Question 1

Pressure has an appreciable effect on the solubility of __________ in liquids.

Accepted Answer

A) gases 
B) solids 
C) liquids 
D) salts 
E) solids and liquids 
A) gases 
B) solids 
C) liquids 
D) salts 
E) solids and liquids A

Question 2

A solution with a solute concentration greater than the solubility is called a supercritical solution.

Accepted Answer

A) True 
 B)False  False

Question 3

Calculate the mole fraction of phosphoric acid (H3PO4)in a 25.4% (by mass)aqueous solution.

Accepted Answer

A) 0.0589 
B) 0.0626 
C) 0.259 
D) 1.00 
E) 4.14 
A) 0.0589 
B) 0.0626 
C) 0.259 
D) 1.00 
E) 4.14 A

Question 4

The solubility of Ar in water at 25°C is 1.6 × 10-3 M when the pressure of the Ar above the solution is 1.0 atm. The solubility of Ar at a pressure of 2.5 atm is __________ M.

Accepted Answer

A) 1.6 × 103 
B) 6.4 × 10-4 
C) 4.0 × 10-3 
D) 7.5 × 10-2 
E) 1.6 × 10-3 
A) 1.6 × 103 
B) 6.4 × 10-4 
C) 4.0 × 10-3 
D) 7.5 × 10-2 
E) 1.6 × 10-3

Question 5

Which component of air is the primary problem in a condition known as "the bends"?

Accepted Answer

A) O2 
B) CO2 
C) He 
D) N2 
E) CO 
A) O2 
B) CO2 
C) He 
D) N2 
E) CO

Question 6

Calculate the vapor pressure of a solution made by dissolving 109 grams of glucose (molar mass = 180.2 g/mol)in 920.0 ml of water at 25°C. The vapor pressure of pure water at 25°C is 23.76 mm Hg. Assume the density of the solution is 1.00 g/ml.

Accepted Answer

A) 0.278 mm Hg 
B) 0.605 mm Hg 
C) 22.98 mm Hg 
D) 23.48 mm Hg 
E) 23.76 mm Hg 
A) 0.278 mm Hg 
B) 0.605 mm Hg 
C) 22.98 mm Hg 
D) 23.48 mm Hg 
E) 23.76 mm Hg

Question 7

A 0.100 m solution of which one of the following solutes will have the lowest vapor pressure?

Accepted Answer

A) KClO4 
B) Ca(ClO4)2 
C) Al(ClO4)3 
D) sucrose 
E) NaCl 
A) KClO4 
B) Ca(ClO4)2 
C) Al(ClO4)3 
D) sucrose 
E) NaCl

Question 8

Which of the following cannot be a colloid?

Accepted Answer

A) an emulsion 
B) an aerosol 
C) a homogenous mixture 
D) a foam 
E) All of the above are colloids. 
A) an emulsion 
B) an aerosol 
C) a homogenous mixture 
D) a foam 
E) All of the above are colloids.

Question 9

Which one of the following is most soluble in hexane (C6H14)?

Accepted Answer

A) CH3OH 
B) CH3CH2CH2OH 
C) CH3CH2OH 
D) CH3CH2CH2CH2OH 
E) CH3CH2CH2CH2CH2OH 
A) CH3OH 
B) CH3CH2CH2OH 
C) CH3CH2OH 
D) CH3CH2CH2CH2OH 
E) CH3CH2CH2CH2CH2OH

Question 10

The concentration of sodium chloride in an aqueous solution that is 2.23 M and that has a density of 1.01 g/mL is __________% by mass.

Accepted Answer

A) 2.21 
B) 7.83 
C) 45.3 
D) 12.9 
E) 10.1 
A) 2.21 
B) 7.83 
C) 45.3 
D) 12.9 
E) 10.1

Question 11

Which of the following statements is false?

