CLASS-01 | SOLUTIONS | TG PCB | ASSISTANT SCIENTIST(ANALYST GRADE-II) | BIOGENESIS -9963697976

Added: 2026-05-24

[00:00:00]Right.

[00:00:03]Hello dear students.

[00:00:06]Right. So previously we completed gaseous state. So the various uh concepts of gaseous state have been discussed. Right. Uh molecular velocities like RMS velocity. Then uh most of probable velocity, average velocity, then kinetic molecular theory of gases. Right? then uh viral theorem and reduced equation of state collision frequency and all those things we have covered in the previous class. So somewhere we can utilize those equations also. Right? Now coming to the part of solutions right. So new chapter solutions.

[00:00:45]What is meant by solution? Right. So whether that may be applicable to physical state various physical states are there, solids are there, liquids are there and gases are there. With the help of that how many kind of solutions we may prepare and what was the syllabus mentioned in our examination. So before that we will go through the detailed classification of solutions all those things right. So what is meant by solution? Solution is a homogeneous mixture. It is a homogeneous mixture of two liquids.

[00:01:27]Homogeneous mixture of two liquids.

[00:01:30]Right?

[00:01:32]So or two or more than two liquids also will be possible. So generally for homogeneous mixture of two liquids means such solution we may call as binary solution.

[00:01:43]This is applicable for binary solution because only two liquids are mentioned.

[00:01:49]If many number of liquids will be there so that is called the corresponding solutions like three will be there tenary four will be there quartinary like that. Right? So the complete homogeneous mixture of two liquids that becomes forms a binary solution. A binary solution right. So means what about those right? So if it may consider a solution so that will be mixing of two liquids. So that is one will be solvent the other will be called as solute. So by mixing of this solvent and solute that can form solution right. So that can form solution.

[00:02:29]The homogeneous mixture of homogeneous mixture of solvent and solute that can forms solution. Right? So what is meant by solvent? What is meant by solute? So that will be respect to the solution.

[00:02:44]Right? So in solution in solution the major component major component that will be present in the solution. Right? In solution major component is considered as or treated as solvent.

[00:03:01]Major component is treated as solvent and minor component minor component which is present in the solution that is called as solute.

[00:03:12]The minor component that will be present in the solution that is called solute.

[00:03:16]Right? Solute is always what? Minor component. So the solute is always minor component. Right? And also here right.

[00:03:26]So how many components? How many liquids are there? Two liquids are there.

[00:03:30]Therefore that becomes what? Binary solution. In that binary solution the homogeneous mixture of homogeneous mixture of solvent and solute that form solution. In this major component is the solvent and minor component is the solute. Right? So the major component is the solvent. That is always one component only.

[00:03:54]that is always or maybe one component right. So the solute may be one or more than one components right.

[00:04:07]So that means maybe one or more components the solute means small portion. So there are many number of components which will be present in the solution. So that is called whenever small portion many number of components are there that becomes treated as what solute but solvent is only one component. So that is the solvent right. So means out of all for example a solution is made with so various number of components what is the maximum component means major component which will be present in the solution that is called solvent. The remaining all will be treated as what?

[00:04:48]Solutes. Right? So the remaining will be treated as solutes. This is the solvent plus solute that becomes solution.

[00:04:55]Right? So in this solution, right? In this homogeneous mixture, right? So the throughout the mixture, right? So the distribution of solvent and solute particles into the solution in throughout that mixture. So that will be same only. Right? So therefore so this is the homogeneous mixture of two solutions right. So whenever the solution is consisting whenever solution is consisting only two liquids that we may call as what binary solution that we may call as binary solution.

[00:05:33]Right? So if solution is consisting three liquids three liquids that we may call as turnary Tinary solution. If solution will be consisting four liquids that becomes what? Quartinary solution.

[00:05:57]Quartonary solution. Right? As we mentioned this is so all are belongs to what? Homogeneous mixture. Right? So sometimes there is a possibility of heterogeneous mixture also will be there means so small portion of solid is converted to the added to the added to the liquid. So that becomes form heterogeneous right. So the example for this homogeneous mixtures homogeneous mixtures means right. So water is mixed with HCl. So that becomes forms a homogeneous mixture. So water will be major component. Therefore that is acts as solvent. So the HCl will be minor component. So that will be act as solute. Some small amount of solute is added to the large amount of water that can make HCl solution. So that solution will be homogeneous mixture solution that is called binary solution and in this two component systems will be there. One is the solvent and other is the solute. So like that if one more will be added so little bit alcohol will be added to that. So two components are there like HCl and alcohol that is overall three components are there that is known as turnary solution. A four components will be there that is quartinary solution right. So this is about solutions right. So solution is nothing but homogeneous mixture of two liquids right or more than two liquids that can make a solution right that can make a solution right.

[00:07:24]Then coming to the part of types of solutions right. So as we discussed that homogeneous and heterogeneous both will be there right.

[00:07:35]So the solutions types of solutions types of solutions right. So that means the first one will be homogeneous solution that is right. Next one will be heterogeneous solution.

[00:08:01]Heterogeneous solution. Homo is nothing but only one phase is present. So there are two different kind of phases will be there that is called heterogeneous.

[00:08:12]Right? So in this homogeneous mixture right homogeneous mixture means right only one component or one phase is present one phase is present either that may be solid phase, liquid phase or gasous phase right morely one phase is present that is called homogeneous solution right so there are more than one phase is present more than one phase is present right? So more than one phase is present that is called what? Heterogeneous solutions right? So in homogeneous mixture right in homogeneous mixture the composition and composition and properties composition and properties are uniformly distributed throughout the solution uniformly distributed throughout The solution right composition will be means whatever is the composition of solvent and solute will be there in homogeneous solution that composition will be distributed uniformly throughout the solution and properties also will be distributed throughout the solution. But in case of heterogeneous right the composition and composition and properties do not uniformly distributed right not uniformly distributed.

[00:09:58]Not uniformly distributed throughout the solution.

[00:10:06]not uniformly distributed throughout the solution. Right? Composion and properties, right? If you may consider the example of homogeneous solutions, right? Simple NAC will be added to water. NaCCl solution, right? Or else sugar solution, some amount of sugar will be added to water. So that can make sugar solution or NaCCl solution that becomes homogeneous consisting only one phase that is the liquid phase only. Right? So here the example of heterogeneous solutions. Example of heterogeneous solutions what sand solution.

