Question 1

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

Accepted Answer

A) 0.274 m 
B) 2.74 m 
C) 3.04 m 
D) 4.33 m 
E) The density of the solution is needed to solve the problem. 
A) 0.274 m 
B) 2.74 m 
C) 3.04 m 
D) 4.33 m 
E) The density of the solution is needed to solve the problem.

Question 2

A solution is prepared by dissolving 6.00 g of an unknown nonelectrolyte in enough water to make 1.00 L of solution. The osmotic pressure of this solution is 0.750 atm at 25.0°C. What is the molecular weight (g/mol)of the unknown solute?

Accepted Answer

A) 16.4 
B) 196 
C) 110 
D) 30.6 
E) 5.12 × 10-3 
A) 16.4 
B) 196 
C) 110 
D) 30.6 
E) 5.12 × 10-3

Question 3

As the concentration of a solute in a solution increases, the freezing point of the solution __________ and the vapor pressure of the solution __________.

Accepted Answer

A) increases, increases 
B) increases, decreases 
C) decreases, increases 
D) decreases, decreases 
E) decreases, is unaffected 
A) increases, increases 
B) increases, decreases 
C) decreases, increases 
D) decreases, decreases 
E) decreases, is unaffected

Question 4

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

Accepted Answer

A) 0.0425 
B) 0.106 
C) -0.0562 
D) -0.158 
E) -0.316 
A) 0.0425 
B) 0.106 
C) -0.0562 
D) -0.158 
E) -0.316

Question 5

Which of the following aqueous solutions will have the highest boiling point?

Accepted Answer

A) 0.10 m Na2SO4 
B) 0.20 m glucose 
C) 0.25 m sucrose 
D) 0.10 m NaCl 
E) 0.10 m SrSO4 
A) 0.10 m Na2SO4 
B) 0.20 m glucose 
C) 0.25 m sucrose 
D) 0.10 m NaCl 
E) 0.10 m SrSO4

Question 6

Emulsifying agents typically have a hydrophobic end and a hydrophilic end.

Accepted Answer

A) True 
 B)False

Question 7

A solution contains 15 ppm of benzene. The density of the solution is 1.00 g/mL. This means that __________.

Accepted Answer

A) there are 15 mg of benzene in 1.0 g of this solution 
B) 100 g of the solution contains 15 g of benzene 
C) 1.0 g of the solution contains 15 × 10-6 g of benzene 
D) 1.0 L of the solution contains 15 g of benzene 
E) the solution is 15% by mass of benzene 
A) there are 15 mg of benzene in 1.0 g of this solution 
B) 100 g of the solution contains 15 g of benzene 
C) 1.0 g of the solution contains 15 × 10-6 g of benzene 
D) 1.0 L of the solution contains 15 g of benzene 
E) the solution is 15% by mass of benzene

Question 8

The mole fraction of He in a gaseous solution prepared from 3.0 g of He, 6.5 g of Ar, and 10.0 g of Ne is __________.

Accepted Answer

A) 0.53 
B) 0.75 
C) 0.20 
D) 0.66 
E) 0.86 
A) 0.53 
B) 0.75 
C) 0.20 
D) 0.66 
E) 0.86

Question 9

The solubility of nitrogen gas in water at 25°C and a nitrogen pressure of 1.0 atm is 6.9 × 10-4 M. The solubility of nitrogen in water at a nitrogen pressure of 5.0 atm is __________ M.

Accepted Answer

A) 0.0035 
B) .00086 
C) 120 
D) 0.00055 
E) 5.0 
A) 0.0035 
B) .00086 
C) 120 
D) 0.00055 
E) 5.0

Question 10

A solution is prepared by dissolving 15.0 g of NH3 in 250.0 g of water. The density of the resulting solution is 0.974 g/mL. The molarity of NH3 in the solution is __________.

