Chapter 9 solutions
In this article, the author has explained the most important chemistry MCQs from the ninth chapter ( Solutions ) of FSC chemistry. All the correct answers have been represented as bold.
1: Which one of the following statements is false about osmotic pressure?
a) It is the pressure of the hydrostatic column set up to osmosis.
b) It is the pressure applied on the solution to prevent the entry of the solvent into it through a semi-permeable membrane.
c) During osmosis, the flow of solvent is only from dilute solution to concentrated solution
d) Osmotic pressure is directly proportional to the temperature of the solution.
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2: Molarity of 4% NaOH solution is
a) 0.1 M
b) 0.01 M
c) 0.5 M
d) 1.0 M
3: A solution which has higher osmotic pressure as compared to other solution is known as
a) Hypotonic
b) Isotonic
c) Hypertonic
d) Normal
4: which of the following solutions will have the highest freezing point?
a) 0.1 M FeCl3
b) 0.1 M NaCl2
c) 0.1 M BaCl2
d) 0.1 M Urea
5: which one of the following statements is incorrect?
A) A solution freezes at a lower temperature than the pure solvent.
b) A solution boils at a higher temperature than the pure solvent.
c) 0.1 NaCl solution and 0.1 M sugar solution have the same boiling point
d) Osmosis cannot take place without a semi-permeable membrane.
6: The freezing point of 1 molal NaCl solution assuming NaCl to be 100% dissociated in water (Kf = 1.853 K.Kg/mol) is
a) -1.860C
b) +1.860C
c) -3.720C
d) +3.720C
7: 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 fixed ratio with that in the lower layer
b) Lower than the lower layer
c) Same as the lower layer
d) Higher than the lower layer
8: The molarity of a solution prepared by adding 7.1 g of Na2SO4 (formula weight 142 amu ) to enough water to make 100 ml volume is
a) 2.0 M
b) 0.5 M
c) 1.0 M
d) 0.05 M
9: An aqueous solution of glucose is 10% in strength. The volume in which 1 gm mole of it is dissolved will be
a) 18 liters
b) 0.9 litres
c) 9 liters
d) 1.8 liters
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10: Molarity of an aqueous solution that produces an elevation of the boiling point of 1.00 K at 1 atm pressure (Kb for water =0.512 K.Kg / mol )
a) 0.512 m
b) 1.95 m
c) 0.915 m
d) 5.12 m
11: Which one of the following salt shows a falling curve of solubility with rise in temperature
a) KNO3
b) NaCl
c) Ce2(SO4)3
d) CaCl2
12: Which of the following solutions has the highest boiling point?
a) 5.85% solution of sodium chloride
b) 6.05 solution of urea
c) 18.0% solution of glucose
d) All have the same boiling points
13: Which of the following, when dissolved in water, gives negative heat of solution?
a) LiCl
b) NaCl
c) KCl
d) Pb(NO3)2
14: The ebullioscopic constant, Kb, depends upon?
a) Amount of solute
b) Nature of solvent
c) Amount of solvent
d) Nature of solute
15: Which of the following solutions will be most concentrated
a) 1m HCl
b) 1 M HCl
c) 1% HCl
d) Same concentration in all
16: The molecular weight of benzoic acid in benzene as determined by depression in freezing point method corresponding to;
a) Ionization of benzoic acid
b) Termerization of benzoic acid
c) Dimerization of benzoic acid
d) Solvation of benzoic acid
17: A solution is obtained by dissolving 5.85g of sodium chloride (mol. Wt= 58.5) in a liter solution, another solution is prepared by dissolving 34.2g of Cane sugar (mol. Wt= 342) in a liter of solution at the same temperature. The lowering of vapor pressure in the first solution is
a) Same as that of 2nd solution
b) Half that of 2nd solution
c) Double that of 2nd solution
d) Nearly 1/5th of 2nd solution
18: A 0.1L 0.5M solution of sulfuric acid is mixed with 0.2L 0.1M phosphoric acid, the concentration of H+ ions in the resultant solution
a) 0.3 M
b) 0.2M
c) 0.5M
d) None of these
19: When mercuric acid is added to the aqueous solution of potassium iodide, the
a) Freezing point is raised
b) Freezing point is lowered
c) Freezing point does not change
d) Boiling point does not change
20: In a depression in freezing point experiment, it is found that
1. The vapor pressure of the solution is less than that of pure solvent
2. The vapor pressure of the solution is more than that of pure solvent
3. Only solute molecules solidify at the freezing point
4. Only solvent molecules solidify at the freezing point
a) 1, 2
b) 2, 3
c) 1, 4
d) 1, 3
21: Which of the following one percent aqueous solution has the lowest freezing point?
