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NEET Chemistry - Chapter 7

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Mole fraction
1. Mole fraction is defined as:
- A. moles of a component divided by total moles (Correct)
- B. mass of solute divided by total mass
- C. moles per litre
- D. grams per 100 mL
Explanation: Mole fraction is a unitless ratio based on moles.
Mass percent
2. Mass percent of a solute is:
- A. mass of solute divided by mass of solution times 100 (Correct)
- B. mass of solute divided by mass of solvent times 100
- C. moles of solute divided by litres of solution
- D. equivalents per litre
Explanation: Mass percent is based on total mass of solution.
Molarity
3. Molarity is the number of moles of solute present in:
- A. 1 litre of solution (Correct)
- B. 1 kilogram of solvent
- C. 100 g of solution
- D. 1 litre of solvent
Explanation: Molarity uses volume of final solution.
Molality
4. Molality is the number of moles of solute present in:
- A. 1 kilogram of solvent (Correct)
- B. 1 litre of solution
- C. 100 g of solvent
- D. 1 mole of solution
Explanation: Molality uses mass of solvent.
Henry law
5. According to Henry's law, solubility of a gas in liquid is proportional to:
- A. partial pressure of the gas (Correct)
- B. molar mass of the gas
- C. surface area only
- D. temperature always
Explanation: Higher gas pressure generally raises dissolved amount.
Raoult law
6. For an ideal solution, partial vapour pressure of a component equals:
- A. mole fraction times vapour pressure of pure component (Correct)
- B. molarity times total pressure
- C. mass fraction times density
- D. temperature divided by mole fraction
Explanation: This is Raoult's law for each volatile component.
Ideal solution
7. An ideal solution obeys Raoult's law over:
- A. the entire composition range (Correct)
- B. only infinite dilution
- C. only at boiling point
- D. only for electrolytes
Explanation: Ideal solutions obey the law at all compositions.
Deviation
8. Positive deviation from Raoult's law means observed vapour pressure is:
- A. greater than ideal value (Correct)
- B. less than ideal value
- C. equal to zero
- D. independent of composition
Explanation: Weaker A-B attraction makes escape easier.
Deviation
9. Negative deviation from Raoult's law means A-B interactions are:
- A. stronger than average (Correct)
- B. weaker than average
- C. zero
- D. always ionic
Explanation: Stronger unlike interactions reduce escaping tendency.
Vapour pressure
10. Adding a non-volatile solute to a solvent generally:
- A. lowers vapour pressure (Correct)
- B. raises vapour pressure
- C. keeps vapour pressure unchanged
- D. makes it zero instantly
Explanation: Fewer solvent molecules are available at surface.
Relative lowering
11. Relative lowering of vapour pressure for dilute solution equals:
- A. mole fraction of solute (Correct)
- B. molarity of solvent
- C. boiling point elevation
- D. osmotic pressure
Explanation: This follows from Raoult's law for non-volatile solute.
Boiling point
12. Elevation in boiling point is a:
- A. colligative property (Correct)
- B. chemical property
- C. nuclear property
- D. surface property
Explanation: It depends on number of solute particles.
Freezing point
13. Depression in freezing point is a:
- A. colligative property (Correct)
- B. kinetic property
- C. magnetic property
- D. optical property
Explanation: It depends on particle concentration, not identity.
Osmosis
14. Osmosis is the flow of solvent through a semipermeable membrane from:
- A. lower solute concentration to higher solute concentration (Correct)
- B. higher solute concentration to lower solute concentration
- C. solution to vacuum only
- D. solute to solvent
Explanation: Solvent moves from dilute side to concentrated side.
Osmotic pressure
15. For dilute solutions, osmotic pressure is given by:
- A. $\pi = CRT$ (Correct)
- B. $\pi = K_b m$
- C. $\pi = K_f m$
- D. $\pi = P x$
Explanation: This is the solution analogue of ideal gas equation.
van't Hoff factor
16. The van't Hoff factor accounts for:
- A. association or dissociation of solute particles (Correct)
- B. molar mass of solvent
- C. density of solution
- D. surface tension
Explanation: It adjusts colligative-property equations for particle count.
