Question 1

The reaction between acetic acid (CH3COOH) and water is written as

Accepted Answer

A)  CH3COOH + H2O   CH2COOH- + H3O+ 
B)  CH3COOH + H2O   CH3COO- + OH- 
C)  CH3COOH + H2O   CH3COOH2+ + OH- 
D)  CH3COOH + H2O   CH3COO- + H3O+ 
E)  CH3COOH + H2O   CH3CO- + OH- + H2O 
A)  CH3COOH + H2O   CH2COOH- + H3O+ 
B)  CH3COOH + H2O   CH3COO- + OH- 
C)  CH3COOH + H2O   CH3COOH2+ + OH- 
D)  CH3COOH + H2O   CH3COO- + H3O+ 
E)  CH3COOH + H2O   CH3CO- + OH- + H2O D

Question 2

Phenolphthalein is an acid-base indicator that is colorless in its acid form and pink in its basic form, changing at pH = 8.5. Bromcresol green is yellow in its acidic form and blue in its basic form, changing at pH = 4.8. A solution is colorless in phenolphthalein and blue in bromcresol green. Therefore we can conclude that the pH of the solution is ____.

Accepted Answer

A)  exactly 7.0 
B)  greater than 8.5 
C)  between 7.0 and 8.5 
D)  between 4.8 and 8.5 
E)  less than 4.8 
A)  exactly 7.0 
B)  greater than 8.5 
C)  between 7.0 and 8.5 
D)  between 4.8 and 8.5 
E)  less than 4.8 D

Question 3

Which cannot act as a Bronsted-Lowry acid?

Accepted Answer

A)  HPO42- 
B)  H3O+ 
C)  CH3COO- 
D)  CH3NH3+ 
E)  HCOOH 
A)  HPO42- 
B)  H3O+ 
C)  CH3COO- 
D)  CH3NH3+ 
E)  HCOOH C

Question 4

If the pH of a solution is raised from 6.27 to 7.57

Accepted Answer

A)  the solution has gone from acidic to basic 
B)  [H3O+] has increased by a factor of 10 
C)  [OH-] has increased by a factor of 10 
D)  the new [OH-] = 2.7 × 10-8 
E)  the new [H3O+] = 5.4 × 10-7 
A)  the solution has gone from acidic to basic 
B)  [H3O+] has increased by a factor of 10 
C)  [OH-] has increased by a factor of 10 
D)  the new [OH-] = 2.7 × 10-8 
E)  the new [H3O+] = 5.4 × 10-7

Question 5

Which substance cannot act as a Bronsted-Lowry base?

Accepted Answer

A)  OH- 
B)  CH3NH2 
C)  NH4+ 
D)  NH3 
E)  HSO4- 
A)  OH- 
B)  CH3NH2 
C)  NH4+ 
D)  NH3 
E)  HSO4-

Question 6

Calculate the pH of a solution where [OH-] = 4.6 × 10-4. Is this solution acidic or basic?

Accepted Answer

A)  3.34; acidic 
B)  3.34; basic 
C)  9.40; basic 
D)  10.66; acidic 
E)  10.66; basic 
A)  3.34; acidic 
B)  3.34; basic 
C)  9.40; basic 
D)  10.66; acidic 
E)  10.66; basic

Question 7

The poison strychnine is a weakly basic compound with Kb = 1.8 × 10-6. What is the pH of a 0.058 M solution of strychnine?

Accepted Answer

A)  3.49 
B)  7.30 
C)  8.26 
D)  10.51 
E)  12.76 
A)  3.49 
B)  7.30 
C)  8.26 
D)  10.51 
E)  12.76

Question 8

In terms of acid strength, which acid does not belong in a category with the others?

Accepted Answer

A)  HNO2 
B)  HClO4 
C)  HCOOH 
D)  HF 
E)  H2SO3 
A)  HNO2 
B)  HClO4 
C)  HCOOH 
D)  HF 
E)  H2SO3

Question 9

Consider a 0.50 M solution of HNO2, a weak acid with Ka = 4.5 × 10-4. Which statement is true?

Accepted Answer

A)  [H3O+] = 0.50 M. 
B)  The acid is mostly ionized. 
C)  pH = 3.35. 
D)  pH = 0.32. 
E)  pH > 0.32. 
A)  [H3O+] = 0.50 M. 
B)  The acid is mostly ionized. 
C)  pH = 3.35. 
D)  pH = 0.32. 
E)  pH > 0.32.

Question 10

Which of the following salts forms an acidic solution when dissolved in water?