a) Sucrose (M.W = 342)
b) Glucose (M.W = 180)
c) Sodium acetate (M.W = 82)
d) Urea (M.W = 60)
22: Molecular weight of a polymer can be best determined by measuring
a) Osmotic pressure of the solution
b) V.P. of solution
c) B.P of solution
d) F.P of solution
23: At constant temperature, with an increase in the concentration of solute, the osmotic pressure
of solution
a) Remains constant
b) Decreases
c) Increases
d) None of these.
24: If two solutions have the same osmotic pressure, they are known as
a) Isotonic solutions
b) Hypotonic solutions
c) Normal solutions
d) Hypertonic-solutions
25: Increasing the temperature of an aqueous solution will cause
a) Molality to increase
b) Mole fraction to decrease
c) Molarity to decrease
d) % by weight to increase
26: The solution of sugar in water contains
a) Free ions
b) Free molecules
c) Free atoms
d) Free, atoms and molecules
27: Mole fraction of water in tap water will
a) Equal to 1
b) Greater than 1
c) Will somewhat equal to 2
d) Less than 1
28: What will be the molality of a solution containing 4.6g ethyl alcohol & 300g H20?
a) 0.3
b) 0.5
c) 0.1
d) None of these
29. x grams Of water is mixed in 69 grams Of ethanol Mole fraction of ethanol in the resultant solution is 0.6. What is the Value Of ‘x’ in grams?
a) 54
b) 36
c) 180
d) 18
30: Water has 2.5×10-3 Of dissolved oxygen in of sample. The concentration of oxygen in
the sample of seawater in parts per million is
a) 3
b) 2.5
c) 0.5
d) 5
31: The number of moles Of NaOH present in 10 liters of 1 molar solution Is
a) 10
b) 5
c) 1
d) 2.5
32: Equal volume 0. 1 M AgNO3 and 0.2 M NaCl are mixed. The concentration of nitrate ions in the mixture will be
a) 0.1M
b) 0.2M
c) 0.05M
d. O.16M
33: The pair of benzene and toluene represents
a) Negative deviation Raoult’s law,
b) No deviation from Raoult’s law
c) Positive deviation from Raoult’s law
d) Variable deviation from Raoult’s law
34: If the solubility of calcium fluoride in water is a moles per litre, its solubility product is given by
a) 2s
b) 4s3
c) 2s2
d) 2s4
35. A binary mixture that forms a non-ideal solution has
a) Boiling point lower than that of the pure solvent
b) Melting point higher than that of the pure solvent
c) Zero heat of solution.
d) Vapour pressure that may be higher or lower than that of the pure solvent.
36. For a solution containing two volatile components, the graph between composition and temperature shows
a) Two curves, one for liquid and the other for vapors
b) Only one curve.
c) Two separate curves for the two liquid components
d) Two curves for vapors only
37: When a crystal of solute is added into the supersaturated solution, then
a) The solute dissolves completely
b) The solution remains supersaturated
c) The excess solute crystallizes our
d) The solution becomes unsaturated
38: Indicate the solution pairs which can be separated into their pure components by fractional distillation:
a) Water and ethanol
b) Water and HNO3
c) Water and HCl
d) Benzene and toluene
39: Vapor pressure of a solution when a non-volatile solute is added, to a solvent is always
a) More than the vapor pressure of the pure solvent
b) Equal to the vapor pressure of the solvent
c) Less than the vapor pressure of the pure solvent
d) Desorbing upon the nature of the solvent
40: The aqueous solution of CuSO4 is
a) Acidic
b) Basic
c) Neutral
d) None of these
41: Which of the following solution has the lowest vapor pressure?