Accepted Answer

A) 0.00353 
B) 0.882 
C) 60.0 
D) 3.24 
E) 3.53 
A) 0.00353 
B) 0.882 
C) 60.0 
D) 3.24 
E) 3.53

Question 11

Which of the following liquids will have the highest 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) 
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)

Question 12

An unsaturated solution is one that __________.

Accepted Answer

A) has no double bonds 
B) contains the maximum concentration of solute possible, and is in equilibrium with undissolved solute 
C) has a concentration lower than the solubility 
D) contains more dissolved solute than the solubility allows 
E) contains no solute 
A) has no double bonds 
B) contains the maximum concentration of solute possible, and is in equilibrium with undissolved solute 
C) has a concentration lower than the solubility 
D) contains more dissolved solute than the solubility allows 
E) contains no solute

Question 13

A solution is prepared by dissolving 22.7 g of CaCl2 in 375 g of water. The density of the resulting solution is 1.05 g/mL. The concentration of CaCl2 is __________% by mass.

Accepted Answer

A) 5.71 
B) 5.99 
C) 0.0599 
D) 0.0571 
E) 6.24 
A) 5.71 
B) 5.99 
C) 0.0599 
D) 0.0571 
E) 6.24

Question 14

A solution contains 11% by mass of sodium chloride. This means that __________.

Accepted Answer

A) there are 11 g of sodium chloride in in 1.0 mL of this solution 
B) 100 g of the solution contains 11 g of sodium chloride 
C) 100 mL of the solution contains 11 g of sodium chloride 
D) the density of the solution is 11 g/mL 
E) the molality of the solution is 11 
A) there are 11 g of sodium chloride in in 1.0 mL of this solution 
B) 100 g of the solution contains 11 g of sodium chloride 
C) 100 mL of the solution contains 11 g of sodium chloride 
D) the density of the solution is 11 g/mL 
E) the molality of the solution is 11

Question 15

The solubility of nitrogen gas at 25°C and 1 atm is 6.8 × 10-4 mol/L. If the partial pressure of nitrogen gas in air is 0.76 atm, what is the concentration (molarity)of dissolved nitrogen?

Accepted Answer

A) 6.8 × 10-4 M 
B) 5.2 × 10-4 M 
C) 4.9 × 10-4 M 
D) 3.8 × 10-4 M 
E) 1.1 × 10-5 M 
A) 6.8 × 10-4 M 
B) 5.2 × 10-4 M 
C) 4.9 × 10-4 M 
D) 3.8 × 10-4 M 
E) 1.1 × 10-5 M

Question 16

A solution containing 20.0 g of an unknown liquid and 110.0 g water has a freezing point of -1.32 °C. Given Kf = 1.86°C/m for water, the molar mass of the unknown liquid is ________g/mol.

Accepted Answer

A) 256 
B) 69.0 
C) 333 
D) 619 
E) 78.1 
A) 256 
B) 69.0 
C) 333 
D) 619 
E) 78.1

Question 17

The process of a substance sticking to the surface of another is called

Accepted Answer

A) absorption 
B) diffusion 
C) effusion 
D) adsorption 
E) coagulation 
A) absorption 
B) diffusion 
C) effusion 
D) adsorption 
E) coagulation

Question 18

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

Accepted Answer

A) pure H2O 
B) aqueous glucose (0.050 m) 
C) aqueous CoI2 (0.030 m) 
D) aqueous FeI3 (0.030 m) 
E) aqueous NaI (0.030 m) 
A) pure H2O 
B) aqueous glucose (0.050 m) 
C) aqueous CoI2 (0.030 m) 
D) aqueous FeI3 (0.030 m) 
E) aqueous NaI (0.030 m)

Question 19

Which one of the following substances would be the most soluble in CCl4?

Accepted Answer

A) CH3CH2OH 
B) H2O 
C) NH3 
D) C10H22 
E) NaCl 
A) CH3CH2OH 
B) H2O 
C) NH3 
D) C10H22 
E) NaCl

Question 20

In a saturated solution of a salt in water, __________.

