Question 1

If Na2HPO4 is added to water, what other compound could also be added in order to make a buffered solution?

Accepted Answer

A)  H3PO4
B)  NaHPO4
C)  NaH2PO4
D)  Na2PO3
E)  NaCl

Question 2

Select the solution below that is the most acidic.

Accepted Answer

A)  [OH-] = 1.0 × 10-4 M
B)  [OH-] = 1.0 × 10-5 M
C)  [H3O+] = 1.0 × 10-6 M
D)  [H3O+] = 1.0 × 10-8 M
E)  [H3O+] = 1.0 × 10-10 M

Question 3

If NaH2PO4 is added to water, what other compound or compounds could also be added in order to make a buffered solution?

Accepted Answer

A)  H3PO4 only
B)  NaHPO4 only
C)  Na2HPO4 only
D)  Na2PO3 only
E)  either H3PO4 or Na2HPO4

Question 4

The substance NaOH(aq) is

Accepted Answer

A)  a strong acid.
B)  a weak acid.
C)  a strong base.
D)  a weak base.
E)  neither an acid nor a base.

Question 5

Which of the following is an amphoteric substance?

Accepted Answer

A)  NaCl
B)  LiOH
C)  KBr
D)  NaHCO3
E)  CH3OH

Question 6

The substance Mg(OH) 2(aq) is

Accepted Answer

A)  a strong acid.
B)  a weak acid.
C)  a strong base.
D)  a weak base.
E)  neither an acid nor a base.

Question 7

If the pH of a blood sample is 7.60, what is the H3O+ concentration in the blood?

Accepted Answer

A)  7.6 M
B)  2.5 × 10-8 M
C)  2.5 × 10-7 M
D)  2.5 × 10-9 M
E)  6.4 M

Question 8

The H3O+ concentration in a 0.010 M solution of NaOH is 0.010 M.

Accepted Answer

A) True 
 B)False

Question 9

All of the following species are weak bases except:

Accepted Answer

A)  NaCN(aq) 
B)  K2CO3(aq) 
C)  KOH(aq) 
D)  CH3NH2(aq) 
E)  NH3(aq)

Question 10

Calculate the pH of a solution that has [H3O+] = 5.9 × 10-5 M.

Accepted Answer

A)  pH = 5.90
B)  pH = 4.23
C)  pH = 5.00
D)  pH = 5.59
E)  pH = 9.77

Question 11

List the species present in order of increasing concentration in a 0.1 M solution of H2C2O4.

Accepted Answer

A)  H2C2O4 2O4− 2O42−
B)  H2C2O4 2O42− 2O4−
C)  C2O42− 2O4− 2C2O4
D)  HC2O4− 2O42− 2C2O4
E)  C2O42− 2C2O4 2O4−

Question 12

Which of the following equations represents the behavior of HCO3− as an acid?

Accepted Answer

A)  HCO3−(aq) + H3O+(aq) ⇌ H2CO3(aq) + H2O(l) 
B)  HCO3−(aq) + HF(aq) ⇌ H2CO3(aq) + F−(aq) 
C)  HCO3−(aq) + HCN(aq) ⇌ H2CO3(aq) + CN−(aq) 
D)  HCO3−(aq) + OH−(aq) ⇌ CO32−(aq) + H2O(l) 
E)  HCO3−(aq) + H2O(l) ⇌ H2CO3(aq) + OH−(aq)

Question 13

Which of the following acids is not normally found in foods or beverages?

Accepted Answer

A)  citric acid
B)  acetic acid
C)  phosphoric acid
D)  carbonic acid
E)  sulfuric acid

Question 14

Which of the following will not change when an acid is added to water?

Accepted Answer

A)  pH
B)  pOH
C)  Kw
D)  hydronium ion concentration
E)  hydroxide ion concentration

Question 15

In pure water at 25°C, the concentration of H3O+ is equal to the concentration of OH-.

Accepted Answer

A) True 
 B)False

Question 16

List the acid, base, conjugate acid, and conjugate base, in that order, for the following reaction: CH3CO2H(aq) + H2O(l) ⇌ CH3CO2−(aq) + H3O+(aq)

Accepted Answer

A)  CH3CO2H, H2O, CH3CO2−, H3O+
B)  H2O, CH3CO2H, CH3CO2−, H3O+
C)  CH3CO2H, H2O, H3O+, CH3CO2−
D)  H2O, CH3CO2H, H3O+, CH3CO2−
E)  CH3CO2−, H3O+, H2O, CH3CO2H

Question 17

If the pH of a coffee sample is 5.15, what is the H3O+ concentration in the coffee?

Accepted Answer

A)  5.2 M
B)  7.1 × 10-8 M
C)  7.1 × 10-7 M
D)  7.1 × 10-6 M
E)  8.8 M

Question 18

Given an H3O+ concentration of 1.0 × 10-4 M, calculate the OH- concentration, and then identify the solution as acidic, basic, or neutral.

