Quiz yourself on basic concepts of Solutions for getting high marks in exams and entrance tests
1. What is a Solution?
A) A homogenepus mixture of two or more substances
B) A mixture of only one substance
C) A solid mixture
D) A liquid mixture
2. Which of the following best describes a Solution?
A) A heterogeneous mixture
B) A mixture with visible components
C) A mixture with uniform distribution
D) A mixture with a fixed composition
3. What is the physical basis for the combination of components in a Solution?
A) Chemical reaction
B) Electrostatic attraction
C) Magnetic force
D) Physical mixing
4. Can dissolved substances in a Solution be seen through a high-power resolving microscope?
A) Yes
B) No
5. What type of composition do Solutions have?
A) Fixed composition
B) High composition
C) Heterogeneous composition
D) Variable composition
6. What are the two components of a Solution?
A) Solutes and solvents
B) Acids and bases
C) Liquids and gases
D) Metals and nonmetals
7. What is another name for Solutions that have two components?
A) Ternary Solutions
B) Binary Solutions
C) Complex Solutions
D) Simple Solutions
8. Which of the following is an example of a Solution?
A) Sugar and sand mixture
B) Oil and water mixture
C) Salt dissolved in water
D) Vinegar and baking soda mixture
9. Which of the following is an example of a gas in gas solution?
A) Smoke
B) Carbon particles
C) Air
D) Vinegar
10. Which of the following is an example of a liquid in gas solution?
A) Sea water
B) Fog
C) Oxygen gas
D) Dental amalgam
11. What type of solution is vinegar?
A) Gas in liquid
B) Liquid in liquid
C) Solid in liquid
D) Gas in solid
12. Which of the following is an example of a liquid in solid solution?
A) Hydrogen in palladium
B) Dental amalgam
C) Sea water
D) Brass (Alloy)
13. What is an example of a solid in solid solution?
A) Hydrogen in palladium
B) HCl solution
C) Vinegar
D) Carbon particles
14. What is the state of the solvent in a gas in solid solution?
A) Solid
B) Liquid
C) Gas
D) Plasma
15. What is an aqueous solution?
A. A solution in which water is not used as a solvent
B. A solution in which water is the only solvent
C. A solution in which solutes are not dissolved
D. A solution in which solvents are not dissolved
16. Which of the following is an example of an aqueous solution?
A. Gasoline and water
B. Salt and oil
C. Sugar and water
D. Oxygen and nitrogen
17. What is a saturated solution?
A. A solution in which no solute is dissolved
B. A solution in which solvents are not dissolved
C. A solution in which no more solute can be dissolved at a particular temperature
D. A solution in which more solute can be dissolved at a particular temperature
18. If 100g of sugar is dissolved in 200ml of water at room temperature, is the solution saturated or unsaturated?
A. Saturated
B. Unsaturated
C. Super-saturated
D. None of the above
19. What is an unsaturated solution?
A. A solution in which no solute is dissolved
B. A solution in which solvents are not dissolved
C. A solution that has less amount of solute than required to become saturated at a particular temperature
D. A solution that has more solute than required to become saturated at a particular temperature
20. Which of the following is an example of a concentrated solution?
A. 50g of salt dissolved in 1L of water B. 20g of sugar dissolved in 500mL of water C. 10g of salt dissolved in 500mL of water D. 30g of sugar dissolved in 1L of water
