Question 1

A 0.1 M aqueous solution of __________ will have a pH of 7.0 at 25.0°C. NaOCl KCl NH4Cl Ca(OAc)2

Accepted Answer

A) NaOCl 
B) KCl 
C) NH4Cl 
D) Ca(OAc)2 
E) KCl and NH4Cl 
A) NaOCl 
B) KCl 
C) NH4Cl 
D) Ca(OAc)2 
E) KCl and NH4Cl

Question 2

The pH of an aqueous solution at 25.0 °C is 10.30. What is the molarity of H+ in this solution?

Accepted Answer

A) 5.0 × 10-11 
B) 2.0 × 10-4 
C) 3.70 
D) 1.0 × 10-13 
E) 2.0 × 1010 
A) 5.0 × 10-11 
B) 2.0 × 10-4 
C) 3.70 
D) 1.0 × 10-13 
E) 2.0 × 1010

Question 3

The Ka of hydrofluoric acid (HF)at 25.0 °C is 6.8 × 10-4. What is the pH of a 0.15 M aqueous solution of HF?

Accepted Answer

A) 4.60 
B) 2.00 
C) 3.64 
D) 0.82 
E) 1.17 
A) 4.60 
B) 2.00 
C) 3.64 
D) 0.82 
E) 1.17

Question 4

A- is a weak base. Which equilibrium corresponds to the equilibrium constant Ka for HA?

Accepted Answer

A) HA (aq)+ H2O (l)   H2A+ (aq)+ OH- (aq) 
B) A- (aq)+ H3O+ (aq)   HA (aq)+ H2O (l) 
C) HA (aq)+ H2O (l)   H3O+ (aq)+ A- (aq) 
D) A- (aq)+ H2O (l)   HA (aq)+ OH- (aq) 
E) A- (aq)+ OH- (aq)   HOA2- (aq) 
A) HA (aq)+ H2O (l)   H2A+ (aq)+ OH- (aq) 
B) A- (aq)+ H3O+ (aq)   HA (aq)+ H2O (l) 
C) HA (aq)+ H2O (l)   H3O+ (aq)+ A- (aq) 
D) A- (aq)+ H2O (l)   HA (aq)+ OH- (aq) 
E) A- (aq)+ OH- (aq)   HOA2- (aq)

Question 5

Determine the pH of a 0.35 M aqueous solution of CH3N H2 (methylamine). The Kb of methylamine is 4.4 × 10-4.

Accepted Answer

A) 10.00 
B) 3.86 
C) 12.09 
D) 1.96 
E) 13.24 
A) 10.00 
B) 3.86 
C) 12.09 
D) 1.96 
E) 13.24

Question 6

A 0.0035 M aqueous solution of a particular compound has pH = 2.46. The compound is __________.

Accepted Answer

A) a weak base 
B) a weak acid 
C) a strong acid 
D) a strong base 
E) a salt 
A) a weak base 
B) a weak acid 
C) a strong acid 
D) a strong base 
E) a salt

Question 7

Of the following acids, __________ is not a strong acid.

Accepted Answer

A) HNO2 
B) H2SO4 
C) HNO3 
D) HClO4 
E) HCl 
A) HNO2 
B) H2SO4 
C) HNO3 
D) HClO4 
E) HCl

Question 8

Using the data in the table, which of the conjugate bases below is the weakest base?

Accepted Answer

A) OAc- 
B) C7H5O2- 
C) NO2- 
D) F- 
E) OAc- and C7H5O2- 
A) OAc- 
B) C7H5O2- 
C) NO2- 
D) F- 
E) OAc- and C7H5O2-

Question 9

Of the acids in the table below, __________ is the strongest acid.

Accepted Answer

A) HOAc 
B) HCHO2 
C) HClO 
D) HF 
E) HOAc and HCHO2 
A) HOAc 
B) HCHO2 
C) HClO 
D) HF 
E) HOAc and HCHO2

Question 10

The pH of a 0.30 M solution of a weak acid is 2.67. What is the Ka for this acid?

