the highest. That is, the value of depression in freezing point should be seen as the highest. Try to think for a moment. When will the highest depression in freezing point be seen? Sir, the depression in freezing point will be highest when the freezing point is minimum. That is, your answer will be decided by the value of I. So, delta TF, the depression in freezing point, you need to see that as the highest. I will give you just one hint. If you put acetic acid in water, it dissociates. When acetic acid is taken in a non-polar solvent, it associates. You must have read in inorganic chemistry that acetic acid can also exist in the form of a dimer. If it is taken in a non-polar solvent. Meaning, if you take acetic acid in a non-polar solvent. It will become like this, COH. This is acetic acid. So, sir, it forms a dimer, sir, due to hydrogen bonding, sir. That is, if it is a non-polar solvent, then acetic acid, benzoic acid. Sir, they form dimers. Just like this benzoic acid, they join together, sir. They start forming dimers. Similarly, acetic acid also starts forming dimers. Do you understand? But if I am told that sir, the most and even in dimer, what is it, sir? Even in dimer, it is said. And like this glucose, sir. Glucose, sir, neither joins nor breaks. Glucose is C6 H12 O6. Sir, this is glucose. Glucose is C6H12 O6, whose van't Hoff factor is equal to one. Whose van't Hoff factor is equal to one. Meaning, one thing is understood, that our acetic acid will start associating. The van't Hoff factor will decrease. Benzoic acid will also start associating. The van't Hoff factor will decrease. The van't Hoff factor of glucose will remain the same. And we will have to estimate a little according to our understanding. So, a little bit, if you try to understand it yourself. Meaning, questions can also be asked from us regarding the van't Hoff factor. So, this is very important. Try to do this once. And let's do more questions. And let's do more in this, like van't Hoff factor questions. Like, for example, this one. Here it is visible that the highest van't Hoff factor is visible in A because it is acetic acid, it has three moles, and when it dissolves in water, it will further dissociate. That is, CH3COOH will further dissociate into CH3COO- + H+. That is, in a polar solvent, acetic acid dissociates, and in a non-polar solvent, acetic acid associates. Meaning, here the value of I will be less than one, and here the value of I will be greater than one. So, one thing is clear. If you add three moles, then more than three will be formed because it is breaking. So, this means that the highest van't Hoff factor will be obtained here. Due to the increase in van't Hoff factor, you will see the highest depression in freezing point in A. Is it clear? Understood? Absolutely easy. Meaning, there is nothing in this. You can create many more such cases. So, there are many questions related to this.

can be done. So many questions can be asked. For example, look at this. And look at this. One mole aqueous solution of an electrolyte A2B3 is 60% ionized. Okay. This means one thing is clear. The value of alpha, 60%, means 0.6. The value of alpha is 0.6. Okay. And looking at A2B3, it seems n is 5. Do you agree? 2A + 3B, meaning the value of n is 5. So, first of all, let's calculate the van't Hoff factor. i = 1 + n - 1 * alpha. 1 + n is 5 - 1 * 0.6. What will this be, brother? This will be 1 + 4 * 0.6 = 1 + 2.4 = 3.4. So the value of I is 3.4. Now tell me, what do we need to find? The boiling point. Wow, wow, wow, sir. Delta TB = I KBM. Do you remember, sir? Delta TB will be equal to I KBM. The value of Delta TB will be equal to I * KB * M. So, this means, sir, if the value of I is 3.4, KB is given in the question as 52, and you have taken a 1 molal solution, then Delta TB can be calculated from this. Tell me quickly, how much will it be? 3.4. To multiply this, 3.4 * 52. Sir, this is 176.8. 176.8. Is this done, sir? This is Delta TB. What do we need to find? We need the boiling point. Okay. So, sir, if you need the boiling point and this is your Delta TB, it means the boiling point is 373. So, the new boiling point that will come, meaning the value of Delta TB is 1.768, right? So, the boiling point of the solution will be the boiling point of the pure solvent, water, which is 373, plus the elevation, which is Delta TB, that is 1.768. So, by adding these two, you will get the new boiling point. Are we doing this correctly? Yes, sir. You have calculated Delta TB. Using Delta TB, you will get the new boiling point. Is it clear? No, we don't need the elevation of the boiling point. This Delta TB is the elevation. We need the new boiling point. So, since the solvent is water, the boiling point of water is 373, and it will elevate by this much. So, this will be added to 373. Do you understand? So, 373 + 1.768 is approximately 375. The answer will be 375. When added, this is 374.768. Rounding off, the answer will be 375. Clear? Understood? So, using this 'i' factor, you can create different cases. Whatever questions you need to do, you can create questions using this 'i'. So, there are many questions that will be given to you to solve. You will try to solve them. They are very interesting, very easy, and very enjoyable questions. For example, here, what are they trying to say, sir? Here they are saying that brother, where will our 'i' factor be the highest? What is 'i', sir? 