21. What is a dilute solution?
A. A solution in which no solute is dissolved
B. A solution in which solvents are not dissolved
C. A solution that has more solute than required to become saturated at a particular temperature
D. A solution that has less amount of solute than required to become saturated at a particular temperature
22. What type of solution has a capacity for dissolution that has not been reached at a particular temperature?
A. Saturated solution
B. Unsaturated solution
C. Super-saturated solution
D. Dilute solution
23. Which of the following is an example of a super-saturated solution?
A. 100g of sugar dissolved in 500mL of water
B. 150g of salt dissolved in 500mL of water
C. 200g of sugar dissolved in 500mL of water
D. 250g of salt dissolved in 1L of water
MCQs on Solubility and Factors affecting solubility
24. What is Solubility?
A. The amount of solute required to saturate 100g of the solvent at a particular temperature.
B. The amount of solvent required to saturate 100g of the solute at a particular temperature.
C. The ability of a solvent to saturate 100g of the solute.
D. The ability of a solute to saturate 100g of the solvent.
25. What is the formula for solubility?
A. Mass of solvent / Mass of solute x 100
B. Mass of solute / Mass of solvent x 100
C. Mass of solvent x Mass of solute x 100
D. Mass of solute - Mass of solvent x 100
26. What does solubility mean?
A. The ability of a solvent to saturate a solute.
B. The ability of a solute to saturate a solvent.
C. The amount of solvent required to saturate a solute.
D. The amount of solute required to saturate a solvent.
27. Which is more soluble in water at a particular temperature, Sodium Nitrate or Silver Chloride?
A. Sodium Nitrate
B. Silver Chloride
C. Both have the same solubility in water at that temperature
D. Not enough information to determine
28. What are completely miscible liquids?
A. Liquids that mix up with each other up to a limited extent.
B. Liquids that do not mix at all.
C. Liquids that mix up with each other in all proportions.
D. Liquids that mix up with each other only under certain conditions.
29. Give an example of completely miscible liquids.
A. Water and carbon-tetra-chloride
B. Water and benzene
C. Water and alcohol
D. Water and carbon-di-Sulphide
30. What are completely immiscible liquids?
A. Liquids which mix up with each other up to a limited extent.
B. Liquids which do not mix at all.
C. Liquids which mix up with each other in all proportions.
D. Liquids which mix up with each other only under certain conditions.
31. Give an example of partially miscible liquids.
A. Water and phenol
B. Water and alcohol
C. Water and benzene
D. Water and carbon-di-Sulphide
32. A heterogeneous mixture of two or more two different substances is called:
A. Solution
B. Suspension
C. Colloid
D. None of the above
33. The solution in which the solution particles are bigger than the solution and smaller than the suspension is called:
A. Solution
B. Suspension
C. Colloid
D. None of the above
34. Colloids are:
A. Homogeneous throughout
B. Heterogeneous throughout
C. Uniform throughout
D. None of the above
35. Suspensions are:
A. Stable and do not separate upon standing
B. Unstable and can separate upon standing
C. Have non-uniform composition throughout
D. None of the above
36. Colloids show:
A. Strong Tyndall effect
B. Weak Tyndall effect
C. No Tyndall effect
D. None of the above
37. Solutions are:
A. Opaque
B. Translucent
C. Transparent
D. None of the above
38. Suspensions are:
A. Highly mobile and can flow easily
B. Less mobile and cannot flow easily
C. Homogeneous throughout
D. None of the above
39. Colloids:
A. Can pass through a filter paper in filtration
B. Cannot pass through a filter paper in filtration
C. Show scattering of light in all directions
D. None of the above
40. What is the definition of concentration?
A. The amount of solvent dissolved in a given amount of solute
B. The amount of solute dissolved in a given amount of solvent
C. The total amount of solution
D. The ratio of solute to solvent
41. What is a standard solution?
A. A solution that is diluted
B. A solution with an unknown concentration
C. A solution with a known concentration
D. A solution with no solute
42. Which concentration units are commonly used?
A. Percentage composition of solution and mass-mass percentage
B. Mass-volume percentage and volume-mass percentage
C. Volume-volume percentage and mass-mass percentage
D. Percentage composition of solution and volume-volume percentage
43. What is percentage composition of solution?
A. The number of parts of solvent present in 100 parts of solution
