Question 1

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

Accepted Answer

A) True 
 B)False

Question 2

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 3

Calculate the molarity of phosphoric acid (H3PO4)in a 22.1% (by mass)aqueous solution.

Accepted Answer

A) 0.0522 m 
B) 0.0992 m 
C) 0.0248 m 
D) 0.0496 m 
E) The density of the solution is needed to solve the problem. 
A) 0.0522 m 
B) 0.0992 m 
C) 0.0248 m 
D) 0.0496 m 
E) The density of the solution is needed to solve the problem.

Question 4

The concentration of lithium chlorate solution is 12.0% by mass. In a ________ g sample of this solution, there are 238.5 g of dissolved lithium chlorate.

Accepted Answer

A) 1990 
B) 28.6 
C) 0.199 
D) 5.03 
E) 0.0503 
A) 1990 
B) 28.6 
C) 0.199 
D) 5.03 
E) 0.0503

Question 5

The mole fraction of HCl in a solution prepared by dissolving 5.5 g of HCl in 200 g of C2H6O is ________. The density of the solution is 0.79 g/mL.

Accepted Answer

A) 0.027 
B) 0.034 
C) 0.028 
D) 0.035 
E) 0.151 
A) 0.027 
B) 0.034 
C) 0.028 
D) 0.035 
E) 0.151

Question 6

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 2.0 atm is ________ M.

Accepted Answer

A) 0.0014 
B) 0.00086 
C) 120 
D) 0.0037 
E) 2.0 
A) 0.0014 
B) 0.00086 
C) 120 
D) 0.0037 
E) 2.0

Question 7

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

Question 8

At 20 °C, a 1.73 M aqueous solution of ammonium chloride has a density of 1.0257 g/mL. What is the mass % of ammonium chloride in the solution? The formula weight of NH4Cl is 53.50 g/mol.

Accepted Answer

A) 1.85 
B) 3.31 
C) 1.68 
D) 0.594 
E) 9.00 
A) 1.85 
B) 3.31 
C) 1.68 
D) 0.594 
E) 9.00

Question 9

The solubility of oxygen gas in water at 25 °C and 1.0 atm pressure of oxygen is 0.041 g/L. The solubility of oxygen in water at 4.0 atm and 25 °C is ________ g/L.

Accepted Answer

A) 0.041 
B) 0.014 
C) 0.31 
D) 0.16 
E) 4.0 
A) 0.041 
B) 0.014 
C) 0.31 
D) 0.16 
E) 4.0

Question 10

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 2.0 × 10-3 M.

Accepted Answer

A) 0.63 
B) 0.68 
C) 1.0 
D) 3.0 
E) 3.2 
A) 0.63 
B) 0.68 
C) 1.0 
D) 3.0 
E) 3.2

Question 11

Which one of the following is least soluble in water?

Accepted Answer

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

Question 12

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 mole fraction of Cl- in this solution is ________.

Accepted Answer

A) 0.0103 
B) 0.0200 
C) 0.0201 
D) 0.0632 
E) 0.0630 
A) 0.0103 
B) 0.0200 
C) 0.0201 
D) 0.0632 
E) 0.0630

Question 13

A solution is prepared by dissolving 10.0 g of benzene (C6H6)in 282 g of carbon tetrachloride (CCl4). The concentration of benzene in this solution is ________ molal. The molar masses of C6H6 and CCl4 are 78.1 g/mol and 154 g/mol, respectively.

Accepted Answer

A) 4.54 × 10-4 
B) 0.454 
C) 0.0654 
D) 0.0342 
E) 3.42 
A) 4.54 × 10-4 
B) 0.454 
C) 0.0654 
D) 0.0342 
E) 3.42

Question 14

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

Accepted Answer

A) True 
 B)False

Question 15

Molality is defined as the ________.

Accepted Answer

A) moles solute/moles solvent 
B) moles solute/liters solution 
C) moles solute/kg solution 
D) moles solute/kg solvent 
E) none (dimensionless) 
A) moles solute/moles solvent 
B) moles solute/liters solution 
C) moles solute/kg solution 
D) moles solute/kg solvent 
E) none (dimensionless)

Question 16

A solution contains 51 ppm of benzene. The density of the solution is 1.00 g/mL. This means that ________.

Accepted Answer

A) there are 51 mg of benzene in 1.0 L of this solution 
B) 100 g of the solution contains 51 g of benzene 
C) 100 g of the solution contains 51 mg of benzene 
D) the solution is 51% by mass of benzene 
E) the molarity of the solution is 51 M 
A) there are 51 mg of benzene in 1.0 L of this solution 
B) 100 g of the solution contains 51 g of benzene 
C) 100 g of the solution contains 51 mg of benzene 
D) the solution is 51% by mass of benzene 
E) the molarity of the solution is 51 M

Question 17

Calculate the molality of a 24.4% (by mass)aqueous solution of phosphoric acid (H3PO4).

Accepted Answer

A) 3.29 m 
B) 323 m 
C) 6.59 m 
D) 1.65 m 
E) The density of the solution is needed to solve the problem. 
A) 3.29 m 
B) 323 m 
C) 6.59 m 
D) 1.65 m 
E) The density of the solution is needed to solve the problem.