Association
17. For association of solute particles, the van't Hoff factor is usually:
- A. less than 1 (Correct)
- B. greater than 1
- C. equal to 2 always
- D. equal to zero
Explanation: Association reduces the number of independent particles.
Dissociation
18. For dissociation of electrolytes, the van't Hoff factor is usually:
- A. greater than 1 (Correct)
- B. less than 1
- C. always 1
- D. always zero
Explanation: Dissociation increases total particles.
Azeotrope
19. A minimum-boiling azeotrope is usually associated with:
- A. positive deviation from Raoult's law (Correct)
- B. negative deviation from Raoult's law
- C. ideal behavior only
- D. solid solutions
Explanation: Higher total vapour pressure lowers boiling point.
Azeotrope
20. A maximum-boiling azeotrope is usually associated with:
- A. negative deviation from Raoult's law (Correct)
- B. positive deviation from Raoult's law
- C. ideal solution only
- D. nonelectrolytes only
Explanation: Lower total vapour pressure raises boiling point.
Concentration unit
21. The concentration unit independent of temperature is:
- A. molality (Correct)
- B. molarity
- C. grams per litre of solution only
- D. normality
Explanation: Mass of solvent does not vary with temperature.
Colligative idea
22. Colligative properties depend mainly on:
- A. number of solute particles (Correct)
- B. chemical nature of solute
- C. color of solution
- D. rate of stirring
Explanation: Particle count is the governing factor.
Semipermeable membrane
23. A semipermeable membrane allows passage of:
- A. solvent molecules only (Correct)
- B. solute particles only
- C. both solute and solvent equally
- D. ions only
Explanation: This selective passage enables osmosis.
Boiling point relation
24. Elevation in boiling point is represented by:
- A. $\Delta T_b = iK_b m$ (Correct)
- B. $\Delta T_b = iK_f m$
- C. $\pi = iCRT$
- D. $P = xP^0$
Explanation: This is the standard colligative equation.
Freezing point relation
25. Depression in freezing point is represented by:
- A. $\Delta T_f = iK_f m$ (Correct)
- B. $\Delta T_f = iK_b m$
- C. $\pi = iCRT$
- D. $P = xP^0$
Explanation: This is the freezing-point colligative equation.
Mole fraction
26. Mole fraction is defined as:
- A. moles of a component divided by total moles (Correct)
- B. mass of solute divided by total mass
- C. moles per litre
- D. grams per 100 mL
Explanation: Mole fraction is a unitless ratio based on moles.
Mass percent
27. Mass percent of a solute is:
- A. mass of solute divided by mass of solution times 100 (Correct)
- B. mass of solute divided by mass of solvent times 100
- C. moles of solute divided by litres of solution
- D. equivalents per litre
Explanation: Mass percent is based on total mass of solution.
Molarity
28. Molarity is the number of moles of solute present in:
- A. 1 litre of solution (Correct)
- B. 1 kilogram of solvent
- C. 100 g of solution
- D. 1 litre of solvent
Explanation: Molarity uses volume of final solution.
Molality
29. Molality is the number of moles of solute present in:
- A. 1 kilogram of solvent (Correct)
- B. 1 litre of solution
- C. 100 g of solvent
- D. 1 mole of solution
Explanation: Molality uses mass of solvent.
Henry law
30. According to Henry's law, solubility of a gas in liquid is proportional to:
- A. partial pressure of the gas (Correct)
- B. molar mass of the gas
- C. surface area only
- D. temperature always
Explanation: Higher gas pressure generally raises dissolved amount.
Raoult law
31. For an ideal solution, partial vapour pressure of a component equals:
- A. mole fraction times vapour pressure of pure component (Correct)
- B. molarity times total pressure
- C. mass fraction times density
- D. temperature divided by mole fraction
Explanation: This is Raoult's law for each volatile component.
