1. A molal solution is one that contains one mole of solute in

(a) one litre of the solvent

(b) 1000 g of the solvent

(c) one litre of the solution

(d) 22.4 litres of solution.

2. Which of the following is independent of temperature?

(a) normality

(b) molarity

(c) molality

(d) formality

3. When \(\mathrm{NaCl}\) is added to water.

(a) freezing point is raised

(b) boiling point is depressed

(c) freezing point does not change

(d) boiling point is raised

4. Which of the following 0.1 \(\mathrm{M}\) aqueous solutions will exert highest osmotic pressure?

(a) \(\mathrm{NaCl}\)

(b) \(\mathrm{BaCl}_2\)

(c) \(\mathrm{MgSO}_4\)

(d) \(\mathrm{Al}\left(\mathrm{SO}_4\right)_3\)

5. According to the Raoult's law, the relative lowering of vapor pressure is equal to the

(a) mole fraction of solvent

(b) mole fraction of solute

(c) independent of mole fraction of solute

(d) molality of solution

6. Partial pressure of solvent in solution of nonvolatile solute is given by equation,

(a) \(\mathrm{p}=\mathrm{x}_2 \mathrm{P}^0\)

(b) \(\mathrm{p}^6=x p\)

(c) \(p=X_1 P^0\)

(d) \(\mathrm{P}^6=\mathrm{x}_1 \mathrm{P}\)

7. When partial pressure of solvent in solution of non-volatile solute is plotted against its mole fraction, nature of graph is

(a) a straight line passing through origin

(b) a straight line parallel to mole fraction of solvent

(c) a straight line parallel to vapor pressure of solvent

(d) a straight line intersecting vapor pressure axis.

8. Lowering of vapor pressure of solution

(a) is a property of solute

(b) is a property of solute as well as solvent

(c) is a property of solvent

(d) is a colligative property

9. Molal elevation constant is elevation in ceiling point produced by

(a) \(1 \mathrm{~g}\) of solute in \(100 \mathrm{~g}\) of solvent

(b) \(100 \mathrm{~g}\) of solute in \(1000 \mathrm{~g}\) of solvent

(c) 1 mole of solute in one litre of solvent

(d) 1 mole of solute in one \(\mathrm{kg}\) of solvent

10. The determination of molar mass from elevation in boiling point is called as

(a) cryoscopy

(b) osmometry

(c) ebullioscopy

(d) spectroscopy

11. Vapour pressure of solution of a non volatile solute is alvays

(a) equal to the vapour pressure of pure solvent

(b) higher than vapour pressure of pare solvent

(c) lower than vapour pressure of pure solvent

(d) constant

12. In osmasis

(a) solvent molecules pass from high

concentration of solute to low concentration.

(b) solvent molecules pass from a solution of low concentration of solute to a solution of high concentration of solute.

(c) solute molecules pass from low concentration to high concentration

(d) solute molecules pass from high concentration to low concentration.

13. The two solutions with same atmotic pressure are called

(a) isotonic

(b) isomeric

(c) hypotonic

(d) hypertonic

14. The values of gas constant and solution constant

(a) are different

(b) almost identical

(c) gas constant is greater than solution constant

(d) gas constant is smaller than solution constant

15. Abnormal molar mass is produced by

(a) association of solute

(b) dissociation of solute

(c) both association and dissociation of solute

(d) separation by semipermeable membrane

16. \(20 \mathrm{~g}\) of \(\mathrm{NaOH}\) (Molar mass \(=40 \mathrm{~g} \mathrm{~mol}^{-1}\) ) is dissolved in \(500 \mathrm{~cm}\) ? of water. Molality of resulting solution is

(a) \(0.1 \mathrm{~m}\)

(b) \(0.5 \mathrm{~m}\)

(c) \(1.5 \mathrm{~m}\)

(d) \(1.0 \mathrm{~m}\)

17. Molarity of solution depends on

(a) temperature

(b) nature of solute dissolved

(c) mass of solvent

(d) pressure

18. Which of the following aqueous solutions will have minimum elevation in boiling point?

(a) \(0.1 \mathrm{M} \mathrm{KCl}\)

(b) \(0.05 \mathrm{M} \mathrm{NaCl}\)

(c) \(1 \mathrm{MAIPO}_4\)

(d) \(0.1 \mathrm{M} \mathrm{MgSO}_4\)

19. Which of the following will have maximum depression in freezing point?

(a) \(0.5 \mathrm{M} \mathrm{Li}_2 \mathrm{SO}_4\)

(b) \(1 \mathrm{M} \mathrm{KCl}\)

(c) \(0.5 \mathrm{MAD2}\left(\mathrm{SO}_4\right)_3\)

(d) \(0.5 \mathrm{M} \mathrm{BaCl}_2\)

20. Relative vapour pressure lowering depends only on

(a) Mole fraction of solute

(b) Nature of solvent

(c) Nature of solute

(d) Nature of solute and solvent

21. If mass is expressed in gram then \(K_b\) is given by

(a) \(\frac{\mathrm{M}_2 \Delta \mathrm{T}_{\mathrm{b}} \times \mathrm{W}_2}{1000 \times \mathrm{W}_1}\)

