Question 1

Which of the following liquids will have the lowest freezing point?

Accepted Answer

A)  pure H2O
B)  aqueous glucose (0.60 m) 
C)  aqueous sucrose (0.60 m) 
D)  aqueous FeI3 (0.24 m) 
E)  aqueous KF (0.50 m) F) A) and C)
G) B) and E)

Question 2

Which one of the following is most soluble in water?

Accepted Answer

A)  CH3OH
B)  CH3CH2CH2OH
C)  CH3CH2OH
D)  CH3CH2CH2CH2OH
E)  CH3CH2CH2CH2CH2OHF) A) and B)
G) C) and D)

Question 3

The mole fraction of urea (MW = 60.0 g/mol) in a solution prepared by dissolving 16 g of urea in 39g of H2O is __________.

Accepted Answer

A)  0.58
B)  0.37
C)  0.13
D)  0.11
E)  9.1F) A) and B)
G) A) and C)

Question 4

The concentration of nitrate ion in a solution that contains 0.900 M aluminum nitrate is _______ M.

Accepted Answer

A)  0.900
B)  0.450
C)  0.300
D)  2.70
E)  1.80F) A) and B)
G) A) and C)

Question 5

Calculate the molality of a 10.0% (by mass) aqueous solution of hydrochloric acid.

Accepted Answer

A)  0.274 m
B)  2.74 m
C)  3.05 m
D)  4.33 m
E)  The density of the solution is needed to solve the problem.F) B) and E)
G) A) and E)

Question 6

On a clear day at sea level, with a temperature of 25°C, the partial pressure of N2 in air is 0.78 atm and the concentration of nitrogen in water is 5.3 × 10-4 M. When the partial pressure of N2 is __________ atm, the concentration in water is 1.1 × 10-3 M.

Accepted Answer

A)  0.63
B)  0.78
C)  1.0
D)  2.1
E)  1.6F) A) and E)
G) B) and E)

Question 7

The molarity of urea in a solution prepared by dissolving 16 g of urea (MW = 60.0 g/mol) in 39g of H2O is __________ M. The density of the solution is 1.3 g/mL.

Accepted Answer

A)  0.11
B)  3.7
C)  6.8
D)  6.3
E)  0.16F) None of the above
G) A) and E)

Question 8

Determine the freezing point (°C) of a 0.015 molal aqueous solution of MgSO4. Assume i = 2.0 for MgSO4. The molal freezing-point-depression constant of water is 1.86°C/m.

Accepted Answer

A)  -0.056
B)  -0.028
C)  -0.17
D)  -0.084
E)  0.000F) A) and B)
G) B) and E)

Question 9

For a dilute aqueous solution, a concentration of 1 ppb also corresponds to a concentration of 1 __________ per liter of solution.

Accepted Answer

The answer of For a dilute aqueous solution, a concentration...

Question 10

The vapor pressure of pure water at 25°C is 23.8 torr. What is the vapor pressure (torr) of water above a solution prepared by dissolving 18.0 g of glucose (a nonelectrolyte, MW = 180.0 g/mol) in 95.0g of water?

Accepted Answer

A)  24.3
B)  23.4
C)  0.451
D)  0.443
E)  23.8F) A) and E)
G) A) and D)

Question 11

A supersaturated solution __________.

Accepted Answer

A)  is one with more than one solute
B)  is one that has been heated
C)  is one with a higher concentration than the solubility
D)  must be in contact with undissolved solid
E)  exists only in theory and cannot actually be preparedF) A) and D)
G) A) and E)

Question 12

The concentration of urea in a solution prepared by dissolving 16 g of urea in 20 g of H2O is __________% by mass. The molar mass of urea is 60.0 g/mol.

Accepted Answer

A)  44
B)  80
C)  0.44
D)  0.80
E)  0.48F) C) and E)
G) D) and E)

Question 13

The Henry's law constant for helium gas in water at 30°C is 3.70 × 10-4 M/atm. When the partial pressure of helium above a sample of water is 0.650 atm, the concentration of helium in the water is __________ M.

