Question 1

Which of the following choices has the compounds correctly arranged in order of increasing solubility in water? (least soluble to most soluble)

Accepted Answer

A) CCl4 3 3 
B) CH3OH 4 4 3 3 
D) LiF 3 3 
E) CH3OH 4 3 
A) CCl4 3 3 
B) CH3OH 4 4 3 3 
D) LiF 3 3 
E) CH3OH 4 3 A

Question 2

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 D

Question 3

The dissolution of water in octane (C8H18)is prevented by ________.

Accepted Answer

A) London dispersion forces between octane molecules 
B) hydrogen bonding between water molecules 
C) dipole-dipole attraction between octane molecules 
D) ion-dipole attraction between water and octane molecules 
E) repulsion between like-charged water and octane molecules 
A) London dispersion forces between octane molecules 
B) hydrogen bonding between water molecules 
C) dipole-dipole attraction between octane molecules 
D) ion-dipole attraction between water and octane molecules 
E) repulsion between like-charged water and octane molecules B

Question 4

-The solubility of MnSO4 monohydrate in water at 20 °C is 70.0 g per 100.0 mL of water. A solution at 20 °C that is 0.401 M in MnSO4 monohydrate is best described as a(n)________ solution. The formula weight of MnSO4 monohydrate is 168.97 g/mol.

Accepted Answer

A) hydrated 
B) solvated 
C) saturated 
D) unsaturated 
E) supersaturated 
A) hydrated 
B) solvated 
C) saturated 
D) unsaturated 
E) supersaturated

Question 5

A 0.100 m solution of which one of the following solutes will have the highest 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 6

-The solubility of MnSO4 monohydrate in water at 20 °C is 70.0 g per 100.0 mL of water. A solution at 20 °C that is 4.22 M in MnSO4 monohydrate is best described as a(n)________ solution. The formula weight of MnSO4 monohydrate is 168.97 g/mol.

Accepted Answer

A) hydrated 
B) solvated 
C) saturated 
D) unsaturated 
E) supersaturated 
A) hydrated 
B) solvated 
C) saturated 
D) unsaturated 
E) supersaturated

Question 7

The principal reason for the extremely low solubility of NaCl in benzene (C6H6)is the ________.

Accepted Answer

A) strong solvent-solvent interactions 
B) hydrogen bonding in C6H6 
C) strength of the covalent bond in NaCl 
D) weak solvation of Na+ and Cl- by C6H6 
E) increased disorder due to mixing of solute and solvent 
A) strong solvent-solvent interactions 
B) hydrogen bonding in C6H6 
C) strength of the covalent bond in NaCl 
D) weak solvation of Na+ and Cl- by C6H6 
E) increased disorder due to mixing of solute and solvent

Question 8

Of the following, a 0.1 M aqueous solution of ________ will have the lowest 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 9

Colligative properties of solutions include all of the following except ________.

Accepted Answer

A) depression of vapor pressure upon addition of a solute to a solvent 
B) elevation of the boiling point of a solution upon addition of a solute to a solvent 
C) depression of the freezing point of a solution upon addition of a solute to a solvent 
D) an increase in the osmotic pressure of a solution upon the addition of more solute 
E) the increase of reaction rates with increase in temperature 
A) depression of vapor pressure upon addition of a solute to a solvent 
B) elevation of the boiling point of a solution upon addition of a solute to a solvent 
C) depression of the freezing point of a solution upon addition of a solute to a solvent 
D) an increase in the osmotic pressure of a solution upon the addition of more solute 
E) the increase of reaction rates with increase in temperature

Question 10

A solution with a concentration higher than the solubility is ________.

Accepted Answer

A) not possible 
B) unsaturated 
C) supercritical 
D) saturated 
E) supersaturated 
A) not possible 
B) unsaturated 
C) supercritical 
D) saturated 
E) supersaturated

Question 11

A 1.35 m aqueous solution of compound X had a boiling point of 101.4 °C. Which one of the following could be compound X? The boiling point elevation constant for water is 0.52 °C/m.

Accepted Answer

A) CH3CH2OH 
B) C6H12O6 
C) Na3PO4 
D) KCl 
E) CaCl2 
A) CH3CH2OH 
B) C6H12O6 
C) Na3PO4 
D) KCl 
E) CaCl2

Question 12

Water (H2O)and the alcohol methanol (CH3OH)are infinitely soluble in each other. The primary intermolecular force responsible for this is ________.

Accepted Answer

Question 13

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 14

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

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

Calculate the molality of a 35.0% (by mass)aqueous solution of nitric acid.

Accepted Answer

A) 6.64 
B) 538 
C) 2.19 
D) 3.32 
E) The density of the solution is needed to solve the problem. 
A) 6.64 
B) 538 
C) 2.19 
D) 3.32 
E) The density of the solution is needed to solve the problem.

Question 17

A solution contains 33% phosphoric acid by mass. This means that ________.

