Question 1

What is the pOH of a 0.0150 M solution of barium hydroxide?

Accepted Answer

A)  12.5 
B)  1.52 
C)  10.4 
D)  1.82 
E)  12.2 
A)  12.5 
B)  1.52 
C)  10.4 
D)  1.82 
E)  12.2

Question 2

A solution of acetic acid is 2.0% dissociated at 25.0 oC. What was the original concentration ( in M) of the acetic acid solution? The Ka at 25.0 oC for acetic acid is 1.8 × 10- 5.

Accepted Answer

Question 3

Of the following, is a weak acid.

Accepted Answer

A)  HF 
B)  HClO4  
C)  HCl 
D)  HBr 
E)  HNO3 
A)  HF 
B)  HClO4  
C)  HCl 
D)  HBr 
E)  HNO3

Question 4

A 0.1 M aqueous solution of will have a pH of 7.0 at 25.0 °C.

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 5

Classify the following compounds as weak acids (W) or strong acids (S):

Accepted Answer

A)  S S S 
B)  W W W 
C)  S W W 
D)  W S W 
E)  W S S 
A)  S S S 
B)  W W W 
C)  S W W 
D)  W S W 
E)  W S S

Question 6

The conjugate acid of HSO4- is

Accepted Answer

A)  H+  
B)  H2SO4  
C)  HSO4+  
D)  HSO3+  
E)  SO42- 
A)  H+  
B)  H2SO4  
C)  HSO4+  
D)  HSO3+  
E)  SO42-

Question 7

Calculate the concentration (in M) of hydronium ions in a solution at 25.0 °C with a pOH of 4.223.

Accepted Answer

A)  5.98 × 10- 5 
B)  5.99 × 10- 19 
C)  1.00 × 10- 7 
D)  1.67 × 104 
E)  1.67 × 10- 10 
A)  5.98 × 10- 5 
B)  5.99 × 10- 19 
C)  1.00 × 10- 7 
D)  1.67 × 104 
E)  1.67 × 10- 10

Question 8

A Lewis acid is an electron- pair acceptor, and a Lewis base is an electron- pair donor.

Accepted Answer

A) True 
 B)False

Question 9

An aqueous solution contains 0.100 M NaOH at 25.0 °C. The pH of the solution is _ .

Accepted Answer

A)  7.00 
B)  - 1.00 
C)  1.00 
D)  0.100 
E)  13.0 
A)  7.00 
B)  - 1.00 
C)  1.00 
D)  0.100 
E)  13.0

Question 10

The acid- dissociation constant, Ka, for gallic acid is 4.57 × 10- 3. What is the base- dissociation constant, Kb, for the gallate ion?

Accepted Answer

A)  7.81 × 10- 6 
B)  5.43 × 10- 5 
C)  2.19 × 10- 12 
D)  2.19 × 102 
E)  4.57 × 10- 3 
A)  7.81 × 10- 6 
B)  5.43 × 10- 5 
C)  2.19 × 10- 12 
D)  2.19 × 102 
E)  4.57 × 10- 3

Question 11

What is the pH of a 0.0150 M aqueous solution of barium hydroxide?

Accepted Answer

A)  12.5 
B)  1.52 
C)  12.2 
D)  1.82 
E)  10.4 
A)  12.5 
B)  1.52 
C)  12.2 
D)  1.82 
E)  10.4

Question 12

Calculate the pOH of a 0.0827 M aqueous sodium cyanide solution at 25.0 °C. Kb for CN- is 4.9 × 10- 10.

Accepted Answer

A)  8.8 
B)  9.3 
C)  5.2 
D)  1.1 
E)  10 
A)  8.8 
B)  9.3 
C)  5.2 
D)  1.1 
E)  10

Question 13

An aqueous solution contains 0.050 M of methylamine. The concentration of hydroxide ion in this solution is _ M. Kb for methylamine is 4.4 × 10- 4.

Accepted Answer

A)  0.050 
B)  4.7 × 10- 3 
C)  2.2 × 10- 5 
D)  - 4.9 × 10- 3 
E)  4.5 × 10- 3 
A)  0.050 
B)  4.7 × 10- 3 
C)  2.2 × 10- 5 
D)  - 4.9 × 10- 3 
E)  4.5 × 10- 3

Question 14

Calculate the pH of a 0.500 M aqueous solution of NH3. The Kb of NH3 is 1.77 × 10- 5.

Accepted Answer

A)  2.52 
B)  8.95 
C)  5.05 
D)  11.5 
E)  3.01 
A)  2.52 
B)  8.95 
C)  5.05 
D)  11.5 
E)  3.01

Question 15

An aqueous solution of _ will produce a basic solution.

Accepted Answer

A)  NaHSO4  
B)  KBr 
C)  Na2SO3  
D)  NaCl 
E)  NH4ClO4 
A)  NaHSO4  
B)  KBr 
C)  Na2SO3  
D)  NaCl 
E)  NH4ClO4

Question 16

In which of the following aqueous solutions does the weak acid exhibit the highest percentage ionization?