B. The fraction of solvent in a solution multiplied by 100
C. The number of parts of solute present in 100 parts of solution
D. The fraction of solute in a solution multiplied by 100
44. What is mass-mass (m/m%) percentage?
A. The number of grams by mass of solute present in 100 grams by mass of a solution
B. The number of grams by mass of solvent present in 100 grams by mass of a solution
C. The number of grams by volume of solute present in 100 mL of a solution
D. The volume in cm3/ml of a solute dissolved per 100 cm3 of solution
45. What is volume-mass (V/m%) percentage?
A. The volume in cm3 of a solute dissolved in 100 g of solution
B. The number of grams by volume of solute present in 100 mL of a solution
C. The number of grams by mass of solute present in 100 grams by mass of a solution
D. The volume in cm3/ml of a solute dissolved per 100 cm3 of solution
46. What is volume-volume (V/V%) percentage?
A. The volume in cm3 of a solute dissolved per 100 cm3 of solution
B. The number of grams by mass of solute present in 100 grams by mass of a solution
C. The number of grams by volume of solute present in 100 mL of a solution
D. The number of parts of solute present in 100 parts of solution
47. What is molarity?
A. The amount of solvent dissolved in a given amount of solute.
B. The amount of solute dissolved in a given amount of solvent.
C. The number of moles of solute and solvent in a given volume of solution.
D. The number of particles of solute and solvent in a given volume of solution.
48. What is the unit of molarity?
A. Gram-per-mole
B. Gram-per-liter
C. Mole-per-liter
D. Mole-per-gram
49. What is the formula for molarity?
A. Molarity (M) = Mass of Solute / Volume of Solution in dm3
B. Molarity (M) = Mass of Solution / Volume of Solute in dm3
C. Molarity (M) = Number of Particles of Solute / Volume of Solution in dm3
D. Molarity (M) = Number of moles of Solute / Volume of Solution in dm3
50. What is the unit of molarity represented in grams?
A. gmol-1
B. gL-1
C. gdm-3
D. gcm-3
50. How do you calculate molarity?
A. M = Number of moles of Solute / (Volume of Solution in dm3 (liter))
B. M = Amount of Solute in gram / (M.wt of Solute x Volume of Solution in dm3 )
C. M = Volume of Solution in dm3 / Number of moles of Solute
D. M = Mass of Solution / Volume of Solution in dm3
51. What is the molarity of a solution containing 12.0 grams of HCl in enough water to make 500 mL of solution? (Molecular weight of HCl is 36.5 g/mol)
A. 1.16 M
B. 0.058 M
C. 0.116 M
D. 11.6 M
52. What is the molarity of a solution containing 5.00 moles of NaOH in enough water to make 2.50 L of solution?
A. 12.5 M
B. 2.00 M
C. 1.00 M
D. 0.800 M
53. What is the molarity of a solution that contains 10 grams of NaOH dissolved in 500 cm3 of solution? (At. mass: Na = 23g, O = 16g, H = 1g)
A) 0.2 M
B) 1 M
C) 2 M
D) 0.5 M
54. What is the molarity of a solution containing 15 g of glucose (C6H12O6) in 250 cm3 of solution? (At. mass: C = 12g, O = 16g, H = 1g)
A) 0.2 M
B) 1 M
C) 2 M
D) 0.5 M
Answer: b) 1 M
0.333
55. How many grams of NaOH are required to prepare 500 cm3 of a 2 M solution? (At. mass: Na = 23g, O = 16g, H = 1g)
A) 20 g
B) 40 g
C) 60 g
D) 80 g
56. What is the molarity of a solution containing 0.5 moles of KCl in 250 cm3 of solution? (At. mass: K = 39g, Cl = 35.5g)
A) 0.2 M
B) 1 M
C) 2 M
D) 0.5 M
Answer: d) 0.5 M.........C..2 M
57. How many grams of CaCl2 are required to prepare 500 cm3 of a 0.5 M solution? (At. mass: Ca = 40g, Cl = 35.5g)
A) 20 g
B) 40 g
C) 60 g
D) 80 g
Answer: b) 40 g
58. What is the molarity of a solution containing 4.5 grams of NaOH dissolved in 250 cm3? (At. mass: Na = 23g, O = 16g, H = 1g)
S) 0.5 M
B) 1 M
C) 2 M
D) 0.2 M
Answer: a) 0.5 M
59. How many grams of glucose (C6H12O6) are required to prepare 500 cm3 of a 1.5 M solution? (At. mass: C = 12g, O = 16g, H = 1g)
A) 67.5 g
B) 90 g
C) 135 g
D) 180 g
Answer: c) 135 g
60. What is the molarity of a solution containing 0.25 moles of NaCl in 500 cm3 of solution? (At. mass: Na = 23g, Cl = 35.5g)
A) 0.25 M
B) 0.5 M
C) 1 M
D) 2 M
Answer: b) 0.5 M
61. How many grams of KCl are required to prepare 500 cm3 of a 1 M solution? (At. mass: K = 39g, Cl = 35.5g)
A) 39 g
B) 74.5 g
C) 118 g
D) 227.5 g
Answer: b) 74.5 g
62. What factor affects the solubility of a solution?
A) Temperature
B) Pressure
C) Both A and B
D) None of the above
Answer: a) Temperature
63. How is solubility related to temperature?
A) Solubility and temperature are directly related.
B) Solubility and temperature are inversely related.
C) Solubility and temperature have no relation.
D) Solubility and temperature are related randomly.
Answer: a) Solubility and temperature are directly related.