Ideal solution
32. An ideal solution obeys Raoult's law over:
- A. the entire composition range (Correct)
- B. only infinite dilution
- C. only at boiling point
- D. only for electrolytes
Explanation: Ideal solutions obey the law at all compositions.
Deviation
33. Positive deviation from Raoult's law means observed vapour pressure is:
- A. greater than ideal value (Correct)
- B. less than ideal value
- C. equal to zero
- D. independent of composition
Explanation: Weaker A-B attraction makes escape easier.
Deviation
34. Negative deviation from Raoult's law means A-B interactions are:
- A. stronger than average (Correct)
- B. weaker than average
- C. zero
- D. always ionic
Explanation: Stronger unlike interactions reduce escaping tendency.
Vapour pressure
35. Adding a non-volatile solute to a solvent generally:
- A. lowers vapour pressure (Correct)
- B. raises vapour pressure
- C. keeps vapour pressure unchanged
- D. makes it zero instantly
Explanation: Fewer solvent molecules are available at surface.
Relative lowering
36. Relative lowering of vapour pressure for dilute solution equals:
- A. mole fraction of solute (Correct)
- B. molarity of solvent
- C. boiling point elevation
- D. osmotic pressure
Explanation: This follows from Raoult's law for non-volatile solute.
Boiling point
37. Elevation in boiling point is a:
- A. colligative property (Correct)
- B. chemical property
- C. nuclear property
- D. surface property
Explanation: It depends on number of solute particles.
Freezing point
38. Depression in freezing point is a:
- A. colligative property (Correct)
- B. kinetic property
- C. magnetic property
- D. optical property
Explanation: It depends on particle concentration, not identity.
Osmosis
39. Osmosis is the flow of solvent through a semipermeable membrane from:
- A. lower solute concentration to higher solute concentration (Correct)
- B. higher solute concentration to lower solute concentration
- C. solution to vacuum only
- D. solute to solvent
Explanation: Solvent moves from dilute side to concentrated side.
Osmotic pressure
40. For dilute solutions, osmotic pressure is given by:
- A. $\pi = CRT$ (Correct)
- B. $\pi = K_b m$
- C. $\pi = K_f m$
- D. $\pi = P x$
Explanation: This is the solution analogue of ideal gas equation.
van't Hoff factor
41. The van't Hoff factor accounts for:
- A. association or dissociation of solute particles (Correct)
- B. molar mass of solvent
- C. density of solution
- D. surface tension
Explanation: It adjusts colligative-property equations for particle count.
Association
42. For association of solute particles, the van't Hoff factor is usually:
- A. less than 1 (Correct)
- B. greater than 1
- C. equal to 2 always
- D. equal to zero
Explanation: Association reduces the number of independent particles.
Dissociation
43. For dissociation of electrolytes, the van't Hoff factor is usually:
- A. greater than 1 (Correct)
- B. less than 1
- C. always 1
- D. always zero
Explanation: Dissociation increases total particles.
Azeotrope
44. A minimum-boiling azeotrope is usually associated with:
- A. positive deviation from Raoult's law (Correct)
- B. negative deviation from Raoult's law
- C. ideal behavior only
- D. solid solutions
Explanation: Higher total vapour pressure lowers boiling point.
Azeotrope
45. A maximum-boiling azeotrope is usually associated with:
- A. negative deviation from Raoult's law (Correct)
- B. positive deviation from Raoult's law
- C. ideal solution only
- D. nonelectrolytes only
Explanation: Lower total vapour pressure raises boiling point.
Concentration unit
46. The concentration unit independent of temperature is:
- A. molality (Correct)
- B. molarity
- C. grams per litre of solution only
- D. normality
Explanation: Mass of solvent does not vary with temperature.
Colligative idea
47. Colligative properties depend mainly on:
- A. number of solute particles (Correct)
- B. chemical nature of solute
- C. color of solution
- D. rate of stirring
Explanation: Particle count is the governing factor.
