Question 1

Define a conjugate acid-base pair and provide an example.

Accepted Answer

A conjugate acid-base pair are

Question 2

Bromocresol green is yellow in its acidic form and blue in its basic form. When is it green?

Accepted Answer

A)  at the equivalence point in a titration 
B)  in its neutral form 
C)  when the solution pH equals its pKa 
D)  when the solution pH equals 7 
E)  at the midpoint in a titration 
A)  at the equivalence point in a titration 
B)  in its neutral form 
C)  when the solution pH equals its pKa 
D)  when the solution pH equals 7 
E)  at the midpoint in a titration

Question 3

Which statement about nitrous acid and nitric acid is correct?

Accepted Answer

A)  They are both weak acids. 
B)  They are both strong acids. 
C)  They both have one ionizable proton. 
D)  Nitrous acid has the formula HNO3. 
E)  Nitric acid has the formula HNO2. 
A)  They are both weak acids. 
B)  They are both strong acids. 
C)  They both have one ionizable proton. 
D)  Nitrous acid has the formula HNO3. 
E)  Nitric acid has the formula HNO2.

Question 4

When pure water autoionizes, the following species are produced: __________

Accepted Answer

A)  O2-, OH-, H3O+, and H2O+. 
B)  OH- and H3O+. 
C)  O2- and H4O2+. 
D)  H+ and OH-. 
E)  2H+ and O2-. 
A)  O2-, OH-, H3O+, and H2O+. 
B)  OH- and H3O+. 
C)  O2- and H4O2+. 
D)  H+ and OH-. 
E)  2H+ and O2-.

Question 5

Boric acid frequently is used as an eyewash to treat eye infections. The pH of a 0.050 M solution of boric acid is 5.28. What is the value of the boric acid ionization constant, Ka?

Accepted Answer

A)  5.25 F1F1F1S1F1F1F10 10-6 
B)  5.51 F1F1F1S1F1F1F10 10-10 
C)  5.43 F1F1F1S1F1F1F10 10-8 
D)  5.79 F1F1F1S1F1F1F10 10-4 
E)  5.33 F1F1F1S1F1F1F10 10-12 
A)  5.25 F1F1F1S1F1F1F10 10-6 
B)  5.51 F1F1F1S1F1F1F10 10-10 
C)  5.43 F1F1F1S1F1F1F10 10-8 
D)  5.79 F1F1F1S1F1F1F10 10-4 
E)  5.33 F1F1F1S1F1F1F10 10-12

Question 6

A cup of coffee has a hydroxide ion concentration of 1.0 F1F1F1S1F1F1F10 10-10 M. What is the pH of this coffee?

Accepted Answer

A)  1.0 F1F1F1S1F1F1F10 10-4 
B)  4 
C)  10 
D)  7 
E)  -10 
A)  1.0 F1F1F1S1F1F1F10 10-4 
B)  4 
C)  10 
D)  7 
E)  -10

Question 7

A solution with a pOH of 4.3 has a [H+] of __________

Accepted Answer

A)  6.8 F1F1F1S1F1F1F10 10-9 M. 
B)  3.2 F1F1F1S1F1F1F10 10-4 M. 
C)  4.8 F1F1F1S1F1F1F10 10-5 M. 
D)  2.0 F1F1F1S1F1F1F10 10-10 M. 
E)  4.3 M. 
A)  6.8 F1F1F1S1F1F1F10 10-9 M. 
B)  3.2 F1F1F1S1F1F1F10 10-4 M. 
C)  4.8 F1F1F1S1F1F1F10 10-5 M. 
D)  2.0 F1F1F1S1F1F1F10 10-10 M. 
E)  4.3 M.

Question 8

The stronger the acid, __________

Accepted Answer

A)  the stronger its conjugate base. 
B)  the weaker its conjugate base. 
C)  the more concentrated the acid. 
D)  the less concentrated the conjugate base. 
E)  the more concentrated the conjugate base. 
A)  the stronger its conjugate base. 
B)  the weaker its conjugate base. 
C)  the more concentrated the acid. 
D)  the less concentrated the conjugate base. 
E)  the more concentrated the conjugate base.

Question 9

What is the pH of a 0.010 M solution of acetic acid? Ka for acetic acid is 1.8 F1F1F1S1F1F1F10 10-5

Accepted Answer

A)  2.74 
B)  4.74 
C)  2.00 
D)  3.37 
E)  6.74 
A)  2.74 
B)  4.74 
C)  2.00 
D)  3.37 
E)  6.74

Question 10

What is the concentration of [OH-] in a 0.20 M solution of ammonia? The Kb value for ammonia is 1.8 F1F1F1S1F1F1F10 10-5.