[00:10:51]Sand solution means so add some sand particles to the water. Right? Water is a solvent. Add some sand particles. So that can make sand solution. In that two different phases will be there. So therefore more than one phase will be present in that solution. Such solutions are called heterogeneous solutions. Only one phase will be there that is called homogeneous solutions. So the homogeneous mixture of two or more components. So can make composition that will be distributed uniformly throughout the solution that is called homogeneous.

[00:11:25]There is no uniform distribution will be there. So like simple take water and add sand particle will be settled down only.

[00:11:31]So that sand may not be distributed in throughout that liquid. So that is not uniformly not uniformly distributed into throughout the solution. So this is about homogeneous solutions and heterogeneous solutions. Right? So one is the homogeneous and other one will be heterogeneous and based on the solvent nature also there are various kind of solutions will be there. Right? That is based on nature of solvent. Right? So the classification so we are going to check so that is based on right one second right based on based on solvent or solvent nature.

[00:12:31]uh based on solvent nature. So there are various kind of solutions will be there right. So whatever is the solvent we'll see solvent is a major component which will be present in the system or solution major component which will be present in the solution. If the solvent will be water right solvent will be water. So such solutions are called as what? Aqua solutions.

[00:12:59]where the water will be solvent. Such solutions are called aquis solutions.

[00:13:05]Right? So water whatever is the substance is dissolved in water that becomes aqua solution. Right? So instead of water if you may right instead of water if you may use other substances that is like C4 right C6 H6 CH3 these all are non-polar solvents therefore CL4 carbon tetrachloride this is a benzene this is the chloroform so such such solvents are such components are acts as the solvent in the solution means major components are These such solutions are called as what? Nonacquest solutions. Nonacquis solutions.

[00:13:49]Non-acquest solutions. Right? If one more will be there, right? So that is third one. So if alcohol will be alcohol will be acts as the solvent means major component is the alcohol.

[00:14:04]Right? So the major component is the alcohol means such solutions are what? Alcoholic solutions. Alcoholic solutions. Such solutions are called as alcoholic solutions. Next fourth one.

[00:14:19]Ether is a major product means a major component. If you may consider any solution that solution consisting major part is ether. Therefore such solutions are what? Ethereal solutions.

[00:14:33]Etheral solutions right. So if the major component will be liquid ammonia liquid ammonia liquid ammonia means so that is such solutions we may call as ammonical solutions ammonical solutions. This is purely based on this is purely based on solvent nature only whether solvent is water aqua solutions solvent is non-polar right that becomes nonqua solutions solvent is alcohol alcoholic solutions solvent is ether etheral solution solvent is liquid ammonia ammonical solutions right so just one more will be there so if one of the component is mercury Right? That may be this maybe either acts as solvent or solute whatever it that is particularly in case of mercury. Right? So the obtained solutions are called what?

[00:15:30]Amalgam solutions.

[00:15:33]Amalgam solutions. Right? So for example of amalgam solution sodium is combined with mercury. So that becomes sodium amalgam or zinc will be combined with mercury that is zinc amalgam solution.

[00:15:47]Right? So one of the component is the mercury. So that mercury is containing solutions are what we may call as amalgams. This is the based on the solvent nature. Particularly what kind of solvent we are using major component what is the nature of that major component based on that we will get the various kind of the solutions right. So then with respect to this right we may go through the classification of solutions right. So there is a huge classification will be there from that uh so we can get so one kind of uh main kind of classification and we are going to discuss about the various properties regarding that right. Next one classification.

[00:16:39]This classification will be based on physical state.

[00:16:45]based on physical states that may be either solid uh solvent or solute. Right? based on the physical states of solvent and solute.

[00:16:57]Physical states of uh solvent is what? Major component.

[00:17:04]Solute is what? Minor component. In any situation, major component is the solvent. Minor component is the solute.

[00:17:12]Right? So based on that, so we can get right type of solutions. So there are various kinds will be there. types of solutions. That is the main category in that physical state of physical state of solute.

[00:17:33]Physical state of solute. Right. Next.

[00:17:36]Physical state of solvent. Right. Next examples.

[00:17:50]based on this. So first how many type of solutions we have right? So we have idea about those three three kind of solutions will be there right. So with the help of the three kind of solutions right these are the three kind of major types of solutions in which so the physical state will be quite different. So the first one will be solid solution.

[00:18:21]The first one will be solid solution.

[00:18:24]Whatever is the solution becomes solid solution means the major component will be what? Solid only. Right? So therefore that is the solid.

[00:18:33]Solid and solid.

[00:18:37]So when major component is solid the minor components that will be belongs to solute right. So that will be once solid is there and liquid possibility is there and gas possibility is there means major component is solid minor component also solid by mixing of both solid and solid.

[00:18:59]Solid solid combinations will be what?

[00:19:02]So we make allies.

[00:19:05]Allies means that is combination of metals right. So we are making ornaments with the help of copper will be added with arum right or else copper is added with zinc. Copper plus zinc, right?

[00:19:19]Copper plus tin, right? Copper plus nickel, right? All those things, these all are what? Allies, right? So, when liquid is present in the solid, right? A small amount of liquid, a small amount of liquid, this will be present in solid, right? Solid will be major component. So, therefore the small amount of liquid will be combined with solid. So just now we discussed that amalgamy will be there right mercury will be small amount that is the liquid mercury in the form of liquid. So therefore mercury with sodium form amalgam right. So that is liquid is the mercury small portion of mercury which is combined with sodium metal that can form sodium amalgam. Right? What is the amalgam? That is sodium amalgam.

[00:20:13]N A H right when gas is in solid means so various times we may use hydrogen gas in platinum or peladium surface right hydrogen gas and present in platinum and paladium. So we make the solution of gas with the solids that becomes will give hydrogen gas in platinum.

[00:20:37]Second kind of solutions will be liquid solutions.

[00:20:43]Liquid solutions. This liquid solutions will be consisting major component is what? Liquid only. Right? So just I am going to write first major component that is liquid. Major component is always liquid. Such solutions are called liquid solutions. The minor may be that becomes a solid right that becomes liquid that becomes gas right. If small amount of solid is dissolved in liquid so that is NaCCl solution. Sodium chloride salt will be dissolved in water. Right? So that is the NaCCl solution. Right? Or sugar solution.