Semipermeable membrane
48. A semipermeable membrane allows passage of:
- A. solvent molecules only (Correct)
- B. solute particles only
- C. both solute and solvent equally
- D. ions only
Explanation: This selective passage enables osmosis.
Boiling point relation
49. Elevation in boiling point is represented by:
- A. $\Delta T_b = iK_b m$ (Correct)
- B. $\Delta T_b = iK_f m$
- C. $\pi = iCRT$
- D. $P = xP^0$
Explanation: This is the standard colligative equation.
Freezing point relation
50. Depression in freezing point is represented by:
- A. $\Delta T_f = iK_f m$ (Correct)
- B. $\Delta T_f = iK_b m$
- C. $\pi = iCRT$
- D. $P = xP^0$
Explanation: This is the freezing-point colligative equation.
Mole fraction
51. Mole fraction is defined as:
- A. moles of a component divided by total moles (Correct)
- B. mass of solute divided by total mass
- C. moles per litre
- D. grams per 100 mL
Explanation: Mole fraction is a unitless ratio based on moles.
Mass percent
52. Mass percent of a solute is:
- A. mass of solute divided by mass of solution times 100 (Correct)
- B. mass of solute divided by mass of solvent times 100
- C. moles of solute divided by litres of solution
- D. equivalents per litre
Explanation: Mass percent is based on total mass of solution.
Molarity
53. Molarity is the number of moles of solute present in:
- A. 1 litre of solution (Correct)
- B. 1 kilogram of solvent
- C. 100 g of solution
- D. 1 litre of solvent
Explanation: Molarity uses volume of final solution.
Molality
54. Molality is the number of moles of solute present in:
- A. 1 kilogram of solvent (Correct)
- B. 1 litre of solution
- C. 100 g of solvent
- D. 1 mole of solution
Explanation: Molality uses mass of solvent.
Henry law
55. According to Henry's law, solubility of a gas in liquid is proportional to:
- A. partial pressure of the gas (Correct)
- B. molar mass of the gas
- C. surface area only
- D. temperature always
Explanation: Higher gas pressure generally raises dissolved amount.
Raoult law
56. For an ideal solution, partial vapour pressure of a component equals:
- A. mole fraction times vapour pressure of pure component (Correct)
- B. molarity times total pressure
- C. mass fraction times density
- D. temperature divided by mole fraction
Explanation: This is Raoult's law for each volatile component.
Ideal solution
57. An ideal solution obeys Raoult's law over:
- A. the entire composition range (Correct)
- B. only infinite dilution
- C. only at boiling point
- D. only for electrolytes
Explanation: Ideal solutions obey the law at all compositions.
Deviation
58. Positive deviation from Raoult's law means observed vapour pressure is:
- A. greater than ideal value (Correct)
- B. less than ideal value
- C. equal to zero
- D. independent of composition
Explanation: Weaker A-B attraction makes escape easier.
Deviation
59. Negative deviation from Raoult's law means A-B interactions are:
- A. stronger than average (Correct)
- B. weaker than average
- C. zero
- D. always ionic
Explanation: Stronger unlike interactions reduce escaping tendency.
Vapour pressure
60. Adding a non-volatile solute to a solvent generally:
- A. lowers vapour pressure (Correct)
- B. raises vapour pressure
- C. keeps vapour pressure unchanged
- D. makes it zero instantly
Explanation: Fewer solvent molecules are available at surface.
Relative lowering
61. Relative lowering of vapour pressure for dilute solution equals:
- A. mole fraction of solute (Correct)
- B. molarity of solvent
- C. boiling point elevation
- D. osmotic pressure
Explanation: This follows from Raoult's law for non-volatile solute.
Boiling point
62. Elevation in boiling point is a:
- A. colligative property (Correct)
- B. chemical property
- C. nuclear property
- D. surface property
Explanation: It depends on number of solute particles.