Accepted Answer

A)  3.6 F1F1F1S1F1F1F10 10-6 M 
B)  1.8 F1F1F1S1F1F1F10 10-5 M 
C)  0.20 M 
D)  1.9 F1F1F1S1F1F1F10 10-3 M 
E)  4.2 F1F1F1S1F1F1F10 10-4 M 
A)  3.6 F1F1F1S1F1F1F10 10-6 M 
B)  1.8 F1F1F1S1F1F1F10 10-5 M 
C)  0.20 M 
D)  1.9 F1F1F1S1F1F1F10 10-3 M 
E)  4.2 F1F1F1S1F1F1F10 10-4 M

Question 11

In evaluating the pH of an aqueous weak acid solution, __________ usually can be ignored.

Accepted Answer

A)  the concentration of the weak acid 
B)  the concentration of hydronium ion produced by the autoionization of water 
C)  the reaction of the weak acid with water 
D)  the concentration of the ionized hydronium ion 
E)  the concentration of the conjugate base 
A)  the concentration of the weak acid 
B)  the concentration of hydronium ion produced by the autoionization of water 
C)  the reaction of the weak acid with water 
D)  the concentration of the ionized hydronium ion 
E)  the concentration of the conjugate base

Question 12

Identify the dominant species that determine the pH at the following points in the titration of a monoprotic weak acid with a strong base, NaOH, and write the relevant reaction equation for each that produces hydronium ion or hydroxide ion.
(1) at the beginning
(2) halfway to the equivalence point
(3) at the equivalence point
(4) past the equivalence point

Accepted Answer

(1) At the beginning, ionization of the

Question 13

A solution of the weak acid, HF, and a solution of the strong acid, HCl, have the same pH. Which solution will require the most sodium hydroxide, NaOH, to neutralize?

Accepted Answer

A)  HCl, because it is a strong acid and dissociates completely. 
B)  HF, because its concentration is larger. 
C)  Both will require the same amount because the concentrations are equal. 
D)  Both will require the same amount because the H3O+ concentrations are the same. 
E)  HCl, because the stronger acid has the higher concentration. 
A)  HCl, because it is a strong acid and dissociates completely. 
B)  HF, because its concentration is larger. 
C)  Both will require the same amount because the concentrations are equal. 
D)  Both will require the same amount because the H3O+ concentrations are the same. 
E)  HCl, because the stronger acid has the higher concentration.

Question 14

The degree of ionization of a weak acid __________
(I) varies with the concentration of the acid.
(II) depends on which weak acid it is.
(III) is 100%.
(IV) is greater than 50% but less than 100%.

Accepted Answer

A)  I only 
B)  II only 
C)  III only 
D)  both I and II 
E)  IV only 
A)  I only 
B)  II only 
C)  III only 
D)  both I and II 
E)  IV only

Question 15

When [H+] = 1.0 F1F1F1S1F1F1F10 10-7 M in water at 25°C, then __________

Accepted Answer

A)  pH = 1. 
B)  pH = 10-7. 
C)  [OH-] = 1.0 F1F1F1S1F1F1F10 10-7 M. 
D)  [OH-] = 1.0 F1F1F1S1F1F1F10 107 M. 
E)  [OH-] = 0 M. 
A)  pH = 1. 
B)  pH = 10-7. 
C)  [OH-] = 1.0 F1F1F1S1F1F1F10 10-7 M. 
D)  [OH-] = 1.0 F1F1F1S1F1F1F10 107 M. 
E)  [OH-] = 0 M.

Question 16

What reaction occurs as a hydrochloric acid solution is added to a solution containing equal concentrations of acetic acid and sodium acetate?

Accepted Answer

A)  CH3COOH + H+ F1F1F1S1F1F1F10 CH3COOH2+ 
B)  CH3COO- + H+ F1F1F1S1F1F1F10 CH3COOH 
C)  CH3COOH + HCl F1F1F1S1F1F1F10 CH3COO- + H2Cl+ 
D)  2CH3COO- + 2H+ F1F1F1S1F1F1F10 CH3COO + H2 
E)  CH3COOH + H+ F1F1F1S1F1F1F10 CH3CO+ + H2O 
A)  CH3COOH + H+ F1F1F1S1F1F1F10 CH3COOH2+ 
B)  CH3COO- + H+ F1F1F1S1F1F1F10 CH3COOH 
C)  CH3COOH + HCl F1F1F1S1F1F1F10 CH3COO- + H2Cl+ 
D)  2CH3COO- + 2H+ F1F1F1S1F1F1F10 CH3COO + H2 
E)  CH3COOH + H+ F1F1F1S1F1F1F10 CH3CO+ + H2O

Define a conjugate acid-base pair and provide an example.

Bromocresol green is yellow in its acidic form and blue in its basic form. When is it green?

Which statement about nitrous acid and nitric acid is correct?

When pure water autoionizes, the following species are produced: __________

Boric acid frequently is used as an eyewash to treat eye infections. The pH of a 0.050 M solution of boric acid is 5.28. What is the value of the boric acid ionization constant, K_a?

