Colligative properties boiling point elevation freezing point depression osmotic pressure - Question Bank

1. What is the osmotic pressure of a 0.1 M NaCl solution at 27°C? (R = 0.0821 L atm mol⁻¹ K⁻¹)
A) 0.246 atm
B) 0.492 atm
C) 1.23 atm
D) 2.46 atm
2. A solution of urea in water freezes at -0.186 °C. If Kf for water is 1.86 K kg mol⁻¹, what is the molality of the solution?
A) 0.01 mol kg⁻¹
B) 0.1 mol kg⁻¹
C) 1.0 mol kg⁻¹
D) 0.186 mol kg⁻¹
3. If a solution boils at 100.52 °C and the Kb for water is 0.52 K kg mol⁻¹, what is the molality of the non-volatile, non-electrolyte solute?
A) 0.01 mol kg⁻¹
B) 0.1 mol kg⁻¹
C) 1.0 mol kg⁻¹
D) 0.52 mol kg⁻¹
4. Which of the following solvents is often used to determine the molar mass of organic compounds due to its high Kf value?
A) Water
B) Ethanol
C) Benzene
D) Acetone
5. Which of the following statements about colligative properties is FALSE?
A) They depend on the number of solute particles.
B) They are useful for determining the molar mass of solutes.
C) They are independent of the nature of the solvent.
D) They are affected by the dissociation or association of the solute.
6. In the context of colligative properties, 'non-volatile' means that the solute:
A) Does not dissolve in the solvent.
B) Does not exert a significant vapor pressure at the boiling point of the solvent.
C) Reacts with the solvent.
D) Is a solid at room temperature.
7. The process of solvent molecules moving from a region of higher solvent concentration to a region of lower solvent concentration through a semipermeable membrane is called:
A) Diffusion
B) Dialysis
C) Osmosis
D) Reverse osmosis
8. Which colligative property is typically measured in terms of pressure difference across a semipermeable membrane?
A) Boiling point elevation
B) Freezing point depression
C) Osmotic pressure
D) Vapor pressure lowering
9. What is the relationship between vapor pressure lowering and other colligative properties?
A) Vapor pressure lowering is independent of other colligative properties.
B) Vapor pressure lowering is inversely related to boiling point elevation.
C) Vapor pressure lowering is directly proportional to boiling point elevation.
D) Vapor pressure lowering is directly proportional to freezing point depression.
10. A 0.1 molal aqueous solution of a salt that dissociates into three ions will have a freezing point depression:
A) Approximately equal to that of a 0.1 molal glucose solution.
B) Approximately three times that of a 0.1 molal glucose solution.
C) Approximately half that of a 0.1 molal glucose solution.
D) Approximately 0.1 times that of a 0.1 molal glucose solution.
11. When 1 mole of NaCl is dissolved in 1 kg of water, the boiling point elevation would be approximately double that of dissolving 1 mole of glucose in 1 kg of water, assuming ideal behavior. This is due to:
A) The higher molar mass of NaCl.
B) The dissociation of NaCl into two ions.
C) The lower solubility of NaCl.
D) The higher Kb of water.
12. Which of the following substances is a strong electrolyte?
A) Glucose
B) Sucrose
C) Hydrochloric acid (HCl)
D) Methanol
13. Which of the following substances is a non-electrolyte?
A) Sodium chloride (NaCl)
B) Potassium nitrate (KNO3)
C) Urea (CO(NH2)2)
D) Sulfuric acid (H2SO4)
14. The molar mass of a non-volatile solute can be determined using the freezing point depression method if:
A) The solute is an electrolyte.
B) The solvent has a high Kf value.
C) The solution is very dilute.
D) The solute is volatile.
15. A solution with a higher concentration of solute particles will have a:
A) Lower boiling point and lower osmotic pressure.
B) Higher boiling point and higher osmotic pressure.
C) Lower boiling point and higher osmotic pressure.
D) Higher boiling point and lower osmotic pressure.
16. Which colligative property is most sensitive to concentration and therefore useful for determining molar masses of very dilute solutions?
A) Boiling point elevation
B) Freezing point depression
C) Osmotic pressure
D) Vapor pressure lowering
17. The modified formula for osmotic pressure considering Van't Hoff factor is:
A) π = i * M R T
B) π = M R T / i
C) π = i R T / M
D) π = M / (i R T)
18. The modified formula for freezing point depression considering Van't Hoff factor is:
A) ΔTf = i * Kf * m
B) ΔTf = Kf * m / i
C) ΔTf = Kf * i / m
D) ΔTf = m / (Kf * i)
19. The modified formula for boiling point elevation considering Van't Hoff factor is:
A) ΔTb = i * Kb * m
B) ΔTb = Kb * m / i
C) ΔTb = Kb * i / m
D) ΔTb = m / (Kb * i)
20. If a solute undergoes dissociation in solution, its observed colligative property will be:
A) Higher than expected, and 'i' will be less than 1.
B) Lower than expected, and 'i' will be less than 1.
C) Higher than expected, and 'i' will be greater than 1.
D) Lower than expected, and 'i' will be greater than 1.
21. If a solute undergoes association in solution, its observed colligative property will be:
A) Higher than expected, and 'i' will be less than 1.
B) Lower than expected, and 'i' will be less than 1.
C) Higher than expected, and 'i' will be greater than 1.
D) Lower than expected, and 'i' will be greater than 1.