Freezing point
63. Depression in freezing point is a:
- A. colligative property (Correct)
- B. kinetic property
- C. magnetic property
- D. optical property
Explanation: It depends on particle concentration, not identity.
Osmosis
64. Osmosis is the flow of solvent through a semipermeable membrane from:
- A. lower solute concentration to higher solute concentration (Correct)
- B. higher solute concentration to lower solute concentration
- C. solution to vacuum only
- D. solute to solvent
Explanation: Solvent moves from dilute side to concentrated side.
Osmotic pressure
65. For dilute solutions, osmotic pressure is given by:
- A. $\pi = CRT$ (Correct)
- B. $\pi = K_b m$
- C. $\pi = K_f m$
- D. $\pi = P x$
Explanation: This is the solution analogue of ideal gas equation.
van't Hoff factor
66. The van't Hoff factor accounts for:
- A. association or dissociation of solute particles (Correct)
- B. molar mass of solvent
- C. density of solution
- D. surface tension
Explanation: It adjusts colligative-property equations for particle count.
Association
67. For association of solute particles, the van't Hoff factor is usually:
- A. less than 1 (Correct)
- B. greater than 1
- C. equal to 2 always
- D. equal to zero
Explanation: Association reduces the number of independent particles.
Dissociation
68. For dissociation of electrolytes, the van't Hoff factor is usually:
- A. greater than 1 (Correct)
- B. less than 1
- C. always 1
- D. always zero
Explanation: Dissociation increases total particles.
Azeotrope
69. A minimum-boiling azeotrope is usually associated with:
- A. positive deviation from Raoult's law (Correct)
- B. negative deviation from Raoult's law
- C. ideal behavior only
- D. solid solutions
Explanation: Higher total vapour pressure lowers boiling point.
Azeotrope
70. A maximum-boiling azeotrope is usually associated with:
- A. negative deviation from Raoult's law (Correct)
- B. positive deviation from Raoult's law
- C. ideal solution only
- D. nonelectrolytes only
Explanation: Lower total vapour pressure raises boiling point.
Concentration unit
71. The concentration unit independent of temperature is:
- A. molality (Correct)
- B. molarity
- C. grams per litre of solution only
- D. normality
Explanation: Mass of solvent does not vary with temperature.
Colligative idea
72. Colligative properties depend mainly on:
- A. number of solute particles (Correct)
- B. chemical nature of solute
- C. color of solution
- D. rate of stirring
Explanation: Particle count is the governing factor.
Semipermeable membrane
73. A semipermeable membrane allows passage of:
- A. solvent molecules only (Correct)
- B. solute particles only
- C. both solute and solvent equally
- D. ions only
Explanation: This selective passage enables osmosis.
Boiling point relation
74. Elevation in boiling point is represented by:
- A. $\Delta T_b = iK_b m$ (Correct)
- B. $\Delta T_b = iK_f m$
- C. $\pi = iCRT$
- D. $P = xP^0$
Explanation: This is the standard colligative equation.
Freezing point relation
75. Depression in freezing point is represented by:
- A. $\Delta T_f = iK_f m$ (Correct)
- B. $\Delta T_f = iK_b m$
- C. $\pi = iCRT$
- D. $P = xP^0$
Explanation: This is the freezing-point colligative equation.
Mole fraction
76. Mole fraction is defined as:
- A. moles of a component divided by total moles (Correct)
- B. mass of solute divided by total mass
- C. moles per litre
- D. grams per 100 mL
Explanation: Mole fraction is a unitless ratio based on moles.
Mass percent
77. Mass percent of a solute is:
- A. mass of solute divided by mass of solution times 100 (Correct)
- B. mass of solute divided by mass of solvent times 100
- C. moles of solute divided by litres of solution
- D. equivalents per litre
Explanation: Mass percent is based on total mass of solution.
Molarity
78. Molarity is the number of moles of solute present in:
- A. 1 litre of solution (Correct)
- B. 1 kilogram of solvent
- C. 100 g of solution
- D. 1 litre of solvent
Explanation: Molarity uses volume of final solution.