Question 18

The concentration of CO2 in a soft drink bottled with a partial pressure of CO2 of 4.0 atm over the liquid at 25 °C is 1.2 × 10-1 M. The Henry's law constant for CO2 at this temperature is ________.

Accepted Answer

A) 3.0 × 10-2 mol/L-atm 
B) 4.5 × 10-3 mol/L-atm 
C) 5.6 × 10-3 mol/L-atm 
D) 2.3 × 10-2 mol/L-atm 
E) More information is needed to solve the problem. 
A) 3.0 × 10-2 mol/L-atm 
B) 4.5 × 10-3 mol/L-atm 
C) 5.6 × 10-3 mol/L-atm 
D) 2.3 × 10-2 mol/L-atm 
E) More information is needed to solve the problem.

Question 19

Which one of the following is most soluble in water?

Accepted Answer

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

Question 20

The freezing point of ethanol (C2H5OH)is -114.6 °C. The molal freezing point depression constant for ethanol is 2.00 °C/m. What is the freezing point (°C)of a solution prepared by dissolving 50.0 g of glycerin (C3H8O3, a nonelectrolyte)in 200.0 g of ethanol?

Accepted Answer

A) -115.0 
B) -5.43 
C) -132.3 
D) -120.0 
E) -114.6 
A) -115.0 
B) -5.43 
C) -132.3 
D) -120.0 
E) -114.6

Exam 13: Properties of Solutions

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

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.

Calculate the molarity of phosphoric acid (H3PO4)in a 22.1% (by mass)aqueous solution.

The concentration of lithium chlorate solution is 12.0% by mass. In a ________ g sample of this solution, there are 238.5 g of dissolved lithium chlorate.

The mole fraction of HCl in a solution prepared by dissolving 5.5 g of HCl in 200 g of C2H6O is ________. The density of the solution is 0.79 g/mL.

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 2.0 atm is ________ M.

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

At 20 °C, a 1.73 M aqueous solution of ammonium chloride has a density of 1.0257 g/mL. What is the mass % of ammonium chloride in the solution? The formula weight of NH4Cl is 53.50 g/mol.

The solubility of oxygen gas in water at 25 °C and 1.0 atm pressure of oxygen is 0.041 g/L. The solubility of oxygen in water at 4.0 atm and 25 °C is ________ g/L.

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 2.0 × 10-3 M.

Which one of the following is least soluble in water?

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 mole fraction of Cl- in this solution is ________.

A solution is prepared by dissolving 10.0 g of benzene (C6H6)in 282 g of carbon tetrachloride (CCl4). The concentration of benzene in this solution is ________ molal. The molar masses of C6H6 and CCl4 are 78.1 g/mol and 154 g/mol, respectively.

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

Molality is defined as the ________.

A solution contains 51 ppm of benzene. The density of the solution is 1.00 g/mL. This means that ________.

Calculate the molality of a 24.4% (by mass)aqueous solution of phosphoric acid (H3PO4).

The concentration of CO2 in a soft drink bottled with a partial pressure of CO2 of 4.0 atm over the liquid at 25 °C is 1.2 × 10-1 M. The Henry's law constant for CO2 at this temperature is ________.

Which one of the following is most soluble in water?

The freezing point of ethanol (C2H5OH)is -114.6 °C. The molal freezing point depression constant for ethanol is 2.00 °C/m. What is the freezing point (°C)of a solution prepared by dissolving 50.0 g of glycerin (C3H8O3, a nonelectrolyte)in 200.0 g of ethanol?

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

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.

Calculate the molarity of phosphoric acid (H₃PO₄)in a 22.1% (by mass)aqueous solution.

The mole fraction of HCl in a solution prepared by dissolving 5.5 g of HCl in 200 g of C₂H₆O is ________. The density of the solution is 0.79 g/mL.

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 2.0 atm is ________ M.

At 20 °C, a 1.73 M aqueous solution of ammonium chloride has a density of 1.0257 g/mL. What is the mass % of ammonium chloride in the solution? The formula weight of NH₄Cl is 53.50 g/mol.

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 2.0 × 10^-3 M.

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 mole fraction of Cl^- in this solution is ________.

A solution is prepared by dissolving 10.0 g of benzene (C₆H₆)in 282 g of carbon tetrachloride (CCl₄). The concentration of benzene in this solution is ________ molal. The molar masses of C₆H₆ and CCl₄ are 78.1 g/mol and 154 g/mol, respectively.

Calculate the molality of a 24.4% (by mass)aqueous solution of phosphoric acid (H₃PO₄).

The concentration of CO₂ in a soft drink bottled with a partial pressure of CO₂ of 4.0 atm over the liquid at 25 °C is 1.2 × 10^-1 M. The Henry's law constant for CO₂ at this temperature is ________.

The freezing point of ethanol (C₂H₅OH)is -114.6 °C. The molal freezing point depression constant for ethanol is 2.00 °C/m. What is the freezing point (°C)of a solution prepared by dissolving 50.0 g of glycerin (C₃H₈O₃, a nonelectrolyte)in 200.0 g of ethanol?