Unit

2

solutions

I. Multiple Choice Questions (Type-I)

1. Which of the following units is useful in relating concentration of solution with its vapour pressure?

(i) mole fraction

(ii) parts per million

(iii) mass percentage

(iv) molality

2. On dissolving sugar in water at room temperature solution feels cool to touch. Under which of the following cases dissolution of sugar will be most rapid?

(i) Sugar crystals in cold water.

(ii) Sugar crystals in hot water.

(iii) Powdered sugar in cold water.

(iv) Powdered sugar in hot water.

3. At equilibrium the rate of dissolution of a solid solute in a volatile liquid solvent is

(i) less than the rate of crystallisation

(ii) greater than the rate of crystallisation

(iii) equal to the rate of crystallisation

(iv) zero

4. A beaker contains a solution of substance ’ $A$ ‘. Precipitation of substance ’ $A$ ’ takes place when small amount of ’ $A$ ’ is added to the solution. The solution is

(i) saturated

(ii) supersaturated

(iii) unsaturated

(iv) concentrated

5. Maximum amount of a solid solute that can be dissolved in a specified amount of a given liquid solvent does not depend upon _______.

(i) Temperature

(ii) Nature of solute

(iii) Pressure

(iv) Nature of solvent

6. Low concentration of oxygen in the blood and tissues of people living at high altitude is due to _______.

(i) low temperature

(ii) low atmospheric pressure

(iii) high atmospheric pressure

(iv) both low temperature and high atmospheric pressure

7. Considering the formation, breaking and strength of hydrogen bond, predict which of the following mixtures will show a positive deviation from Raoult’s law?

(i) Methanol and acetone.

(ii) Chloroform and acetone.

(iii) Nitric acid and water.

(iv) Phenol and aniline.

8. Colligative properties depend on _______.

(i) the nature of the solute particles dissolved in solution.

(ii) the number of solute particles in solution.

(iii) the physical properties of the solute particles dissolved in solution.

(iv) the nature of solvent particles.

9. Which of the following aqueous solutions should have the highest boiling point?

(i) $1.0 M NaOH$

(ii) $1.0 M Na_2 SO_4$

(iii) $1.0 M NH_4 NO_3$

(iv) $1.0 M KNO_3$

10. The unit of ebulioscopic constant is _______.

(i) $K kg mol^{-1}$ or $K$ (molality) ${ }^{-1}$

(ii) $mol kg K^{-1}$ or $K^{-1}$ (molality)

(iii) $kg mol^{-1} K^{-1}$ or $K^{-1}$ (molality) ${ }^{-1}$

(iv) $K mol kg^{-1}$ or $K$ (molality)

11. In comparison to a $0.01 M$ solution of glucose, the depression in freezing point of a $0.01 M MgCl_2$ solution is

(i) the same

(ii) about twice

(iii) about three times

(iv) about six times

12. An unripe mango placed in a concentrated salt solution to prepare pickle, shrivels because _______.

(i) it gains water due to osmosis.

(ii) it loses water due to reverse osmosis.

(iii) it gains water due to reverse osmosis.

(iv) it loses water due to osmosis.

13. At a given temperature, osmotic pressure of a concentrated solution of a substance _______.

(i) is higher than that at a dilute solution.

(ii) is lower than that of a dilute solution.

(iii) is same as that of a dilute solution.

(iv) cannot be compared with osmotic pressure of dilute solution.

14. Which of the following statements is false?

(i) Two different solutions of sucrose of same molality prepared in different solvents will have the same depression in freezing point.

(ii) The osmotic pressure of a solution is given by the equation $\Pi=C R T$ ( where $C$ is the molarity of the solution).

(iii) Decreasing order of osmotic pressure for $0.01 M$ aqueous solutions of barium chloride, potassium chloride, acetic acid and sucrose is

$BaCl_2>KCl>CH_3 COOH>$ sucrose.

(iv) According to Raoult’s law, the vapour pressure exerted by a volatile component of a solution is directly proportional to its mole fraction in the solution.