Molality
79. Molality is the number of moles of solute present in:
- A. 1 kilogram of solvent (Correct)
- B. 1 litre of solution
- C. 100 g of solvent
- D. 1 mole of solution
Explanation: Molality uses mass of solvent.
Henry law
80. According to Henry's law, solubility of a gas in liquid is proportional to:
- A. partial pressure of the gas (Correct)
- B. molar mass of the gas
- C. surface area only
- D. temperature always
Explanation: Higher gas pressure generally raises dissolved amount.
Raoult law
81. For an ideal solution, partial vapour pressure of a component equals:
- A. mole fraction times vapour pressure of pure component (Correct)
- B. molarity times total pressure
- C. mass fraction times density
- D. temperature divided by mole fraction
Explanation: This is Raoult's law for each volatile component.
Ideal solution
82. An ideal solution obeys Raoult's law over:
- A. the entire composition range (Correct)
- B. only infinite dilution
- C. only at boiling point
- D. only for electrolytes
Explanation: Ideal solutions obey the law at all compositions.
Deviation
83. Positive deviation from Raoult's law means observed vapour pressure is:
- A. greater than ideal value (Correct)
- B. less than ideal value
- C. equal to zero
- D. independent of composition
Explanation: Weaker A-B attraction makes escape easier.
Deviation
84. Negative deviation from Raoult's law means A-B interactions are:
- A. stronger than average (Correct)
- B. weaker than average
- C. zero
- D. always ionic
Explanation: Stronger unlike interactions reduce escaping tendency.
Vapour pressure
85. Adding a non-volatile solute to a solvent generally:
- A. lowers vapour pressure (Correct)
- B. raises vapour pressure
- C. keeps vapour pressure unchanged
- D. makes it zero instantly
Explanation: Fewer solvent molecules are available at surface.
Relative lowering
86. Relative lowering of vapour pressure for dilute solution equals:
- A. mole fraction of solute (Correct)
- B. molarity of solvent
- C. boiling point elevation
- D. osmotic pressure
Explanation: This follows from Raoult's law for non-volatile solute.
Boiling point
87. Elevation in boiling point is a:
- A. colligative property (Correct)
- B. chemical property
- C. nuclear property
- D. surface property
Explanation: It depends on number of solute particles.
Freezing point
88. Depression in freezing point is a:
- A. colligative property (Correct)
- B. kinetic property
- C. magnetic property
- D. optical property
Explanation: It depends on particle concentration, not identity.
Osmosis
89. Osmosis is the flow of solvent through a semipermeable membrane from:
- A. lower solute concentration to higher solute concentration (Correct)
- B. higher solute concentration to lower solute concentration
- C. solution to vacuum only
- D. solute to solvent
Explanation: Solvent moves from dilute side to concentrated side.
Osmotic pressure
90. For dilute solutions, osmotic pressure is given by:
- A. $\pi = CRT$ (Correct)
- B. $\pi = K_b m$
- C. $\pi = K_f m$
- D. $\pi = P x$
Explanation: This is the solution analogue of ideal gas equation.
van't Hoff factor
91. The van't Hoff factor accounts for:
- A. association or dissociation of solute particles (Correct)
- B. molar mass of solvent
- C. density of solution
- D. surface tension
Explanation: It adjusts colligative-property equations for particle count.
Association
92. For association of solute particles, the van't Hoff factor is usually:
- A. less than 1 (Correct)
- B. greater than 1
- C. equal to 2 always
- D. equal to zero
Explanation: Association reduces the number of independent particles.
Dissociation
93. For dissociation of electrolytes, the van't Hoff factor is usually:
- A. greater than 1 (Correct)
- B. less than 1
- C. always 1
- D. always zero
Explanation: Dissociation increases total particles.
Azeotrope
94. A minimum-boiling azeotrope is usually associated with:
- A. positive deviation from Raoult's law (Correct)
- B. negative deviation from Raoult's law
- C. ideal behavior only
- D. solid solutions
Explanation: Higher total vapour pressure lowers boiling point.