22. For a strong electrolyte that dissociates into three ions (e.g., CaCl2), the theoretical Van't Hoff factor (i) is:
A) 1
B) 2
C) 3
D) 4
23. For a strong electrolyte that dissociates into two ions (e.g., NaCl), the theoretical Van't Hoff factor (i) is:
A) 1
B) 2
C) 3
D) 0.5
24. For a non-electrolyte solute like glucose, the Van't Hoff factor (i) is:
A) 0
B) 1
C) 2
D) Greater than 1
25. The Van't Hoff factor (i) accounts for:
A) The volume of the solute.
B) The effect of solute association or dissociation on colligative properties.
C) The solubility of the solute.
D) The color of the solution.
26. Reverse osmosis is a process used for:
A) Increasing the concentration of a solution.
B) Purifying water.
C) Separating isomers.
D) Detecting radioactivity.
27. When a solution is placed in contact with pure solvent through a semipermeable membrane, osmosis will occur:
A) From the solution to the solvent.
B) From the solvent to the solution.
C) In both directions equally.
D) Not at all.
28. Isotonic solutions have:
A) Different osmotic pressures but the same concentration.
B) The same osmotic pressure but different concentrations.
C) The same osmotic pressure at the same temperature.
D) Different osmotic pressures at different temperatures.
29. Osmotic pressure is a colligative property because it depends on:
A) The size of the solute particles.
B) The chemical potential of the solvent.
C) The concentration of solute particles.
D) The boiling point of the solvent.
30. Which of the following is an example of a semipermeable membrane?
A) Platinum foil
B) Cellophane
C) Glass plate
D) Rubber sheet
31. What is a semipermeable membrane?
A) A membrane that allows all molecules to pass through.
B) A membrane that allows only solvent molecules to pass through, but not solute molecules.
C) A membrane that allows only solute molecules to pass through.
D) A membrane that blocks all molecular movement.
32. The relationship between osmotic pressure (π), molarity (M), gas constant (R), and absolute temperature (T) is given by:
A) π = M R T
B) π = M / R T
C) π = R T / M
D) π = M + R T
33. Osmotic pressure is defined as:
A) The pressure exerted by the solvent molecules on the membrane.
B) The minimum pressure required to prevent the passage of solvent into the solution through a semipermeable membrane.
C) The pressure at which the solution boils.
D) The pressure at which the solution freezes.
34. Which solvent has the highest Kf value, making it suitable for determining molar masses of solutes?
A) Water
B) Ethanol
C) Benzene
D) Acetic acid
35. Pure water freezes at 0°C. If a solution of a non-volatile solute is prepared, its freezing point will be:
A) Higher than 0°C
B) Lower than 0°C
C) Exactly 0°C
D) Dependent on the molarity
36. For a non-volatile, non-electrolyte solute, the freezing point depression is directly proportional to:
A) The mole fraction of the solvent
B) The molality of the solution
C) The molarity of the solution
D) The vapor pressure of the solution
37. The formula for freezing point depression is ΔTf = Kf * m. What does 'm' represent?
A) Molarity of the solution
B) Molality of the solution
C) Mole fraction of the solute
D) Mass of the solute
38. Which of the following units is commonly used for Kf?
A) K kg mol⁻¹
B) mol kg⁻¹ K
C) K mol⁻¹ kg
D) mol K kg⁻¹
39. The molal freezing point depression constant (Kf) is also known as:
A) Ebullioscopic constant
B) Cryoscopic constant
C) Osmotic coefficient
D) Van't Hoff factor
40. The depression in freezing point of a solvent on dissolving a non-volatile solute is called:
A) Ebullioscopy
B) Osmometry
C) Cryoscopy
D) Viscosity
41. Adding a non-volatile solute to a solvent will generally:
A) Increase the boiling point and decrease the freezing point
B) Decrease the boiling point and increase the freezing point
C) Increase the boiling point and increase the freezing point
D) Decrease the boiling point and decrease the freezing point
42. For a non-volatile, non-electrolyte solute, the boiling point elevation is directly proportional to:
A) The mole fraction of the solvent
B) The molality of the solution
C) The molarity of the solution
D) The vapor pressure of the solvent
43. The formula for boiling point elevation is ΔTb = Kb * m. What does 'm' represent?
A) Molarity of the solution
B) Molality of the solution
C) Mole fraction of the solute
D) Mass of the solvent
44. Which of the following units is commonly used for Kb?
A) K kg mol⁻¹
B) mol kg⁻¹ K
C) K mol⁻¹ kg
D) mol K kg⁻¹
45. The molal boiling point elevation constant (Kb) is also known as:
A) Ebullioscopic constant
B) Cryoscopic constant
C) Osmotic coefficient
D) Van't Hoff factor
46. Which factor directly influences the boiling point elevation of a solution?
A) Nature of the solvent
B) Concentration of solute particles
C) Pressure of the atmosphere
D) Chemical reactivity of the solute
47. The elevation in boiling point of a solvent on dissolving a non-volatile solute is called:
A) Molality
B) Ebullioscopy
C) Cryoscopy
D) Osmometry
48. Which of the following is NOT a colligative property?
A) Boiling point elevation
B) Freezing point depression
C) Osmotic pressure
D) Surface tension
49. What is the primary definition of a colligative property?
A) A property that depends on the chemical nature of the solute.
B) A property that depends on the concentration of solute particles, irrespective of their identity.
C) A property that depends on the volume of the solvent.
D) A property that depends on the temperature of the solution.
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