SOLUTIONS – 8

1) In a pair of immiscible liquids, a common solute dissolves in both and the equilibrium is reached, then the concentration of the solute in the upper layer is
a) In a fixed ratio with that in the lower layer
b) Same as the lower layer
c) Lower than the lower layer
d) Higher than the lower layer

2) Which one of the following salt will have the same value of vant Hoff factor (i) as that of ?
a)
b) NaCl
c)
d)

3) The solution of sugar in water contains
a) free atoms
b) free ions
c) free molecules
d) free atoms and molecules

4) Which of the following is not a colligative property?
a) Depression in freezing point
b) Elevation of boiling point
c) Osmotic pressure
d) Modification of refractive index

5) 12 g of urea is dissolved in 1 litre of water and 68.4 g of sucrose is dissolved in 1 litre of water. The lowering of vapour pressure in the first case is
a) equal to that of the second
b) greater than in the second
c) less than in the second
d) double that of the second

6) Isotonic solutions of nonelectrolytes have the same
a) Molar concentration
b) Molality
c) Normality
d) None of these

7) When a mango is placed in dilute aqueous solution of hydrochloric acid, it
a) Shrinks
b) Swells
c) Bursts
d) Nothing happens

8) Which of the following is a colligative property?
a) Change in free energy
b) Change in pressure
c) Heat of vaporisation
d) Osmotic pressure

9) The freezing point of equimolal aqueous solution will be highest for
a)
b)
c)
d)

10) A solution of 18g of glucose in 200g of water will boil at: (mw of glucose=180;Kb of water=0.5130 C Kg mol-1).
a)
b)
c)
d)

11) The normal boiling point of water is 373 K (at 760 mm). The vapour pressure of water at 298 K is 23 mm. If the enthalpy of vaporisation is 40.656 KJ , the boiling point of water at 23 mm pressure will be
a) 250 K
b) 298 K
c) 51.6 K
d) 12.5 K

12) If the elevation in boiling point of a solution of 10 gm of solute (mol. wt. = 100) in 100 gm of water is , the ebullioscopic constant of water is
a) 10
b)
c)
d)

13) @ The latent heat of vaporisation of water is 9700 cal/mole and if the boiling point is , the ebullioscopic constant of water is
a)
b)
c)
d)

14) The molal elevation constant for water is per kg of water. The boiling point of solution made by dissolving 6.0 g of urea in 200 g of water is
a)
b)
c)
d) none of these

15) 10 g of solute with molecular mass 100 g is dissolved in 100 g solvent to show elevation in boiling point. The value of the molal ebullioscopic constant will be
a) 10
b) 3
c) 0.3
d) unpredictable

16) The boiling point of 0.1 molal solution of urea is at 1 atm. The molal elevation constant of the solvent is
a) 1.8
b) 0.18
c) 18
d) 18.6

17) At a certain hill-station, pure water boils at . If for water is kg , the boiling point of 0.69 M solution of urea at the same place will be
a)
b)
c)
d) unpredictable

18) What is the molality of solution of a certain solute in a solvent if there is a freezing point depression of and if the freezing point constant is 18.4?
a) 0.01
b) 1
c) .001
d) 100

19) A solution of 1.25 g of non-electrolyte in 20 g of water freezes at 271.94 K. If kg , then the molecular weight of the solute will be
a)
b)
c)
d)

20) The amount of urea to be dissolved in 500 c.c. of water (K=1.86) to produce a depression of in the freezing point is
a) 0.3 gm
b) 3 gm
c) 6 gm
d) 9 gm

21) The freezing point of a 0.05 molal solution of a non-electrolyte in water (Kf=1.86) is
a)
b)
c)
d)

22) @ The molar freezing point constant for water is C/mol. If 342 gm of cane sugar is dissolved in 1000 g of water, the solution will freeze at
a)
b)
c)
d)