[00:21:26]A small amount of sugar will be added to water. Water is a liquid. That is a physical state of solvent will be liquid. The physical state of solute will be solid. NaCCl are sugar solution.

[00:21:38]Now both are liquids. Right? Both are liquids means the solution of right H2O plus C2 H5O. Alcohol plus water.

[00:21:50]Alcohol is the liquid and water is the liquid. The combination of alcohol and water that becomes make liquid liquid solutions. Then gas in liquid. Gas in liquid means what? So carbon dioxide gas which will be dissolved in water. Right?

[00:22:06]CO2 in water.

[00:22:11]Right? Carbon dioxide is dissolved in water or oxygen gas is dissolved in water. That is the example for gas in liquid. Right? So coming to the part of third category. So that are what?

[00:22:21]Gaseous solutions.

[00:22:25]Gaseous solutions. In gasous solutions, what about the major component? The major component will be gas only. Right?

[00:22:34]The major component will be gas. So same kind of terminology we will utilize in even collides also. Right? But here in place of this physical state of solute and solvent, we may use what? Dispersion medium and dispersion phase. With respect to the dispersion phase and dispersion medium we can get various kind of the components like soles, aerosols, gels, aerogels, right?

[00:22:56]Emulsions all kind of collision collides we will get. So at the time of collides we able to discuss all those things. So such kind of solutions we will get except gas and gas right that is in collision collides sorry that is in collides right here the minor component is what? So again we have to take solid then liquid.

[00:23:20]So then gases right solid and gas the major component is the gas only. So therefore the examples will be right. So camper is the solid. Therefore camper is present in nitrogen gas. So a small amount of camp which will be dissolved or present in nitrogen gas right. Liquid in gas.

[00:23:46]Liquid in gas means what? So liquid is a chloroform. So this chloroform is present in nitrogen gas. Right? So when gas and gas will be there atmosphere will be there that will be consisting gasous mixtures or mixture of gas.

[00:24:03]Mixture of gases that will be present in air. This is the example. Right? So these all are right examples for the corresponding solutions. Right? So there are nine kind of solutions will be there but the majorly type of solutions will be solid solution, liquid solution and gas solution. So but in our syllabus they mentioned right. So type of solutions will be what? Liquid solutions we are going to discuss about liquid solutions only. Right? So means what is the solubility of solid in liquid? What is the solubility of gas in liquid? Then what about the concept which will be related to liquid and liquid that will be mentioned in our syllabus. So right the solid solutions and gases solutions just for example point of view. So we will discuss Right. We are going to discuss about right. So directly what is the syllabus mentioned in the solutions means. So directly that are solubility heading will be there. So but we have to know the solubility concept. Before that some basic concepts will be there. Definitely we have to know all those things. With the help of that we have to discuss about the solubility and that is particularly about what liquid liquid solutions. This entire syllabus will be mentioned right. All these three we are going to discuss that is solid in liquid then liquid in liquid and gas in liquid.

[00:25:49]All these three topics elaborately we have to discuss that is our main syllabus. Right? In addition to this classification some other kind of types of solutions will be there. Right?

[00:26:02]So particularly what liquid and liquid only right. So liquid liquid solutions are different kind of solutions will be there. After that we have to discuss about the what solid and liquid and gas in liquid. What is the solubility that we are going to discuss right? So then coming to the part of one more types of solutions are liquid solutions. Right.

[00:26:26]So just putting liquid solutions. This is very important means what kind of solutions we have in our syllabus that is liquid solutions.

[00:26:45]Liquid solutions means what? Liquid in liquid particularly liquid in liquid. This liquid will be what? Solute. So this liquid will be what? solvent then combination of liquid and liquid that becomes forms liquid solutions. The combination of what? Solvent and solute that can give solution. Simply mixing of solvent and solute together that can make a solution. That particular solution is what? Liquid solution.

[00:27:17]Because liquid is a solute and liquid also solvent both are mixing together we can get liquid solutions. Right? So these are three types.

[00:27:26]Right?

[00:27:34]Three types will be there. So the first one will be completely missible solutions.

[00:27:44]Completely missible solutions.

[00:27:53]Right? Completely missible solutions means both solvent and solute mixed together that can make a homogeneous mixture solution means that completely solute is dissolved in solvent that can make a solution. Such solutions are called completely misable solutions.

[00:28:14]Right? For completely misable solutions examples will be take small amount of hydrochloric acid that will be added to water. Right? small amount of hydrochloric acid that will be added to water. So that can give completely visible solution. So therefore we may call as solution will be aqua solution.

[00:28:32]That is aqua solution of HCL aqua solution because water is solvent right water is solvent. Such solutions are what? Aqua solutions. This is about completely emissibility right. Second one is about partial missible solutions.

[00:28:56]Partial missible solutions only small extent will be dissolved. Right? Only small extent will be dissolved. Such solutions are called partially missible solutions. Right? So what are the examples of partially missible solutions? Right?

[00:29:16]The examples for partially missible solutions. Whenever phenol added to water only small portion of phenol is soluble right so that can make partially missible solutions. Here we are going to discuss this is the liquid solution only but partially missible solution right. This is the liquid solution partially misable solutions where we are going to discuss about the word critical solution temperature concepts.

[00:29:46]CST concept we are going to discuss right so that is mentioned in our syllabus that is particularly what partially missible solutions what is meant by CST critical solution temperature right critical solution temperature that is a minimum critical solution temperature maximum critical solution temperature all those things will be mentioned in our syllabus right okay coming to the part of third category partially missible next one will be immissible ible solutions.