a) 0.1m Urea
b) 0.1m Glucose
c) 0.1m NaCl
d) 0.1m Sucrose
42: Pure water boils at 373K and boils at 359K. the azeotropic mixture of water and HNO3 boils at 393.5K. By distilling the azeotropic mixture
a) Pure nitric acid will distill over first
b) Pure water will distill
c) One of them will distill over in a small amount of the other
d) Both of them will distill over in the same composition as that of the mixture being distilled
43: When the attraction between A –B is more than that of the A-A and B-B, the solution will show deviation from Raoult’s law
a) positive
b) Negative
c) No deviation
d) Cannot be predicted
44: The vapor pressure of two liquids P and Q are 80 and 60 torr respectively. The total vapor pressure of solution obtained by mixing 3 moles of P and 3 moles of Q would be
a) 20 torr
b) 68 torr
c) 72 torr
d) 140 torr
45: A solution containing 1 mole of CHCl3 and 4 moles of acetone has a vapor pressure of 0.400 atmospheres. At this temperature, the vapor pressure of pure CHCl3 is 0.359 atm and that of acetone is 0.453 atm. From the data, it is correctly concluded
a) That the solution shows a negative deviation from Raoult’s law
b) That of the solution maximum-boiling azeotrope
c) Heat is evolved
d) All of these
46. If a compound has a negative heat of solution, at high temperature it dissolves
a) More rapidly and is more soluble
b) Less rapidly and is less soluble
c) More rapidly and is less soluble
d) Less rapidly and is more soluble.
47: The correct order of hydration for the following ions is
a) K+ > H+> Cl– > OH–
b) H+> K+ > Cl– > OH–
c) Cl– > K+ > H+> OH–
d) H+> OH– > Cl– > K+
48: In CuS04.5H20, out of five water molecules. How much water surrounds Cu+2
a) 1
b) 2
c) 3
d) 4
49: Azeotropic mixture can be separated by
a) Vaccum distillation
b) Fractional distillation
c) Chemical method
d) Both a’ and ‘c’
50: Which one of the following salt produces acidic solution on hydrolysis
a) Na2CO3
b) CH3COONa
c) Na2SO4
d) CuSO4
51: Molarity of 4 % NaOH solution is
a) 0.1 M
b) 0.5 M
c) 0.01 M
d) 1.0 M
52: The molarity of a solution prepared by adding 7.1 g of Na2SO4 ( formula weight 142 amu) to enough water to make 100 ml volume is
a) 2.0 M
b) 1.0 M
c) 0.5
d) 0.05
53: An aqueous solution of glucose is 10% in strength. The volume in which 1 gm mole of it is dissolved will be
a) 18 liters
b) 9 liters
c) 0.9 liters
d) 1.8 liters
54: Molality of an aqueous solution that produces an elevation of the boiling point of 1.00 K at 1 atm pressure ( Kb for water = 0.512 K.Kg.mol-1)
a) 0.512 m
b) 0.915 m
c) 1.95 m
d) 5.12 m
55: Which Of the following solutions will be most concentrated?
a) 1m HCI
b) 1M HCI
c) 1% HCI
d) Same in all
56: A 0.1L 0.5M solution of sulfuric acid is mixed with 0.2L 0.1M phosphoric acid, the concentration of H+ ions in the resultant solution.
a) 0.3M
b) 0.2M
c) 0.53M
d) None of these
57: Which Of the following unit of concentration is not independent of temperature?
a) Molarity
b) Molality
c) Mole fraction
d) All
58. Increasing the temperature of an aqueous solution will cause
a) Molality to increase
b) Mole fraction to decrease
c) Molarity to decrease
d) % by weight to increase
59: Mole fraction of water in tap water will
a) Equal to 1
b) Greater than 1
c) Will be somewhat equal to 2
d) Less than
60. What will be the molality of a solution containing 4.6g ethyl alcohol & 300g H20?
a) 0.3
b) 0.5
c) 0.1
d) None