'i' is dissociation. The more the dissociation, the greater the van't Hoff factor will be. This means if a solute is dissociating, the greater its degree of dissociation, the greater its 'i' factor will be. Understand, 'i' was equal to what? i = 1 + n - 1 * alpha. Okay? So, if you are saying that my degree of dissociation... See, 'n' is common because the solute is fixed. Its 'n' value is 2. NaCl means one Na and one Cl, meaning it will break into how many? Two. Okay. Now, if the value of n is 2. Increasing alpha will increase 'i'. This means, okay? This means if alpha is greater, then 'i' is greater. Okay? And alpha is greater when dilution is greater. This is Ostwald's dilution law. The more you dilute the solution, the greater its degree of dissociation will become. So, our most diluted solution is the third one, meaning the C solution. So, IC will be the largest. IC will be the largest. Then IB will be there, and after that, IA will be there. Clear? Understood? Absolutely easy. So, in this way, you can do many questions. Now, I will talk a little further on this. I will give some questions to solve. You will try to solve them. Now I will move a little further on this. This will be my last section, which is related to Henry's Law. So, let's quickly discuss Henry's Law. This is the last section we need to discuss. What does Henry's Law say? Henry's Law actually talks about the solubility of gases, about how the solubility of gases will be more or less in a solvent or water, and it talks about some related things. And the law is very clear. The law states that when you place a gas above any solvent, the gas dissolves in the solvent to the extent it needs to dissolve. And after some time, an equilibrium is established between the undissolved gas and the dissolved gas. The amount of gas that dissolves is called the solubility of that gas. This means the meaning is very simple: the definition is that the maximum amount of gas dissolved in a solvent per liter at a particular temperature is known as solubility. This means the amount of gas that dissolves in 1 liter of solvent at a particular temperature is given the name solubility. So, I said this is very easy, sir. Whatever dissolves is solubility. So, if you bring 1 liter of water, whatever gas dissolves in it is solubility. Henry's Law is not involved here anywhere. It is just talking about solubility. Okay? So, sir, in this solubility, if I ask you, can you tell me on which factors this solubility will depend? So, the logic is that temperature must be a very big factor. And there is no doubt that increasing the temperature will decrease your solubility. Sir, if I talk about gas. This means if you talk about a gaseous system, if you talk about dissolving gas, then increasing the temperature will cause the gas to bubble out of the solvent. Its solubility will decrease. But if we talk about the dissolution of a solid, then it dissolves more when heated. You know, like when you are making sugar syrup, dissolving sugar, the more you heat it, the more sugar dissolves. This means in the case of solids, the situation is different. For solids, temperature increase leads to solubility increase. But for gases, increasing temperature decreases solubility. Without much thinking, let's learn this first. Clear? This means the solubility of gases should decrease with an increase in temperature. Okay? Understood? Alright, sir. Second, sir, the second factor. The second factor is this, sir. Look, try to understand. This is cold water. This is hot water. A fish is smiling in cold water and crying in hot water. Why? Because the dissolution of O2 in cold water is higher. If you heat the water, O2 will come out because solubility decreases. So, this poor thing starts crying because oxygen is gone. So, aquatic life is happy in cold water, and aquatic life is a bit troubled in hot water. Okay? Well, the second factor is pressure. What is the relation of pressure with solubility? This is Henry's Law. The talk about pressure you are doing here, from here, the talk related to Henry's Law starts. Henry's saying is that if you increase the pressure above a gas, that gas will dissolve more in the solvent. We said, what chemistry is there in this? This is very straightforward. If you try to press the gas by placing a stone, it will dissolve less. If you increase the stone above this gas, the pressure of the gas will increase. With increased pressure, its dissolution will also increase. So, Henry's Law states that the solubility of a gas depends on the pressure of the gas. The higher the partial pressure of the gas, the greater its solubility in the solvent. Understood? This means solubility of a