Azeotrope
95. A maximum-boiling azeotrope is usually associated with:
- A. negative deviation from Raoult's law (Correct)
- B. positive deviation from Raoult's law
- C. ideal solution only
- D. nonelectrolytes only
Explanation: Lower total vapour pressure raises boiling point.
Concentration unit
96. The concentration unit independent of temperature is:
- A. molality (Correct)
- B. molarity
- C. grams per litre of solution only
- D. normality
Explanation: Mass of solvent does not vary with temperature.
Colligative idea
97. Colligative properties depend mainly on:
- A. number of solute particles (Correct)
- B. chemical nature of solute
- C. color of solution
- D. rate of stirring
Explanation: Particle count is the governing factor.
Semipermeable membrane
98. A semipermeable membrane allows passage of:
- A. solvent molecules only (Correct)
- B. solute particles only
- C. both solute and solvent equally
- D. ions only
Explanation: This selective passage enables osmosis.
Boiling point relation
99. Elevation in boiling point is represented by:
- A. $\Delta T_b = iK_b m$ (Correct)
- B. $\Delta T_b = iK_f m$
- C. $\pi = iCRT$
- D. $P = xP^0$
Explanation: This is the standard colligative equation.
Freezing point relation
100. Depression in freezing point is represented by:
- A. $\Delta T_f = iK_f m$ (Correct)
- B. $\Delta T_f = iK_b m$
- C. $\pi = iCRT$
- D. $P = xP^0$
Explanation: This is the freezing-point colligative equation.
Mole fraction
101. Mole fraction is defined as:
- A. moles of a component divided by total moles (Correct)
- B. mass of solute divided by total mass
- C. moles per litre
- D. grams per 100 mL
Explanation: Mole fraction is a unitless ratio based on moles.
Mass percent
102. Mass percent of a solute is:
- A. mass of solute divided by mass of solution times 100 (Correct)
- B. mass of solute divided by mass of solvent times 100
- C. moles of solute divided by litres of solution
- D. equivalents per litre
Explanation: Mass percent is based on total mass of solution.
Molarity
103. Molarity is the number of moles of solute present in:
- A. 1 litre of solution (Correct)
- B. 1 kilogram of solvent
- C. 100 g of solution
- D. 1 litre of solvent
Explanation: Molarity uses volume of final solution.
Molality
104. Molality is the number of moles of solute present in:
- A. 1 kilogram of solvent (Correct)
- B. 1 litre of solution
- C. 100 g of solvent
- D. 1 mole of solution
Explanation: Molality uses mass of solvent.
Henry law
105. According to Henry's law, solubility of a gas in liquid is proportional to:
- A. partial pressure of the gas (Correct)
- B. molar mass of the gas
- C. surface area only
- D. temperature always
Explanation: Higher gas pressure generally raises dissolved amount.
Raoult law
106. For an ideal solution, partial vapour pressure of a component equals:
- A. mole fraction times vapour pressure of pure component (Correct)
- B. molarity times total pressure
- C. mass fraction times density
- D. temperature divided by mole fraction
Explanation: This is Raoult's law for each volatile component.
Ideal solution
107. An ideal solution obeys Raoult's law over:
- A. the entire composition range (Correct)
- B. only infinite dilution
- C. only at boiling point
- D. only for electrolytes
Explanation: Ideal solutions obey the law at all compositions.
Deviation
108. Positive deviation from Raoult's law means observed vapour pressure is:
- A. greater than ideal value (Correct)
- B. less than ideal value
- C. equal to zero
- D. independent of composition
Explanation: Weaker A-B attraction makes escape easier.
Deviation
109. Negative deviation from Raoult's law means A-B interactions are:
- A. stronger than average (Correct)
- B. weaker than average
- C. zero
- D. always ionic
Explanation: Stronger unlike interactions reduce escaping tendency.