[00:30:18]Imissible solutions means so both solvent and solute may not mix together in any extent right. So as it is that can make two layers right so that we may get right example of imisible liquids means HCL is combined with carbon tetrachloride this is one polar right another one is non-polar so that mixing of this polar and non-polar that makes immisible liquids so this can make two layer system two layer system immissible liquids means we can get two layer system so that two layer system one more example will be there water with nhexane nhexane and water are immissible liquids. So where we are going to discuss about distribution law where we are going to discuss about distribution law right so these all three will be mentioned in the syllabus right so first completely missible solutions means we can get various kind of solutions like ideal solutions and non ideal solutions we will get right So that we are going to discuss then solubility also mentioned that solubility concept also will be discussed in that we will get Henry's law and R's law will get so that is also will be discussed that is applicable for what completely missible solutions then coming to the part of part partial missible solutions means so critical solution temperature we have to discuss CST concept will be introduced so that will be for particularly partially misable solutions what is meant by CST so what are the phenol water system how we are getting the concept from that we'll see and somewhere will be there immissible last will be mentioned distribution law in our syllabus therefore we are going to discuss about the word distribution law also these two are doesn't mix together that can make two layer systems right one will be above layer one will be below layer based on the density whose density will be less that can make occupy above layer density will be more that can make below layer right so one is the water other one is the organic substance And therefore we make called as two layer system that is organic layer and aquas layer. Right? This is the overall entire syllabus that is in liquid solutions.

[00:32:40]Which part we have been discussed that is liquids in liquids only. Liquids in liquids. Other two also will be there.

[00:32:48]Solid in liquid and gas in liquid that is the will be discussed in terms of solubility. What is the solubility of solid in liquid? What is the solubility of liquid gases in liquids? So that three we are going to discuss in detail.

[00:33:05]So before going to that so we have to know some terminology so that which will be related to that solutions right. So whatever is the solution is there how we have to say the concentration of the solution.

[00:33:19]For example water is there water is a solvent or that may be combined with some minerals. So that can acts as solution. Right? If is a pure will be there that is a solvent. If any components are mixed like hardness of water means calcium and magnesium salts are present in the water that can make hardness. So such minor components will be present in that water. Therefore water will be act as a solvent and minor components will be act as solute. So therefore that solution we are going to discuss then what is the concentration terms right the concentration terms will be denoted to the solutions that is based on the solute based on the amount of solute how much amount of solute is present in the solution based on that we can get so various methods for expression of concentrations right methods nexting methods for expression of concentrations, right?

[00:34:22]Methods for methods of expression concentration.

[00:34:37]Methods of expression concentration.

[00:34:47]Right. So there are various methods are there. What are those methods to express the concentration? This is based on amount of solute.

[00:35:06]This is based on amount of solute with respect to solvent.

[00:35:14]What kind of solvent is there? Right?

[00:35:17]Then how much amount of solute will be present in that solvent that can make solution. Right? So based on this, there are various methods are there to express that concentration. Just we are going to see. So the first one will be weight by weight percentage method. Right? The second one will be weight by volume percentage method. Right? Weight by volume percentage method. Then the third one will be volume by volume percentage method. Volume by volume percentage method. Right? So then the fourth one will be marity that will be denoted with M. The fifth one will be normality that is N. Sixth one will be mality that is m. Seventh one will be mole fraction that is x. Then eighth one will be mality marity normality marity mole fraction. Then eighth one will be ppm parts per million. So then ninth one will be solubility right even strength of the solution also will be there. So that will be come under this only right these are the major part of methods to express the concentrations right that concentration will be based on what how much amount of solute that will be present in the solution that solution will be related to solvent right so actually this will be what this will be how much amount of solute which will be present in the solution right so that solution will be related to But solvent right this is the conditions that can make the concentration terms right so we are going to discuss about all those things here we have to keep it in mind these three first three will be weight by weight percentage weight by volume percentage will be applicable for 100 right so the next will be next four will be R3 so this next three will be applicable for 1,000 this is 1,000 ml or 1,000 g Right here 100 ml or 100 g right. So just we have to keep it in mind. Therefore from that we will get the definitions.

[00:37:57]So this is first three will be related to 100 that is either in ml or gs. The next three will be related to 1,000 ml or 1,000 g. Right? So somehow three will be quite different independently. Right?

[00:38:11]So individual we have to make the definitions of all these three. Right?

[00:38:15]So now we'll go with the little bit right just for information only. So we'll do some questions also based on this right weight by weight percentage.

[00:38:25]First one will be what? Weight by weight percentage right.

[00:38:32]First one will be weight by weight percentage method.

[00:38:43]What is meant by weight by weight percentage method means the first weight is belongs to solute. The below weight is belongs to solution that we have to keep it in mind. So this will be belongs to what? Solute.

[00:38:57]This will be belongs to what? Solution not solvent solution. Therefore, how can make a definition? Means amount of solute will be grams present in or dissolved in present in 100 g of solution.

[00:39:21]In total 100 g of solution, how much amount of solute is present? So that can give percentage of weight by weight method, right? So simply weight by weight percentage we have to written as weight of solute weight of solute in grams divided by weight of solute in grams divided by weight of solution divided by weight of solution that is also in grams multiplied with 100 that can give percentage right. So this is the weight by weight percentage only right by weight percentage right for example right 10% 10 weight by weight percentage of 10 weight by weight percentage of NaOH 10 weight by weight percentage of NO means what we have to Okay. NaOH solution, right? Solution means combined with water, right? So this we have to say how many grams NaOH 10 weight means this first will be belongs to solute that is 10 g of NaOH 10 g of NaOH which is combined with how many grams of solvent the total solution will be by combining of this total solution will be how much? 100 g.

[00:40:57]What is the definition? The amount of solute which is present in 100 g of solution. Total solution must be 100 g.

[00:41:04]But how many grams of solute is there?

[00:41:06]40 g of solute is there. Therefore, what about the remaining right? Remaining 90 g will be solvent.

[00:41:15]90 g will be solvent. That is the solvent will be water. 10 g of NaOH 90 g of water. The total becomes 100 ml. So that is the 100 ml NaOH solution.

[00:41:28]100 g of NaOH solution. Sorry 100 g means 10 g plus 90 g overall 100 g.

[00:41:36]Already we discussed that this weight by weight will be applicable for what? 100.

[00:41:40]Whether it is a weight means applicable for 100 g. Right? In this 100 g in this 100 g solution how much amount of solute is present that will be expressed in terms of weight by weight only. Right?

[00:41:53]Weight by weight. Similarly weight by volume, volume by volume also similar to this only just we have to understand easily right.

[00:42:02]So then see similar to this the next one will be second one will be weight by volume percentage weight by volume percentage. So this first W already I told that this will be related to solute. The V will be related to solution.