gas in a particular solvent is directly proportional to the partial pressure of the gas above the liquid surface. This means the higher the partial pressure of the gas above the liquid, the more the gas will enter. And you know the very simple logic for this. CO2 is filled in cold drinks at very high pressure. As soon as the cap is opened, the external pressure decreases. So, CO2 feels that the pressure has decreased, so its solubility also decreases, and that CO2 starts coming out with bubbles. Have you seen it? This means Henry's Law states that the solubility of any gas, meaning if we want to write Henry's Law properly, how will we write it? Henry's Law states that the solubility of a gas is directly linked with the pressure of the gas. If you want to put an equality sign, then P gas is equal to some constant KH * mole fraction of gas, and this KH is known as Henry's constant. Sir, this is Henry's constant. KH is Henry's constant. So, you will give it the name of Henry's constant. Clear? Okay. Alright, sir. Let's talk about the next thing within this. Does nature also... Will we come back to Henry's Law again? Does nature also affect the solubility of a gas? What is nature? Sir, absolutely, sir. Like dissolves like, sir. A very big rule of chemistry, sir. What is like dissolves like? Sir, a person of one type dissolves a person of their own type. If a gas is polar, it dissolves more in a polar solvent. If it is non-polar, it dissolves more in a non-polar solvent. This means polar gases dissolve more in polar solvents. This means the dissolution of gases or their solubility is also affected by the nature of the gas and the solvent in which the gas is being introduced. Clear about this? This means, overall, if we look, the solubility of a gas is mainly dependent on three factors. The first factor that emerges is temperature. The second factor is pressure, where Henry's Law will come. And the third factor is the nature of the gas. So, what does the nature of the gas say? Polar gases dissolve more in polar solvents. Now, if I talk about the applications of Henry's Law, there are three major applications. When you go to high altitudes, you have difficulty breathing. The reason is? As you go up, the pressure decreases. When the pressure decreases, the oxygen dissolved in our blood starts dissolving less. Brother, if you increase pressure, dissolution increases. You just studied Henry's Law. So, if the pressure decreases above, the gas starts coming out of the blood. O2 starts decreasing from the blood. Due to this, there is difficulty in breathing. Okay? Second, scuba divers. These scuba divers go inside the water, and they go at their own pace. Right? So, when they go inside, the pressure gradually increases. When the pressure increases, whatever gas they are inhaling starts dissolving more in the blood. This means O2 and nitrogen start dissolving more in the blood. Because the pressure is increasing from above, as they are going down. So, due to the pressure of the water, the dissolution of nitrogen and oxygen in the blood increases. But when they start coming up after their fun and games, what happens? Sir, the pressure starts decreasing again. Now, when the pressure starts decreasing, the same O2 and N2 that dissolved more in the blood now start coming out. So, if they come out quickly, the gas comes out very rapidly, causing a lot of pain in our veins when that gas comes out. This is called the bends. This is called the bends. So, scuba divers are told, "Look, it's like this. Come up slowly." When you come up slowly, the gas will be released very slowly from your veins, from your blood vessels, it will come out slowly, so you won't have trouble. If you come out quickly, nitrogen will come out very rapidly, which will cause you trouble. Okay? And the last one is that if you talk about applications, it is difficult to survive in hot water. Absolutely correct, sir. It is difficult for aquatic life to survive in hot water because in hot water, due to higher temperature, the dissolution of oxygen decreases. Solubility decreases. Therefore, it is considered easier for fish to survive in cold water and difficult to survive in hot water. Alright, very good, sir. Now, let's get to the important part, sir. What is the important part? Listen very carefully, brother. The important part is that you just said there is a Henry's constant, KH. Okay. Let's tell you a hidden fact about this Henry's constant. Henry's constant mainly depends on whether the solubility of the gas is high or low. Try to understand my point. We said, meaning, if Henry's constant is low, it means the solubility of the gas is high. It is visible from here, right? Brother, KH and mole fraction are inversely proportional. If KH increases, mole fraction decreases. If KH decreases, mole fraction increases. If the pressure of the gases is kept the same. This means if different gases are taken, and the pressure is the same, then KH and mole fraction have an inverse relationship. So, the gas with a higher KH means its solubility