Question 1

When 12.1 g of the sugar sucrose (a nonelectrolyte) is dissolved in exactly 800.0 g of water, the solution has a freezing point of -0.082°C.What is the molar mass of sucrose? Kf of water is 1.86°C/m.

Accepted Answer

A)  426 g
B)  99.2 g
C)  178 g
D)  266 g
E)  343 gF) A) and E)
G) None of the above

Question 2

A solution made of pentane and hexane has a mole fraction, X = 0.250 of pentane.Which substance is the solvent?

Accepted Answer

The answer of A solution made of pentane and hexane...

Question 3

A 100.-mL sample of water is taken from the Pacific Ocean, and the water is allowed to evaporate.The salts that remain (mostly NaCl)have a mass of 3.85 g.Calculate the original concentration of NaCl, in g per liter, in the water sample.

Accepted Answer

The answer of A 100.-mL sample of water is taken...

Question 4

In which of the following solvents would you expect KBr to be most soluble?

Accepted Answer

A)  C6H14 (hexane) 
B)  CH3CH2OH (ethanol) 
C)  C6H6 (benzene) 
D)  CCl4 (carbon tetrachloride) 
E)  C6H12 (cyclohexane) F) A) and E)
G) B) and C)

Question 5

A 15.00 % by mass solution of lactose (C12H22O11, 342.30 g/mol) in water has a density of 1.0602 g/mL at 20°C.What is the molarity of this solution?

Accepted Answer

A)  0.03097 M
B)  0.4133 M
C)  0.4646 M
D)  1.590 M
E)  3.097 MF) All of the above
G) B) and D)

Question 6

Using your knowledge of osmosis or osmotic pressure explain the following statement: Drinking salt water actually dehydrates our tissues.

Accepted Answer

The water passes fro...

Question 7

A solution is 35.0% by mass carbon tetrachloride (CCl4) in benzene (C6H6) at 20°C.The vapor pressure of pure benzene and pure carbon tetrachloride at this temperature is 74.61 mmHg and 91.32 mmHg, respectively.Calculate the vapor pressure of the solution at 20°C:

Accepted Answer

A)  58.1 mmHg
B)  78.2 mmHg
C)  80.5 mmHg
D)  82.9 mmHg
E)  83.0 mmHgF) C) and E)
G) A) and B)

Question 8

Calculate the mass of solute in the following solution: 50.0 mL of 0.0300 M C12H22O11.

Accepted Answer

Question 9

Assuming 100% dissociation, which of the following compounds is listed correctly with its van't Hoff factor i?

Accepted Answer

A)  Ca(ClO3) 2, i = 2
B)  (NH4) 2SO4, i = 3
C)  (NH4) 3PO4, i = 5
D)  Urea, i = 2
E)  Sc2(SO4) 3, i = 6F) A) and D)
G) C) and D)

Question 10

What is the percent CdSO4 by mass in a 1.00 m aqueous CdSO4 solution?

Accepted Answer

A)  1.00 × 10-3 %
B)  0.100 %
C)  17.2 %
D)  20.8 %
E)  24.4 %F) A) and B)
G) A) and C)

Question 11

How many grams of propanol (C3H7OH, 60.10 g/mol)would be needed to make 750 mL of a solution with an osmotic pressure of 25 atm at 25°C? (R = 0.0821 L.atm/K.mol)

Accepted Answer

Question 12

Oxygen gas makes up 21 % of the atmosphere by volume.What is the solubility of O2(g) in water at 25°C if the atmospheric pressure is 741 mmHg? The Henry's law constant for oxygen gas at 25°C is 1.3 × 10-3 mol/L·atm.

Accepted Answer

A)  2.7 × 10-4 M
B)  1.3 × 10-3 M
C)  6.2 × 10-3 M
D)  9.6 × 10-3 M
E)  0.96 MF) A) and B)
G) None of the above

Question 13

Consider a solution made from a nonvolatile solute and a volatile solvent.Which statement is true?

