CET
WORKSHEET
1. A solution is
a) a mixture of two components b) a compound of two components c) A homogenous mixture of two
components d) All the above
2. 50 g. of a solvent is dissolved in 0.95 kg of the solvent. The weight percent of the solution is
a) 50 b) 0.95
c) 5 d) 0.095
3. A solution is 0.25% by weight. The weight of the solvent containing 1.25 g of solute would be
a) 500 g b) 498.75 g
c) 500.25 g d) 501.25 g
4. 200 g of a 5% solution (by weight) of the solute A is mixed with 300 g of a 10% solution (by weight) of solute B. The weight percent of A and B in the mixture are respectively
a) 3.33 and 15 b) 5 and 10
c) 2 and 16 d) 6 and 2
5. Equal volumes of a 10% solution (by weight) of the solute 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
6. 400 cm3 of water is added to 600 g of a 6%
(weight percent) aqueous soln. of a solute. The final weight percent of the solute is
a) 10 b) 1.5
c) 9 d) 3.6
7. 2 mole of ethanol is dissolved in 8 mole of water. The mole fraction of water in the solution
a) 0.2 b) 0.8
c) 0.4 d) 1
8. 92 g of ethanol is dissolved in 108 g of water. The mole fraction of ethanol in the soln is
a) 0.25 b) 0.75
c) 92/108 d) 108/92
9. 4.9 gm of H SO2 4 is present in 500 cm3 of the
solution. Its molarity will be
a) 0.2 b) 0.1
c) 0.05 d) 0.025
10. A centi-molar solution is diluted 10 times. Its molarity would be
a) 0.01 b) 0.1
c) 0.001 d) 0.005
11. If 20 gm. of sodium hydroxide is dissolved in 3
1 dm of water, the molality of the solution will be
a) 0.5 b) 1
c) 0.01 d) 0.2
12. Which 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 13. 30 gm of acetic acid is dissolved in 1dm of the 3
solvent. The molality of the soln. will be (Given, density of solvent = 1.25 g. cm−3)
a) 0.4 b) 0.3
c) 0.5 d) 0.45
14. Colligative properties of a solution are there whose values depend on
a) No. of molecules present in it b) No. of ions present in it c) No. of particles present in it d) None of these
15. Which one of the following is a colligative property ? a) Boiling point
b) Freezing point c) Vapour pressure
d) lowering of vapour pressure 16. Some of the statements are given below
A] lowering of vapour pressure is a colligative property
B] Freezing point of a soln. depends on its concentration
C] Higher the vapour pressure of a liquid, lower is its boiling point
D] Vapour pressure of a solution is always more than that of pure solvent. Among the above the true statements are
a) only A and B b) only A and C
c) A, B and D d) A, B and C
17. If “n” mole of solute are dissolved in “N” mole of solvent and if vapour pressure of pure solvent is ‘P’, then the partial vapour pressure of the solvent in the solution. Will be
a) + P n N b) + nP n N c) + NP n N d) nP N
Solutions and Colligative Properties
18. The vapour pressure of pure solvent and solutions are 120mm and 108mm respectively. The mole fraction of the solvent in the soln is
a) 0.1 b) 0.9
c) 120/108 d) 1.08
19. The vapour pressure of the solution and pure solvent are P and Po respectively. If P/Po is 0.15. then the mole fraction of the solute in the solution is
a) 0.85 b) 0.15
c) 1/0.15 d) 1/0.85
20. In ostwald’s and walkes’s method for determining the lowering of vapour pressure, the loss in weight of solvent bulb is 50 times less than the gain in weight of CaCl2 tubes. The vapour pressure of the soln. would be (Given v.p of pure solvent = 100mm)