Accepted Answer

A)  LiF 
B)  K3PO4 
C)  NH4ClO4 
D)  NaOCl 
E)  NaNO3 
A)  LiF 
B)  K3PO4 
C)  NH4ClO4 
D)  NaOCl 
E)  NaNO3

Question 11

The value of the ionization constant for a weak acid HA is 4.2 × 10-7. What is the pH of a 0.35 M solution of this acid?

Accepted Answer

A)  6.83 
B)  6.38 
C)  3.42 
D)  3.19 
E)  2.96 
A)  6.83 
B)  6.38 
C)  3.42 
D)  3.19 
E)  2.96

Question 12

The pH of a 0.172 M solution of benzoic acid (Ka = 6.31 × 10-5) is

Accepted Answer

A)  2.48. 
B)  3.44. 
C)  4.37. 
D)  4.96. 
E)  5.63. 
A)  2.48. 
B)  3.44. 
C)  4.37. 
D)  4.96. 
E)  5.63.

Question 13

The reaction between the ion of a weak acid or a weak base and water is called a(n) ____ reaction.

Accepted Answer

A)  autoionization 
B)  hydrolysis 
C)  decomposition 
D)  neutralization 
E)  proteomic 
A)  autoionization 
B)  hydrolysis 
C)  decomposition 
D)  neutralization 
E)  proteomic

Question 14

Which compound is the most acidic?

Accepted Answer

A)  GeH4 
B)  H2Se 
C)  HBr 
D)  AsH3 
E)  H2O 
A)  GeH4 
B)  H2Se 
C)  HBr 
D)  AsH3 
E)  H2O

Question 15

Which reaction illustrates water acting as a base?

Accepted Answer

A)  Cu(H2O)42+ + 4 NH3 Cu(NH3)42+ + 4 H2O 
B)  H2CO3 H2O + CO2 
C)  NH3 + H2O NH4+ + OH- 
D)  H2PO4- + H2O OH- + H3PO4 
E)  HSO4- + H2O H3O+ + SO42- 
A)  Cu(H2O)42+ + 4 NH3 Cu(NH3)42+ + 4 H2O 
B)  H2CO3 H2O + CO2 
C)  NH3 + H2O NH4+ + OH- 
D)  H2PO4- + H2O OH- + H3PO4 
E)  HSO4- + H2O H3O+ + SO42-

Question 16

In this reaction

Accepted Answer

A)  NH3 acts as a base and OH- as an acid. 
B)  H2O acts as an acid and NH3 as a base. 
C)  H2O acts as a base and NH4+ as an acid. 
D)  H2O acts as an acid and NH4+ as a base. 
E)  NH3 acts as an acid and OH- as a base. 
A)  NH3 acts as a base and OH- as an acid. 
B)  H2O acts as an acid and NH3 as a base. 
C)  H2O acts as a base and NH4+ as an acid. 
D)  H2O acts as an acid and NH4+ as a base. 
E)  NH3 acts as an acid and OH- as a base.

Question 17

Answer the following questions:
A)	Write the reaction for the ionization of the weak acid HA in water.
B)	Write the reaction for the hydrolysis of the conjugate base of the weak acid HA in water.
C)	Using equilibrium constant expressions for the reaction of HA and of its conjugate base A- with water, prove that the product of Ka for a weak acid and Kb for its conjugate base equals 1.0 ´ 10-14 at 25°C.

Accepted Answer

A) HA + H₂O ⇌ A^- + H₃O⁺ B) A^- + H₂O

Question 18

The pH of a solution of a 0.15 M solution of HOCl is 4.14. What is the Ka for HOCl?

Accepted Answer

A)  5.7 × 10-2 
B)  8.8 × 10-3 
C)  4.8 × 10-4 
D)  7.2 × 10-5 
E)  3.5 × 10-8 
A)  5.7 × 10-2 
B)  8.8 × 10-3 
C)  4.8 × 10-4 
D)  7.2 × 10-5 
E)  3.5 × 10-8

Question 19

The pH of a 0.50 M solution of the weak monoprotic acid HA is 4.76. The value of Ka is

Accepted Answer

A)  6.0 × 10-10 
B)  1.7 × 10-5 
C)  3.5 × 10-5 
D)  7.6 × 10-4 
E)  9.24 
A)  6.0 × 10-10 
B)  1.7 × 10-5 
C)  3.5 × 10-5 
D)  7.6 × 10-4 
E)  9.24

Question 20

As the pH of a solution rises, [H3O+] ____, pOH ____, and [OH-] ____.