Accepted Answer

A)  5.69 × 10-4
B)  1.76 × 103
C)  1.30
D)  2.41 × 10-4
E)  3.70 × 10-4F) A) and C)
G) B) and D)

Question 14

A solution is prepared by dissolving 23.7 g of CaCl2 in 375 g of water. The density of the resulting solution is 1.05 g/mL. The concentration of Cl- in this solution is __________ M.

Accepted Answer

A)  0.214
B)  0.562
C)  1.12
D)  1.20
E)  6.64 × 10-2F) B) and D)
G) B) and E)

Question 15

A solution is prepared by dissolving 23.7 g of CaCl2 in 375 g of water. The density of the resulting solution is 1.05 g/mL. The concentration of CaCl2 in this solution is __________ molar.

Accepted Answer

A)  0.564
B)  0.571
C)  0.569
D)  0.537
E)  0.214F) B) and C)
G) C) and D)

Question 16

Which one of the following substances is more likely to dissolve in CCl4?

Accepted Answer

A)  CBr4
B)  HBr
C)  HCl
D)  CH3CH2OH
E)  NaClF) B) and E)
G) None of the above

Question 17

A solution contains 28% phosphoric acid by mass. This means that __________.

Accepted Answer

A)  1 mL of this solution contains 28 g of phosphoric acid
B)  1 L of this solution has a mass of 28 g
C)  100 g of this solution contains 28 g of phosphoric acid
D)  1 L of this solution contains 28 mL of phosphoric acid
E)  the density of this solution is 2.8 g/mLF) D) and E)
G) A) and B)

Question 18

An aqueous solution of a soluble compound (a nonelectrolyte) is prepared by dissolving 33.2 g of the compound in sufficient water to form 250 mL of solution. The solution has an osmotic pressure of 1.2 atm at25°C. What is the molar mass (g/mole) of the compound?

Accepted Answer

A)  1.0 × 103
B)  2.7 × 103
C)  2.3 × 102
D)  6.8 × 102
E)  28F) C) and D)
G) A) and D)

Question 19

The concentration of urea (MW = 60.0 g/mol) in a solution prepared by dissolving 16 g of urea in 39g of H2O is __________ molal.

Accepted Answer

A)  96
B)  6.8
C)  0.68
D)  6.3
E)  0.11F) B) and D)
G) C) and E)

Question 20

Adding a nonvolatile solute to a solution decreases the vapor pressure of the solution.

Accepted Answer

A) True 
 B)False

Exam 13: Properties of Solutions

Which one of the following is most soluble in water?

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A solution is prepared by dissolving 23.7 g of CaCl2 in 375 g of water. The density of the resulting solution is 1.05 g/mL. The concentration of Cl- in this solution is __________ M.

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The concentration of urea (MW = 60.0 g/mol) in a solution prepared by dissolving 16 g of urea in 39g of H2O is __________ molal.

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A supersaturated solution __________.

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The mole fraction of urea (MW = 60.0 g/mol) in a solution prepared by dissolving 16 g of urea in 39g of H2O is __________.

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Which one of the following substances is more likely to dissolve in CCl4?

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For a dilute aqueous solution, a concentration of 1 ppb also corresponds to a concentration of 1 __________ per liter of solution.

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The concentration of nitrate ion in a solution that contains 0.900 M aluminum nitrate is _______ M.

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An aqueous solution of a soluble compound (a nonelectrolyte) is prepared by dissolving 33.2 g of the compound in sufficient water to form 250 mL of solution. The solution has an osmotic pressure of 1.2 atm at25°C. What is the molar mass (g/mole) of the compound?

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The concentration of urea in a solution prepared by dissolving 16 g of urea in 20 g of H2O is __________% by mass. The molar mass of urea is 60.0 g/mol.