Accepted Answer

A)  The vapor pressure of the solution is always greater than the vapor pressure of the pure solvent.
B)  The boiling point of the solution is always greater than the boiling point of the pure solvent.
C)  The freezing point of the solution is always greater than the freezing point of the pure solvent.D) B) and C)
E) A) and B)

Question 14

The solubility of gases in water always decreases with increasing temperature.

Accepted Answer

A) True 
 B)False

Question 15

What is the molality of a solution that is 3.68 % by mass calcium chloride.

Accepted Answer

A)  0.0332 m
B)  0.332 m
C)  0.344 m
D)  0.464 m
E)  0.506 mF) B) and C)
G) A) and D)

Question 16

Which of the following concentration units will not change with temperature: molarity, percent mass, mole fraction, and molality.

Accepted Answer

Percent mass, mole f...

Question 17

How many liters of ethylene glycol antifreeze (C2H6O2)would you add to your car radiator containing 15.0 L of water if you needed to protect your engine to -17.8°C? (The density of ethylene glycol is 1.1 g/mL.For water, Kf = 1.86°C/m.)

Accepted Answer

Question 18

Calculate the mass percent of HOCH2CH2OH in a solution made by dissolving 3.2 g of HOCH2CH2OH in 43.5g of water.

Accepted Answer

A)  2.9%
B)  6.9%
C)  7.4%
D)  22%
E)  29%F) None of the above
G) B) and E)

Question 19

The vapor pressure of water at 45.0 °C is 71.93 mmHg.Calculate the vapor pressure of a solution of 1.50m K2CO3 at this temperature (assume 100% dissociation)

Accepted Answer

A)  1.89 mmHg
B)  5.39 mmHg
C)  66.5 mmHg
D)  70.0 mmHg
E)  108 mmHgF) A) and B)
G) A) and D)

Question 20

What is the percent by mass of sodium phosphate in a 0.142 M Na3PO4(aq)solution that has a density of 1.015 g/mL?

Accepted Answer

Exam 12: Physical Properties of Solutions

In which of the following solvents would you expect KBr to be most soluble?

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What is the percent by mass of sodium phosphate in a 0.142 M Na3PO4(aq)solution that has a density of 1.015 g/mL?

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Calculate the mass percent of HOCH2CH2OH in a solution made by dissolving 3.2 g of HOCH2CH2OH in 43.5g of water.

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How many grams of propanol (C3H7OH, 60.10 g/mol)would be needed to make 750 mL of a solution with an osmotic pressure of 25 atm at 25°C? (R = 0.0821 L.atm/K.mol)

Correct AnswerverifiedShow Answer

Calculate the mass of solute in the following solution: 50.0 mL of 0.0300 M C12H22O11.

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What is the percent CdSO4 by mass in a 1.00 m aqueous CdSO4 solution?

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When 12.1 g of the sugar sucrose (a nonelectrolyte) is dissolved in exactly 800.0 g of water, the solution has a freezing point of -0.082°C.What is the molar mass of sucrose? Kf of water is 1.86°C/m.

Correct AnswerverifiedShow Answer

A 100.-mL sample of water is taken from the Pacific Ocean, and the water is allowed to evaporate.The salts that remain (mostly NaCl)have a mass of 3.85 g.Calculate the original concentration of NaCl, in g per liter, in the water sample.

Correct AnswerverifiedShow Answer

Oxygen gas makes up 21 % of the atmosphere by volume.What is the solubility of O2(g) in water at 25°C if the atmospheric pressure is 741 mmHg? The Henry's law constant for oxygen gas at 25°C is 1.3 × 10-3 mol/L·atm.

Correct AnswerverifiedShow Answer

Which of the following concentration units will not change with temperature: molarity, percent mass, mole fraction, and molality.

Correct AnswerverifiedPercent mass, mole f...View AnswerShow Answer

Assuming 100% dissociation, which of the following compounds is listed correctly with its van't Hoff factor i?