a) 2 mm b) 0.5 mm
c) 98 mm d) 100 mm
21. The 0.1 molar aqueous soln. of glucose boils at
0
100.16 C . The boiling point of 0.5 molal aqueous soln. of sucrose will be
a) 500.80 C 0 b) 100.80 C 0
c) 20.16 C0 d) 20.8 C0
22. Which one of the following aqueous soln. will have the highest boiling point ?
a) 0.1 M urea
b) 30 g of glucose per dm3
c) 3.42 g of sucrose in 100 ml d) 0.2 M glucose
23. If kb denotes the molal elevation constant of water, then the boiling point, of an aqueous soln. containing 36 g. of glucose per dm3 in 0C will be
a) 100 2 10 + kb b) 100 10 + kb c) (100 + kb) d) (100 + 2 kb) 24. For a solvent =5 −1 b
k K kg mol . Using this solvent the solution records the elevation of boiling point of 0.5 C . The molality of the 0
solution is
a) 0.25 b) 0.1
c) 10 d) Unpredictable
25. Which one of the following aqueous solution will have the highest freezing point ?
a) 0.1 M urea b) 0.2 M cane sugar c) 6 g of glucose in 100 cm3
d) 1.5 g of urea in 500 cm3
26. The values of Kf for solvents A,B,C and D are 1.86, 1.99, 5.12 and 4.4 K kg mol−1
respectively. The equimolal solutions of a solute in there solvents will have the freezing in order of solvents as
a) C > D > B > A b) A > C > D > B c) A > B > D > C d) C > B > A > D 27. The solution containing 6 g of urea (mol. Wt =
60) per dm3 of water and another containing 9 g
of solute A per dm3 of water freeze at the same
temperature. The molecular weight of ‘A’ is
a) 120 b) 90
c) 54 d) 900
28. Osmosis is the flow, through semi permeable membrane of
a) Solvent molecules from pure solvent to solution
b) Solvent molecules from a solution of lower concentration to that at hiqher concentration
c) Solute molecules from a solution of higher
concentration to that at lower
concentration d) Both (a) and (b) 29. 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 of the pure solvent till it becomes equal to the vapour pressure of the solution
d) All the above
30. When a solution is separated from the solvent by a semi-permeable membrane, the solution rises to maximum height of 10cm. The osmotic pressure of the solution in Pascal is (Given, Density of solution = 1.1 kg dm3)
a) 1079.1 b) 107.91
c) 10791 d) 10.791
31. The osmotic pressure of a solution is directly proportional to
a) Its molarity b) Its temperature c) Both (a) and (b) d) None of these 32. The isotonic solutions have same
a) Molarities b) Osmotic pressure
33. A 0.1m solution of a solute A is isotonic with a solution of B containing 1.5 g of it per 100cm3.
The molecular weight of B is
a) 150 b) 15
c) 75 d) 750
34. A 0.2 M solution of a solute is isotonic with a solution containing
a) 3.42 g of sucrose in 100cm3
b) 18 g of glucose per dm3
c) 6 g of urea in 500cm3
d) 27 g of fructose per dm3
35. For isotonic solutions which one of the following is equal ?
a) Molality b) Normality
c) Weight percent d) Molarity 36. Solution ‘A’ contains 5.85 g of NaCl in 500
3
cm of water and 1 solution B is 0.2 m glucose in water. Temperature being same, which one of the following is true ?