[00:42:28]So similarly here this first term will be related to solute. Below term will be related to solution. Here also same right. So therefore how we will define means the amount of solute right? Amount of solute. Amt means amount of solute.

[00:42:50]amount of solute that solute will be in what grams present in right or dissolved in 100 ml of solution because that solution will be expressed in terms of volume only right amount of solute is present in or dissolved in 100 ml of solution. So therefore what was the formula we have to use weight by volume percentage is equals to weight of solute weight of solute in g divided by volume of solution volume of solution multiplied with 100 right as similar to that only right so this is the formula right so therefore here just we'll go with example or question directly Right. So what is meant by 10 uh 15%.

[00:43:45]15 weight by volume percent 15 weight by volume percentage sucrose solution.

[00:44:00]Sucross solution or sugar solution whatever it right. So we may take this.

[00:44:06]So that means what is the 15 g means this will be belongs to solute that is a sucrose right. So therefore 15 g of sucrose this 15 g of sucrose which will be present in how much 100 ml right 100 ml solution.

[00:44:28]So therefore how much amount we have to take the solvent right 15 g will be so that is 100 ml of solvent water right so these both will be combined together we can get 100 ml solution sir by adding 15 g to the 100 ml little bit volume will be increased right so then how we have to prepare that solution means so first we have to take a 100 ml standard flask In that take some amount of water around 30 ml or 40 ml then add 15 g of sucros dissolve it right then after that you have to make up up to the mark with water that becomes exact 100 ml. If you take direct 100 ml and adding 15 g little bit water quantity will be increases right. So the volume will be increases at that time you will get 100 plus volume right. So how we'll get this exact means first we have to take small amount then dissolve this solute and after that we have to make up to the 100 that is becomes total 100 ml solution right so therefore sol solvent volume is equals to solution volume in this case of weight by volume percentage right. So then coming to the part of volume by volume both are in volume only similar to this weight by weight right. So volume of solute is present in right the third category is volume by volume percentage right so directly I'm giving definition right volume by volume percentage is equals to way uh sorry volume of right amount of solute this amount of solute will be present In word ml only right divided by volume of volume of solution this is also in ml multiplied with 100 right both are in ml only volume by volume right so therefore we'll go with one example right 5% of hcl solution 5% of solution five means weight by weight sorry volume by volume volume by volume percentage of HCl solution. So this first will be related to what solute volume. So therefore 5 ml we have to take 5 ml of HCl. This is combined with how much? So therefore we will get total volume becomes what 100 ml by combined with 5 ml is combined with 95 ml of water. So that can gives total 100 ml HCl solution right 95 ml. So make it clearly understand that right weight by weight by volume. Next volume by volume these are very important which we can utilize in further determination of concentrations in terms of marity normality mole fraction and all those things also. Right? So this is the equation and examples. Okay. This is the volume by volume percentage. This all will be applicable for what? 100 only.

[00:47:54]If it is weight, express it in grams. If it is volume, expressed in ml. Right?

[00:48:01]So, coming to the part of next concentration term that is the marity.

[00:48:07]Right?

[00:48:20]Right. The next one will be what? Fourth one will be marity.

[00:48:29]Marity will be denoted with m. So I told that already these are belongs to what,000 right? 1,000 ml or 1,000 g.

[00:48:40]Okay 1,000 ml is nothing but what?

[00:48:43]one liter. Remember that marity will be related to one liter. After that that will be converted into ml that will be very easy only. Right? In that one liter solution how many number of moles of solute is present. Right? So simple the definition will be number of moles of solute. Number of moles of solute is present in is present in one liter solution. So total how much solution is there? One liter is there. In one liter how many number of moles of solute is there? That becomes marity. That will be n by v.

[00:49:26]V in lit. V in liters. But number of moles n is equals to we know that weight by g molecular weight by w by gmw g molecular weight. So both w also is present in grams. Right? So this is also is present in grams. Therefore weight by gram molecular weight we have to take.

[00:49:50]Therefore marity is equals to weight by g molecular weight into 1 by v in l.

[00:49:58]Right? If these liters will be converted into ml that becomes marity capital m will be right capital m will be weight by g molecular weight into 1,000 divided by v in ml right so this is the these all the three equations which are related to what marity so if it is in ml we have to use this equation if it is volume in liters we have to use this equation so then volume is uh in liters But number of moles will be given.

[00:50:30]Therefore, we have to use this equation.

[00:50:33]Right?

[00:50:49]Right. So here so many transformations are there. Right? So what are those transformations that we will see? Right.

[00:50:57]This is the important equations we have to remember. So because we are not getting direct equation. So by examiner we'll make confusions to get right.

[00:51:07]Okay. Here weight by volume right. So here weight by volume will be considered as right weight by volume that is multiplied with 100. So that becomes converted as what? M is equals to weight by volume percentage into 10 divided by g molecular weight.

[00:51:33]Right? So that means this 1,000 will be considered as 100 into 10 that 100 will be multiplied to this that becomes weight by volume percentage we will get right. So even this I am going to change a little bit right. So for our convenient so that will be that will be multiplied with 100 by V in ml this is multiplied with 10 100 into 10 means 1,000 only right so therefore this weight by volume percentage the overall weight by volume percentage right by volume into 100 that becomes weight by volume percentage weight by volume percentage into 100 whenever weight by volume percentage is given therefore the marity will be considered as like is right. So but in addition to this density is known right but density is mass by volume. Density is equals to mass by volume. Right? So mass means that is about weight by volume. Weight by volume. Right? Density will be weight by volume.

[00:52:44]So therefore this will be considered as right. So in case of weight by volume means what we have to write density right. So density weight by volume is there. So therefore where in case of volume we have to write weight by density right. So from this equation volume is equals to weight by density.

[00:53:05]Weight by density. So in place of volume you have to write weight by density that is marity is equals to weight by gram molecular weight is there right first one will be weight by g molecular weight is there into 1,000 divided by in case of v what we have to write w by d w by d right in case of volume in ml that is w by d means in case of v in this equation in case of V I am going to write W by D right now what I have to consider means this 100 will be multiplied with 10 right now this weight by weight into 100 I will get this density will come numerator therefore marity will be equals to weight by weight percentage into density into 10 divided by g molecular weight if weight by weight is given this is the formula we have to utilize if weight by volume is given this is the formula we have to utilize right so this is the formula we have to utilize right so the with the help of this so I'm going to calculate the concentration of water every day we are using water daily right what is the concentration of water how we will get C right so concentration of water Right? Or else marity of water is the question. Marity of water is the question. Right? So water density density of water is what?