Vapour pressure
110. Adding a non-volatile solute to a solvent generally:
- A. lowers vapour pressure (Correct)
- B. raises vapour pressure
- C. keeps vapour pressure unchanged
- D. makes it zero instantly
Explanation: Fewer solvent molecules are available at surface.
Relative lowering
111. Relative lowering of vapour pressure for dilute solution equals:
- A. mole fraction of solute (Correct)
- B. molarity of solvent
- C. boiling point elevation
- D. osmotic pressure
Explanation: This follows from Raoult's law for non-volatile solute.
Boiling point
112. Elevation in boiling point is a:
- A. colligative property (Correct)
- B. chemical property
- C. nuclear property
- D. surface property
Explanation: It depends on number of solute particles.
Freezing point
113. Depression in freezing point is a:
- A. colligative property (Correct)
- B. kinetic property
- C. magnetic property
- D. optical property
Explanation: It depends on particle concentration, not identity.
Osmosis
114. Osmosis is the flow of solvent through a semipermeable membrane from:
- A. lower solute concentration to higher solute concentration (Correct)
- B. higher solute concentration to lower solute concentration
- C. solution to vacuum only
- D. solute to solvent
Explanation: Solvent moves from dilute side to concentrated side.
Osmotic pressure
115. For dilute solutions, osmotic pressure is given by:
- A. $\pi = CRT$ (Correct)
- B. $\pi = K_b m$
- C. $\pi = K_f m$
- D. $\pi = P x$
Explanation: This is the solution analogue of ideal gas equation.
van't Hoff factor
116. The van't Hoff factor accounts for:
- A. association or dissociation of solute particles (Correct)
- B. molar mass of solvent
- C. density of solution
- D. surface tension
Explanation: It adjusts colligative-property equations for particle count.
Association
117. For association of solute particles, the van't Hoff factor is usually:
- A. less than 1 (Correct)
- B. greater than 1
- C. equal to 2 always
- D. equal to zero
Explanation: Association reduces the number of independent particles.
Dissociation
118. For dissociation of electrolytes, the van't Hoff factor is usually:
- A. greater than 1 (Correct)
- B. less than 1
- C. always 1
- D. always zero
Explanation: Dissociation increases total particles.
Azeotrope
119. A minimum-boiling azeotrope is usually associated with:
- A. positive deviation from Raoult's law (Correct)
- B. negative deviation from Raoult's law
- C. ideal behavior only
- D. solid solutions
Explanation: Higher total vapour pressure lowers boiling point.
Azeotrope
120. A maximum-boiling azeotrope is usually associated with:
- A. negative deviation from Raoult's law (Correct)
- B. positive deviation from Raoult's law
- C. ideal solution only
- D. nonelectrolytes only
Explanation: Lower total vapour pressure raises boiling point.
Concentration unit
121. The concentration unit independent of temperature is:
- A. molality (Correct)
- B. molarity
- C. grams per litre of solution only
- D. normality
Explanation: Mass of solvent does not vary with temperature.
Colligative idea
122. Colligative properties depend mainly on:
- A. number of solute particles (Correct)
- B. chemical nature of solute
- C. color of solution
- D. rate of stirring
Explanation: Particle count is the governing factor.
Semipermeable membrane
123. A semipermeable membrane allows passage of:
- A. solvent molecules only (Correct)
- B. solute particles only
- C. both solute and solvent equally
- D. ions only
Explanation: This selective passage enables osmosis.
Boiling point relation
124. Elevation in boiling point is represented by:
- A. $\Delta T_b = iK_b m$ (Correct)
- B. $\Delta T_b = iK_f m$
- C. $\pi = iCRT$
- D. $P = xP^0$
Explanation: This is the standard colligative equation.
Freezing point relation
125. Depression in freezing point is represented by:
- A. $\Delta T_f = iK_f m$ (Correct)
- B. $\Delta T_f = iK_b m$
- C. $\pi = iCRT$
- D. $P = xP^0$
Explanation: This is the freezing-point colligative equation.

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