Accepted Answer

A)  rises; falls; rises 
B)  falls; rises; falls 
C)  falls; falls; rises 
D)  rises; falls; falls 
E)  falls, falls, falls 
A)  rises; falls; rises 
B)  falls; rises; falls 
C)  falls; falls; rises 
D)  rises; falls; falls 
E)  falls, falls, falls

The reaction between acetic acid (CH₃COOH) and water is written as

Which cannot act as a Bronsted-Lowry acid?

If the pH of a solution is raised from 6.27 to 7.57

Which substance cannot act as a Bronsted-Lowry base?

Calculate the pH of a solution where [OH^-] = 4.6 × 10^-4. Is this solution acidic or basic?

The poison strychnine is a weakly basic compound with K_b = 1.8 × 10^-6. What is the pH of a 0.058 M solution of strychnine?

In terms of acid strength, which acid does not belong in a category with the others?

Consider a 0.50 M solution of HNO₂, a weak acid with K_a = 4.5 × 10^-4. Which statement is true?

Which of the following salts forms an acidic solution when dissolved in water?

The value of the ionization constant for a weak acid HA is 4.2 × 10^-7. What is the pH of a 0.35 M solution of this acid?

The pH of a 0.172 M solution of benzoic acid (K_a = 6.31 × 10^-5) is

The reaction between the ion of a weak acid or a weak base and water is called a(n) ____ reaction.

Which compound is the most acidic?

Which reaction illustrates water acting as a base?

In this reaction

The pH of a solution of a 0.15 M solution of HOCl is 4.14. What is the K_a for HOCl?

The pH of a 0.50 M solution of the weak monoprotic acid HA is 4.76. The value of K_a is

As the pH of a solution rises, [H₃O⁺] , pOH , and [OH^-] .

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Exam 15: Acids and Bases

The reaction between acetic acid (CH3COOH) and water is written as

Which cannot act as a Bronsted-Lowry acid?

If the pH of a solution is raised from 6.27 to 7.57

Which substance cannot act as a Bronsted-Lowry base?

Calculate the pH of a solution where [OH-] = 4.6 × 10-4. Is this solution acidic or basic?

The poison strychnine is a weakly basic compound with Kb = 1.8 × 10-6. What is the pH of a 0.058 M solution of strychnine?

In terms of acid strength, which acid does not belong in a category with the others?

Consider a 0.50 M solution of HNO2, a weak acid with Ka = 4.5 × 10-4. Which statement is true?

Which of the following salts forms an acidic solution when dissolved in water?

The value of the ionization constant for a weak acid HA is 4.2 × 10-7. What is the pH of a 0.35 M solution of this acid?

The pH of a 0.172 M solution of benzoic acid (Ka = 6.31 × 10-5) is

The reaction between the ion of a weak acid or a weak base and water is called a(n) ____ reaction.

Which compound is the most acidic?

Which reaction illustrates water acting as a base?

In this reaction

The pH of a solution of a 0.15 M solution of HOCl is 4.14. What is the Ka for HOCl?

The pH of a 0.50 M solution of the weak monoprotic acid HA is 4.76. The value of Ka is

As the pH of a solution rises, [H3O+] ____, pOH ____, and [OH-] ____.

The Nature of Chemistry

Atoms and Elements

Chemical Compounds

Quantities of Reactants and Products

Chemical Reactions

Energy and Chemical Reactions

Electron Configurations and the Periodic Table

Covalent Bonding

Molecular Structure

Gases and the Atmosphere

Liquids, Solids, and Materials

Chemical Kinetics: Rates of Reactions

Chemical Equilibrium

The Chemistry of Solutes and Solutions

Additional Aqueous Equilibria

Thermodynamics: Directionality of Chemical Reactions

Electrochemistry and Its Applications

Nuclear Chemistry

Filters

The reaction between acetic acid (CH₃COOH) and water is written as

Calculate the pH of a solution where [OH^-] = 4.6 × 10^-4. Is this solution acidic or basic?

The poison strychnine is a weakly basic compound with K_b = 1.8 × 10^-6. What is the pH of a 0.058 M solution of strychnine?

Consider a 0.50 M solution of HNO₂, a weak acid with K_a = 4.5 × 10^-4. Which statement is true?

The value of the ionization constant for a weak acid HA is 4.2 × 10^-7. What is the pH of a 0.35 M solution of this acid?

The pH of a 0.172 M solution of benzoic acid (K_a = 6.31 × 10^-5) is

The pH of a solution of a 0.15 M solution of HOCl is 4.14. What is the K_a for HOCl?

The pH of a 0.50 M solution of the weak monoprotic acid HA is 4.76. The value of K_a is

As the pH of a solution rises, [H₃O⁺] , pOH , and [OH^-] .