Question 1

Hydration is a specific example of the phenomenon known generally as ________.

Accepted Answer

A) salutation 
B) disordering 
C) solvation 
D) condensation 
E) dilution 
A) salutation 
B) disordering 
C) solvation 
D) condensation 
E) dilution

Question 2

Which produces the greatest number of ions when one mole dissolves in water?

Accepted Answer

A) K2SO4 
B) NaF 
C) LiMnO4 
D) NH4Br 
E) sucrose 
A) K2SO4 
B) NaF 
C) LiMnO4 
D) NH4Br 
E) sucrose

Question 3

A solution is prepared by dissolving 0.60 g of nicotine (a nonelectrolyte)in water to make 12 mL of solution. The osmotic pressure of the solution is 7.55 atm at 25 °C. The molecular weight of nicotine is ________ g/mol.

Accepted Answer

A) 28 
B) 43 
C) 50 
D) 160 
E) 0.60 
A) 28 
B) 43 
C) 50 
D) 160 
E) 0.60

Question 4

Which of the following cannot be a colloid?

Accepted Answer

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

Question 5

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 6

The concentration of sodium sulfate solution is 18.6% by mass. There are ________ g of sodium sulfate present in a 236.5 g sample of this solution.

Accepted Answer

A) 44.0 
B) 4400 
C) 0.000786 
D) 7.86 
E) 1270 
A) 44.0 
B) 4400 
C) 0.000786 
D) 7.86 
E) 1270

Question 7

Pairs of liquids that will mix in all proportions are called ________ liquids.

Accepted Answer

A) miscible 
B) unsaturated 
C) polar liquids 
D) saturated 
E) supersaturated 
A) miscible 
B) unsaturated 
C) polar liquids 
D) saturated 
E) supersaturated

Question 8

The concentration of sodium chloride in an aqueous solution that is 2.13 M and that has a density of 1.01 g/mL is ________% by mass.

Accepted Answer

A) 2.11 
B) 7.83 
C) 124 
D) 12.3 
E) 14.2 
A) 2.11 
B) 7.83 
C) 124 
D) 12.3 
E) 14.2

Question 9

At 20 °C, a 3.13 M aqueous solution of ammonium chloride has a density of 1.0457 g/mL. What is the molality of ammonium chloride in the solution? The formula weight of NH4Cl is 53.50 g/mol.

Accepted Answer

A) 3.56 
B) 0.0611 
C) 3.13 
D) 0.334 
E) 16.00 
A) 3.56 
B) 0.0611 
C) 3.13 
D) 0.334 
E) 16.00

Question 10

Calculate the mole fraction of phosphoric acid (H3PO4)in a 38.5% (by mass)aqueous solution.

Accepted Answer

A) 0.103 
B) 0.115 
C) 0.206 
D) 0.0516 
E) The density of the solution is needed to solve the problem. 
A) 0.103 
B) 0.115 
C) 0.206 
D) 0.0516 
E) The density of the solution is needed to solve the problem.

Question 11

The most likely van't Hoff factor for an 0.01 m CaI2 solution is ________.

Accepted Answer

A) 1.00 
B) 3.00 
C) 1.27 
D) 2.69 
E) 3.29 
A) 1.00 
B) 3.00 
C) 1.27 
D) 2.69 
E) 3.29

Question 12

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 13

Calculate the mole fraction of phosphoric acid (H3PO4)in a 29.1% (by mass)aqueous solution.

Accepted Answer

A) 0.0702 
B) 0.0755 
C) 0.140 
D) 0.0351 
E) The density of the solution is needed to solve the problem. 
A) 0.0702 
B) 0.0755 
C) 0.140 
D) 0.0351 
E) The density of the solution is needed to solve the problem.

Question 14

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 15

The phrase "like dissolves like" refers to the fact that ________.

Accepted Answer

A) gases can only dissolve other gases 
B) polar solvents dissolve polar solutes and nonpolar solvents dissolve nonpolar solutes 
C) solvents can only dissolve solutes of similar molar mass 
D) condensed phases can only dissolve other condensed phases 
E) polar solvents dissolve nonpolar solutes and vice versa 
A) gases can only dissolve other gases 
B) polar solvents dissolve polar solutes and nonpolar solvents dissolve nonpolar solutes 
C) solvents can only dissolve solutes of similar molar mass 
D) condensed phases can only dissolve other condensed phases 
E) polar solvents dissolve nonpolar solutes and vice versa

Question 16

Calculate the freezing point of a solution containing 20 grams of KCl and 2200.0 grams of water. The molal-freezing-point-depression constant (Kf)for water is 1.86 °C/m.

