Subject : Chemistry Class : XII Chapter-2.Solutions Work Sheet ( WS 2. 1) Topic- 2.1 Henry s & Raoult s Laws

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1 Work Sheet ( WS 2. 1) Topic- 2.1 Henry s & Raoult s Laws Name -. Class/ sec.. Roll No.. A. Fill in the blanks: 1. Solutions are mixtures of two or more than two components. 2. Generally, the component that is present in the largest quantity is known as. 3. Mass percentage (w/w): The mass percentage of a component of a solution is defined as: Mass % of a component = 4. Mole fraction of a component = 5. In a given solution sum of all the mole fractions is. 6. Molarity (M) is defined as number of moles of solute dissolved in one litre (or one cubic decimetre) of. 7. Molality (m) is defined as the number of moles of the solute per kilogram (kg) of the. 8. A solution in which no more solute can be dissolved at the same temperature and pressure is called a solution. 9. solution is one in which more solute can be dissolved at the same temperature. 10. The solubility of a solid in a liquid is significantly affected by changes. 11. Pressure does not have any significant effect on solubility of in liquids. 12. law states that at a constant temperature, the solubility of a gas in a liquid is directly proportional to the pressure of the gas. 13. The mole fraction of gas in the solution is proportional to the of the gas over the solution. 14. s law states that the partial pressure of the gas in vapour phase (p) is proportional to the mole fraction of the gas (x) in the solution. 15. Higher the value of KH at a given pressure, the is the solubility of the gas in the liquid. 16. Solubility of gases in liquids decreases with in temperature. 17. For a solution of volatile liquids, the partial vapour pressure of each component in the solution is proportional to its mole fraction. 18. According to s law of partial pressures, the total pressure over the solution phase in the container will be the sum of the partial pressures of the components of the solution. 19. The solutions which show a large positive deviation from Raoult s law form boiling azeotrope at a specific composition. 20. Some liquids on mixing, form which are binary mixtures having the same composition in liquid and vapour phase and boil at a constant temperature.

2 Work Sheet ( WS 2. 2) Topic- 2.2 Colligative Properties Name -. Class/ sec.. Roll No.. A. Fill in the blanks: 1. properties depend on the number of solute particles irrespective of their nature relative to the total number of particles present in the solution. 2. In a solution containing several non-volatile solutes, the lowering of the vapour pressure depends on the of the mole fraction of different solutes. 3. Relative lowering of vapour pressure and is to the mole fraction of the solute. 4. The boiling point of a solution is always than that of the boiling point of the pure solvent in which the solution is prepared. 5. is called Boiling Point Elevation Constant or Molal Elevation Constant or Constant. 6. The unit of Kb is. 7. The lowering of vapour pressure of a solution causes a of the freezing point compared to that of the pure solvent. 8. The freezing point of a substance may be defined as the temperature at which the vapour pressure of the substance in its liquid phase is equal to its vapour pressure in the phase. 9. Solvent molecules will flow through the membrane from pure solvent to the solution. This process of flow of the solvent is called. 10. Pressure that just the flow of solvent is called osmotic pressure of the solution. 11. Osmotic pressure is proportional to the of the solution at a given temperature T. 12. widely used to determine molar masses of proteins, polymers and other macromolecules. 13. Two solutions having same osmotic pressure at a given temperature are called solutions. 14. If the salt concentration is less than 0.9% (mass/volume), the solution is said to be. 15. When placed in water containing less than 0.9% (mass/volume) salt, blood cells collapse due to loss of water by. 16. osmosis occurs when a pressure larger than the osmotic pressure is applied to the solution. 17. A molar mass that is either lower or higher than the expected or normal value is called as molar mass. 18. The extent to which a solute is or can be expressed by van t Hoff factor. 19. factor has been defined as ratio of normal molar mass to experimentally determined molar mass. 20. Solutes which dissociate in solution exhibit molar mass than the actual molar mass.

