Q. If 0.5 moles of a non-volatile solute are dissolved in 1 kg of water, what is the expected change in boiling point? (Kb for water = 0.52 °C kg/mol) (2021)
A.
0.26 °C
B.
0.52 °C
C.
1.04 °C
D.
0.78 °C
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Solution
Boiling point elevation = i * Kb * m = 1 * 0.52 * 0.5 = 0.26 °C, so change = 0.52 °C.
Correct Answer: C — 1.04 °C
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Q. If 0.5 moles of a non-volatile solute are dissolved in 1 kg of water, what is the expected vapor pressure lowering? (2021)
A.
0.5 P0
B.
0.25 P0
C.
0.75 P0
D.
0.1 P0
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Solution
Vapor pressure lowering = X_solute * P0 = (0.5 / (0.5 + 55.5)) * P0 ≈ 0.25 P0.
Correct Answer: B — 0.25 P0
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Q. If 0.5 moles of a non-volatile solute is dissolved in 1 kg of water, what is the expected vapor pressure lowering? (2020)
A.
0.5 P0
B.
0.25 P0
C.
0.75 P0
D.
0.1 P0
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Solution
Vapor pressure lowering = (moles of solute / moles of solvent) * P0 = (0.5 / 55.5) * P0 ≈ 0.25 P0.
Correct Answer: B — 0.25 P0
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Q. If 1 mole of a non-volatile solute is dissolved in 1 kg of water, what is the expected freezing point depression? (2019)
A.
1.86 °C
B.
3.72 °C
C.
0.93 °C
D.
2.0 °C
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Solution
Freezing point depression (ΔTf) = i * Kf * m = 1 * 1.86 °C kg/mol * 1 mol/kg = 1.86 °C.
Correct Answer: A — 1.86 °C
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Q. If the freezing point of a solution is -5°C, what is the molality of the solution if the freezing point depression constant (Kf) is 1.86°C kg/mol? (2022)
A.
1.34 m
B.
2.68 m
C.
0.5 m
D.
3.72 m
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Solution
ΔTf = Kf * m; -5 = -1.86 * m; m = 5 / 1.86 = 2.68 m.
Correct Answer: B — 2.68 m
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Q. If the freezing point of pure water is 0 °C, what will be the freezing point of a solution containing 1 mole of NaCl in 1 kg of water? (2023)
A.
-1.86 °C
B.
-3.72 °C
C.
-2.26 °C
D.
-0.93 °C
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Solution
Freezing point depression = i * Kf * m = 2 * 1.86 °C kg/mol * 1 mol/kg = 3.72 °C. Thus, freezing point = 0 - 3.72 = -3.72 °C.
Correct Answer: B — -3.72 °C
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Q. What is the boiling point elevation for a solution with 0.5 moles of a non-volatile solute in 1 kg of water? (Kb for water = 0.512 °C kg/mol) (2022)
A.
0.256 °C
B.
0.512 °C
C.
1.024 °C
D.
0.128 °C
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Solution
Boiling point elevation (ΔTb) = Kb * m = 0.512 °C kg/mol * 0.5 mol/kg = 0.256 °C.
Correct Answer: A — 0.256 °C
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Q. What is the effect of adding a non-volatile solute to a solvent on its boiling point? (2019)
A.
Increases boiling point
B.
Decreases boiling point
C.
No effect
D.
Depends on the solute
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Solution
Adding a non-volatile solute increases the boiling point due to boiling point elevation.
Correct Answer: A — Increases boiling point
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Q. What is the effect of adding a non-volatile solute to a solvent on its vapor pressure? (2023)
A.
Increases vapor pressure
B.
Decreases vapor pressure
C.
No effect
D.
Depends on the solute
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Solution
Adding a non-volatile solute decreases the vapor pressure of the solvent due to the solute particles occupying space at the surface.
Correct Answer: B — Decreases vapor pressure
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Q. What is the freezing point depression of a solution containing 1 mole of NaCl in 1 kg of water? (2022)
A.
1.86 °C
B.
3.72 °C
C.
2.52 °C
D.
0.93 °C
Show solution
Solution
Freezing point depression = i * Kf * m = 2 * 1.86 * 1 = 3.72 °C (i = 2 for NaCl).
Correct Answer: A — 1.86 °C
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Q. What is the freezing point depression of a solution containing 3 moles of KCl in 1 kg of water? (Kf for water = 1.86 °C kg/mol) (2022)
A.
5.58 °C
B.
3.72 °C
C.
1.86 °C
D.
7.44 °C
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Solution
Freezing point depression = i * Kf * m = 3 * 1.86 * 3 = 5.58 °C (i = 2 for KCl).
Correct Answer: A — 5.58 °C
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Q. What is the osmotic pressure of a solution containing 0.1 moles of glucose in 1 L of solution at 25 °C? (R = 0.0821 L·atm/(K·mol)) (2020)
A.
2.03 atm
B.
1.96 atm
C.
0.82 atm
D.
0.25 atm
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Solution
Osmotic pressure (π) = nRT/V = (0.1 mol)(0.0821 L·atm/(K·mol))(298 K) = 2.03 atm.
Correct Answer: A — 2.03 atm
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Q. What is the osmotic pressure of a solution containing 0.1 moles of glucose in 1 liter of solution at 25 °C? (R = 0.0821 L atm/K mol) (2020)
A.
2.06 atm
B.
0.82 atm
C.
1.01 atm
D.
0.25 atm
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Solution
Osmotic pressure (π) = nRT/V = (0.1 mol)(0.0821 L atm/K mol)(298 K) = 2.06 atm.
Correct Answer: A — 2.06 atm
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Q. What is the osmotic pressure of a solution containing 0.1 moles of solute in 1 liter of solution at 25 °C? (R = 0.0821 L·atm/(K·mol)) (2020)
A.
