Question 1

The ionization constant for ammonia is 1.8 × 10-5. What is the pH of a solution labeled 0.50 M ammonia?

Accepted Answer

A)  7.30 
B)  9.12 
C)  10.26 
D)  11.48 
E)  12.52 
A)  7.30 
B)  9.12 
C)  10.26 
D)  11.48 
E)  12.52 D

Question 2

The term pH = -ln [H+].

Accepted Answer

A) True 
 B)False  False

Question 3

Choose the Br∅nsted-Lowry acids and bases in the following equation: HSO4- + C2H3O2- ⇌ HC2H3O2 + SO42-

Accepted Answer

A)  acids HSO4- , SO42- bases HC2H3O2, C2H3O2- 
B)  acids HSO4- , HC2H3O2 bases SO42-, C2H3O2- 
C)  acids SO42-, HC2H3O2 bases HSO4- , C2H3O2- 
D)  acids SO42-, C2H3O2- bases HSO4- , HC2H3O2 
E)  acids HSO4- -, C2H3O2-- bases HC2H3O2, SO42- 
A)  acids HSO4- , SO42- bases HC2H3O2, C2H3O2- 
B)  acids HSO4- , HC2H3O2 bases SO42-, C2H3O2- 
C)  acids SO42-, HC2H3O2 bases HSO4- , C2H3O2- 
D)  acids SO42-, C2H3O2- bases HSO4- , HC2H3O2 
E)  acids HSO4- -, C2H3O2-- bases HC2H3O2, SO42- B

Question 4

What is the pH of a 0.250 M solution of formic acid? Ka = 1.8 × 10-4

Accepted Answer

A)  11.8 
B)  2.2 
C)  0.60 
D)  5.4 
E)  8.6 
A)  11.8 
B)  2.2 
C)  0.60 
D)  5.4 
E)  8.6

Question 5

What is the pH of a 0.563 M solution of ethylammonium bromide? Kb (ethylammonia) = 4.3 × 10-4

Accepted Answer

A)  8.58 
B)  1.79 
C)  8.68 
D)  5.32 
E)  5.44 
A)  8.58 
B)  1.79 
C)  8.68 
D)  5.32 
E)  5.44

Question 6

According to the Arrhenius theory, a neutralization reaction involves the combination of hydrogen ions and hydroxide ions to form water.

Accepted Answer

A) True 
 B)False

Question 7

A saturated aqueous solution of calcium hydroxide is approximately 0.13% calcium hydroxide, by mass, and has a density of 1.02 g ml-1. What is the pH of such a solution?

Accepted Answer

A)  11.95 
B)  12.25 
C)  12.55 
D)  12.75 
E)  13.00 
A)  11.95 
B)  12.25 
C)  12.55 
D)  12.75 
E)  13.00

Question 8

Proton acceptor is an abbreviated definition of:

Accepted Answer

A)  Br∅nsted-Lowry base 
B)  Br∅nsted-Lowry acid 
C)  Lewis base 
D)  Lewis acid 
E)  Arrhenius acid 
A)  Br∅nsted-Lowry base 
B)  Br∅nsted-Lowry acid 
C)  Lewis base 
D)  Lewis acid 
E)  Arrhenius acid

Question 9

What is the indication of the relative acid strengths of the following acids? CH3CH2CHClCOOH   &emsp; CH3CHClCH2COOH   &emsp; CH2ClCH2CH2COOH

Accepted Answer

A)  CH3CHClCH2COOH > CH2ClCH2CH2COOH > CH3CH2CHClCOOH 
B)  CH2ClCH2CH2COOH > CH3CH2CHClCOOH > CH3CHClCH2COOH 
C)  CH2ClCH2CH2COOH > CH3CHClCH2COOH > CH3CH2CHClCOOH 
D)  CH3CH2CHClCOOH > CH3CHClCH2COOH > CH2ClCH2CH2COOH 
E)  CH3CH2CHClCOOH > CH2ClCH2CH2COOH > CH3CHClCH2COOH 
A)  CH3CHClCH2COOH > CH2ClCH2CH2COOH > CH3CH2CHClCOOH 
B)  CH2ClCH2CH2COOH > CH3CH2CHClCOOH > CH3CHClCH2COOH 
C)  CH2ClCH2CH2COOH > CH3CHClCH2COOH > CH3CH2CHClCOOH 
D)  CH3CH2CHClCOOH > CH3CHClCH2COOH > CH2ClCH2CH2COOH 
E)  CH3CH2CHClCOOH > CH2ClCH2CH2COOH > CH3CHClCH2COOH

Question 10

If one mole of Ba(OH)2 is added to enough water to make 10 liters of solution, the pH of the resulting solution is ________.