a) Both the solutions are isotonic
b) A is hypotonic solution with respect to B c) B is hypertonic solution with respect to A d) A is hypertonic solution with respect to B
37. The weight of glucose to be dissolved in 250 cm3 of water, to set a solution which is
isotonic with 0.2 M solution of urea, is
a) 36 g b) 9 g
c) 18 g d) 4.5 g
38. The solutions of electrolytes have higher values of colligative properties than the equimolar solutions of non-electrolytes. This is because
a) of ionization of electrolytes b) non-electrolytes do not ionize
c) electrolytes ionize to increase the number of particles in the solution
d) the number of particles in the solution of electrolytes increases due to ionization and the value of colligative property depends on number of particles in the solution 39. The boiling point of a decimolal aqueous
solution of glucose could be (Given kb= 0.52 l kg mol−1)
a) 100.52 C 0 b) 99.48 C 0
c) 99.948 C 0 d) 100.052 C 0
40. osmotic pressure of a 0.6% solution of urea is 300mm Hg at 298 k. The osmotic pressure of a 0.2m cane sugar solution at the same temperature would be
a) 300 mm b) 600 mm
c) 150 mm d) 30 mm
41. The vapour pressure of a solvent is decreased by 2.5mm by adding a solute. The mole fraction of the solute in the solution is (Given v. p of pure solvent B = 250 mm)
a) 0.1 b) 0.9
c) 0.01 d) 1.01
42. The relative lowering of vapour pressure in a solution is 0.23. The mole fraction of the solvent in the solution is
a) 0.23 b) 0.43
c) 0.77 d) 0.34
43. The example of solution of liquid in gas is
a) Dry air b) Aerated water
c) Amalgam d) Moist air
44. The vapour pressure of pure solvent is Po. The mole fraction of a non-volatile solute in the solution is x. The vapour pressure of the solution will be
a) Po (1 – x) b) Po / (1 – x)
c) Pox d) Po/x
45. The lowering of vapor pressure of solvent occurs
a) When the solvent is volatile b) When the solute is non-electrolyte c) When the solute is non-volatile d) In all the above cases
46. Arrange the following aqueous solutions in the order of there increasing boiling points i) 10−4M NaCl ii) 10−3M Urea iii) 3
2
10−M MgCl iv) 10−2M NaCl a) (i) < (ii) < (iii) <
(iv)
b) (ii) < (i) = (iii) < (iv)
c) (ii) < (i) < (iii) < (iv)
d) (iv) > (iii) > (i) = (ii)
47. Which one of the following aqueous solution will have the lowest freezing point ? (Assume complete ionization)
a) 0.1 m urea b) 0.1 m NaCl
c) 0.2 m sucrose d) 0.15 m BaCl2
48. If π1 is the osmotic pressure of a solution containing 6 g of acetic acid per dm3 and
2 π is that of a solution containing 5.85 g of NaCl per
3
dm at the some temperature, then a) π < π1 2 b) π > π1 2
Solutions and Colligative Properties
49. At constant temperature, the osmotic pressure
( )
π and the molarity (M) of the solution are related asa) π α M b) π α 1
M
c) π α M d) π α 1
M
50. The osmotic pressure
( )
π is given as equal toa) M/RT b) MR/T
c) MRT d) RT/M
51. The osmotic pressure (in atm) of a 1 M solution a non-electrolyte at O C0 will be
a) 1 b) 22.4
c) 0.0821 d) 10
52. Equimolar solutions of urea and KCl are separated by a semi permeable membrane. Which one of the following will take place ?