3 Subject : Chemistry Class : XII [Special assignment-2.1] Chapter-2.Solutions 1) When is the value of Van t Hoff Factor more than one? [1 mark] 2) Why is an increase in the temperature observed on mixing chloroform with acetone? 3) How is that alcohol and water miscible in all proportions? 4) What temperature change is expected during the mixing of two liquids whose solution shows a negative deviation from Raoult s law? 5) Why is Benzene insoluble in water but soluble in toluene? 6) Define an ideal solution? 7) What do you understand by Colligative properties? 8) Give an example of a compound in which hydrogen bonding results in the formation of a dimer. 9) State any two characteristics of ideal solutions? 10) Why is vapour pressure of solution of glucose in water lower than that of water? 11) Why does the molality of a solution remain unchanged with temperature? 12) How does the molarity of a solution change with temperature? 13) How is osmotic pressure dependant upon number of mole of solute? 14) Distinguish between molarity and molality. 15) State Raoult s Law. 16) Why is osmotic pressure considered a colligative property? 17) What possible value of i will it have if solute molecules undergo association in solution. 18) Explain the term Mole Fraction. [2 marks] 19) Give one example each of miscible liquid pairs showing positive and negative deviations from Raoult s law. Give one reason each for such deviations. 20) An aqueous solution of glucose is made by dissolving 10g of glucose (C 6 H 12 O 6 ) in 90g of water at 303K. If vapour pressure of pure water at 303 K be 32.8mm Hg. What would be the vapour pressure of the solution? 21) Define the following terms: (i) Mole Fractions (ii) Ideal solution 22) Explain with suitable diagram and appropriate examples why some non ideal solutions show positive from ideal behavior. 23) What is meant by abnormal molecular mass of solute? Discuss the factors, which bring abnormality in the experimentally determined molecular masses of solutes using colligative properties. 24) What is molar concentration of solute particles in a human blood if the osmotic pressure is 7.2 atm at the body temperature of 37 C? (R= Latm K -1 mol -1 ) [0.283 mol L -1 ] 25) Vapour pressure of pure water at 35 C is mm Hg. When 27.0 g of Solute is dissolved in 100 g of water (at the same temperature) vapour pressure of the solution thus formed is mm Hg. Calculate the molecular mass of the solute. [ g mol -1 ] 26) The vapour pressure of pure liquids A and B are 70mm and 90 mm Hg respectively at 25 C. The mole fraction of A in a solution of the two is 0.3.Assuming that A and B form an ideal solution, calculate the partial pressure of each component in equilibrium with the solution. [21 mm, 63mm] 27) (i) What is osmotic pressure and how is it related with the molecular mass of Non-volatile solute? (ii) What advantages the osmotic pressure method has over elevation in boiling point method for determining molecular masses? 28) Calculate molarity and molality of a 13% solution (by weight) of sulphuric acid? Its density is g cm -3 (Atomic mass H=1,0=16, S=32 a.m.u.) [1.353 M, m] 29) With the help of a suitable diagram show that the lower vapour pressure of a solution than the pure solvent, causes a lowering of freezing point for the solution compared to that of pure solvent.

4 Subject : Chemistry Class : XII [Special assignment-2.2] Chapter-2.Solutions 1. A solution containing 2.56g of sulphur in100g of CS 2 gave a freezing point lowering of K. Calculate the molecular formula of sulphur. (K f for CS 2 in 3.83 K kg mol -1 ) At.wt. of S=32. [S 8 ] 2. Differentiate between molarity and molality of a solution. When and why is molality preferred over molarity in handling solutions in chemistry? 3. With the help of suitable diagrams, illustrate the two types of non-ideal solutions. 4. Illustrate elevation in boiling point with the help of vapour pressure-temperature curve of a solution. Show that elevation in boiling point is a colligative property. 5. Explain why freezing point of a solvent is lowered on dissolving a non- volatile solute into it? Give an important application of the phenomenon of depression in freezing point. 6. The solubility of Ba (OH) 2.8 H 2 O in water at 288 K is 5.6 g per 100 g of water. What is the molality of the hydroxide ions in saturated solution of Ba (OH) 2.8H 2 O at 288 K? (At. Mass of Ba = 137, O = 16, H = 1) [0.356 m] 7. Osmotic pressure of a solution containing 7 g of dissolved protein per 100 cm 3 of the solution is 20 mm Hg at 310 K. Calculate the molar mass of protein. (R = L atm mol -1 k -1 ) [67699 g mol -1 ] 8. Define mole fraction. A 95 mass percent aqueous solution of ethanol is further diluted with water. The mole fraction of ethanol diluted is What is the mole fraction of water in the solution? It is an ideal solution. Justify your answer. [0.75] 9. What is meant by abnormal molecular mass? Illustrate it with an example. 10. Define osmotic pressure. How does it depend upon the temperature and atmospheric pressure? 11. What is Van t Hoff factor? How does it modify the equation for elevation in boiling point? 12. Calculate the molality of KCI solution in water given that the depression in freezing point is 2K (K f for water = 1.86 K kg mol 1 ) [ m] 13. Find the molality of water solution, which freezes at K. [K f = 1.85] 14. The normal freezing point of nitrobenzene (C 6 H 5 NO 2 ) is K. A 0.25 molal solution of a certain solute in nitrobenzene causes a freezing point depression of 2 degrees. Calculate the value of K f for nitrobenzene. [8 K Kg mol 1 ] 15. The freezing point of pure nitrobenzene is K. When 2.5 g of unknown substance is dissolved in 100g of nitrobenzene, the freezing point of solution is found to be K. If the freezing point depression constant of nitrobenzene is 8.0 K kg mol -1. What is the molar mass of unknown substance? [100 g mol -1 ] 16. Define vapour pressure of a liquid. What happens to the vapour pressure when (a) volatile solute dissolves in the liquid (b) The dissolved solute is non-volatile? 17. On dissolving 3.24 g of sulphur in 40 g of benzene boiling point of solution was higher than that of benzene by 0.81 K. k b value for benzene is 2.53 K Kg mol 1. What is molecular formula of sulphur? (Atomic mass of sulphur = 32 g mol 1 ) [S 8 ] 18. The vapour pressure of pure benzene at 25 C is mm Hg and the vapour pressure of a solution of a non-volatile solute in benzene at the same temperature is mm Hg. Calculate mole fraction of solute and molality of solution. [0.0122, ] 19. Assuming complete ionization, calculate the expected freezing point of the solution prepared by dissolving 6.00 g of Glauber s salt, Na 2 SO 4 10H 2 O in 0.1 kg of H 2 0 (K f for H 2 0 = 1.86 K kg mol -1 at mass of Na = 23, S= 32, O=16, H= 1 a.m.u.) [ K] 20. An aqueous solution freezes at k, while pure water at 273 K. Determine [i] the molality of the solution [ii] Boiling point of the solution [iii] Lowering of vapour pressure of water at 298 K. (given K = 1.86 K kg mol -1, K b = K kg mol -1 and vapour pressure of pure water is mm Hg) [(i) (ii) (iii) mm]