Accepted Answer

A)  13.3 
B)  1.0 
C)  0.7 
D)  13.0 
E)  12.5 
A)  13.3 
B)  1.0 
C)  0.7 
D)  13.0 
E)  12.5

Question 11

What is the pH of a 0.120 M solution of the sodium salt of acetylsalicylic acid (aspirin)? Ka (aspirin) = 3.3 × 10-4

Accepted Answer

A)  7.0 
B)  11.8 
C)  2.2 
D)  5.7 
E)  8.3 
A)  7.0 
B)  11.8 
C)  2.2 
D)  5.7 
E)  8.3

Question 12

What is the [K+] of a solution prepared by dissolving 0.140 g of potassium hydroxide in sufficient pure water to prepare 250.0 ml of solution?

Accepted Answer

A)  10-5 M 
B)  10-8 M 
C)  10-12 M 
D)  10-4 M 
E)  10-2 M 
A)  10-5 M 
B)  10-8 M 
C)  10-12 M 
D)  10-4 M 
E)  10-2 M

Question 13

What is the pH for a solution labeled 0.10 M arsenic acid (H3AsO4)? [Ka1 = 6 × 10-3, Ka2 = 1 × 10-7, Ka3 = 3 × 10-12]

Accepted Answer

A)  1.6 
B)  4.0 
C)  6.3 
D)  1.0 
E)  3.2 
A)  1.6 
B)  4.0 
C)  6.3 
D)  1.0 
E)  3.2

Question 14

A saturated aqueous solution of calcium hydroxide has a pH of 12.25. What is the [Ca2+] of such a solution?

Accepted Answer

A)  0.018 
B)  5.6 × 10-13 
C)  2.3 × 10-5 
D)  0.035 
E)  8.9 × 10-3 
A)  0.018 
B)  5.6 × 10-13 
C)  2.3 × 10-5 
D)  0.035 
E)  8.9 × 10-3

Question 15

In the reaction BF3 + NH3 ⇌ F3B:NH3, BF3 acts as:

Accepted Answer

A)  an Arrhenius base 
B)  a Lewis base 
C)  a Br∅nsted acid 
D)  a Lewis acid 
E)  an Arrhenius acid 
A)  an Arrhenius base 
B)  a Lewis base 
C)  a Br∅nsted acid 
D)  a Lewis acid 
E)  an Arrhenius acid

Question 16

What is the pH of a 0.052 M solution of sodium acetate? Ka (acetic acid)= 1.8 × 10-5

Accepted Answer

A)  10.0 
B)  5.3 
C)  11.0 
D)  8.7 
E)  3.0 
A)  10.0 
B)  5.3 
C)  11.0 
D)  8.7 
E)  3.0

Question 17

In the equilibrium system described by: PO43-(aq) + H2O(l) ⇌ HPO42-(aq) + OH-, Br nsted-Lowry theory would designate:

Accepted Answer

A)  PO43- and H2O as the bases 
B)  H2O and OH- as a conjugate pair 
C)  HPO42- and OH- as the acids 
D)  HPO42- and H2O as a conjugate pair 
E)  PO43- as amphiprotic 
A)  PO43- and H2O as the bases 
B)  H2O and OH- as a conjugate pair 
C)  HPO42- and OH- as the acids 
D)  HPO42- and H2O as a conjugate pair 
E)  PO43- as amphiprotic

Question 18

What is the pH of a 0.375 M solution of methylammonium chloride? Kb (CH3NH2) = 4.2 × 10-4

Accepted Answer

A)  12.1 
B)  1.9 
C)  5.5 
D)  8.5 
E)  11.0 
A)  12.1 
B)  1.9 
C)  5.5 
D)  8.5 
E)  11.0

Question 19

Choose the strongest acid.

Accepted Answer

A)  HF 
B)  H2CO3 
C)  HCN 
D)  HC2H3O2 
E)  HClO4 
A)  HF 
B)  H2CO3 
C)  HCN 
D)  HC2H3O2 
E)  HClO4

Question 20

Choose the Br∅nsted-Lowry acids and bases in the following equation: HCN + OH- ⇌ H2O + CN-

Accepted Answer

A)  acids HCN, CN- bases OH-, H2O 
B)  acids CN-, OH- bases HCN, H2O 
C)  acids HCN, H2O bases OH-, CN- 
D)  acids OH-, H2O bases CN-, HCN 
E)  acids HCN, OH- bases H2O, CN- 
A)  acids HCN, CN- bases OH-, H2O 
B)  acids CN-, OH- bases HCN, H2O 
C)  acids HCN, H2O bases OH-, CN- 
D)  acids OH-, H2O bases CN-, HCN 
E)  acids HCN, OH- bases H2O, CN-

Exam 16: Acids and Bases

The ionization constant for ammonia is 1.8 × 10-5. What is the pH of a solution labeled 0.50 M ammonia?