Accepted Answer

A) 2.1 × 10-4 
B) 4.4 × 10-4 
C) 1.5 × 10-4 
D) 6.6 × 10-4 
E) none of the above 
A) 2.1 × 10-4 
B) 4.4 × 10-4 
C) 1.5 × 10-4 
D) 6.6 × 10-4 
E) none of the above

Question 11

Which of the following acids will be the strongest?

Accepted Answer

A) H2SO4 
B) HSO4- 
C) H2SO3 
D) H2SeO4 
E) HSO3- 
A) H2SO4 
B) HSO4- 
C) H2SO3 
D) H2SeO4 
E) HSO3-

Question 12

The pH of a 0.25 M aqueous solution of hydrofluoric acid, HF, at 25.0°C is 2.03. What is the value of Ka for HF?

Accepted Answer

A) 2.0 × 10-9 
B) 1.1 × 10-9 
C) 6.0 × 10-5 
D) 3.5 × 10-4 
E) none of the above 
A) 2.0 × 10-9 
B) 1.1 × 10-9 
C) 6.0 × 10-5 
D) 3.5 × 10-4 
E) none of the above

Question 13

Calculate the pOH of a 0.0627 M aqueous sodium cyanide solution at 25.0°C. Kb for CN- is 4.9 × 10-10.

Accepted Answer

A) 9.33 
B) 10.00 
C) 5.25 
D) 1.20 
E) 8.75 
A) 9.33 
B) 10.00 
C) 5.25 
D) 1.20 
E) 8.75

Question 14

The Ka of hypochlorous acid (HClO)is 3.0 × 10-8 at 25.0°C. Calculate the pH of a 0.0335 M hypochlorous acid solution.

Accepted Answer

A) 3.02 
B) 9.50 
C) 4.50 
D) 6.52 
E) -3.02 
A) 3.02 
B) 9.50 
C) 4.50 
D) 6.52 
E) -3.02

Question 15

What is the pOH of a 0.035 M solution of barium hydroxide?

Accepted Answer

A) 12.85 
B) 12.54 
C) 1.46 
D) 1.15 
E) 10.41 
A) 12.85 
B) 12.54 
C) 1.46 
D) 1.15 
E) 10.41

Question 16

An aqueous solution contains 0.10 M NaOH. The solution is __________.

Accepted Answer

A) very dilute 
B) highly colored 
C) basic 
D) neutral 
E) acidic 
A) very dilute 
B) highly colored 
C) basic 
D) neutral 
E) acidic

Question 17

According to the Arrhenius concept, an acid is a substance that __________.

Accepted Answer

A) is capable of donating one or more H+ 
B) causes an increase in the concentration of H+ in aqueous solutions 
C) can accept a pair of electrons to form a coordinate covalent bond 
D) reacts with the solvent to form the cation formed by autoionization of that solvent 
E) tastes bitter 
A) is capable of donating one or more H+ 
B) causes an increase in the concentration of H+ in aqueous solutions 
C) can accept a pair of electrons to form a coordinate covalent bond 
D) reacts with the solvent to form the cation formed by autoionization of that solvent 
E) tastes bitter

Question 18

Calculate the pH of a 0.100 M aqueous solution of NH3. The Kb of NH3 is 1.77 × 10-5.

Accepted Answer

A) 8.95 
B) 11.12 
C) 2.88 
D) 12.12 
E) 1.87 
A) 8.95 
B) 11.12 
C) 2.88 
D) 12.12 
E) 1.87

Question 19

Which of the following aqueous solutions has the lowest [OH-]?

Accepted Answer

A) a solution with a pH of 3.0 
B) a 1 × 10-4 M solution of HNO3 
C) a solution with a pOH of 12.0 
D) pure water 
E) a 1 × 10-3 M solution of NH4Cl 
A) a solution with a pH of 3.0 
B) a 1 × 10-4 M solution of HNO3 
C) a solution with a pOH of 12.0 
D) pure water 
E) a 1 × 10-3 M solution of NH4Cl

Question 20

Of the compounds below, a 0.1 M aqueous solution of __________ will have the highest pH.