5 Home Assignment ( HA 2. 1 ) : Topic- 2.1 Henry s & Raoult s Laws (To be done In Home Work Register) NCERT EXERCISE Question numbers 2.4, 2.5, 2.6, 2.8, 2.11, 2.15, 2.16 to Concentrated nitric acid used in laboratory work is 68% nitric acid by mass in aqueous solution. What should be the molarity of such a sample of the acid if the density of the solution is g ml 1? 2.5 A solution of glucose in water is labelled as 10% w/w, what would be the molality and mole fraction of each component in the solution? If the density of solution is 1.2 g ml 1, then what shall be the molarity of the solution? 2.6 How many ml of 0.1 M HCl are required to react completely with 1 g mixture of Na2CO3 and NaHCO3 containing equimolar amounts of both? 2.8 An antifreeze solution is prepared from g of ethylene glycol (C2H6O2) and 200 g of water. Calculate the molality of the solution. If the density of the solution is g ml 1, then what shall be the molarity of the solution? 2.11 Why do gases always tend to be less soluble in liquids as the temperature is raised? 2.15 An aqueous solution of 2% non-volatile solute exerts a pressure of bar at the normal boiling point of the solvent. What is the molar mass of the solute? 2.16 Heptane and octane form an ideal solution. At 373 K, the vapour pressures of the two liquid components are kpa and 46.8 kpa respectively. What will be the vapour pressure of a mixture of 26.0 g of heptane and 35 g of octane? 2.17 The vapour pressure of water is 12.3 kpa at 300 K. Calculate vapour pressure of 1 molal solution of a non-volatile solute in it Calculate the mass of a non-volatile solute (molar mass 40 g mol 1 ) which should be dissolved in 114 g octane to reduce its vapour pressure to 80% A solution containing 30 g of non-volatile solute exactly in 90 g of water has a vapour pressure of 2.8 kpa at 298 K. Further, 18 g of water is then added to the solution and the new vapour pressure becomes 2.9 kpa at 298 K. Calculate: (i) molar mass of the solute (ii) vapour pressure of water at 298 K.

6 (To be done In Home Work Register) Home Assignment ( HA 2. 2 ) : Topic- 2.2 Colligative Properties NCERT EXERCISE Question number 2.20, 2.21, 2.22, 2.27, 2.31 to 2.33 & A 5% solution (by mass) of cane sugar in water has freezing point of 271K. Calculate the freezing point of 5% glucose in water if freezing point of pure water is K Two elements A and B form compounds having formula AB2 and AB4. When dissolved in 20 g of benzene (C6H6), 1 g of AB2 lowers the freezing point by 2.3 K whereas 1.0 g of AB4 lowers it by 1.3 K. The molar depression constant for benzene is 5.1 K kg mol 1. Calculate atomic masses of A and B At 300 K, 36 g of glucose present in a litre of its solution has an osmotic pressure of 4.98 bar. If the osmotic pressure of the solution is 1.52 bars at the same temperature, what would be its concentration? 2.27 If the solubility product of CuS is , calculate the maximum molarity of CuS in aqueous solution The depression in freezing point of water observed for the same amount of acetic acid, trichloroacetic acid and trifluoroacetic acid increases in the order given above. Explain briefly Calculate the depression in the freezing point of water when 10 g of CH3CH2CHClCOOH is added to 250 g of water. Ka = , Kf = 1.86 K kg mol g of CH2FCOOH is dissolved in 500 g of water. The depression in the freezing point of water observed is C. Calculate the van t Hoff factor and dissociation constant of fluoroacetic acid g of liquid A (molar mass 140 g mol 1 ) was dissolved in 1000 g of liquid B (molar mass 180 g mol 1 ). The vapour pressure of pure liquid B was found to be 500 torr. Calculate the vapour pressure of pure liquid A and its vapour pressure in the solution if the total vapour pressure of the solution is 475 Torr.

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