is lower. The one with a lower KH means its solubility is higher. Okay up to here. So, this means if we can find out which gas is more soluble, then we will also know whose KH is lower and whose KH is higher, because the more soluble gas has a lower KH, and the less soluble gas has a higher KH. Okay up to here. This means it is clearly written here: Gases having more force of attraction. Now, sir, which gases are more soluble? Gases in which the force of attraction is greater are more soluble. And if they are more soluble, then their KH is less. And which gases have greater force of attraction? Polar gases, sir. Polar gases, sir, dissolve more in water. Because they can interact with water, as they are polar and water is also polar. Now, if they dissolve more, their KH will be less, sir. This means polar gases have lower KH, and non-polar gases have higher KH. First point. Second point. Sir, second point is, if we compare KH among non-polar gases, then in non-polar gases, the gas whose size or molecular weight, the molecular weight of which gas is higher, its dissolution is higher. If its dissolution is higher, then its KH will be less. This means in non-polar gases, increasing molecular weight increases solubility and decreases the KH value. This means two cases are formed. KH of polar and KH of non-polar. KH of polar is less because their solubility is higher in water. KH of non-polar is higher. Clear? If I have to compare among non-polar gases, then the gas with higher molecular weight has lower KH because its solubility is higher. This means ultimately, I have to remember both things. For non-polar gases, the gases having more molecular weight will have less KH because more molecular weight means more dissolution in the solvent. These two points are important. Okay? This means two points are covered. If we are ever asked to compare, brother, whether the KH value of SO2 is higher or H2 is higher? Then, from what I know from inorganic chemistry, SO2 is a polar molecule, and H2 is just H2. And if it is polar, then there is no doubt. Its solubility will be higher than this. And if the solubility of SO2 is higher, then its Henry's constant will definitely be seen to be lower. This means the Henry's constant of SO2 is less than the Henry's constant of H2. So, if I have to find the answer, it is clearly visible that KH of SO2 will be less than H2. If it were a question of solubility, then sir, the one with lower KH has higher solubility. Do you understand my point? So, its solubility will be higher. Alright, sir. Let's draw a graph. Let's draw a graph between P gas and mole fraction of gas. It's a very easy graph, sir. You just told me that P gas is equal to KH * mole fraction of gas. This is Henry's Law. So, if I want to draw a graph of P gas and mole fraction of gas, it is very clear. Sir, this graph can be drawn like this. And if I want to draw it for different gases, I can definitely draw it. It is very clear to me that if I draw this curve for different gases. So, this is gas A. Huh? This is gas A. This is gas B. This is gas C. This is gas D. So, it is very clear that the slope of this curve of P gas and mole fraction of gas will be KH. This is y = mx. See, this is the y-axis, this is m, and this is x. So, in y = mx, the slope, my slope, is KH. So, it is very clear that the higher the slope, the higher its KH. This means KH of D > KH of C > KH of B > KH of A. And if we know the ratio or relation of solubility and Henry's constant, then we will also know the relation of solubility. Solubility of D is less than solubility of C is less than solubility of B is less than solubility of A. Why? Because with higher KH, solubility decreases, and with lower KH, solubility increases. So, this is for P gas and mole fraction of gas. If I draw a graph of P gas and solvent. Look, sir, this is also very beautiful, sir. This is a question itself, sir. Look, this is very easy. Tell me quickly, what relation will come? What, what, which answer is correct, sir? KH of B is higher. If KH of B is higher, then its solubility is lower. So, KH of B is higher. This answer is correct. And solubility is lower. This is the answer. B and C. Clear? Can everyone do it? It's absolutely straightforward. Alright, sir. Now, if we draw a graph of P gas and mole fraction of solvent. You just told me that P gas is equal to KH * mole fraction of gas. Very good, sir. Okay, sir. This means P gas = KH * mole fraction of gas. So, we can do one more thing, sir. If I write 1 - mole fraction of solvent instead of mole fraction of gas. Okay, sir. We put the gas into the solvent, right? So, you can write the mole fraction of the solvent instead of the mole fraction of the gas. So, this curve, sir, let's write it properly, sir. This is P gas = - of KH * mole fraction of solvent. KH * mole fraction of solvent + KH. Sir, if I look at this carefully, this is the y-axis, this is x, this is m, which is negative, and this is c. So, this is y = mx + c. This means one thing is clear, sir. This is a person with a negative slope, sir. And this person with a negative slope.