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The Henry's law constant for helium gas in water at 30°C is 3.70 × 10-4 M/atm. When the partial pressure of helium above a sample of water is 0.650 atm, the concentration of helium in the water is __________ M.

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Which of the following liquids will have the lowest freezing point?

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A solution contains 28% phosphoric acid by mass. This means that __________.

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A solution is prepared by dissolving 23.7 g of CaCl2 in 375 g of water. The density of the resulting solution is 1.05 g/mL. The concentration of CaCl2 in this solution is __________ molar.

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Calculate the molality of a 10.0% (by mass) aqueous solution of hydrochloric acid.

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The molarity of urea in a solution prepared by dissolving 16 g of urea (MW = 60.0 g/mol) in 39g of H2O is __________ M. The density of the solution is 1.3 g/mL.

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The vapor pressure of pure water at 25°C is 23.8 torr. What is the vapor pressure (torr) of water above a solution prepared by dissolving 18.0 g of glucose (a nonelectrolyte, MW = 180.0 g/mol) in 95.0g of water?

Correct AnswerverifiedShow Answer

On a clear day at sea level, with a temperature of 25°C, the partial pressure of N2 in air is 0.78 atm and the concentration of nitrogen in water is 5.3 × 10-4 M. When the partial pressure of N2 is __________ atm, the concentration in water is 1.1 × 10-3 M.

Correct AnswerverifiedShow Answer

Adding a nonvolatile solute to a solution decreases the vapor pressure of the solution.

Correct AnswerverifiedShow Answer

Determine the freezing point (°C) of a 0.015 molal aqueous solution of MgSO4. Assume i = 2.0 for MgSO4. The molal freezing-point-depression constant of water is 1.86°C/m.

Correct AnswerverifiedShow Answer

Correct Answer
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A solution is prepared by dissolving 23.7 g of CaCl₂ in 375 g of water. The density of the resulting solution is 1.05 g/mL. The concentration of Cl^- in this solution is __________ M.

Correct Answer
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The concentration of urea (MW = 60.0 g/mol) in a solution prepared by dissolving 16 g of urea in 39g of H₂O is __________ molal.

Correct Answer
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Correct Answer
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The mole fraction of urea (MW = 60.0 g/mol) in a solution prepared by dissolving 16 g of urea in 39g of H₂O is __________.

Correct Answer
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Which one of the following substances is more likely to dissolve in CCl₄?

Correct Answer
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Correct Answer
verified

The concentration of urea in a solution prepared by dissolving 16 g of urea in 20 g of H₂O is __________% by mass. The molar mass of urea is 60.0 g/mol.

Correct Answer
verified

The Henry's law constant for helium gas in water at 30°C is 3.70 × 10^-4 M/atm. When the partial pressure of helium above a sample of water is 0.650 atm, the concentration of helium in the water is __________ M.

Correct Answer
verified

Correct Answer
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Correct Answer
verified

A solution is prepared by dissolving 23.7 g of CaCl₂ in 375 g of water. The density of the resulting solution is 1.05 g/mL. The concentration of CaCl₂ in this solution is __________ molar.

Correct Answer
verified

Correct Answer
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The molarity of urea in a solution prepared by dissolving 16 g of urea (MW = 60.0 g/mol) in 39g of H₂O is __________ M. The density of the solution is 1.3 g/mL.

Correct Answer
verified

Correct Answer
verified

On a clear day at sea level, with a temperature of 25°C, the partial pressure of N₂ in air is 0.78 atm and the concentration of nitrogen in water is 5.3 × 10^-4 M. When the partial pressure of N₂ is __________ atm, the concentration in water is 1.1 × 10^-³ M.

Correct Answer
verified

Correct Answer
verified

Determine the freezing point (°C) of a 0.015 molal aqueous solution of MgSO₄. Assume i = 2.0 for MgSO₄. The molal freezing-point-depression constant of water is 1.86°C/m.

Correct Answer
verified