Question 1

How many moles of KF are contained in 347 g of water in a 0.175 m KF solution?

Accepted Answer

A)   1.65 × 10-2 mol KF
B)   5.04 × 10-2 mol KF
C)   6.07 × 10-2 mol KF
D)   3.22 × 10-2 mol KF
E)   1.98 × 10-2 mol KFF) B) and E)
G) A) and D)

Question 2

A solution of LiCl in water is 20.0 wt% LiCl.What is the mole fraction of LiCl?

Accepted Answer

A)   0.0960
B)   0.106
C)   0.472
D)   4.44E) B) and C)
F) All of the above

Question 3

Match between columns Premises: 0.020 m NH₄Cl 0.0050 m CO₂ 0.050 m NaCl 0.010 m Al(NO₃)₃ 0.050 m C₆H₁₂O₆(aqueous)

Accepted Answer

The Answer of largest van't Hoff factor and solution that is...

Question 4

A solution is 0.0480 m LiF.What is the molarity of the solution if the density is 1.10 g/mL?

Accepted Answer

A)   0.0441 M
B)   0.0480 M
C)   0.0436 M
D)   0.0528 M
E)   0.0417 MF) None of the above
G) B) and C)

Question 5

Choose the aqueous solution below with the highest freezing point.These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable.

Accepted Answer

A)   0.200 m Mg(ClO4) 2
B)   0.200 m Na3PO3
C)   0.200 m HOCH2CH2OH
D)   0.200 m Ba(NO3) 2
E)   These all have the same freezing point.F) A) and D)
G) A) and B)

Question 6

Choose the statement below that is TRUE.

Accepted Answer

A)   A solution will form between two substances if the solute-solvent interactions are of comparable strength to the solute-solute and solvent-solvent interactions.
B)   A solution will form between two substances if the solute-solvent interactions are small enough to be overcome by the solute-solute and solvent-solvent interactions.
C)   A solution will form between two substances if the solute-solute interactions are strong enough to overcome the solvent-solvent interactions.
D)   A solution will form between two substances only if the solvent-solvent interactions are weak enough to overcome the solute-solvent interactions.
E)   None of the above are true.F) B) and E)
G) A) and B)

Question 7

The vapor pressure of a solution is always that of the pure solvent

Accepted Answer

A)   equal to
B)   twice
C)   one half
D)   higher than
E)   lower thanF) All of the above
G) A) and E)

Question 8

What is the freezing point of a solution of 7.15 g MgCl2 in 100 g of water? Kf for water is1.86°C/m.

Accepted Answer

A)   -0.140°C
B)   - 1.40°C
C)   - 2.80°C
D)   - 4.18°CE) A) and B)
F) B) and C)

Question 9

A solution is prepared by dissolving 76.3 g NaI in 545 g of water.Determine the mole fraction of NaI if the final volume of the solution is 576 mL.

Accepted Answer

A)   6.04 × 10-3
B)   1.65 × 10-2
C)   1.40 × 10-3
D)   1.32 × 10-2
E)   8.84 × 10-2F) D) and E)
G) C) and E)

Question 10

What is the expected freezing point of a 0.50 m solution of Li2SO4 in water? Kf for water is 1.86°C/m.

Accepted Answer

A)   -0.93°C
B)   -1.9°C
C)   -2.8°C
D)   -6.5°CE) B) and C)
F) A) and D)

Question 11

Choose the aqueous solution below with the lowest freezing point.These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable.

Accepted Answer

A)   0.075 m Li Cl
B)   0.075 m (NH4) 3PO4
C)   0.075 m NaBrO4
D)   0.075 m KCN
E)   0.075 m KNO2F) A) and C)
G) A) and E)

Question 12

Calculate the mole fraction of the total ions in an aqueous solution prepared by dissolving 0.400 moles of Ca F2 in 850.0 g of water.

Accepted Answer

A)   0.00841
B)   0.0270
C)   0.00900
D)   0.0248
E)   0.0167F) A) and E)
G) A) and D)

Question 13

A solution is prepared by dissolving 1.928 g of KNO3 into enough water to make 651 mL.What is the molarity of the solution?

Accepted Answer

A)   0.159 M
B)   0.381 M
C)   0.0293 M
D)   2.48 M
E)   0.0832 MF) B) and D)
G) A) and B)

Question 14

Which of the following statements is generally TRUE?