15. The values of Van’t Hoff factors for $KCl, NaCl$ and $K_2 SO_4$, respectively, are _______.

(i) 2, 2 and 2

(ii) 2, 2 and 3

(iii) 1, 1 and 2

(iv) 1,1 and 1

16. Which of the following statements is false?

(i) Units of atmospheric pressure and osmotic pressure are the same.

(ii) In reverse osmosis, solvent molecules move through a semipermeable membrane from a region of lower concentration of solute to a region of higher concentration.

(iii) The value of molal depression constant depends on nature of solvent.

(iv) Relative lowering of vapour pressure, is a dimensionless quantity.

17. Value of Henry’s constant $K_{H}$ _______.

(i) increases with increase in temperature.

(ii) decreases with increase in temperature.

(iii) remains constant.

(iv) first increases then decreases.

18. The value of Henry’s constant $K_{H}$ is _______.

(i) greater for gases with higher solubility.

(ii) greater for gases with lower solubility.

(iii) constant for all gases.

(iv) not related to the solubility of gases.

19. Consider the Fig. 2.1 and mark the correct option.

(i) water will move from side (A) to side (B) if a pressure lower than osmotic pressure is applied on piston (B).

(ii) water will move from side (B) to side (A) if a pressure greater than osmotic pressure is applied on piston (B).

(iii) water will move from side (B) to side (A) if a pressure equal to osmotic pressure is applied on piston (B).

(iv) water will move from side (A) to side (B) if pressure equal to osmotic pressure is applied on piston (A).

Fig. 2.1

20. We have three aqueous solutions of $NaCl$ labelled as ‘A’, ‘B’ and ’ $C$ ’ with concentrations $0.1 M, 0.01 M$ and $0.001 M$, respectively. The value of van’t Hoff factor for these solutions will be in the order _______.

(i) $i_{A}<i_{B}<i_{C}$

(ii) $i_{A}>i_{B}>i_{C}$

(iii) $i_{A}=i_{B}=i_{C}$

(iv) $i_{A}<i_{B}>i_{C}$

21. On the basis of information given below mark the correct option.

Information:

(A) In bromoethane and chloroethane mixture intermolecular interactions of A-A and B-B type are nearly same as A-B type interactions.

(B) In ethanol and acetone mixture $A-A$ or $B-B$ type intermolecular interactions are stronger than $A-B$ type interactions.

(C) In chloroform and acetone mixture A-A or B-B type intermolecular interactions are weaker than $A-B$ type interactions.

(i) Solution (B) and (C) will follow Raoult’s law.

(ii) Solution (A) will follow Raoult’s law.

(iii) Solution (B) will show negative deviation from Raoult’s law.

(iv) Solution (C) will show positive deviation from Raoult’s law.

22. Two beakers of capacity $500 mL$ were taken. One of these beakers, labelled as “A”, was filled with $400 mL$ water whereas the beaker labelled " $B$ " was filled with $400 mL$ of $2 M$ solution of $NaCl$. At the same temperature both the beakers were placed in closed containers of same material and same capacity as shown in Fig. 2.2.

Fig. 2.2

At a given temperature, which of the following statement is correct about the vapour pressure of pure water and that of $NaCl$ solution.

(i) vapour pressure in container (A) is more than that in container (B).

(ii) vapour pressure in container (A) is less than that in container (B).

(iii) vapour pressure is equal in both the containers.

(iv) vapour pressure in container (B) is twice the vapour pressure in container (A).

23. If two liquids $A$ and $B$ form minimum boiling azeotrope at some specific composition then _______.

(i) A-B interactions are stronger than those between $A-A$ or $B-B$.

(ii) vapour pressure of solution increases because more number of molecules of liquids A and B can escape from the solution.

(iii) vapour pressure of solution decreases because less number of molecules of only one of the liquids escape from the solution.

(iv) A-B interactions are weaker than those between $A-A$ or $B-B$.

24. $4 L$ of $0.02 M$ aqueous solution of $NaCl$ was diluted by adding one litre of water. The molality of the resultant solution is _______.

(i) 0.004

(ii) 0.008

(iii) 0.012

(iv) 0.016

25. On the basis of information given below mark the correct option.

Information : On adding acetone to methanol some of the hydrogen bonds between methanol molecules break.