It has an intercept equal to KH, sir. That is, this is confirmed, sir. This graph that is going to be formed, sir, is going to be a line drawn something like this. Are you understanding what I'm saying? In which one thing is clear, that if you talk about the slope, the slope will be equal to -KH, and the intercept, sir, will be equal to KH. Is it clear? Understood? That is, if I make a graph of P gas and mole fraction of solvent, then a tremendous graph can be made. And what is the interesting thing? That JEE has asked me a question on this graph once. So if I talk about a question on this graph, this. Can you quickly tell me the answer? Whose graph is it, sir? Partial pressure and mole fraction of solvent. What kind of graph will it be, sir? It will be of negative slope, sir. If it will be of negative slope, then go to hell. Go to hell. Now, who is left, sir? These two are left. If you look closely at these two, the one with the largest intercept will be the one whose KH is the largest. And the smallest intercept will be of the one whose KH is the smallest. So, sir, the smallest KH appears to be of the first person. And who is the first person? Sir, the first one is W. This means, sir, the smallest KH is of W, sir. See this, W, sir. The answer is correct. Go to hell. After W will come X, sir. Who is X, sir? X is our second person. The second person has this less. Absolutely correct. Then will come the third, then will come the fourth. Absolutely correct, sir. W, X, Y, Z. The answer will be A. Clear? Clear. Understood? Everyone understood? No. Look at these. There's a difference in slope too, isn't there, man? There's a difference in slope too, isn't there? That also has to be seen, hasn't it? So ultimately, the correct answer should be A. Is it clear? Let's talk more, sir. Now, sir, let's try one or two similar questions. Sir, these are very straightforward questions. O2 gas is bubbled through water at 33 Kelvin. The number of millimoles of O2 gas that dissolve in 1 liter of water is. Let's go, sir. So this means that the pressure of the gas is 92. That is, P gas = 0.92 bar, and the KH given for the gas is 46.82 * 10 raised to the power 3 bar. It's given in kilo bar, right? It's given. Okay, sir. So I think according to the formula, P bar, sorry, P gas equals KH. What is KH? KH, that is 46.82 * 10 to the power 3 * mole fraction of mole fraction of O2. Let's put the values. The value of mole fraction of O2 will be 0.92 / 46.82 * 10 to the power -3. Sir, this is mole fraction. How is mole fraction written? Moles of O2. We need to find this, right? If O2 is this much, if how much to find? The number of millimoles. So the moles of O2 will be divided by moles of O2 plus moles of water. And water is 1 liter. So 1 liter means 1 kilogram. The mole of 1 kilogram is 55.55. Clear? Now, he said to assume the solubility of O2 in water is very small. So this means that the moles of O2 can be neglected. You can neglect the moles of O2 with respect to water. So, the moles of O2 will come from here. So the moles of O2 that you need to find, you will calculate them. And remember, we need the number of millimoles. So, multiply the moles obtained by 10 to the power 3 to get millimoles. So from here you can calculate. That is, only one formula is to be applied. Apply that formula repeatedly. It's over. There's nothing to do in it. Let's see more and more. Same, same, same questions, same formula ones, all together. Look here, the oxygen dissolved in water exerts a partial pressure of 20. That is, the partial pressure is 20 kilopascals. This is equal to KH. What is it? 8 * 10 raised to the power 4 * 10 raised to the power 3. No, one second. That is also in kilopascals, so let's keep this in kilopascals too. So this is 10 raised to the power 4 * mole fraction of gas. It's the same question, sir, again. Calculate the mole fraction of gas. Everything is given the same. So, if it comes to mole fraction and moles, mole fraction of gas means moles of gas upon moles of water. And if we are talking about molar solubility, what does molar solubility mean? How many moles dissolve in 1 liter? You need to find it per liter, right? Look here. So this means the weight of water is 1 liter. So you can do it exactly the same way. The value of x gas will be 20 * 10 raised to the power 3 / 8 * 10 raised to the power 4. This is our x gas. Whose value should be? Moles of gas, which one is ours? O2. Moles of O2 / Moles of water. So, calculate the moles of O2 from here. It's the same question. There's nothing new in it. And the weight of water, the moles of water are 55.5. Why? Because, sir, when molar solubility is talked about, 1 liter of water is taken. And these will be the moles of 1 liter of water. In many books, I have seen that the answer is not 1389. They give some other answer. They actually just calculate the moles of gas. Whereas, it means they just calculate the mole fraction. They call this the answer. Whereas it is not so. This is not the answer. Understand the point. The answer