a) No net flow of solvent in either direction b) Solvent will flow from KCl to urea
solution
c) Solvent will flow from urea to KCl solution
d) Nothing can be predicted
53. For NaBr solution, M = 0.5, α =0.8 and 400
π = mm and for Na Po3 4 solution, m = 0.25, α =0.6 and π = P2. Temperature being same, the value of P2 will be
a) 533.3 atm b) 1200 mm
c) 300 mm d) 2133. mm
54. The molecular weights of CaCl2, NaCl and glucose, as determined from osmotic pressure are A, B and C respectively. Assuming CaCl2
and NaCl to be completely ionized the order observed molecules weights will be
a) C > B > A b) A > C > B c) C > A > B d) B > A > C 55. The plant cell will shrink when it is placed in
a) A hypertonic soln b) A hypotonic soln c) An isotonic soln d) None of these
56. The molal elevation constant is the ratio of the elevation of boiling point to
a) Molarity b) Molality c) Normality
d) Mole fraction of solute
57. The value of Kb for a solvent is x K kg mol−1,
A 0.2m solution, of a non-electrolyte, in this solvent will boil at
(Given, B.P of solvent = A ) 0c a)
(
)
0 + A x c b) 0 10 + x A c c) 0 5 + x A c d) 5 + x A k 58. For water =1.86 −1 f k K kg mol . Assuming complete ionization, the freezing point of 1 molal aqueous solution of KCl would bea) 3.72 c 0 b) −3.720c
c) −1.860c d) Unpredictable
59. The freezing point of a 0.05 molal solution of a non-electrolyte in water is
(
=1.86 −1)
f K K kg mol a) 0.093 c 0 b) 273.093 K c) 272.907 K d) -0.093 K60. The best solvent to determine the depression of freezing point accurately is that which has
a) A low value of K f
b) A high value of K f
c) A low freezing point d) A high freezing point
61. Molal elevation constant of water is 0.51. The boiling of a decimolal aqueous KCl is hearly equal to
a) 100.1 c 0 b) 100.05 c 0
c) 105.1 c 0 d) 101.5 c 0
62. The elevation of boiling point of a solution of 10g of a binary strong electrolyte (mol. wt = 100) in 100g. of water is ∆T . The value of Kb
for water is
a) 10 b) 2
c) 2 ∆T d) ∆T/ 2
63. Equal volumes of centimolar solutions of glucose and fructose are mixed. The osmotic pressure of the mixture is
a) equal to either of the solution b) less than either of the solution c) more than either of the solution
d) the sum of osmotic pressure of individual solution
64. The ratio of the value of any colligative property for BaCl2 and Na PO3 4, assuming α to be same for both, is
a) 3 : 4 b) 1 : 4
c) 1 : 2 d) 4 : 3
65. A 5% solution of glucose is isotonic with a 1% solution of solute A. The mol. wt of A is
a) 900 b) 180
c) 36 d) 90
66. A non-volatile solute lowers the vapour pressure of a solvent by 20 mm when its mole fraction in the solution is 0.3. To obtain a lowering of vapour pressure of 40 mm, the mole fraction of the solvent should be
a) 0.6 b) 0.3
c) 0.4 d) 0.15
67. The osmotic pressure of 1% urea solution
( )
1
π , 2% glucose
( )
π2 and 3.42% sucrose solution( )
π3 , at same temperature are in the ordera) π > π > π3 2 1 b) π > π > π1 2 3 c) π > π > π3 1 2 d) π > π > π2 1 3 68. One mole of urea is dissolved in 36 g of water.
The V.P of the solution and pure water are in the ratio of
a) 1 : 1 b) 1 : 3
c) 2 : 3 d) 1 : 2
69. The elevation of boiling point for 0.1 m sucrose, 0.2 m urea and 0.2 m NaCl are in the ratio of
a) 1 : 2 : 4 b) 1 : 2 : 2
c) 1 : 1 : 2 d) 1 : 1 : 4
70. How much glucose per 100 cm3 should be
present to get a solution which would be isotonic with a 3.42% sucrose solution ?