(i) At specific composition methanol-acetone mixture will form minimum boiling azeotrope and will show positive deviation from Raoult’s law.

(ii) At specific composition methanol-acetone mixture forms maximum boiling azeotrope and will show positive deviation from Raoult’s law.

(iii) At specific composition methanol-acetone mixture will form minimum boiling azeotrope and will show negative deviation from Raoult’s law.

(iv) At specific composition methanol-acetone mixture will form maximum boiling azeotrope and will show negative deviation from Raoult’s law.

26. $K_{H}$ value for $Ar(g), CO_2(g), HCHO(g)$ and $CH_4(g)$ are $40.39,1.67,1.83 \times 10^{-5}$ and 0.413 respectively.

Arrange these gases in the order of their increasing solubility.

(i) $HCHO<CH_4<CO_2<Ar$

(ii) $HCHO<CO_2<CH_4<Ar$

(iii) $Ar<CO_2<CH_4<HCHO$

(iv) $Ar<CH_4<CO_2<HCHO$

II. Multiple Choice Questions (Type-II)

Note : In the following questions two or more options may be correct.

27. Which of the following factor (s) affect the solubility of a gaseous solute in the fixed volume of liquid solvent?

(a) nature of solute

(b) temperature

(c) pressure

(i) (a) and (c) at constant $T$

(ii) (a) and (b) at constant $P$

(iii) (b) and (c) only

(iv) (c) only

28. Intermolecular forces between two benzene molecules are nearly of same strength as those between two toluene molecules. For a mixture of benzene and toluene, which of the following are not true?

(i) $\Delta_{\text {mix }} H=$ zero

(ii) $\Delta_{\text {mix }} V=$ zero

(iii) These will form minimum boiling azeotrope.

(iv) These will not form ideal solution.

29. Relative lowering of vapour pressure is a colligative property because _______.

(i) It depends on the concentration of a non electrolyte solute in solution and does not depend on the nature of the solute molecules.

(ii) It depends on number of particles of electrolyte solute in solution and does not depend on the nature of the solute particles.

(iii) It depends on the concentration of a non electrolyte solute in solution as well as on the nature of the solute molecules.

(iv) It depends on the concentration of an electrolyte or nonelectrolyte solute in solution as well as on the nature of solute molecules.

30. Van’t Hoff factor $i$ is given by the expression _______.

(i) $\quad i=\frac{\text { Normal molar mass }}{\text { Abnormal molar mass }}$

(ii) $\quad i=\frac{\text { Abnormal molar mass }}{\text { Normal molar mass }}$

(iii) $\quad i=\frac{\text { Observed colligative property }}{\text { Calculated colligative property }}$

(iv) $\quad i=\frac{\text { Calculated colligative property }}{\text { Observed colligative property }}$

31. Isotonic solutions must have the same _______.

(i) solute

(ii) density

(iii) elevation in boiling point

(iv) depression in freezing point

32. Which of the following binary mixtures will have same composition in liquid and vapour phase?

(i) Benzene - Toluene

(ii) Water-Nitric acid

(iii) Water-Ethanol

(iv) $n$-Hexane - $n$-Heptane

33. In isotonic solutions _______.

(i) solute and solvent both are same. (ii) osmotic pressure is same.

(iii) solute and solvent may or may not be same.

(iv) solute is always same solvent may be different.

34. For a binary ideal liquid solution, the variation in total vapour pressure versus composition of solution is given by which of the curves?

(i)

(iii)

(ii)

(iv)

35. Colligative properties are observed when

(i) a non volatile solid is dissolved in a volatile liquid.

(ii) a non volatile liquid is dissolved in another volatile liquid.

(iii) a gas is dissolved in non volatile liquid.

(iv) a volatile liquid is dissolved in another volatile liquid.

III. Short Answer Type

36. Components of a binary mixture of two liquids A and B were being separated by distillation. After some time separation of components stopped and composition of vapour phase became same as that of liquid phase. Both the components started coming in the distillate. Explain why this happened.

37. Explain why on addition of $1 mol$ of $NaCl$ to 1 litre of water, the boiling point of water increases, while addition of $1 mol$ of methyl alcohol to one litre of water decreases its boiling point.