23) @ A solution containing 6.8 g of a nonionic solute in 100 g of water was found to freeze at . The freezing point depression constant of water is 1.86. Calculate the molecular weight of the solute.
a) 13.6
b) 34
c) 68
d) 136

24) The freezing point of 1.0 M solution of glucose is . If an equal volume of 3.0 M glucose Solution is added, the freezing point of the mixture will be
a)
b)
c)
d)

25) A 0.5 molal solution of ethylene glycol in water is used as coolant in a car. If the freezing point constant of water be mole, the mixture will freeze at
a)
b)
c)
d)

26) What is the freezing point of a solution containing 8.1 g HBR in 100 g water assuming the acid to be 90% ionised ( for water = 1.86 K Kg )?
a)
b)
c)
d)

27) If 15 gm of a solute in 100 gm of water makes a solution that freezes at , then 30 gm of the same solute in 100 gm of water will make a solution that freezes at
a)
b)
c)
d)

28) An aqueous solution of a non-electrolyte solute boils at . The freezing point of the solution will be (Kb=0.52, Kt=1.86)
a)
b)
c)
d) none of the above

29) The molal depression constant for a solvent is 4.9. The depression in freezing point for a millimolal solution of a non-electrolyte in the solvent is
a) 0.49
b) 4.9
c) 4.9+0.001
d) 0.0049

30) An aqueous solution freezes at what is the elevation in boiling point?
a) 0.186
b) 0.512
c) 0.86
d) 0.0512

31) The molal freezing point constant for water is . Therefore, the freezing point of 0.1 M NaCl solution in water is expected to be
a)
b)
c)
d)

32) The depression in freezing point of 0.01 M aqueous solution urea, sodium chloride and sodium sulphate is in the ratio of
a) 1:1:1
b) 1:2:3
c) 1:2:4
d) 2:2:3

33) @ The molal elevation constant of water = . The boiling point of 1.0 molal aqueous KCI solution (assuming complete dissociation of KCI), should be
a)
b)
c)
d)

34) A chemical reaction will be spontaneous if it is accompanied by a decrease of
a) entropy of the system
b) enthalpy of the system
c) internal energy of the system
d) free energy of the system

35) free energy G, enthalpy H and entropy S are related to one another by
a) G = H + TS
b) G = H – TS
c) G – TS = H
d) S = H – G

36) Consider the following reaction occurring in an automobile . The sign of would be
a) +, -, +
b) -, +, –
c) -, +, +
d) +, +, –

37) The pH of a neutral solution is 7. The value of pOH of this solution is
a) <7
b) >7
c) 7
d) More than 7 but less than 10

38) In a certain first order reaction, the concentration of the reactants is reduced to 25% in one hour. The half life period of the reaction is

a) 2 hours
b) 4 hours
c) 1/2 hour
d) 1/4 hour

39) The percentage ionization of 0.01 M NH3 solution is ( kb = 1. 8 x 10-5 )

a) 0.4
b) 0.04
c) 4
d) None of these

40) The fraction of H COOH molecules dissociated in 0.015 m solution is ( Ka = 17.7 x 10-5 )
a) 0.012
b) 0.19
c) 0.18
d) 0.11

41) An aqueous solution whose pH = 0 is
a) Acidic
b) Neutral
c) Basic
d) Amphoters

42) A solution contains 10 ml of 0.1 N NaOH and 10 ml of 0 . 05 N H2 SO4. The pH of this solution is
a) 7
b) Less than 7
c) Greater than 7
d) Zero

43) 1c.c. of 0.1 N HCl is added to 999 c.c. aqueous solution of sodium chloride. The pH of the resulting solution will be
a) 7
b) 4
c) 5
d) 2

44) The PH value of the solution obtained by adding 1 c.c. of 10-5 M HCl to one litre of water is
a) Less than 7
b) Greater than 7
c) Nearly 7
d) Exactly 7

45) The degree of dissociation of HCl is 95% . 0.1920 gm of the acid is present in 0.5 litre of a solution. The pH of this solution is approximately
a) 4
b) 2
c) 2.192
d) 1.92