(b) \(\frac{\mathrm{W}}{\Delta \mathrm{T}_{\mathrm{i}} \times \mathrm{W}_1 \times \mathrm{M}_2} \times 1000\)

(c) \(\frac{\mathrm{M}_2 \Delta \mathrm{T}_{\mathrm{b}} \times \mathrm{W}_1}{1000 \times \mathrm{W}_2}\)

(d) \(\frac{\mathrm{W}_2}{\mathrm{ST}_{\mathrm{b}} \times \mathrm{W}_2 \times \mathrm{M}_2} \times 1000\)

22. A solution is

(a) a mixture of two components

(b) a compound of two components

(c) a homogeneous mixture of two components

(d) all the above

23. A solution is \(0.25 \%\) by weight. The weight of solvent containing \(1.25 \mathrm{~g}\) - of solute would be

(a) \(500 \mathrm{~g}\).

(b) \(498.75 \mathrm{~g}\).

(c) \(50025 \mathrm{~g}\)

(d) \(501.25 \mathrm{~g}\).

24. Equal volumes of a \(10 \%\) solution (by weight of the solute \(\mathrm{A}\) and \(15 \%\) solution (by weight) of the solute \(B\) are mixed. The weight percent of \(A\) and \(B\) in the mixture would be respectively

(a) 5 and 7.5

(b) 10 and 15

(c) 15 and 10

(d) 20 and 30

25. \(1 \mathrm{dm}^3\) of water contains \(90 \mathrm{~g}\). of glucose. The mole fraction of glucose in the solution is

(a) 0.33

(b) 0.66

(c) \(0.5 / 56.05\)

(d) \(0.5 / 55.55\)

26. Two solutions \(A\) and \(B\) have same mole fractions of the solute. If \(1 \mathrm{dm}^3\) of \(\mathrm{A}\) is mixed with \(2 \mathrm{dm}^3\) of \(\mathrm{B}\), the mole fraction of the solute in the mixture would

(a) decrease

(b) increase

(c) remain unchanged

(d) change unpredictably

27. Which one of the following statements is true for a solution?

(a) Normality is always equal to molarity

(b) Normality is always less than molarity

(c) Molarity is always less than normality

(d) Molarity is either equal to or less than normality

28. For a solution of tartaric acid (HOOC.CHOH.CHOH.COOH) the molarity (M) and normality ( \(\mathrm{N})\) are related as

(a) \(\mathrm{N}=\mathrm{M} / 2\)

(b) \(2 \mathrm{M}=\mathrm{N}\)

(c) \(\mathrm{M}=\mathrm{N}\)

(d) \(\mathrm{M}>\mathrm{N}\)

29. Which one of the following is a colligative property?

(a) Boiling point

(b) Freezing point

(c) Vapour pressure

(d) Lowering of vapour pressure

30. For a solution, Vapour pressure of solution = Partial vapour pressure of solvent. This means that

(a) the solution is dilute

(b) the solute is non-volatile

(c) the solvent is volatile

(d) the solution is at room temperature

31. The plot of partial vapour pressure of solvent versus its mole fraction in the solution, at a constant temperature is

(a) a straight line

(b) a straight line parallel to one axis

(c) a straight line passing through the origin

(d) none of the above

32. The vapour pressures of pure solvent and solution are \(120 \mathrm{~mm} \mathrm{Hg}\) and \(108 \mathrm{~mm} \mathrm{Hg}\) respectively. The mole fraction of the solvent in the solution is

(a) 0.1

(b) 0.9

(c) \(120 / 108\)

(d) 1.08

33. In Ostwald and Walker's method for determining the lowering of vapour pressure, the loss in mass of solvent bulbs in \(\mathbf{5 0}\) times less than the gain in mass of \(\mathrm{CaCl}_2\) tubes. The vapour pressure of the solution would be (Given V.P. of pure solvent \(=100 \mathrm{~mm} \mathrm{Hg}\) )

(a) \(2 \mathrm{~mm} \mathrm{Hg}\)

(b) \(0.5 \mathrm{~mm} \mathrm{Hg}\)

(c) \(98 \mathrm{~mm} \mathrm{Hg}\)

(d) \(100 \mathrm{~mm} \mathrm{Hg}\)

34. Boiling point of a liquid under given conditions is the temperature at which its vapour pressure

(a) is equal to \(760 \mathrm{~mm} \mathrm{Hg}\)

(b) is equal to atmospheric pressure

(c) is equal to \(1 \mathrm{~atm}\).

(d) changes very rapidly

35. The elevation of boiling point is directly proportional to

(a) molality of the solution

(b) depression of freezing point in the same solution

(c) both these

(d) none of these

36. Which one of the following aqueous solutions will have the highest boiling point?

(a) \(0.1 \mathrm{M}\) urea

(b) \(30 \mathrm{~g}\). of glucose per \(\mathrm{dm}^3\)

(c) \(3.42 \mathrm{~g}\). of sucrose in \(100 \mathrm{ml}\)

(d) \(0.2 \mathrm{M}\) glucose

37. Which one of the following aqueous solutions will have same boiling point as that of \(0.2 \mathrm{M}\) aqueous solution of fructose?