that will come out will be in terms of moles. Not in terms of mole fraction. Solubility means how many moles dissolve in 1 liter. So the answer will be calculated from moles only. We will have to calculate that. Clear? Understood? So there are many such questions that are calculation-based, which can be given. Look, this is also a very good question. In this, they are saying that if I give you the Henry's constant, what can you refer to from this table? This is very important. What does this table tell? So, first of all, is this statement correct? Tell me. Solubility of gamma at 300 Kelvin is less than 298. Sir, this is correct, sir. Solubility decreases with increasing temperature. This is absolutely correct. But sir, this is not given from this graph. It is not implied from this data. Therefore, I will not consider it the correct option. The statement is correct, but this table implies that. Absolutely not, sir. There is nothing in the table that indicates that the solubility of the gas at 308 Kelvin decreases as compared to 298. This is what happens. Solubility decreases with increasing temperature. But it has nothing to do with the table, sir. Are you understanding? So most children get confused that sir, this option is also correct. What is wrong with it? The mistake is that it has nothing to do with this table. What has to do with this table, if you look closely, is this option C. Let's try this option C once. The pressure of a 55.5 molar solution of delta is 250 bar. Sir, let's check. Sir, the pressure is KH * mole fraction of gas. Okay, sir. Let's put the values. What is the value of KH? You are talking about delta. Delta's KH is 5. And sir, what will be the mole fraction, sir? Molality is 55.5. Then how will the mole fraction be calculated? Molality means moles upon what? Weight of solvent. So if molality is 55.5, then that means 55.5 grams in 1 gram of solvent. This is what it means. So if I calculate the mole fraction, then moles, which is 55.5, how will we write it, man? Today we learned an English line. 55.5 will be written as moles. 55.5 moles in 1000 grams of water. This is what it means. So, sir, if I need the mole fraction of the gas, then how many moles of gas are there? 55.5 moles of gas are 55.5 / moles of water. What are the moles of water? For mole fraction, 55.5 plus moles of water. 55.50 grams means how many moles? 1000 / 18 = 55.5. So this is also 55.5, this is also 55.5. So this 5, in what unit is it? It is in kilobar. So this means if I multiply by 10 to the power 3, the answer will be in bar. So this will be 1/2. 500 / how much? 500 / 2 = 250 bar. Clear? That is, this option is correct, sir. Option C is correct. Most children think that sir, option B is also correct. The rest are fine anyway. Sir, option B is correct. Option B is not correct. A is completely wrong anyway. Alpha has the highest solubility. Alpha's K is the largest. So its solubility should be the least. It cannot be the highest. So A is completely wrong. Children only have doubt in B, that B is also correct. Yes, B is correct, but it has nothing to do with this table. Therefore, the correct answer should be C. Clear? Everyone understood? So, brother, we will do this much for today. We have also completed Henry's Law. We have discussed everything in great detail. So, in my opinion, everything is done. Obviously, some questions will be given for you to do. You can see this PDF on the app and prepare from here. In my opinion, we have discussed everything in great detail. If we just practice a little, this chapter will be completely ready. So I don't think there is anything else to study. All the questions are given. Practice the excellent questions. It's over. Nothing to do. Okay? So, those children who were connected from beginning to end would have got an idea that there is nothing very new in this chapter. We need to find Delta TB, its formula is there. If we put I, it will become a new formula. Similarly, sir, there are some cases of vapor pressures and some cases of concentrations. So there is a very limited source on which questions are formed. So if I just brush them up a little, prepare them, my work will be done. Provided that NTA is not doing anything very new. Which seems to be the case, although looking at the questions of 2025, it seems that thinking has improved a bit. But still, you see that everything is the same as what you were taught. Okay? So, let's do this much. We will meet in the next class. Keep at it, try, work hard because the more you work hard, the more you will get the fruit because there is very little time left now. So, those children whose exams have one month left, 40 days left, they should try to gather everything very wisely at this time. It is not necessary that you get 100 out of 100 marks. But at least after giving the paper, you should feel that okay. I prepared this much. I got decent marks. This is my purpose. Okay? So, let's do this much for today. We will meet again. We will meet you in the next series of destinations. Thank you. Thank you so much.