A cup of coffee has a hydroxide ion concentration of 1.0  10^-¹⁰ M. What is the pH of this coffee?

A solution with a pOH of 4.3 has a [H⁺] of __________

The stronger the acid, __________

What is the pH of a 0.010 M solution of acetic acid? K_a for acetic acid is 1.8  10^-⁵

What is the concentration of [OH^-] in a 0.20 M solution of ammonia? The K_b value for ammonia is 1.8  10^-⁵.

In evaluating the pH of an aqueous weak acid solution, __________ usually can be ignored.

A solution of the weak acid, HF, and a solution of the strong acid, HCl, have the same pH. Which solution will require the most sodium hydroxide, NaOH, to neutralize?

The degree of ionization of a weak acid __________ (I) varies with the concentration of the acid. (II) depends on which weak acid it is. (III) is 100%. (IV) is greater than 50% but less than 100%.

When [H⁺] = 1.0  10^-⁷ M in water at 25°C, then __________

What reaction occurs as a hydrochloric acid solution is added to a solution containing equal concentrations of acetic acid and sodium acetate?

Matter, Energy, and the Origins of the Universe

Atoms, Ions, and Compounds

Chemical Reactions and Earths Composition

Solution Chemistry and the Hydrosphere

Thermochemistry

Properties of Gases: the Air We Breathe

Electrons in Atoms and Periodic Properties

Chemical Bonding and Climate Change

Molecular Geometry and Bonding Theories

Forces Between Ions and Molecules

Solutions and Their Colligative Properties

The Chemistry of Solids

Organic Chemistry: Fuels, Pharmaceuticals, and Materials

Thermodynamics: Spontaneous Processes, Entropy, and Free Energy

Chemical Kinetics

Chemical Equilibrium

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Electrochemistry and the Quest for Clean Energy

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Exam 17: Equilibrium in the Aqueous Phase

Define a conjugate acid-base pair and provide an example.

Bromocresol green is yellow in its acidic form and blue in its basic form. When is it green?

Which statement about nitrous acid and nitric acid is correct?

When pure water autoionizes, the following species are produced: __________

Boric acid frequently is used as an eyewash to treat eye infections. The pH of a 0.050 M solution of boric acid is 5.28. What is the value of the boric acid ionization constant, Ka?

A cup of coffee has a hydroxide ion concentration of 1.0  10-10 M. What is the pH of this coffee?

A solution with a pOH of 4.3 has a [H+] of __________

The stronger the acid, __________

What is the pH of a 0.010 M solution of acetic acid? Ka for acetic acid is 1.8  10-5

What is the concentration of [OH-] in a 0.20 M solution of ammonia? The Kb value for ammonia is 1.8  10-5.

In evaluating the pH of an aqueous weak acid solution, __________ usually can be ignored.

A solution of the weak acid, HF, and a solution of the strong acid, HCl, have the same pH. Which solution will require the most sodium hydroxide, NaOH, to neutralize?

The degree of ionization of a weak acid __________ (I) varies with the concentration of the acid. (II) depends on which weak acid it is. (III) is 100%. (IV) is greater than 50% but less than 100%.

When [H+] = 1.0  10-7 M in water at 25°C, then __________

What reaction occurs as a hydrochloric acid solution is added to a solution containing equal concentrations of acetic acid and sodium acetate?

Matter, Energy, and the Origins of the Universe

Atoms, Ions, and Compounds

Chemical Reactions and Earths Composition

Solution Chemistry and the Hydrosphere

Thermochemistry

Properties of Gases: the Air We Breathe

Electrons in Atoms and Periodic Properties

Chemical Bonding and Climate Change

Molecular Geometry and Bonding Theories

Forces Between Ions and Molecules

Solutions and Their Colligative Properties

The Chemistry of Solids

Organic Chemistry: Fuels, Pharmaceuticals, and Materials

Thermodynamics: Spontaneous Processes, Entropy, and Free Energy

Chemical Kinetics

Chemical Equilibrium

The Colorful Chemistry of Metals

Electrochemistry and the Quest for Clean Energy

Biochemistry: the Compounds of Life

Nuclear Chemistry

Life and the Periodic Table

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Boric acid frequently is used as an eyewash to treat eye infections. The pH of a 0.050 M solution of boric acid is 5.28. What is the value of the boric acid ionization constant, K_a?

A cup of coffee has a hydroxide ion concentration of 1.0  10^-¹⁰ M. What is the pH of this coffee?

A solution with a pOH of 4.3 has a [H⁺] of __________

What is the pH of a 0.010 M solution of acetic acid? K_a for acetic acid is 1.8  10^-⁵

What is the concentration of [OH^-] in a 0.20 M solution of ammonia? The K_b value for ammonia is 1.8  10^-⁵.

When [H⁺] = 1.0  10^-⁷ M in water at 25°C, then __________