Accepted Answer

A) KCN, Ka of HCN = 4.0 × 10-10 
B) NH4NO3, Kb of NH3 = 1.8 × 10-5 
C) NaOAc, Ka of HOAc = 1.8 × 10-5 
D) NaClO, Ka of HClO = 3.2 × 10-8 
E) NaHS, Kb of HS- = 1.8 × 10-7 
A) KCN, Ka of HCN = 4.0 × 10-10 
B) NH4NO3, Kb of NH3 = 1.8 × 10-5 
C) NaOAc, Ka of HOAc = 1.8 × 10-5 
D) NaClO, Ka of HClO = 3.2 × 10-8 
E) NaHS, Kb of HS- = 1.8 × 10-7

Exam 16: Acid-Base Equilibria

A 0.1 M aqueous solution of __________ will have a pH of 7.0 at 25.0°C. NaOCl KCl NH4Cl Ca(OAc)2

The pH of an aqueous solution at 25.0 °C is 10.30. What is the molarity of H+ in this solution?

The Ka of hydrofluoric acid (HF)at 25.0 °C is 6.8 × 10-4. What is the pH of a 0.15 M aqueous solution of HF?

A- is a weak base. Which equilibrium corresponds to the equilibrium constant Ka for HA?

Determine the pH of a 0.35 M aqueous solution of CH3N H2 (methylamine). The Kb of methylamine is 4.4 × 10-4.

A 0.0035 M aqueous solution of a particular compound has pH = 2.46. The compound is __________.

Of the following acids, __________ is not a strong acid.

Using the data in the table, which of the conjugate bases below is the weakest base?

Of the acids in the table below, __________ is the strongest acid.

The pH of a 0.30 M solution of a weak acid is 2.67. What is the Ka for this acid?

Which of the following acids will be the strongest?

The pH of a 0.25 M aqueous solution of hydrofluoric acid, HF, at 25.0°C is 2.03. What is the value of Ka for HF?

Calculate the pOH of a 0.0627 M aqueous sodium cyanide solution at 25.0°C. Kb for CN- is 4.9 × 10-10.

The Ka of hypochlorous acid (HClO)is 3.0 × 10-8 at 25.0°C. Calculate the pH of a 0.0335 M hypochlorous acid solution.

What is the pOH of a 0.035 M solution of barium hydroxide?

An aqueous solution contains 0.10 M NaOH. The solution is __________.

According to the Arrhenius concept, an acid is a substance that __________.

Calculate the pH of a 0.100 M aqueous solution of NH3. The Kb of NH3 is 1.77 × 10-5.

Which of the following aqueous solutions has the lowest [OH-]?

Of the compounds below, a 0.1 M aqueous solution of __________ will have the highest pH.

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

Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

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 0.1 M aqueous solution of __________ will have a pH of 7.0 at 25.0°C. NaOCl KCl NH₄Cl Ca(OAc)₂

The pH of an aqueous solution at 25.0 °C is 10.30. What is the molarity of H⁺ in this solution?

The K_a of hydrofluoric acid (HF)at 25.0 °C is 6.8 × 10^-4. What is the pH of a 0.15 M aqueous solution of HF?

A- is a weak base. Which equilibrium corresponds to the equilibrium constant K_a for HA?

Determine the pH of a 0.35 M aqueous solution of CH₃N H₂ (methylamine). The K_b of methylamine is 4.4 × 10^-⁴.

The pH of a 0.30 M solution of a weak acid is 2.67. What is the K_a for this acid?

The pH of a 0.25 M aqueous solution of hydrofluoric acid, HF, at 25.0°C is 2.03. What is the value of K_a for HF?

Calculate the pOH of a 0.0627 M aqueous sodium cyanide solution at 25.0°C. K_b for CN^- is 4.9 × 10^-10.

The K_a of hypochlorous acid (HClO)is 3.0 × 10^-8 at 25.0°C. Calculate the pH of a 0.0335 M hypochlorous acid solution.

Calculate the pH of a 0.100 M aqueous solution of NH₃. The K_b of NH₃ is 1.77 × 10^-5.

Which of the following aqueous solutions has the lowest [OH^-]?