[00:54:48]1.00 g per ml. Right? Next weight of water. Molecular weight of water is how much? Right? That is 18.

[00:55:01]Right? Percent of purity. Right?

[00:55:13]right? The marity is equals to weight by weight percentage means this percentage of purity this will be weight by weight means percentage that will be 100 right multiplied with the density is 1 0 multiplied with 10 divided by 18 therefore this is the 1,000 by 18 right therefore 55.55 m what is the water concentration 55.55 m right any liquid will be there not only the water with the help of density and percentage of purity. So we can get the concentration that is with the help of this equation only. These are common equations right marity. So but this is the equation weight by weight percentage into density into 10 divided by molecular weight. If density is given if there is no density weight by volume we have to get weight by volume percentage into 10 by g molecular weight. So these are the two equations we have to utilize to get the concentration in terms of marity right. So here also one dilution formula is there right. So that is also we have to written right dilution formula continuation dilution formula right so what is the dilution formula m1 v1 is equals to m_sub_2 v_sub_2 right m1 a1 is equals to m_sub_2 v_sub_2 where number of moles are same.

[00:56:50]Number of moles same. If number of moles are same means n_sub_1 is equals to n_sub_2. Right? So if we have to use m1 v1 by n1 is equals to m_sub_2 vsub2 by m_sub_2 v2 by n_sub_2 where number of moles are not equal. Right? So whenever we are going to discuss about the dilution process of redux reactions for the redux reactions the number of moles not at all equal. So therefore we have to utilize this formula. Wherever the number of moles will be same for example acid based reactions acid base reactions number of moles will be same. So therefore we have to use this like HCl versus NaOH. HCl versus NaOH. Right? So then here what redux reactions we have to use redux reactions for redux reactions number of moles are unequal therefore we have to use this formula right so coming to the part of right any solution is consisting 1 molar 1 m solution is there that 1 m solution we may call as what molar solution 1 m solution is called as what molar solution right 0.1 m solution is Say sorry 0.5 we have to take first right 0.5 molar is there right so 0.5 m is there what is meant by 0.5 means mar solution this terminology exam right solution semiar solution solution Right?

[00:58:39]Semiolar solution. Semiolar solution means what is the concentration? 0.5.

[00:58:46]Right? Therefore, decimar solution.

[00:58:49]Decimar solution means decimar solution that is 0.1 molar. Right? Centar solution that is centar solution means centimolar solution that is 0.01 m. Next 0.001 001 m that is what millolar solution millar solution right so this terminology we will get in the question right so whenever a decimar solution will be undergo undergo dilution therefore what is the concentration of the resultant solution like that we will get the questions right so one molar means molar solution 5 means semimolar 0.1 means AC centime means 0.01 then mill means 0.001 0001 molar. Right?

[00:59:43]Whenever mixture solutions are there, right? For mixture solutions, how we can get the concentration of resultant solution, right? So for mixture of solutions, right?

[00:59:58]For mixture solutions, for mixture of solutions, right? So what is the concentration we will get?

[01:00:10]Concentration for mixture of solutions.

[01:00:13]So the solution A will be consisting marity is M A VA right? So the solution B consisting MB VB uh we have to use small right? M A VA this is MB VB. So when these two are mixed together these two solutions are mixed together.

[01:00:37]So what about the resultant solution right? Resultant solution marity is what right? So that resultant solution marity will be M is equals to what we have to take MA VA plus MB VB divided by VA plus VB right so this VA plus VB also we may call as V total also right this is the formula we have to utilize for the mixture of solutions whether acid mixture will be there base mixture will be there so therefore we have to use these conditions for mixture of solutions right this is about marity various equations we have been discussed for the marity so all kind of equations will be applicable for the normality also but instead of number of moles we have to use gram equivalent right so the same all equations we are going to written for normality also right so just we will move little bit first with normality because as we understand all those things. Therefore we can get normality will be easily righting normality normality will be denoted with n right so these all are formulas only so just we have to remember all those formulas right so which formula can be useful for uh solving of the problem. So where we have to use that formula, right? When marity is applicable for number of moles, normality will be applicable for what? Number of gram equivalents.

[01:02:47]number of gram equivalents. Right? So what about gram equivalent that we'll be we'll see after this. Right? Right. What is the definition? Definition of normality means number of gram equivalents present in gram number of gram equivalents of solute present in one liter solution.

[01:03:15]One liter solution right. Similarly here N also what g equivalence g equivalence that is weight by g equivalent weight.

[01:03:28]So previously we considered as molecular weight equivalent right for example weight so that becomes getting equivalent weight Right? So equivalent weight for that person means so that molecular weight divided with n factor. What is the n factor with respect that we can get the equivalent weight right? So that is weight by g equivalent weight is the n. So therefore all the formulas what we wrote for marity. So that all will be utilized for normality also. Normality is equals to n by v. But n is equals to weight by g equivalent weight into 1 by v n in lit.

[01:04:32]1x v in liters. Right. Next equation that n is equals to weight by g equivalent weight.

[01:04:43]Right? G equivalent weight. This is the gram.

[01:04:47]Right? G equivalent weight into 1,000 by V in ml. Right? So these are the three common equations. Next equation will be normality will be expressed in terms of weight by volume percentage. Weight by volume percentage into 10 divided by g equivalent weight. Right?

[01:05:10]G equivalent weight. If weight by weight is given. So if weight by sorry weight by volume percentage is given right if weight by weight is given normality is equals to weight by weight percentage into density will be added. So just now all those how the conversions will be there we have been discussed right. So divided by g equivalent weight what is this equivalent weight we will discuss later right. So then coming to the next formula right after these two dilution formula will be there.

[01:05:54]Dilution formula is what? N1 V_sub1 is equals to N_sub_2 V_sub_2 only one formula right. So here we used to say number of gram equivalent always same means similarly n1= to n_sub_2 ns1 is not equals to n_sub_2 possibility number of equivalent is always same only Right? So whatever the number of equivalents will be there that all are same and always N1 is equals to N_sub_2. Therefore we have to use one dilution formula. This is only right. So this is the important thing for mixture of mixture of acid and base.