Accepted Answer

A)  0.01 M HC2H3O2 (Ka = 1.8 × 10- 5) 
B)  0.01 M HClO (Ka = 3.0 × 10- 8) 
C)  0.01 M HNO2 (Ka = 4.5 × 10- 4) 
D)  0.01 M HF (Ka = 6.8 × 10- 4) 
E)  These will all exhibit the same percentage ionization. 
A)  0.01 M HC2H3O2 (Ka = 1.8 × 10- 5) 
B)  0.01 M HClO (Ka = 3.0 × 10- 8) 
C)  0.01 M HNO2 (Ka = 4.5 × 10- 4) 
D)  0.01 M HF (Ka = 6.8 × 10- 4) 
E)  These will all exhibit the same percentage ionization.

Question 17

What is the pH of an aqueous solution at 25.0 °C that contains 3.98 × 10- 9 M hydroxide ion?

Accepted Answer

A)  3.98 
B)  5.60 
C)  7.00 
D)  8.40 
E)  9.00 
A)  3.98 
B)  5.60 
C)  7.00 
D)  8.40 
E)  9.00

Question 18

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

Accepted Answer

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

Question 19

The Ka of hypochlorous acid (HClO) is 3.00 × 10- 8 at 25.0 °C. Calculate the pH of a 0.0385 M hypochlorous acid solution.

Accepted Answer

A)  - 1.41 
B)  7.52 
C)  1.41 
D)  8.94 
E)  4.47 
A)  - 1.41 
B)  7.52 
C)  1.41 
D)  8.94 
E)  4.47

Question 20

Which of the following acids will be the strongest?

Accepted Answer

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

Exam 16: Acid-Base Equilibria

What is the pOH of a 0.0150 M solution of barium hydroxide?

A solution of acetic acid is 2.0% dissociated at 25.0 oC. What was the original concentration ( in M) of the acetic acid solution? The Ka at 25.0 oC for acetic acid is 1.8 × 10- 5.

Of the following, is a weak acid.

A 0.1 M aqueous solution of will have a pH of 7.0 at 25.0 °C.

Classify the following compounds as weak acids (W) or strong acids (S):

The conjugate acid of HSO4- is

Calculate the concentration (in M) of hydronium ions in a solution at 25.0 °C with a pOH of 4.223.

A Lewis acid is an electron- pair acceptor, and a Lewis base is an electron- pair donor.

An aqueous solution contains 0.100 M NaOH at 25.0 °C. The pH of the solution is _ .

The acid- dissociation constant, Ka, for gallic acid is 4.57 × 10- 3. What is the base- dissociation constant, Kb, for the gallate ion?

What is the pH of a 0.0150 M aqueous solution of barium hydroxide?

Calculate the pOH of a 0.0827 M aqueous sodium cyanide solution at 25.0 °C. Kb for CN- is 4.9 × 10- 10.

An aqueous solution contains 0.050 M of methylamine. The concentration of hydroxide ion in this solution is _ M. Kb for methylamine is 4.4 × 10- 4.

Calculate the pH of a 0.500 M aqueous solution of NH3. The Kb of NH3 is 1.77 × 10- 5.

An aqueous solution of _ will produce a basic solution.

In which of the following aqueous solutions does the weak acid exhibit the highest percentage ionization?

What is the pH of an aqueous solution at 25.0 °C that contains 3.98 × 10- 9 M hydroxide ion?

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

The Ka of hypochlorous acid (HClO) is 3.00 × 10- 8 at 25.0 °C. Calculate the pH of a 0.0385 M hypochlorous acid solution.

Which of the following acids will be the strongest?

Introduction: Matter and Measurement

Atoms, Molecules, and Ions

Stoichiometry: Calculations With Chemical Formulas and Equations

Aqueous Reactions and Solution Stoichiometry

Electronic Structure of Atoms

Periodic Properties of the Elements

Basic Concepts of Chemical Bonding

Gases

Intermolecular Forces, Liquids, and Solids

Modern Materials

Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Additional Aspects of Equilibria

Chemistry of the Environment

Chemical Thermodynamics

Electrochemistry

Nuclear Chemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Chemistry of Coordination Compounds

The Chemistry of Life: Organic and Biological Chemistry

Filters

A solution of acetic acid is 2.0% dissociated at 25.0 ^oC. What was the original concentration ( in M) of the acetic acid solution? The K_aat 25.0 ^oC for acetic acid is 1.8 × 10^-⁵.

The conjugate acid of HSO₄^-is

The acid- dissociation constant, K_a, for gallic acid is 4.57 × 10^-³. What is the base- dissociation constant, K_b, for the gallate ion?

Calculate the pOH of a 0.0827 M aqueous sodium cyanide solution at 25.0 °C. K_bfor CN^-is 4.9 × 10^-¹⁰.

An aqueous solution contains 0.050 M of methylamine. The concentration of hydroxide ion in this solution is _ M. K_bfor methylamine is 4.4 × 10^-⁴.

Calculate the pH of a 0.500 M aqueous solution of NH₃. The K_bof NH₃is 1.77 × 10^-⁵.

What is the pH of an aqueous solution at 25.0 °C that contains 3.98 × 10^-⁹M hydroxide ion?

The K_aof hypochlorous acid (HClO) is 3.00 × 10^-⁸at 25.0 °C. Calculate the pH of a 0.0385 M hypochlorous acid solution.