46) The value of pkw  at   298 K is
a) 
1 x 10-4
b) 0.014
c) 1.4
d) 14

47) A 0.1 N solution of sodium bicarbonate has a pH value of  
a) 5.6
b) 7.0
c) 8.4
d) 4.0

48) The pH of 0 .1 M acetic acid solution is 
a) 0
b) 1
c) Greater than 1
d) 7

49) Pick a poor electrolytic conductor complex in solution.
a)
b)
c)
d)

50) The molality of a solution prepared by dissolving 18 gms of glucose in 500 gms of water will be
a) 1.2 m
b) 0.4 m
c) 0.1 m
d) 0.2 m

51) For preparation of one litre of N / 10 H2SO4 solution we need  H2SO4 equal to
a) 98 gm
b) 4.9 gm
c) 10 gm
d) 2.45 gm

52) Isotonic solutions are
a) somolal
b) Equi – normal
c) Equimolar
d) All of these

53) How many grams of NaOH will be needed to prepare 250 ml of 0.1 M solution?
a) 1 g
b) 10 g
c) 4 g
d) 6 g

54) What is the volume of water to be mixed in 500 ml of 0.5 M NaOH solution so that its concentration becomes 10 g NaOH per litre ?
a) 100 ml
b) 200 ml
c) 250 ml
d) 500 ml

55) If more solvent is added to a solution, the magnitude of heat of reaction
a) Decreases
b) Increases
c) Remains constant
d) None of these

56) The solution with the highest pH is
a) 
0. 1 MH2 SO4
b) 
0.1 M H2 C2 O4
c) 
0.1 M H NO3
d) 
0.1 M H C l O4

57) Soda water has a pH value
a) Less than 7
b) More than 7
c) 7
d) Greater than 14

58) If NH3 is dissolved in water, the pH of the solution 
a) Decreases
b) Increases
c) Remains unchanged
d) May increase or decrease

59) The compound which is not a Lewis acid is
a) BF
b) 
AlCl 3
c) 
SnCl4
d) 
Be Cl2

60) The molal concentration of a solution containing 0.5 mole of H3PO4 dissolved in 500 gm water is

a) 1 m
b) 1 M
c) 1 N
d) 0.5 M

61) CuSO4. 5 H2O is a
a) Solution of solid in a liquid
b) Solution of liquid in a solid
c) Salt only and cannot be called a solution
d) Co- ordination compound of copper with water molecules as the ligands

62) The vapour pressure of a dilute aqueous solution of glucose is 750 m.m. of mercury at 373 K. The mole fraction of the solute is
a)
b)
c)
d)

63) At one atmosphere which of the following solutions has the maximum boiling point?
a) 0.1 m Na Cl
b) 0.1 m  C12 H22 O 11 
c) 
0 .1 m  C6 H12O6
d) 
0.1 m Ba Cl2

64) The osmotic pressure of 6% urea solution in water at 300 k is 24. 63 atmosphere. The molecular mass of urea will be
a) 60
b) 63
c) 59
d) 65

65) Osmotic pressure is measured by
a) Berkley and Hartley method
b) Ostwald’s method
c) Haber’s method
d) Henry’s method

66) The osmotic pressure of a solution increases if the
a) Temperature is decreased
b) Solution constant is increased
c) Number of solute molecules are increased
d) Volume is increased

67) 5 % solution of cane sugar is isotonic with 0.877 % solution of X. The molecular weight of substance X is
a) 59.98
b) 69.98
c) 49.98
d) 39.98

68) For a non – electrolytic solution, van’t Hoff factor is equal to
a) Zero
b) 1
c) 2
d) Between 0 and 1

69) The values of the observed and calculated molecular weights of silver nitrate are 92.64 and 170 respectively. The degree of dissociation of silver nitrate will be
a) 60 %
b) 83.5 %
c) 85.3 %
d) 41.6 %