38. Explain the solubility rule “like dissolves like” in terms of intermolecular forces that exist in solutions.

39. Concentration terms such as mass percentage, ppm, mole fraction and molality are independent of temperature, however molarity is a function of temperature. Explain.

40. What is the significance of Henry’s Law constant $K_{H}$ ?

41. Why are aquatic species more comfortable in cold water in comparison to warm water?

42. (a) Explain the following phenomena with the help of Henry’s law.

(i) Painful condition known as bends.

(ii) Feeling of weakness and discomfort in breathing at high altitude.

(b) Why soda water bottle kept at room temperature fizzes on opening?

43. Why is the vapour pressure of an aqueous solution of glucose lower than that of water?

44. How does sprinkling of salt help in clearing the snow covered roads in hilly areas? Explain the phenomenon involved in the process.

45. What is “semi permeable membrane”?

46. Give an example of a material used for making semipermeable membrane for carrying out reverse osmosis.

IV. Matching Type

Note : In the following questions match the items given in Column I and Column II.

47. Match the items given in Column I and Column II.

Column I

(i) Saturated solution

(ii) Binary solution

(iii) Isotonic solution

(iv) Hypotonic solution

(v) Solid solution

(vi) Hypertonic solution

Column II

(a) Solution having same osmotic pressure at a given temperature as that of given solution.

(b) A solution whose osmotic pressure is less than that of another.

(c) Solution with two components.

(d) A solution which contains maximum amount of solute that can be dissolved in a given amount of solvent at a given temperature.

(e) A solution whose osmotic pressure is more than that of another.

(f) A solution in solid phase.

48. Match the items given in Column I with the type of solutions given in Column II.

Column I

(i) Soda water

(ii) Sugar solution

(iii) German silver

(iv) Air

(v) Hydrogen gas in palladium

Column II

(a) A solution of gas in solid

(b) A solution of gas in gas

(c) A solution of solid in liquid

(d) A solution of solid in solid

(e) A solution of gas in liquid

(f) A solution of liquid in solid

49. Match the laws given in Column I with expresions given in Column II.

Column I

(i) Raoult’s law

(ii) Henry’s law

(iii) Elevation of boiling point

(iv) Depression in freezing point

(v) Osmotic pressure

Column II

(a) $\Delta T_{f}=Km_{f}$

(b) $\Pi=C R T$

(c) $\quad p=x_1 p_1^{0}+x_2 p_2^{0}$

(d) $\Delta T_{b}=K_{b} m$

(e) $p=K_{H} \cdot x$

50. Match the terms given in Column I with expressions given in Column II.

Column I

(i) Mass percentage

(ii) Volume percentage

(iii) Mole fraction

(iv) Molality

(v) Molarity

Column II

(a) $\frac{\text{Number of moles of the solute component}}{\text{Volume of solution in litres }} $

(b) $\frac{\text { Number of moles of a component }}{\text { Total number of moles of all the components }}$

(c) $\frac{\text { Volume of the solute component in solution}}{\text { Total volume of solution }}$ x 100

(d) $\frac{\text { Mass of the solute component in solution}}{\text { Total mass of the solution }}$ x 100

(e) $\frac{\text { Number of moles of the solute components}}{\text { Mass of solvent in kilograms }}$

V. Assertion and Reason Type

Note : In the following questions a statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices.

(i) Assertion and reason both are correct statements and reason is correct explanation for assertion.

(ii) Assertion and reason both are correct statements but reason is not correct explanation for assertion.

(iii) Assertion is correct statement but reason is wrong statement.

(iv) Assertion and reason both are incorrect statements.

(v) Assertion is wrong statement but reason is correct statement.

51. Assertion : Molarity of a solution in liquid state changes with temperature.

Reason : The volume of a solution changes with change in temperature.

52. Assertion : When methyl alcohol is added to water, boiling point of water increases.

Reason : When a volatile solute is added to a volatile solvent elevation in boiling point is observed.

53. Assertion : When $NaCl$ is added to water a depression in freezing point is observed.

Reason : The lowering of vapour pressure of a solution causes depression in the freezing point.