Accepted Answer

A) 100 g of this solution contains 33 g of phosphoric acid 
B) 1 mL of this solution contains 33 g of phosphoric acid 
C) 1 L of this solution has a mass of 33 g 
D) 1 L of this solution contains 33 mL of phosphoric acid 
E) the density of this solution is 3.3 g/mL 
A) 100 g of this solution contains 33 g of phosphoric acid 
B) 1 mL of this solution contains 33 g of phosphoric acid 
C) 1 L of this solution has a mass of 33 g 
D) 1 L of this solution contains 33 mL of phosphoric acid 
E) the density of this solution is 3.3 g/mL

Question 18

The Henry's law constant for helium gas in water at 30 °C is 3.70 × 10-4 M/atm. When the partial pressure of helium above a sample of water is 0.400 atm, the concentration of helium in the water is ________ M.

Accepted Answer

A) 9.25 × 10-4 
B) 1.08 × 103 
C) 0.800 
D) 1.48 × 10-4 
E) 3.70 × 10-4 
A) 9.25 × 10-4 
B) 1.08 × 103 
C) 0.800 
D) 1.48 × 10-4 
E) 3.70 × 10-4

Question 19

When solutions of strong electrolytes in water are formed, the ions are surrounded by water molecules. These interactions are described as a case of ________.

Accepted Answer

A) hydration 
B) supersaturation 
C) crystallization 
D) dehydration 
E) saturation 
A) hydration 
B) supersaturation 
C) crystallization 
D) dehydration 
E) saturation

Question 20

A solution contains 39% phosphoric acid by mass. This means that ________.

Accepted Answer

A) 100 g of this solution contains 39 g of phosphoric acid 
B) 1 mL of this solution contains 39 g of phosphoric acid 
C) 1 L of this solution has a mass of 39 g 
D) 1 L of this solution contains 39 mL of phosphoric acid 
E) the density of this solution is 3.9 g/mL 
A) 100 g of this solution contains 39 g of phosphoric acid 
B) 1 mL of this solution contains 39 g of phosphoric acid 
C) 1 L of this solution has a mass of 39 g 
D) 1 L of this solution contains 39 mL of phosphoric acid 
E) the density of this solution is 3.9 g/mL

Exam 13: Properties of Solutions

Which of the following choices has the compounds correctly arranged in order of increasing solubility in water? (least soluble to most soluble)

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

The dissolution of water in octane (C8H18)is prevented by ________.

-The solubility of MnSO4 monohydrate in water at 20 °C is 70.0 g per 100.0 mL of water. A solution at 20 °C that is 0.401 M in MnSO4 monohydrate is best described as a(n)________ solution. The formula weight of MnSO4 monohydrate is 168.97 g/mol.

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

-The solubility of MnSO4 monohydrate in water at 20 °C is 70.0 g per 100.0 mL of water. A solution at 20 °C that is 4.22 M in MnSO4 monohydrate is best described as a(n)________ solution. The formula weight of MnSO4 monohydrate is 168.97 g/mol.

The principal reason for the extremely low solubility of NaCl in benzene (C6H6)is the ________.

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

Colligative properties of solutions include all of the following except ________.

A solution with a concentration higher than the solubility is ________.

A 1.35 m aqueous solution of compound X had a boiling point of 101.4 °C. Which one of the following could be compound X? The boiling point elevation constant for water is 0.52 °C/m.

Water (H2O)and the alcohol methanol (CH3OH)are infinitely soluble in each other. The primary intermolecular force responsible for this is ________.

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

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

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?

Calculate the molality of a 35.0% (by mass)aqueous solution of nitric acid.

A solution contains 33% phosphoric acid by mass. This means that ________.

The Henry's law constant for helium gas in water at 30 °C is 3.70 × 10-4 M/atm. When the partial pressure of helium above a sample of water is 0.400 atm, the concentration of helium in the water is ________ M.

When solutions of strong electrolytes in water are formed, the ions are surrounded by water molecules. These interactions are described as a case of ________.

A solution contains 39% phosphoric acid by mass. This means that ________.

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

The dissolution of water in octane (C₈H₁₈)is prevented by ________.

-The solubility of MnSO₄ monohydrate in water at 20 °C is 70.0 g per 100.0 mL of water. A solution at 20 °C that is 0.401 M in MnSO₄ monohydrate is best described as a(n)________ solution. The formula weight of MnSO₄ monohydrate is 168.97 g/mol.

-The solubility of MnSO₄ monohydrate in water at 20 °C is 70.0 g per 100.0 mL of water. A solution at 20 °C that is 4.22 M in MnSO₄ monohydrate is best described as a(n)________ solution. The formula weight of MnSO₄ monohydrate is 168.97 g/mol.

The principal reason for the extremely low solubility of NaCl in benzene (C₆H₆)is the ________.

Water (H₂O)and the alcohol methanol (CH₃OH)are infinitely soluble in each other. The primary intermolecular force responsible for this is ________.

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?

The Henry's law constant for helium gas in water at 30 °C is 3.70 × 10^-4 M/atm. When the partial pressure of helium above a sample of water is 0.400 atm, the concentration of helium in the water is ________ M.