[01:06:51]Right? For mixture of acid and base solutions.

[01:06:58]Mixture of acid base solutions right. So for acid what we have to consider for acid normality will be NA volume will be VA. For base for base normality will be NB volume will be VB. Therefore so what is the mixture of solution right? So the resultant mixture of solution that is depending on this if N A VA is greater than NB VB. NAV VA is greater than NB VB. Whose concentration is more? Acid concentration is more. Therefore, we can get the resultant concentration. Our solution will be hydrogen only.

[01:07:40]Therefore, H+ concentration acid means H+ concentration. So this is the H+ concentration or normality resultant normality that will be equals to NA VA minus N A VA minus NB VB divided by VA + VB VA plus VB Hence the resultant solution is what acidic in nature acidic solution because acid concentration will be solution H+ right that is one condition. So then coming to the part of second condition right if N A VA is less than NB VB NB VB and base right base concentration base concentration O minus concentration or resultant solution normality is equals to base right so NB VB NB VB minus N A VA divided by VA + VB. The resultant solution is what? Basic solution.

[01:09:10]Basic solution. Resultant solution and basic solution. Right? So my third condition and third condition, right? If N A VA is equals to NB VB, right? So rendered concentrations same what about the resultant concentration resultant concentration will be means that is the resultant normality so that will be 10 ^ of -7 only because NAVA minus NB VB that becomes same only these both are same therefore that concentration will be equals to 10 ^ of - 7 therefore whose concentration means pH is equals to 7 therefore such solution is neutral solution.

[01:10:01]This is the kind of various kind of solutions we will get with the help of normalities. Right? These all are definitions of normality, normality equations. Then that will be applicable for dilution formula and a mixture of acids and bases. Right? So this uh we have to get important because by mixing of acid with base the resultant solution will be acidic in nature or basic in nature or neutral in nature and also whose pH will be so getting how right just copied all all concepts are very important.

[01:10:47]Right? So this was not mentioned but whenever we are going to discuss about the concept definitely normality all those things marity mole fraction all those things we have to know right so ppm particularly mole fraction we have to utilize in R's law and Henry's law right so at that time we have to know all those things before only we are discussing about all those things after that we'll discuss our main topic Right. So similar to similar to marity. So one more we have to write here. So what about that means?

[01:11:39]Right.

[01:11:41]If 1 N will be there that is called as what? Normal solution.

[01:11:47]Normal solution. 0.5N will be there.

[01:11:51]That is the what? Semnormal solution.

[01:11:58]Semnormal solution 0.1N will be there.

[01:12:01]That is basormal solution. Right? Normal means nothing but what? Normality.

[01:12:08]Right? 0.0 01 normality is there normal solution 0.001 001 normality is there right? Millie normal solution as similar to the marity also right right. So then here we have discussed that equivalent weight right equivalent Right. What is meant by equivalent weight? So just we'll go with the definition. Right. So I have the substance right this substance either combined with 1.008 008 parts of hydrogen are 35.5 parts by hydrogen or 35.5 parts by chlorine or eight parts by oxygen.

[01:13:33]This substance either it may combine with hydrogen or combined with chlorine or combined with oxygen by how many parts? This is the parts 1.008 parts by hydrogen or 35.5 parts by chlorine or eight parts by oxygen. Either this may be combine or displace. Right? Combine or displace.

[01:14:00]either displace in any parts of hydrogen will be combined to this substance or so this 1.008 008 parts removed by the hydrogen from the substance that will be equals to what? This will be equals to what?

[01:14:18]Its equivalent weight.

[01:14:21]That will be equals to its equivalent weight. Right? So that is actual definition. So simply we will get the equivalent weight. Equivalent weight with the help of equation that is whatever it molecular weight divided by n factor.

[01:14:38]This n factor is different for different substances.

[01:14:42]N factor is different for different substances. That is called equivalent weight. Right? So just I will give some examples for this equivalent weight. So from that you will understand that right.

[01:15:04]What is meant by equivalent weight and n factor? N factor will be different for different substances right so just I am giving N factor n factor for different substances right so N factor for acids N factor for acids what we will get basicity N factor for acids is what? Basicity.

[01:15:42]What is mean by basicity? Means number of replaceable hydrogens. Number of replaceable hydrogens. Right? So then N factor for bases.

[01:15:56]N factor for bases that is called what?

[01:15:59]Sed.

[01:16:01]What is meant by SD? That is how many number of replaceable O groups. Number of replaceable O groups will be how many number will be there? That is called acidity. N factor will be acidity for bases. Right? So then N factor for salts salts, right? So salts in this charge on either kan or anion. Charge on kan or anion.

[01:16:38]Right. So charge on kan or anion that will be equals to n factor. Right. Next ions.

[01:16:50]Ions right. Charge on ion.

[01:16:56]If it is ion is there how we'll get the equivalent weight means with the help of charge on ion. Right? Last one oxidizing agent or reducing agents. Right?

[01:17:09]Oxidizing agent or reducing agent.

[01:17:11]Right? Here number of number of electrons either lost or gained.

[01:17:20]number of electrons either lost or gained. So that can give the n factor for various substances. Right? So for example here I am going to calculate right HCl is there. What is the equivalent weight of HCl? E of HCL will be right molecular weight of HCl divided by right. How many H+ it will give? Molecular will be denoted with M only M divided with how many replaceable H+ will be there? 1. Therefore, M by 1.

[01:17:52]Right. Next, H2S4 is there. H2S4 is there. Equivalent weight of H2S4.

[01:18:02]Equivalent weight of H2SO4 is that molecular weight divided by 2 because two replaceable hydrogen's will be there. Right? Like H3 P4 if you may consider H3 P4 means equivalent weight is equals to M by 3. Three replaceable hydrogens's are there. Here two replaceable here one replaceable here three replaceable hydrogens's are there so that's why this is the thing right so then coming to the part of bases right so space is not sufficient we'll move like other also right so this is about what base right for base equivalent of any base is equals to molecular weight divided by acid n factor is what acid for base. So here also same definition or formula for acids E of acid is equals to molecular weight by basicity. Right?