54. Assertion : When a solution is separated from the pure solvent by a semipermeable membrane, the solvent molecules pass through it from pure solvent side to the solution side.

Reason : Diffusion of solvent occurs from a region of high concentration solution to a region of low concentration solution.

VI. Long Answer Type

55. Define the following modes of expressing the concentration of a solution. Which of these modes are independent of temperature and why?

(i) $\quad w / w$ (mass percentage)

(ii) $\quad V / V$ (volume percentage)

(iii) w/V (mass by volume percentage)

(iv) ppm. (parts per million) (v) $x$ (mole fraction)

(vi) M (Molarity)

(vii) m (Molality)

56. Using Raoult’s law explain how the total vapour pressure over the solution is related to mole fraction of components in the following solutions.

(i) $CHCl_3(l)$ and $CH_2 Cl_2(l)$

(ii) $\quad NaCl(s)$ and $H_2 O(l)$

57. Explain the terms ideal and non-ideal solutions in the light of forces of interactions operating between molecules in liquid solutions.

58. Why is it not possible to obtain pure ethanol by fractional distillation? What general name is given to binary mixtures which show deviation from Raoult’s law and whose components cannot be separated by fractional distillation. How many types of such mixtures are there?

59. When kept in water, raisin swells in size. Name and explain the phenomenon involved with the help of a diagram. Give three applications of the phenomenon.

60. Discuss biological and industrial importance of osmosis.

61. How can you remove the hard calcium carbonate layer of the egg without damaging its semiprermiable membrane? Can this egg be inserted into a bottle with a narrow neck without distorting its shape? Explain the process involved.

62. Why is the mass determined by measuring a colligative property in case of some solutes abnormal? Discuss it with the help of Van’t Hoff factor.

ANSWERS

I. Multiple Choice Questions (Type-I)

1. (i)

2. (iv)

3. (iii)

4. (ii), [Hint : If added substance dissolves, the solution is unsaturated. If it does not dissolve solution is saturated. If precipitation occurs solution is supersaturated.]

5. (iii)

6. (ii), [Hint : Body temperature of human beings remains constant.]

7. (i)

8. (ii)

9. (ii)

10. (i)

11. (iii)

12. (iv)

13. (i)

14. (i)

15. (ii)

16. (ii)

17. (i)

18. (ii)

19. (ii)

20. (iii)

21. (ii)

22. (i)

23. (i)

24. (iv)

25. (ii)

26. (iii)

II. Multiple Choice Guestions (Type-II)

III. Short Answer Type

36. Since both the components are appearing in the distillate and composition of liquid and vapour is same, this shows that liquids have formed azeotropic mixture and hence cannot be separated at this stage by distillation.

37. $NaCl$ is a non volatile solute, therefore, addition of $NaCl$ to water lowers the vapour pressure of water. As a result boiling point of water increases. Methyl alcohol on the other hand is more volatile than water, therefore its addition increases, the total vapour pressure over the solution and a decrease in boiling point of water results.

38. A substance (solute) dissolves in a solvent if intermolecular interactions are similar in both the components; for example, polar solutes dissolve in polar solvents and non polar solutes in non polar solvents thus we can say “like dissolves like”.

39. Molarity of a solution is defined as the number of moles of solute dissolved in one litre of solution. Since volume depends on temperature and undergoes a change with change in temperature, the molarity will also change with change in temperature. On the other hand, mass does not change with change in temperature, as a result other concentration terms given in the question remain unchanged by changing temperature. According to the definition of all these terms, mass of the solvent used for making the solution is related to the mass of solute.

40. Higher the value of Henry’s law constant $K_{H}$, the lower is the solubility of the gas in the liquid.

41. At a given pressure the solubility of oxygen in water increases with decrease in temperature. Presence of more oxygen at lower temperature makes the aquatic species more comfortable in cold water.

42. Refer to the NCERT textbook for Class XII.

43. In pure liquid water the entire surface of liquid is occupied by the molecules of water. When a non volatile solute, for example glucose is dissolved in water, the fraction of surface covered by the solvent molecules gets reduced because some positions are occupied by glucose molecules. As a result number of solvent molecules escaping from the surface also gets reduced, consequently the vapour pressure of aqueous solution of glucose is reduced.