Accepted Answer

A)  [OH-] = 1.0 × 10-7, neutral
B)  [OH-] = 1.0 × 10-4, acidic
C)  [OH-] = 1.0 × 10-10, acidic
D)  [OH-] = 1.0 × 10-10, basic
E)  [OH-] = 1.0 × 10-4, basic

Question 19

Select the two Brønsted-Lowry bases in the following equation: NH3(aq) + H2O(aq) ⇌ NH4+(aq) + OH−(aq)

Accepted Answer

A)  NH3 and  H2O
B)  NH3 and OH−
C)  H2O and OH−
D)  NH3 and NH4+
E)  NH4+ and OH−

Question 20

Given an OH− concentration of 1.0 × 10−4 M, calculate the H3O+ concentration, and then identify the solution as acidic, basic, or neutral.

Accepted Answer

A)  [H3O+] = 1.0 × 10-7, neutral
B)  [H3O+] = 1.0 × 10-4, acidic
C)  [H3O+] = 1.0 × 10-10, acidic
D)  [H3O+] = 1.0 × 10-10, basic
E)  [H3O+] = 1.0 × 10-4, basic

Exam 13: Acids and Bases

Given an OH− concentration of 1.0 × 10−4 M, calculate the H3O+ concentration, and then identify the solution as acidic, basic, or neutral.

Correct AnswerverifiedShow Answer

If Na2HPO4 is added to water, what other compound could also be added in order to make a buffered solution?

Correct AnswerverifiedShow Answer

If the pH of a coffee sample is 5.15, what is the H3O+ concentration in the coffee?

Correct AnswerverifiedShow Answer

The H3O+ concentration in a 0.010 M solution of NaOH is 0.010 M.

Correct AnswerverifiedShow Answer

If the pH of a blood sample is 7.60, what is the H3O+ concentration in the blood?

Correct AnswerverifiedShow Answer

The substance Mg(OH) 2(aq) is

Correct AnswerverifiedShow Answer

Select the two Brønsted-Lowry bases in the following equation: NH3(aq) + H2O(aq) ⇌ NH4+(aq) + OH−(aq)

Correct AnswerverifiedShow Answer

All of the following species are weak bases except:

Correct AnswerverifiedShow Answer

Given an H3O+ concentration of 1.0 × 10-4 M, calculate the OH- concentration, and then identify the solution as acidic, basic, or neutral.

Correct AnswerverifiedShow Answer

Which of the following is an amphoteric substance?

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Calculate the pH of a solution that has [H3O+] = 5.9 × 10-5 M.

Correct AnswerverifiedShow Answer

Select the solution below that is the most acidic.

Correct AnswerverifiedShow Answer

The substance NaOH(aq) is

Correct AnswerverifiedShow Answer

In pure water at 25°C, the concentration of H3O+ is equal to the concentration of OH-.

Correct AnswerverifiedShow Answer

If NaH2PO4 is added to water, what other compound or compounds could also be added in order to make a buffered solution?

Correct AnswerverifiedShow Answer

Which of the following acids is not normally found in foods or beverages?

Correct AnswerverifiedShow Answer

List the species present in order of increasing concentration in a 0.1 M solution of H2C2O4.

Correct AnswerverifiedShow Answer

Which of the following will not change when an acid is added to water?

Correct AnswerverifiedShow Answer

List the acid, base, conjugate acid, and conjugate base, in that order, for the following reaction: CH3CO2H(aq) + H2O(l) ⇌ CH3CO2−(aq) + H3O+(aq)

Correct AnswerverifiedShow Answer

Which of the following equations represents the behavior of HCO3− as an acid?

Correct AnswerverifiedShow Answer

Given an OH⁻ concentration of 1.0 × 10⁻⁴ M, calculate the H₃O⁺ concentration, and then identify the solution as acidic, basic, or neutral.

Correct Answer
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If Na₂HPO₄ is added to water, what other compound could also be added in order to make a buffered solution?

Correct Answer
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If the pH of a coffee sample is 5.15, what is the H₃O⁺ concentration in the coffee?

Correct Answer
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The H₃O⁺ concentration in a 0.010 M solution of NaOH is 0.010 M.

Correct Answer
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If the pH of a blood sample is 7.60, what is the H₃O⁺ concentration in the blood?

Correct Answer
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The substance Mg(OH) ₂(aq) is

Correct Answer
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Select the two Brønsted-Lowry bases in the following equation: NH₃(aq) + H₂O(aq) ⇌ NH₄⁺(aq) + OH⁻(aq)

Correct Answer
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Correct Answer
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Given an H₃O⁺ concentration of 1.0 × 10^-4 M, calculate the OH^- concentration, and then identify the solution as acidic, basic, or neutral.

Correct Answer
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Correct Answer
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Calculate the pH of a solution that has [H₃O⁺] = 5.9 × 10^-5 M.

Correct Answer
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Correct Answer
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Correct Answer
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In pure water at 25°C, the concentration of H₃O⁺ is equal to the concentration of OH^-.

Correct Answer
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If NaH₂PO₄ is added to water, what other compound or compounds could also be added in order to make a buffered solution?

Correct Answer
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Correct Answer
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List the species present in order of increasing concentration in a 0.1 M solution of H₂C₂O₄.

Correct Answer
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Correct Answer
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List the acid, base, conjugate acid, and conjugate base, in that order, for the following reaction: CH₃CO₂H(aq) + H₂O(l) ⇌ CH₃CO₂⁻(aq) + H₃O⁺(aq)

Correct Answer
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Which of the following equations represents the behavior of HCO₃− as an acid?

Correct Answer
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