Accepted Answer

A) -0.45 °C 
B) +0.45 °C 
C) -0.23 °C 
D) +0.23 °C 
E) 1.23 °C 
A) -0.45 °C 
B) +0.45 °C 
C) -0.23 °C 
D) +0.23 °C 
E) 1.23 °C

Question 17

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 18

The magnitudes of Kf and of Kb depend on the identity of the ________.

Accepted Answer

A) solute 
B) solvent 
C) solution 
D) solvent and on temperature 
E) solute and solvent 
A) solute 
B) solvent 
C) solution 
D) solvent and on temperature 
E) solute and solvent

Question 19

At 20 °C, an aqueous solution that is 12.0% by mass in ammonium chloride has a density of 1.0344 g/mL. What is the molarity of ammonium chloride in the solution? The formula weight of NH4Cl is 53.50 g/mol.

Accepted Answer

A) 2.55 
B) 0.232 
C) 2.32 
D) 0.0862 
E) 11.6 
A) 2.55 
B) 0.232 
C) 2.32 
D) 0.0862 
E) 11.6

Question 20

The molarity of urea in a solution prepared by dissolving 16 g of urea (MW = 60.0 g/mol)in 39 g 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) 0.16 
A) 0.11 
B) 3.7 
C) 6.8 
D) 6.3 
E) 0.16

Exam 13: Properties of Solutions

Hydration is a specific example of the phenomenon known generally as ________.

Which produces the greatest number of ions when one mole dissolves in water?

A solution is prepared by dissolving 0.60 g of nicotine (a nonelectrolyte)in water to make 12 mL of solution. The osmotic pressure of the solution is 7.55 atm at 25 °C. The molecular weight of nicotine is ________ g/mol.

Which of the following cannot be a colloid?

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

The concentration of sodium sulfate solution is 18.6% by mass. There are ________ g of sodium sulfate present in a 236.5 g sample of this solution.

Pairs of liquids that will mix in all proportions are called ________ liquids.

The concentration of sodium chloride in an aqueous solution that is 2.13 M and that has a density of 1.01 g/mL is ________% by mass.

At 20 °C, a 3.13 M aqueous solution of ammonium chloride has a density of 1.0457 g/mL. What is the molality of ammonium chloride in the solution? The formula weight of NH4Cl is 53.50 g/mol.

Calculate the mole fraction of phosphoric acid (H3PO4)in a 38.5% (by mass)aqueous solution.

The most likely van't Hoff factor for an 0.01 m CaI2 solution is ________.

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

Calculate the mole fraction of phosphoric acid (H3PO4)in a 29.1% (by mass)aqueous solution.

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

The phrase "like dissolves like" refers to the fact that ________.

Calculate the freezing point of a solution containing 20 grams of KCl and 2200.0 grams of water. The molal-freezing-point-depression constant (Kf)for water is 1.86 °C/m.

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

The magnitudes of Kf and of Kb depend on the identity of the ________.

At 20 °C, an aqueous solution that is 12.0% by mass in ammonium chloride has a density of 1.0344 g/mL. What is the molarity of ammonium chloride in the solution? The formula weight of NH4Cl is 53.50 g/mol.

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

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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At 20 °C, a 3.13 M aqueous solution of ammonium chloride has a density of 1.0457 g/mL. What is the molality of ammonium chloride in the solution? The formula weight of NH₄Cl is 53.50 g/mol.

Calculate the mole fraction of phosphoric acid (H₃PO₄)in a 38.5% (by mass)aqueous solution.

The most likely van't Hoff factor for an 0.01 m CaI₂ solution is ________.

Calculate the mole fraction of phosphoric acid (H₃PO₄)in a 29.1% (by mass)aqueous solution.

Calculate the freezing point of a solution containing 20 grams of KCl and 2200.0 grams of water. The molal-freezing-point-depression constant (K_f)for water is 1.86 °C/m.

The magnitudes of K_f and of K_b depend on the identity of the ________.

At 20 °C, an aqueous solution that is 12.0% by mass in ammonium chloride has a density of 1.0344 g/mL. What is the molarity of ammonium chloride in the solution? The formula weight of NH₄Cl is 53.50 g/mol.

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