2.5 atm
B.
0.82 atm
C.
1.0 atm
D.
0.25 atm
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Solution
Osmotic pressure (π) = nRT/V = (0.1 moles * 0.0821 * 298) / 1 = 2.5 atm.
Correct Answer: A — 2.5 atm
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Q. What is the osmotic pressure of a solution containing 0.5 moles of solute in 1 liter of solution at 25 °C? (2021)
A.
12.3 atm
B.
24.6 atm
C.
6.1 atm
D.
3.1 atm
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Solution
Osmotic pressure (π) = nRT/V = (0.5 moles)(0.0821 L·atm/(K·mol))(298 K) = 12.3 atm.
Correct Answer: B — 24.6 atm
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Q. What is the osmotic pressure of a solution containing 0.5 moles of solute in 1 liter of solution at 25 °C? (R = 0.0821 L·atm/(K·mol)) (2021)
A.
12.3 atm
B.
10.2 atm
C.
8.2 atm
D.
6.1 atm
Show solution
Solution
Osmotic pressure (π) = nRT/V = (0.5 moles * 0.0821 L·atm/(K·mol) * 298 K) / 1 L = 12.3 atm.
Correct Answer: B — 10.2 atm
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Q. What is the osmotic pressure of a solution containing 2 moles of glucose in 1 liter of solution at 25 °C? (2021)
A.
0.0821 atm
B.
1.0 atm
C.
2.0 atm
D.
4.0 atm
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Solution
Osmotic pressure (π) = iCRT = 1 * 2 * 0.0821 * 298 = 4.0 atm (i = 1 for glucose).
Correct Answer: C — 2.0 atm
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Q. What is the osmotic pressure of a solution containing 2 moles of glucose in 1 liter of solution at 25 °C? (R = 0.0821 L·atm/(K·mol)) (2020)
A.
0.82 atm
B.
1.64 atm
C.
2.46 atm
D.
4.92 atm
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Solution
Osmotic pressure (π) = nRT/V = (2 moles * 0.0821 L·atm/(K·mol) * 298 K) / 1 L = 4.92 atm.
Correct Answer: B — 1.64 atm
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Q. What is the relationship between the vapor pressure of a solution and the mole fraction of the solvent? (2023)
A.
Directly proportional
B.
Inversely proportional
C.
No relationship
D.
Exponential relationship
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Solution
The vapor pressure of a solution is directly proportional to the mole fraction of the solvent.
Correct Answer: A — Directly proportional
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Q. What is the van 't Hoff factor (i) for a non-electrolyte solute? (2023)
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Solution
The van 't Hoff factor (i) for a non-electrolyte solute is 1, as it does not dissociate into ions.
Correct Answer: A — 1
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Q. What is the van 't Hoff factor (i) for a solution of glucose (C6H12O6)? (2023)
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Solution
Glucose does not dissociate in solution, so the van 't Hoff factor (i) = 1.
Correct Answer: A — 1
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Q. What is the van 't Hoff factor (i) for a strong electrolyte like Na2SO4 in solution? (2023)
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Solution
Na2SO4 dissociates into 3 ions (2 Na⁺ and 1 SO4²⁻), so i = 3.
Correct Answer: C — 3
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Q. What is the vapor pressure of a solution containing 1 mole of solute in 10 moles of solvent, assuming ideal behavior? (2019)
A.
0.1 P0
B.
0.9 P0
C.
0.5 P0
D.
0.2 P0
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Solution
Using Raoult's law, the vapor pressure of the solution = (moles of solvent / total moles) * P0 = (10 / 11) * P0 ≈ 0.909 P0.
Correct Answer: B — 0.9 P0
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Q. What is the vapor pressure of a solution containing 1 mole of solute in 9 moles of solvent, assuming ideal behavior? (2019)
A.
0.1 P0
B.
0.9 P0
C.
0.5 P0
D.
0.2 P0
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Solution
Using Raoult's law, the vapor pressure of the solution = (moles of solvent / total moles) * P0 = (9 / 10) * P0 = 0.9 P0.
Correct Answer: B — 0.9 P0
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Q. What is the vapor pressure of a solution containing 2 moles of solute and 3 moles of solvent, assuming ideal behavior? (2022)
A.
0.4 P0
B.
0.6 P0
C.
0.2 P0
D.
0.8 P0
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Solution
Vapor pressure of solution = (moles of solvent / total moles) * P0 = (3 / (2 + 3)) * P0 = 0.6 P0.
Correct Answer: B — 0.6 P0
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Q. What is the vapor pressure of a solution containing 2 moles of solute and 4 moles of solvent compared to pure solvent? (2022)
A.
1/3
B.
1/2
C.
2/3
D.
1/4
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Solution
Vapor pressure lowering = (moles of solute / total moles) = 2 / (2 + 4) = 2/6 = 1/3. Thus, vapor pressure is 1/2 of pure solvent.
Correct Answer: B — 1/2
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Q. What is the vapor pressure of a solution containing 2 moles of solute and 4 moles of solvent, assuming ideal behavior? (2022)
A.
0.33 P0
B.
0.50 P0
C.
0.67 P0
D.
0.75 P0
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Solution
Vapor pressure = (moles of solvent / total moles) * P0 = (4 / (2 + 4)) * P0 = (4/6) * P0 = 0.67 P0.
Correct Answer: C — 0.67 P0
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Q. Which of the following statements about solutions is true? (2023)
A.
Solutes increase the boiling point of solvents
B.
Solutes decrease the freezing point of solvents
C.
Both A and B
D.
Neither A nor B
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Solution
Both statements are true; solutes affect the colligative properties of solvents.
Correct Answer: C — Both A and B
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