Accepted Answer

A)   The solubility of a solid is not dependent on either temperature or pressure.
B)   The solubility of a solid is highly dependent on pressure.
C)   The solubility of a solid is highly dependent on both pressure and temperature.
D)   The solubility of a solid is highly dependent on temperature.
E)   None of the above.F) A) and C)
G) C) and D)

Question 15

Calculate the molality of a solution formed by dissolving 34.8 g of LiI in 500.0 mL of water.

Accepted Answer

A)   0.254 m
B)   0.130 m
C)   0.696 m
D)   0.260 m
E)   0.520 mF) All of the above
G) B) and C)

Question 16

Explain why the van't Hoff factor for MgCl2 is less than it's predicted value.

Accepted Answer

The hydrated Mg²⁺ and Cl⁻ ions ...

Question 17

Determine the solubility of N2 in water exposed to air at 25°C if the atmospheric pressure is 2.0 atm.Assume that the mole fraction of nitrogen is 0.78 in air and the Henry's law constant for nitrogen in water at this temperature is 6.1 × 10-4 M/atm.

Accepted Answer

A)   1.6 × 10-4 M
B)   6.4 × 10-4 M
C)   9.5 × 10-4 M
D)   1.1 × 10-4 M
E)   1.2 × 10-4 MF) A) and C)
G) B) and E)

Question 18

Identify the compound whose solubility decreases with increasing temperature.

Accepted Answer

A)   Na2SO4
B)   K2Cr2O7
C)   NaNO3
D)   KClO3
E)   CaCl2F) A) and B)
G) D) and E)

Question 19

Calculate the freezing point of a solution of 40.0 g methyl salicylate,C7H6O2,dissolved in 800.g of benzene,C6H6.Kf for benzene is 5.10°C/m and the freezing point is 5.50°C for benzene.

Accepted Answer

A)   - 2.09°C
B)   2.09°C
C)   3.41°C
D)   7.59°CE) B) and C)
F) A) and B)

Question 20

A 4.55 L sample of water contains 0.115 g of sodium ions.Determine the concentration of sodium ions in ppm if the density of the solution is 1.00 g/mL.

Accepted Answer

A)   52.3 ppm
B)   13.2 ppm
C)   12.7 ppm
D)   25.3 ppm
E)   36.5 ppmF) A) and B)
G) A) and C)

Exam 14: Solutions

Which of the following statements is generally TRUE?

Correct Answer
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A 4.55 L sample of water contains 0.115 g of sodium ions.Determine the concentration of sodium ions in ppm if the density of the solution is 1.00 g/mL.

Correct Answer
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Calculate the freezing point of a solution of 40.0 g methyl salicylate,C₇H₆O₂,dissolved in 800.g of benzene,C₆H₆.K_f for benzene is 5.10°C/m and the freezing point is 5.50°C for benzene.

Correct Answer
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Choose the aqueous solution below with the highest freezing point.These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable.

Correct Answer
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What is the freezing point of a solution of 7.15 g MgCl₂ in 100 g of water? K_f for water is1.86°C/m.

Correct Answer
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A solution of LiCl in water is 20.0 wt% LiCl.What is the mole fraction of LiCl?

Correct Answer
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A solution is prepared by dissolving 76.3 g NaI in 545 g of water.Determine the mole fraction of NaI if the final volume of the solution is 576 mL.

Correct Answer
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How many moles of KF are contained in 347 g of water in a 0.175 m KF solution?

Correct Answer
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Determine the solubility of N₂ in water exposed to air at 25°C if the atmospheric pressure is 2.0 atm.Assume that the mole fraction of nitrogen is 0.78 in air and the Henry's law constant for nitrogen in water at this temperature is 6.1 × 10^-4 M/atm.

Correct Answer
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Explain why the van't Hoff factor for MgCl₂ is less than it's predicted value.

Correct Answer
verified
The hydrated Mg²⁺ and Cl⁻ ions ...
View Answer

Identify the compound whose solubility decreases with increasing temperature.

Correct Answer
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Choose the statement below that is TRUE.

Correct Answer
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Calculate the molality of a solution formed by dissolving 34.8 g of LiI in 500.0 mL of water.

Correct Answer
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Calculate the mole fraction of the total ions in an aqueous solution prepared by dissolving 0.400 moles of Ca F₂ in 850.0 g of water.

Correct Answer
verified

Match the following.

A solution is 0.0480 m LiF.What is the molarity of the solution if the density is 1.10 g/mL?

Correct Answer
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What is the expected freezing point of a 0.50 m solution of Li₂SO₄ in water? K_f for water is 1.86°C/m.

Correct Answer
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A solution is prepared by dissolving 1.928 g of KNO3 into enough water to make 651 mL.What is the molarity of the solution?