a) 18 g b) 9 g
c) 1.8 g d) 3.6 g
71. The weight of urea, to be dissolved per dm3, to
get a solution which is isotonic with a 0.1m aqueous solution of BaCl2
(
α =1)
would bea) 108 g b) 1.8 g
c) 6 g d) 18 g
72. Some statements are given below :
A] In solution of a non-volatile solute, the V.P of solution is equal to partial V.P of solvent B] For a given solution ∆Tb and ∆Tf will be equal if Kb=Kf
C] Among a set of solution, that which has highest F. pt and will also have highest B. pt. D] Equimolar solutions of all solutes are isotonic
Among the above the false statements are
a) B, C and D b) A, B and C
c) C and D d) B and C
73. Assuming the degree of ionization to be equal the ratio of osmotic pressure of equimolar solutions of Al2
(
SO4)
3,Na PO3 4 and(
)
4 6 K Fe CN a) 5 : 5 : 4 b) 4 : 5 : 4 c) 1 : 0.8 : 1 d) 0.8 : 1 : 1 74. To 100 ml of a 0.5 M solution, 400 ml of water is added. The final molarity would bea) 0.125 b) 0.1
c) 0.25 d) 0.15
75. 800 ml of 0.1 M H SO2 4 is mixed with 200 ml of 0.8 M H SO2 4. The molarity of the mixture. is
a) 0.32 b) 0.24
c) 0.2 d) 0.45
76. 400 ml of 0.2 m H SO2 4 is mixed with 100 ml of 0.1 N H SO2 4. The final normality is
a) 0.17 b) 0.45
c) 0.25 d) 0.34
77. The lowering of vapour pressures is 0.1 m aqueous solutions of NaCl, CuSO4 and K SO2 4 are in the ratio of
a) 1 : 2.5 : 1.5 b) 1 : 1 : 3
c) 1 : 1 : 1.5 d) None of these
78. The factor of ∆Tb k/ b is equal to
a) Molality b) Molarity
c) Mole fraction d) None of these 79. Osmotic pressure can be increased by
a) Increasing temperature b) Decreasing temperature c) Increasing volume d) All of these
80. Which of the following is not a colligative property ?
Solutions and Colligative Properties
81. When a solution is diluted the mole fraction of the solvent
a) Decreases b) Increases
c) Remains unchanged d) Changes unpredictably
82. When to a solution, the solvent is added, the value of lowering of vapour pressure
a) Decreases b) Increases
c) Remains unchanged
d) Records an unpredictable change
83. A molal solution is that which contains one mole of solute in
a) one litr. of solvent b) one litr. of solution c) one kg of solution d) one kg of solvent
84. The osmotic pressure, of a solution of benzoic acid in benzene, is less than expected. This is because
a) Benzene is a non-polar solvent b) Benzoic acid is an organic solute
c) Benzoic acid is in associated state in benzene
d) Benzoic acid gets dissociated in benzene 85. The Raoult’s law of lowering of V.P is best
applicable in determination of correct mol. wt. in case of
a) Volatile solute in a concentrated solution b) Volatile solute in a dilute solution c) Non-volatile solute in a concentrated
solution
d) Non-volatile solute in a dilute solution 86. The plot of partial vapour pressure of a volatile
component of a solution vs its mole fraction at a constant temp. is a straight line with
a) Negative slope b) With positive slope
c) With positive slope passing though the origin and reaching a maxima
d) With a positive slope and passing through the origin
87. The vapour pressure of a liquid depends on a) Its surface area
b) Its volume c) Temperature d) All of these
88. The normal molecular wt. of on electrolyte is 1
M and its molecular wt. obtained from a colligative property is M2. Then
a) M1=2M2 b) M1>M2
c) M1<M2 d) 2M1=M2
89. Which of the following happens, in case of solution, when the mole fraction of a solute in the solution decreases ?
a) V.P increases b) F. pt.. increases
c) Osmotic pressure increases d) Both (a) and (b)
90. The molarity of a 10% NaOH solution is
a) 2.5 b) 0.5
c) 0.25 d) 0.05
91. The mole fraction of nitrogen lima mixture of 7 g of N2 and 16 g of O2, is
a) 0.5 b) 0.75
c) 0.66 d) 0.33
92. 100 ml of 2NHCl is mixed with 400 ml of 5N
2 4
H SO and the mixture is made 2 litr by water. The normality of the resulting mixture is
a) 2.2 b) 1.4
c) 1.1 d) 0.7
93. Which of the following solutions has highest normality ?
a) 1 M HCl b) 0.5M H SO2 4
c) 0.4M H PO3 4 d) 0.55M H SO2 4
94. Colligative properties of a solution depends upon:
a) Nature of both solvent and solute
b) The relative number of solvent and solute particles
c) Nature of solute only d) Nature of solvent only 95. Isotonic solution have the same
a) Density
b) Molar concentration c) Strength
d) Normality