64. Which process occurs when solutes absorb heat?
A) Hyperthermic process
B) Exothermic process
C) Neither A nor B
D) Both A and B
Answer: C)
65. When does the solubility of sugar in water increase?
A) When heat is released
B) When there is no change in temperature
C) When heat is absorbed
D) None of the above
Answer: c) When heat is absorbed
66. Which of the following solutes releases heat?
A) Sugar
B) Calcium oxide (CaO)
C) Sodium chloride (NaCl)
D) Potassium bromide (KBr)
Answer: b) Calcium oxide (CaO)
67. Does the solubility of NaCl and KBr change with an increase or decrease in temperature?
A) Yes, it increases with an increase in temperature
B) Yes, it decreases with an increase in temperature
C) No, it remains unchanged
D) None of the above
Answer: c) No, it remains unchanged
68. What happens to the solubility of sodium sulphate dehydrate (Na2SO4.10H2O) above 32.4 ℃?
A) It remains the same
B) It increases
C) It decreases
D) It becomes anhydrous
Answer: d) It becomes anhydrous
69. How does the solubility of a solute that releases heat change with temperature?
A) It increases with an increase in temperature
B) It decreases with an increase in temperature
C) It remains the same
D) It depends on the solute
Answer: b) It decreases with an increase in temperature
70. Which of the following processes is characterized by the absorption of heat?
A) Exothermic process
B) Endothermic process
C) Neither A nor B
D) Both A and B
Answer: b) Endothermic process
71. What happens to the solubility of a solute that absorbs heat when temperature is increased?
A) It increases
B) It decreases
C) It remains the same
D) It depends on the solute
Answer: a) It increases
72. How does pressure affect the solubility of gases?
A) Pressure has no effect on the solubility of gases
B) Increase in pressure increases the solubility of gases
C) Decrease in pressure increases the solubility of gases
D) Increase in pressure decreases the solubility of gases
Answer: b) Increase in pressure increases the solubility of gases
73. What is the effect of pressure on the solubility of solids and liquids?
A) Solids and liquids become more soluble with increase in pressure
B) Solids and liquids become less soluble with increase in pressure
C) Pressure has no effect on the solubility of solids and liquids
D) Solids become more soluble and liquids become less soluble with increase in pressure
Answer: c) Pressure has no effect on the solubility of solids and liquids
74. How does the nature of solvent affect solubility?
A) Solubility decreases when the solute and solvent have similar properties
B) Solubility increases when the solute and solvent have similar properties
C) The nature of the solvent has no effect on solubility
D) The effect of the nature of the solvent on solubility depends on the nature of the solute
Answer: b) Solubility increases when the solute and solvent have similar properties
75. What is the effect of an endothermic process on solubility?
A) Solubility increases with increase in temperature
B) Solubility decreases with increase in temperature
C) Solubility remains constant with increase in temperature
D) Solubility decreases with decrease in temperature
Answer: a) Solubility increases with increase in temperature
76. What is the effect of an exothermic process on solubility?
A) Solubility increases with increase in temperature
B) Solubility decreases with increase in temperature
C) Solubility remains constant with increase in temperature
D) Solubility decreases with decrease in temperature
Answer: b) Solubility decreases with increase in temperature
77. What is the effect of the nature of solute on solubility?
A) Solubility always increases with increase in the nature of the solute
B) Solubility always decreases with increase in the nature of the solute
C) The effect of the nature of solute on solubility depends on the nature of the solvent
D) The nature of the solute has no effect on solubility
Answer: c) The effect of the nature of solute on solubility depends on the nature of the solvent
78. Why does the solubility of gases increase with increase in pressure?
A) Gases become more polar with increase in pressure
B) Gases become less polar with increase in pressure
C) Gases become more compressible with increase in pressure
D) Gases become less compressible with increase in pressure
Answer: c) Gases become more compressible with increase in pressure
79. What is Solute Solvent Interaction?
A) The force of attraction between the solute and solvent molecules
B) The force of attraction between solute and solvent of same nature cl
C) The force of attraction between solute and solvent of different nature
D) The force of attraction between solute and solute molecules
80. What is the role of solute solvent interaction in solubility?
A) It determines the nature of solute
B) It determines the nature of solvent
C) It determines the extent of solubility
D) It determines the concentration of solute
Answers
1. A 2. C 3. D 4. B 5. D 6. A 7. B 8. C 9. C 10. B 11. B 12. B 13. A 14. A 15. B 16. C 17. C 18. B 19. C 20. A 21. D 22. B 23. C 24. A 25. B 26. B 27. A 28. C 29. C 30. B 31. A 32. B 33. C 34. B 35. B 36. B 37. C 38. B 39. 40. B 41. C 42. A 43. D 44. A 45. A 46. A 47. B 48. C 49. D 50. A 51. C 52. B 53. D 54. 55. B 56. 57. 58. 59. 60. 61. 62. 63. 64. 65. 66. 67. 68. 69. 70. 71. 72. 73. 74. 75. 76. 77. 78. 79. 80. 81. 82. 83. 84. 85. 86. 87. 88. 89. 90. 91. 92. 93.
Make 10 standarized MCQs along with providing four options in the form A. B C. D. as well as correct answers indicated among these four options for the given
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