Correct Answer
verified

The vapor pressure of a solution is always that of the pure solvent

Correct Answer
verified

Choose the aqueous solution below with the lowest freezing point.These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable.

Correct Answer
verified

Exam 14: Solutions

Which of the following statements is generally TRUE?

Correct AnswerverifiedShow Answer

A 4.55 L sample of water contains 0.115 g of sodium ions.Determine the concentration of sodium ions in ppm if the density of the solution is 1.00 g/mL.

Correct AnswerverifiedShow Answer

Calculate the freezing point of a solution of 40.0 g methyl salicylate,C7H6O2,dissolved in 800.g of benzene,C6H6.Kf for benzene is 5.10°C/m and the freezing point is 5.50°C for benzene.

Correct AnswerverifiedShow Answer

Choose the aqueous solution below with the highest freezing point.These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable.

Correct AnswerverifiedShow Answer

What is the freezing point of a solution of 7.15 g MgCl2 in 100 g of water? Kf for water is1.86°C/m.

Correct AnswerverifiedShow Answer

A solution of LiCl in water is 20.0 wt% LiCl.What is the mole fraction of LiCl?

Correct AnswerverifiedShow Answer

A solution is prepared by dissolving 76.3 g NaI in 545 g of water.Determine the mole fraction of NaI if the final volume of the solution is 576 mL.

Correct AnswerverifiedShow Answer

How many moles of KF are contained in 347 g of water in a 0.175 m KF solution?

Correct AnswerverifiedShow Answer

Determine the solubility of N2 in water exposed to air at 25°C if the atmospheric pressure is 2.0 atm.Assume that the mole fraction of nitrogen is 0.78 in air and the Henry's law constant for nitrogen in water at this temperature is 6.1 × 10-4 M/atm.

Correct AnswerverifiedShow Answer

Explain why the van't Hoff factor for MgCl2 is less than it's predicted value.

Correct AnswerverifiedThe hydrated Mg2⁺ and Cl⁻ ions ...View AnswerShow Answer

Identify the compound whose solubility decreases with increasing temperature.

Correct AnswerverifiedShow Answer

Choose the statement below that is TRUE.

Correct AnswerverifiedShow Answer

Calculate the molality of a solution formed by dissolving 34.8 g of LiI in 500.0 mL of water.

Correct AnswerverifiedShow Answer

Calculate the mole fraction of the total ions in an aqueous solution prepared by dissolving 0.400 moles of Ca F2 in 850.0 g of water.

Correct AnswerverifiedShow Answer

Match the following.

A solution is 0.0480 m LiF.What is the molarity of the solution if the density is 1.10 g/mL?

Correct AnswerverifiedShow Answer

What is the expected freezing point of a 0.50 m solution of Li2SO4 in water? Kf for water is 1.86°C/m.

Correct AnswerverifiedShow Answer

A solution is prepared by dissolving 1.928 g of KNO3 into enough water to make 651 mL.What is the molarity of the solution?

Correct AnswerverifiedShow Answer

The vapor pressure of a solution is always that of the pure solvent

Correct AnswerverifiedShow Answer

Choose the aqueous solution below with the lowest freezing point.These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable.

Correct AnswerverifiedShow Answer

Correct Answer
verified

Correct Answer
verified

Calculate the freezing point of a solution of 40.0 g methyl salicylate,C₇H₆O₂,dissolved in 800.g of benzene,C₆H₆.K_f for benzene is 5.10°C/m and the freezing point is 5.50°C for benzene.

Correct Answer
verified

Correct Answer
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What is the freezing point of a solution of 7.15 g MgCl₂ in 100 g of water? K_f for water is1.86°C/m.

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Determine the solubility of N₂ in water exposed to air at 25°C if the atmospheric pressure is 2.0 atm.Assume that the mole fraction of nitrogen is 0.78 in air and the Henry's law constant for nitrogen in water at this temperature is 6.1 × 10^-4 M/atm.

Correct Answer
verified

Explain why the van't Hoff factor for MgCl₂ is less than it's predicted value.

Correct Answer
verified
The hydrated Mg²⁺ and Cl⁻ ions ...
View Answer

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Calculate the mole fraction of the total ions in an aqueous solution prepared by dissolving 0.400 moles of Ca F₂ in 850.0 g of water.

Correct Answer
verified

Correct Answer
verified

What is the expected freezing point of a 0.50 m solution of Li₂SO₄ in water? K_f for water is 1.86°C/m.

Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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