44. When salt is spread over snow covered roads, snow starts melting from the surface because of the depression in freezing point of water and it helps in clearing the roads.

45. Continuous sheets or films (natural or synthetic) which contain a network of submicroscopic holes or pores through which small solvent molecules like water can pass; but the passage of bigger molecules of solute is hindered, are known as semi permeable membrane.

46. Cellulose acetate.

IV. Matching Type

47. $\quad$ (i) $\rightarrow$ (d)

(ii) $\rightarrow$ (c)

(iii) $\rightarrow$ (a)

(iv) $\rightarrow$ (b)

$(v) \rightarrow(f)$

(vi) $\rightarrow$ (e)

48. $\quad$ (i) $\rightarrow(e)$

(ii) $\rightarrow$ (c)

(iii) $\rightarrow$ (d)

(iv) $\rightarrow$ (b)

(v) $\rightarrow$ (a)

49. (i) $\rightarrow$ (c)

(ii) $\rightarrow$ (e)

(iii) $\rightarrow$ (d)

(iv) $\rightarrow$ (a)

(v) $\rightarrow$ (b)

(i) $\rightarrow$ (d)

(ii) $\rightarrow$ (c)

(iii) $\rightarrow$ (b)

(iv) $\rightarrow$ (e)

(v) $\rightarrow$ (a)

V. Assertion and Reason Type

51. (i)

52. (iv)

53. (i)

54. (ii)

VI. Long Answer Type

55. Refer to NCERT textbook for Class XII.

56. Hint : Discuss the following formulas

(i) for a binary solution having both components as volatile liquids, the total pressure will be

$ \begin{aligned} p & =p_1=x_1 p_1^{0}+x_2 p_2^{0} \\ & =x_1 p_1^{0}+(1-x_1) p_2^{0} \\ & =(p_1^{0}-p_2^{0}) x_1+p_2^{0} \\ p & =\text { total vapour pressure } \\ p_1 & =\text { partial vapour pressure of component } 1 \\ p_2 & =\text { partial vapour pressure of component } 2 . \end{aligned} $

(ii) For a solution containing non-volatile solute, the Raoult’s law is applicable only to vaporisable component (1) and total vapour pressure is written as

$ p=p_1=x_1 p_1^{0} $

57. Refer to page 45 of NCERT textbook for Class XII.

58. See page 46 of NCERT textbook for Class XII.

59. [Hint : Explain it with the help of a diagram (Fig. 2.3) illustrating the osmosis of water into raisin.]

60. Hint : The process of osmosis is of immense biological and industrial importance as is evident from the following examples :

(i) Movement of water from soil into plant roots and subsequently into upper portion of the plant is partly due to

Fig. 2.3

(ii) Preservation of meat against bacterial action by adding salt.

(iii) Preservation of fruits against bacterial action by adding sugar. Bacterium in canned fruit loses water through the process of osmosis, shrivels and dies.

(iv) Reverse osmosis is used for desalination of water.

61. Hint :

62. Certain compounds when dissolved in suitable solvents either dissociate or associate.

For example ethanoic acid dimerises in benzene due to hydrogen bonding, while in water, it dissociates and forms ions. As a result the number of chemical species in solution increases or decreases as compared to the number of chemical species of solute added to form the solution. Since the magnitude of colligative property depends on the number of solute particles, it is expected that the molar mass determined on the basis of colligative properties will be either higher or lower than the expected value or the normal value and is called abnormal molar mass.

In order to account for the extent of dissociation or association of molecules in solution, Van’t Hoff introduced a factor, $i$, known as the Van’t Hoff factor. It can be defined as follows.

$ \begin{aligned} i & =\frac{\text { Expected molar mass }}{\text { Abnormal molar mass }} \\ & =\frac{\text { Observed colligative property }}{\text { Calculated colligative property }} \\ & =\frac{\text { Total number of moles of particles after association/dissociation }}{\text { Number of moles of particles before association/dissociation }} \end{aligned} $