Accepted Answer

A) the rate of crystallization > the rate of dissolution 
B) the rate of dissolution > the rate of crystallization 
C) seed crystal addition may cause massive crystallization 
D) the rate of crystallization = the rate of dissolution 
E) addition of more water causes massive crystallization 
A) the rate of crystallization > the rate of dissolution 
B) the rate of dissolution > the rate of crystallization 
C) seed crystal addition may cause massive crystallization 
D) the rate of crystallization = the rate of dissolution 
E) addition of more water causes massive crystallization

Exam 13: Properties of Solutions

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

A solution is prepared by dissolving 6.00 g of an unknown nonelectrolyte in enough water to make 1.00 L of solution. The osmotic pressure of this solution is 0.750 atm at 25.0°C. What is the molecular weight (g/mol)of the unknown solute?

As the concentration of a solute in a solution increases, the freezing point of the solution __________ and the vapor pressure of the solution __________.

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

Which of the following aqueous solutions will have the highest boiling point?

Emulsifying agents typically have a hydrophobic end and a hydrophilic end.

A solution contains 15 ppm of benzene. The density of the solution is 1.00 g/mL. This means that __________.

The mole fraction of He in a gaseous solution prepared from 3.0 g of He, 6.5 g of Ar, and 10.0 g of Ne is __________.

The solubility of nitrogen gas in water at 25°C and a nitrogen pressure of 1.0 atm is 6.9 × 10-4 M. The solubility of nitrogen in water at a nitrogen pressure of 5.0 atm is __________ M.

A solution is prepared by dissolving 15.0 g of NH3 in 250.0 g of water. The density of the resulting solution is 0.974 g/mL. The molarity of NH3 in the solution is __________.

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

An unsaturated solution is one that __________.

A solution is prepared by dissolving 22.7 g of CaCl2 in 375 g of water. The density of the resulting solution is 1.05 g/mL. The concentration of CaCl2 is __________% by mass.

A solution contains 11% by mass of sodium chloride. This means that __________.

The solubility of nitrogen gas at 25°C and 1 atm is 6.8 × 10-4 mol/L. If the partial pressure of nitrogen gas in air is 0.76 atm, what is the concentration (molarity)of dissolved nitrogen?

A solution containing 20.0 g of an unknown liquid and 110.0 g water has a freezing point of -1.32 °C. Given Kf = 1.86°C/m for water, the molar mass of the unknown liquid is ________g/mol.

The process of a substance sticking to the surface of another is called

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

Which one of the following substances would be the most soluble in CCl4?

In a saturated solution of a salt in 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

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As the concentration of a solute in a solution increases, the freezing point of the solution and the vapor pressure of the solution .

The solubility of nitrogen gas in water at 25°C and a nitrogen pressure of 1.0 atm is 6.9 × 10^-4 M. The solubility of nitrogen in water at a nitrogen pressure of 5.0 atm is __________ M.

A solution is prepared by dissolving 15.0 g of NH₃ in 250.0 g of water. The density of the resulting solution is 0.974 g/mL. The molarity of NH₃ in the solution is __________.

A solution is prepared by dissolving 22.7 g of CaCl₂ in 375 g of water. The density of the resulting solution is 1.05 g/mL. The concentration of CaCl₂ is __________% by mass.

The solubility of nitrogen gas at 25°C and 1 atm is 6.8 × 10^-4 mol/L. If the partial pressure of nitrogen gas in air is 0.76 atm, what is the concentration (molarity)of dissolved nitrogen?

A solution containing 20.0 g of an unknown liquid and 110.0 g water has a freezing point of -1.32 °C. Given K_f = 1.86°C/m for water, the molar mass of the unknown liquid is ________g/mol.

Which one of the following substances would be the most soluble in CCl₄?