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Using your knowledge of osmosis or osmotic pressure explain the following statement: Drinking salt water actually dehydrates our tissues.

Correct AnswerverifiedThe water passes fro...View AnswerShow Answer

A solution made of pentane and hexane has a mole fraction, X = 0.250 of pentane.Which substance is the solvent?

Correct AnswerverifiedShow Answer

How many liters of ethylene glycol antifreeze (C2H6O2)would you add to your car radiator containing 15.0 L of water if you needed to protect your engine to -17.8°C? (The density of ethylene glycol is 1.1 g/mL.For water, Kf = 1.86°C/m.)

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What is the molality of a solution that is 3.68 % by mass calcium chloride.

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A solution is 35.0% by mass carbon tetrachloride (CCl4) in benzene (C6H6) at 20°C.The vapor pressure of pure benzene and pure carbon tetrachloride at this temperature is 74.61 mmHg and 91.32 mmHg, respectively.Calculate the vapor pressure of the solution at 20°C:

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Consider a solution made from a nonvolatile solute and a volatile solvent.Which statement is true?

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The vapor pressure of water at 45.0 °C is 71.93 mmHg.Calculate the vapor pressure of a solution of 1.50m K2CO3 at this temperature (assume 100% dissociation)

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A 15.00 % by mass solution of lactose (C12H22O11, 342.30 g/mol) in water has a density of 1.0602 g/mL at 20°C.What is the molarity of this solution?

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The solubility of gases in water always decreases with increasing temperature.

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What is the percent by mass of sodium phosphate in a 0.142 M Na₃PO₄(aq)solution that has a density of 1.015 g/mL?

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Calculate the mass percent of HOCH₂CH₂OH in a solution made by dissolving 3.2 g of HOCH₂CH₂OH in 43.5g of water.

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How many grams of propanol (C₃H₇OH, 60.10 g/mol)would be needed to make 750 mL of a solution with an osmotic pressure of 25 atm at 25°C? (R = 0.0821 L.atm/K.mol)

Correct Answer
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Calculate the mass of solute in the following solution: 50.0 mL of 0.0300 M C₁₂H₂₂O₁₁.

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What is the percent CdSO₄ by mass in a 1.00 m aqueous CdSO₄solution?

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When 12.1 g of the sugar sucrose (a nonelectrolyte) is dissolved in exactly 800.0 g of water, the solution has a freezing point of -0.082°C.What is the molar mass of sucrose? K_f of water is 1.86°C/m.

Correct Answer
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Correct Answer
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Oxygen gas makes up 21 % of the atmosphere by volume.What is the solubility of O₂(g) in water at 25°C if the atmospheric pressure is 741 mmHg? The Henry's law constant for oxygen gas at 25°C is 1.3 × 10^-3 mol/L·atm.

Correct Answer
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Correct Answer
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Percent mass, mole f...
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The water passes fro...
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How many liters of ethylene glycol antifreeze (C₂H₆O₂)would you add to your car radiator containing 15.0 L of water if you needed to protect your engine to -17.8°C? (The density of ethylene glycol is 1.1 g/mL.For water, K_f = 1.86°C/m.)

Correct Answer
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Correct Answer
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A solution is 35.0% by mass carbon tetrachloride (CCl₄) in benzene (C₆H₆) at 20°C.The vapor pressure of pure benzene and pure carbon tetrachloride at this temperature is 74.61 mmHg and 91.32 mmHg, respectively.Calculate the vapor pressure of the solution at 20°C:

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Correct Answer
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The vapor pressure of water at 45.0 °C is 71.93 mmHg.Calculate the vapor pressure of a solution of 1.50m K₂CO₃ at this temperature (assume 100% dissociation)

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A 15.00 % by mass solution of lactose (C₁₂H₂₂O₁₁, 342.30 g/mol) in water has a density of 1.0602 g/mL at 20°C.What is the molarity of this solution?

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Correct Answer
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