70) The freezing point of an equimolal aqueous solution will be highest for
a) C6 H5 NH3 Cl
b) 
Ca ( NO3) 2
c) 
La ( NO3)
d) 
C6 H12 O6

71) The molal elevation constant of water which can be evaporated at 100 deg C with the absorption of 2260 J per gm ( R = 8.3 Jk -1 mol -1 ) is
a) 2.32
b) 0.511
c) 1.38
d) 2.02

72) The molecular mass of CHCl 3 can be determined by
a) Osmotic pressure
b) the Rast method
c) Both the above
d) Neither of these

73) The mixture which cannot be separated by simple distillation is
a) n – Hexane and n – Heptane
b) Benzene and Toluene
c) H2O and HNO3
d) All the above

74) Ruby glass is a
a) Colloid
b) Solution
c) Gel
d) Emulsion

75) In the colloidal state, particle size ranges from
a) 1 to 10 A¦
b) 
10 – 1000 A¦ 
c) 
10 – 20 A¦
d) 
100 – 280 A¦

76) The Tyndall effect in colloidal systems is due to the
a) Scattering of light
b) Reflection of light
c) Absorption of light
d) Presence of electrically charged particles

77) Fog is a colloidal state of
a) Gaseous particles dispersed in gas
b) Liquid particles dispersed in a gas
c) Solid particles dispersed in a liquid
d) Solid particles dispersed in gas

78) A colloidal solution can be purified by
a) Filtration
b) Peptization
c) Sedimentation
d) Dialysis

79) The random motion of colloidal particles in the dispersion medium is referred to as
a) Adsorption
b) Coagulation
c) Brownian movement
d) Tyndall effect

80) Purple of cassius is a colloidal solution of
a) Gold
b) Pt
c) Hg
d) All transition elements

81) On adding a few drops of dilute HCl to freshly precipitated ferric hydroxide, a red coloured colloidal state is obtained. This phenomenon is known as
a) Peptisation
b) Coagulation
c) Focculation
d) Dissolution

82) Brownian movement is due to the
a) Temperature fluctuation within the liquid phase
b) Attraction and repulsion between charges on the colloidal particles
c) Impact of molecules of the dispersion medium on the colloidal particles
d) Convective currents

83) The blue colour of water in sea is due to the
a) Absorption of other colours except blue by water molecules
b) Scattering of blue light by water molecules
c) Refraction of blue light by impurities in sea water
d) All of these

84) When a colloidal solution is observed under a ultra microscope, we can see the
a) Light scattered by colloidal particles
b) Size of colloidal particles
c) Shape of the colloidal particles
d) None of these

85) A freshly prepared precipitate of Fe ( OH ) 3 in the presence of water containing some Fe Cl3 becomes colloidal on gentle shaking. This is an example of
a) Peptization
b) Emulsification
c) Electrophoresis
d) Coagulation

86) The ability of an ion to bring about coagulation of a given colloid depends upon
a) It’s size
b) The magnitude of its charge only
c) The sign of its charge alone
d) Both the magnitude and sign of its charge

87) What is ultra filtration?
a) It is the process of separating the dispersed phase from colloidal systems
b) It is the process of separating solutes from suspensions
c) It is the process of separating colloidal systems from suspensions
d) None of these

88) The magnitude of osmotic pressure, relative lowering of vapour pressure, depression in freezing point and elevation in boiling point in all colloidal dispersions is
a) Large
b) Very large
c) Negligible
d) Small

89) The minimum amount of an electrolyte required to a coagulate one litre of the solution is called the coagulation value of the electrolyte. The amount of the electrolyte is expressed in
a) Milligrams
b) Grams
c) Millimoles
d) Moles

90) The phenomenon when the composition of the activated complex includes a substance which does not take part stoichiometrically in the chemical process, but changes the kinetic properties of the system is called
a) Chemical equilibrium
b) Catalysis
c) Osmosis
d) None of these

91) The reaction 2 SO2 ( g ) + O2 ( g ) is an example of

 

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