(a) \(34.2 \mathrm{~g}\) sucrose per \(\mathrm{dm}^3\)

(b) \(36 \mathrm{~g}\). glucose in \(500 \mathrm{~cm}^3\)

(c) \(180 \mathrm{~g}\). glucose in \(10 \mathrm{dm}^3\)

(d) \(12 \mathrm{~g}\). urea per \(\mathrm{dm}^3\)

38. To determine the elevation of boiling point more accurately, the solvent used should have

(a) higher value of \(K_b\)

(b) lower value of \(\mathrm{K}_{\mathrm{b}}\)

(c) high mol, mass

(d) low mol. mass

39. Some statements are given below about depression of freezing point in a solution

(A) It is directly proportional to lowering of vapour pressure

(B) It is directly proportional to relative lowering of vapour pressure

(C) It is independent of the molarity of the solution

(D) It is directly proportional to the elevation of boiling point in the same solution

Among the above, the correct statements are

(a) only \(A\) and \(D\)

(b) A, C and D

(c) A, B and D

(d) all

40. The scale of the Beckmann's thermometer is only of \(5^{\circ}-6^{\circ} \mathrm{C}\) but the thermometer can be used over a wide range of temperature. This is due to

(a) its large length

(b) bigger size of the bulb

(c) large amount of mercury present

(d) the facility of adjusting the quantity of mercury in the bulb as per requirement

41. The values of \(K_t\) for solvents \(A, B, C\) and \(D\) are \(1.86,1.99,5.12\) and \(4.7 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\) respectively. The equimolal solutions of a solute in these solvents will have the freezing points in order of solvent as

(a) \(\mathrm{C}>\mathrm{D}>\mathrm{B}>\mathrm{A}\)

(b) A \(>\) C \(>\) D \(>\) B

(c) \(\mathrm{A}>\mathrm{B}>\mathrm{D}>\mathrm{C}\)

(d) \(\mathrm{C}>\mathrm{B}>\mathrm{A}>\mathrm{D}\)

42. Osmotic pressure is defined as

(a) the excess pressure which must be applied to a solution to stop osmosis

(b) the excess pressure which must be applied to a solution to increase its vapour pressure till it becomes equal to the vapour pressure of pure solvent

(c) the decrease in pressure on the pure solvent to decrease its vapour pressure till it becomes equal to the vapour pressure of solution

(d) all the above

43. The Van't Hoff factor for \(0.1 \mathrm{M} \mathrm{Ba}\left(\mathrm{NO}_3\right)_2\) solution is 2.74. The degree of dissociation is

(a) \(91.3 \%\)

(b) \(87 \%\)

(c) \(100 \%\)

(d) \(74 \%\)

44. A \(0.2 \mathrm{M}\) solution of a solute is isotonic with a solution containing

(a) 3.42 g. of sucrose in \(100 \mathrm{~cm}^3\)

(b) \(18 \mathrm{~g}\). of glucose per \(\mathrm{dm}^3\)

(c) 6 g. of urea in \(500 \mathrm{~cm}^3\)

(d) \(27 \mathrm{~g}\). of fructose per \(\mathrm{dm}^3\)

45. For isotonic solutions of non-electrolytes which one of the following is equal?

(a) Molality

(b) Normality

(c) Weight percent

(d) Molarity

46. A 0.1 \(\mathrm{M}\) aqueous solution of urea has osmotic pressure of 2 atm. A mixture is prepared by mixing

(i) \(50 \mathrm{ml}\) of \(0.2 \mathrm{M}\) glucose and

(ii) \(150 \mathrm{ml}\) of \(0.4 \mathrm{M}\) canesugar. Temperature being same, the osmotic pressure of the mixture would be

(a) \(7 \mathrm{~atm}\)

(b) \(8 \mathrm{~atm}\)

(c) \(12 \mathrm{~atm}\)

(d) \(6 \mathrm{~atm}\)

47. The mass of glucose to be dissolved in \(250 \mathrm{~cm}^3\) of water, to get a solution which is isotonic with 0.2 M solution of urea, is

(a) \(36 \mathrm{~g}\)

(b) \(9 \mathrm{~g}\)

(c) \(18 \mathrm{~g}\)

(d) \(4.5 \mathrm{~g}\)

48. In an aqueous solution the molecular mass of sodium chloride, as obtained from the colligative properties, is

(a) its normal molecular weight

(b) more than its normal molecular weight

(c) less than its normal molecular weight

(d) unpredictable

49. The boiling point of a decimolal aqueous solution of glucose would be

\(\left(\right.\) Given \(\mathrm{K}_{\mathrm{b}}=0.52 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\) )

(a) \(100.52^{\circ} \mathrm{C}\)

(b) \(99.48^{\circ} \mathrm{C}\)

(c) \(99.948^{\circ} \mathrm{C}\)

(d) \(100.052^{\circ} \mathrm{C}\)

50. The example of solution of liquid in gas is

(a) dry air

(b) aerated water

(c) amalgam

(d) moist air