Accepted Answer

A) Nonpolar liquids tend to be insoluble in polar liquids. 
B) The weaker the attraction between the solute and solvent molecules, the greater the solubility. 
C) Substances with similar intermolecular attractive forces tend to be soluble in one another. 
D) The solubility of a gas increases in direct proportion to its partial pressure above the solution. 
E) The solubility of gases in water decreases with increasing temperature. 
A) Nonpolar liquids tend to be insoluble in polar liquids. 
B) The weaker the attraction between the solute and solvent molecules, the greater the solubility. 
C) Substances with similar intermolecular attractive forces tend to be soluble in one another. 
D) The solubility of a gas increases in direct proportion to its partial pressure above the solution. 
E) The solubility of gases in water decreases with increasing temperature.

Question 12

Calculate the freezing point of a 0.08500 m aqueous solution of NaNO3. The molal freezing-point-depression constant of water is 1.86°C/m.

Accepted Answer

A) 0.0425 
B) -0.0790 
C) 0.0790 
D) -0.158 
E) -0.316 
A) 0.0425 
B) -0.0790 
C) 0.0790 
D) -0.158 
E) -0.316

Question 13

A solution is prepared by adding 1.43 mol of KCl to 889 g of water. The concentration of KCl is __________ molal.

Accepted Answer

A) 1.61 × 10-3 
B) 622 
C) 0.622 
D) 1.27 × 103 
E) 1.61 
A) 1.61 × 10-3 
B) 622 
C) 0.622 
D) 1.27 × 103 
E) 1.61

Question 14

Which of the following substances is least likely to dissolve in water?

Accepted Answer

A) HOCH2CH2OH 
B) CHCl3 
C) O 
CH3(CH2)9CH 
D) CH3(CH2)8CH2OH 
E) CCl4 
A) HOCH2CH2OH 
B) CHCl3 
C) O 
CH3(CH2)9CH 
D) CH3(CH2)8CH2OH 
E) CCl4

Question 15

The largest value of the Henry's Law constant for the liquid solvent H2O will be obtained with __________ gas as the solute and a temperature of __________°C.

Accepted Answer

A) C2H4, 45 
B) Ar, 11 
C) HCl, 49 
D) CO2, 32 
E) N2, 15 
A) C2H4, 45 
B) Ar, 11 
C) HCl, 49 
D) CO2, 32 
E) N2, 15

Question 16

What is the mole fraction of sodium chloride in solution that is 13.0% by mass sodium chloride and that has a density of 1.10 g/mL?

Accepted Answer

A) 0.0442 
B) 0.0462 
C) 0.223 
D) 0.483 
E) 0.505 
A) 0.0442 
B) 0.0462 
C) 0.223 
D) 0.483 
E) 0.505

Question 17

Of the concentration units below, only __________ is temperature dependent.

Accepted Answer

A) mass % 
B) ppm 
C) ppb 
D) molarity 
E) molality 
A) mass % 
B) ppm 
C) ppb 
D) molarity 
E) molality

Question 18

A saturated solution __________.

Accepted Answer

A) contains as much solvent as it can hold 
B) contains no double bonds 
C) contains dissolved solute in equilibrium with undissolved solute 
D) will rapidly precipitate if a seed crystal is added 
E) cannot be attained 
A) contains as much solvent as it can hold 
B) contains no double bonds 
C) contains dissolved solute in equilibrium with undissolved solute 
D) will rapidly precipitate if a seed crystal is added 
E) cannot be attained

Question 19

Of the following, a 0.1 M aqueous solution of __________ will have the highest freezing point.

Accepted Answer

A) NaCl 
B) Al(NO3)3 
C) K2CrO4 
D) Na2SO4 
E) sucrose 
A) NaCl 
B) Al(NO3)3 
C) K2CrO4 
D) Na2SO4 
E) sucrose

Question 20

The vapor pressure of pure water at 25°C is 23.8 torr. Determine the vapor pressure (torr)of water at 25°C above a solution prepared by dissolving 21 g of urea (a nonvolatile, non-electrolyte, MW = 60.0g/mol)in 75 g of water.