[01:18:57]So we'll see like examples N AOH NaOH is equivalent weight of NaOH is equals to what? Molecular weight divided by one only because it can replace only one. Calcium hydroxide right equivalent weight of calcium hydroxide that is equals to M by 2. Right? Next aluminium hydroxide whose equivalent weight will be what?

[01:19:25]How many replaceable O groups are there?

[01:19:27]Three. Therefore molecular weight by three. These all will be helpful in electrochemistry also. That's why I'm going in detail. Right here 27 by3 that means what is the equivalent weight? 9.

[01:19:40]Here calcium hydroxide will be calcium will be 40. 40 + 2 oxygen means 32. 40 + 32 means 72 + 2 74 by2 74 by 2 that becomes 36.

[01:19:56]Oh sorry 37 right? So this is the equivalent weight is 40 only. So with the help of this any base is there whose equivalent weight will be calculated like this like any salt is there ion is there oxidizing and reducing agent is there. So therefore we are going to calculate the equivalent weight with the help of equivalent weight. So we can get the concentration that is the normality right.

[01:20:23]So that is the n factor for various substances right n factor for various substances.

[01:20:29]So just I am going with salts and other three right.

[01:20:34]So I will get that equivalent weight right now salt I may consider E of salt is equals to molecular weight by charge on kion or charge on anion right so charge on kion or charge on anion. So what is the charge on kion for example right the salt we have to take KCL KCL will give K plus and Cl minus right. So therefore equivalent weight of KCL is equals to molecular weight by charge on cation is how much that is the + one only right. So or else next calcium chloride calcium chloride will give calcium + 2 plus 2 CL minus two negatives are there or two positives are there. Therefore equivalent weight of calcium chloride will be molecular weight by two that is for salts. Right?

[01:21:40]If any ion is there, right? If any ion is there, ion means consider as write N3 minus NZ ion. This is right. N3 minus means equivalent weight of N3 minus is equals to molecular weight divided by charge ion is only 1.

[01:22:02]Right? Next CO3 minus2 E of CO3 minus2 is equals to molecular weight divided by 2 because charge will be 2 irrespective of the positive and negative. So whatever the charge will be there that will be considered as N factorus right +2 + only number irrespective of the sign right. So this is about salts and ions like similarly oxidizing agent and reducing agents number of electrons will be lost and gain. So that uh will be explicit in case of electrochemistry in detail. Right? So then we are moving to the next right. Next one that is the mality.

[01:22:50]Right? After normality the next one will be what? Expression of mality.

[01:22:56]Right?

[01:22:58]Mality this is denoted with what small m this is applicable here we have to remember 1,000 g of solvent right this is only expressing the concentration with respect to solvent irrespective of the solution right so simple how we are getting the definition means number of moles of solute number of moles of solute which is dissolved in 1 kg of solvent.

[01:23:36]See here solvent only not solution. Just you have to identify this difference compared to marity and normality. So therefore what we have to write m small m is equals to number of moles by weight of solvent.

[01:23:53]Right? Weight of solvent. So but n is equals to what? Weight by g molecular weight. Right? Weight by gram molecular weight. So therefore mality m is equals to weight by g molecular weight into 1 by w of solvent in kg. Right? So if we have to written M is equals to W by g molecular weight into 1,000 divided by W of solvent in g right. So this is the only mality.

[01:24:35]So that can give small M right. So that can give the word solvent weight we have to consider. Right? Solvent weight we have to consider. Right? So then coming to the mole fraction this is very important uh that is denoted with X right simple definition just to go through it X is equals to the ratio of ratio of directly I am giving equation X is equals to the ratio of number of moles of number of moles of particular component particular component by total number of moles of component.

[01:25:27]Total number of moles of components components number of moles that is the mole fraction. This is very important. And we are going to discuss even further topics with the help of mole fraction only. So that will be related with the vapor pressure all those things. Right? So therefore here consider A is a solvent.

[01:25:58]B is a solute.

[01:26:01]A is a solvent. B is a solute. What about number of moles of A that is N A.

[01:26:07]Number of moles of B NB. So therefore what is the mole fraction of solvent? X A is equals to how many number of moles of A is there? N A by what about total number of moles? It is a binary solution.

[01:26:23]Binary solution, right? Therefore, N A + NB, right? Similarly, XB is equals to what we have to write XB is equals to mole fraction of B solute. That is number of moles will be B. By total number of moles NA + NB right? If you add sum X A + XB is equals to N A by N A + NB plus NB by N A + NB. So that will be we will get NA + NB by NA + NB. So the sum of all the mole fractions always equals to always equals to 1. So therefore for two component system X a + xb is equ= to 1.

[01:27:13]For three component system x a + xb + x c is equals to 1. For four component system x a + xb + x c + x d is equ= to 1. Like that we will get the mole fraction. Right? So this is the one of the concentration term.

[01:27:35]Okay.

[01:27:36]After this small fraction right one more will be there that is what ppm parts per mill right parts per million that will be used for hardness of water right this mality and parts per million will be used for hardness of water.

[01:28:07]Right.

[01:28:10]Right. So the next one will be ppm.

[01:28:15]ppm will be parts per million means how many number of parts of solute is present in 1 million part of solution. Right?

[01:28:33]Number of parts of solute present in 10 ^ of six parts of solution. What is mean by this 10 ^ of six? That is million million part of solution. Right? So therefore we have to written as parts per million is equals to number of parts of uh solute by total number of parts of total parts of solution multiplied with 100 total parts of solution sorry multiplied with 10 ^ of six that is the million Right. So this ppm will be used to express the hardness of water.

[01:29:34]Hardness of water concentration will be expressed in terms of ppm. And the relation between ppm will be equals to 1 ppm is equals to 1 mg per liter.

[01:29:48]1 ppm is equals to 1 mg per liter.

[01:29:51]Right?

[01:29:53]That is some other also will be there degree degree clark and degree French right degree French and degree clark units also will be there to express the hardness of water but here our aim will be what parts per million right ppm after this there is a solubility is there right what is meant by solubility what is the solubility of solid in liquid right what is the solubility of gas in liquid liquid after that what about liquid liquid properties that are like rula and what are the composition so that solubility concept will be mentioned in our syllabus so we'll go in detailed with the solubility and whose properties in the next class okay thank