Accepted Answer

A) 2.9 
B) 0.35 
C) 22 
D) 27 
E) 0.92 
A) 2.9 
B) 0.35 
C) 22 
D) 27 
E) 0.92

Exam 13: Properties of Solutions

Pressure has an appreciable effect on the solubility of __________ in liquids.

A solution with a solute concentration greater than the solubility is called a supercritical solution.

Calculate the mole fraction of phosphoric acid (H3PO4)in a 25.4% (by mass)aqueous solution.

The solubility of Ar in water at 25°C is 1.6 × 10-3 M when the pressure of the Ar above the solution is 1.0 atm. The solubility of Ar at a pressure of 2.5 atm is __________ M.

Which component of air is the primary problem in a condition known as "the bends"?

Calculate the vapor pressure of a solution made by dissolving 109 grams of glucose (molar mass = 180.2 g/mol)in 920.0 ml of water at 25°C. The vapor pressure of pure water at 25°C is 23.76 mm Hg. Assume the density of the solution is 1.00 g/ml.

A 0.100 m solution of which one of the following solutes will have the lowest vapor pressure?

Which of the following cannot be a colloid?

Which one of the following is most soluble in hexane (C6H14)?

The concentration of sodium chloride in an aqueous solution that is 2.23 M and that has a density of 1.01 g/mL is __________% by mass.

Which of the following statements is false?

Calculate the freezing point of a 0.08500 m aqueous solution of NaNO3. The molal freezing-point-depression constant of water is 1.86°C/m.

A solution is prepared by adding 1.43 mol of KCl to 889 g of water. The concentration of KCl is __________ molal.

Which of the following substances is least likely to dissolve in water?

The largest value of the Henry's Law constant for the liquid solvent H2O will be obtained with __________ gas as the solute and a temperature of __________°C.

What is the mole fraction of sodium chloride in solution that is 13.0% by mass sodium chloride and that has a density of 1.10 g/mL?

Of the concentration units below, only __________ is temperature dependent.

A saturated solution __________.

Of the following, a 0.1 M aqueous solution of __________ will have the highest freezing point.

The vapor pressure of pure water at 25°C is 23.8 torr. Determine the vapor pressure (torr)of water at 25°C above a solution prepared by dissolving 21 g of urea (a nonvolatile, non-electrolyte, MW = 60.0g/mol)in 75 g of water.

Introduction: Matter and Measurement

Atoms, Molecules, and Ions

Stoichiometry: Calculations With Chemical Formulas and Equations

Aqueous Reactions and Solution Stoichiometry

Thermochemistry

Electronic Structure of Atoms

Periodic Properties of the Elements

Basic Concepts of Chemical Bonding

Molecular Geometry and Bonding Theories

Gases

Liquids and Intermolecular Forces

Solids and Modern Materials

Chemical Kinetics

Chemical Equilibrium

Acid-Base Equilibria

Additional Aspects of Aqueous Equilibria

Chemistry of the Environment

Chemical Thermodynamics

Electrochemistry

Nuclear Chemistry

Chemistry of the Nonmetals

Transition Metals and Coordination Chemistry

The Chemistry of Life: Organic and Biological Chemistry

Filters

Calculate the mole fraction of phosphoric acid (H₃PO₄)in a 25.4% (by mass)aqueous solution.

The solubility of Ar in water at 25°C is 1.6 × 10^-3 M when the pressure of the Ar above the solution is 1.0 atm. The solubility of Ar at a pressure of 2.5 atm is __________ M.

Which one of the following is most soluble in hexane (C₆H₁₄)?

Calculate the freezing point of a 0.08500 m aqueous solution of NaNO₃. The molal freezing-point-depression constant of water is 1.86°C/m.

The largest value of the Henry's Law constant for the liquid solvent H₂O will be obtained with gas as the solute and a temperature of °C.