The term pH = -ln [H+].

Choose the Br∅nsted-Lowry acids and bases in the following equation: HSO4- + C2H3O2- ⇌ HC2H3O2 + SO42-

What is the pH of a 0.250 M solution of formic acid? Ka = 1.8 × 10-4

What is the pH of a 0.563 M solution of ethylammonium bromide? Kb (ethylammonia) = 4.3 × 10-4

According to the Arrhenius theory, a neutralization reaction involves the combination of hydrogen ions and hydroxide ions to form water.

A saturated aqueous solution of calcium hydroxide is approximately 0.13% calcium hydroxide, by mass, and has a density of 1.02 g ml-1. What is the pH of such a solution?

Proton acceptor is an abbreviated definition of:

What is the indication of the relative acid strengths of the following acids? CH3CH2CHClCOOH CH3CHClCH2COOH CH2ClCH2CH2COOH

If one mole of Ba(OH)2 is added to enough water to make 10 liters of solution, the pH of the resulting solution is ________.

What is the pH of a 0.120 M solution of the sodium salt of acetylsalicylic acid (aspirin)? Ka (aspirin) = 3.3 × 10-4

What is the [K+] of a solution prepared by dissolving 0.140 g of potassium hydroxide in sufficient pure water to prepare 250.0 ml of solution?

What is the pH for a solution labeled 0.10 M arsenic acid (H3AsO4)? [Ka1 = 6 × 10-3, Ka2 = 1 × 10-7, Ka3 = 3 × 10-12]

A saturated aqueous solution of calcium hydroxide has a pH of 12.25. What is the [Ca2+] of such a solution?

In the reaction BF3 + NH3 ⇌ F3B:NH3, BF3 acts as:

What is the pH of a 0.052 M solution of sodium acetate? Ka (acetic acid)= 1.8 × 10-5

In the equilibrium system described by: PO43-(aq) + H2O(l) ⇌ HPO42-(aq) + OH-, Br nsted-Lowry theory would designate:

What is the pH of a 0.375 M solution of methylammonium chloride? Kb (CH3NH2) = 4.2 × 10-4

Choose the strongest acid.

Choose the Br∅nsted-Lowry acids and bases in the following equation: HCN + OH- ⇌ H2O + CN-

Matter - Its Properties and Measurement

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Chemical Compounds

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Introduction to Reactions in Aqueous Solutions

Gases

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Electrons in Atoms

The Periodic Table and Some Atomic Properties

Chemical Bonding I: Basic Concepts

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Intermolecular Forces: Liquids and Solids

Solutions and Their Physical Properties

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Principles of Chemical Equilibrium

Additional Aspects of Acid-Base Equilibria

Solubility and Complex-Ion Equilibria

Spontaneous Change: Entropy and Free Energy

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Main Group Elements I: Groups 1, 2, 13, and 14

Main Group Elements II: Groups 18, 17, 16, 15, and Hydrogen

The Transition Elements

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The ionization constant for ammonia is 1.8 × 10^-5. What is the pH of a solution labeled 0.50 M ammonia?

Choose the Br∅nsted-Lowry acids and bases in the following equation: HSO₄^-+ C₂H₃O₂^- ⇌ HC₂H₃O₂ + SO₄^2-

What is the pH of a 0.250 M solution of formic acid? Ka = 1.8 × 10^-4

What is the pH of a 0.563 M solution of ethylammonium bromide? Kb (ethylammonia) = 4.3 × 10^-4

What is the indication of the relative acid strengths of the following acids? CH₃CH₂CHClCOOH CH₃CHClCH₂COOH CH₂ClCH₂CH₂COOH

If one mole of Ba(OH)₂ is added to enough water to make 10 liters of solution, the pH of the resulting solution is ________.

What is the pH of a 0.120 M solution of the sodium salt of acetylsalicylic acid (aspirin)? Ka (aspirin) = 3.3 × 10^-4

What is the pH for a solution labeled 0.10 M arsenic acid (H₃AsO₄)? [Ka1 = 6 × 10^-3, Ka₂ = 1 × 10^-7, Ka₃ = 3 × 10^-12]

A saturated aqueous solution of calcium hydroxide has a pH of 12.25. What is the [Ca²⁺] of such a solution?

In the reaction BF₃ + NH₃ ⇌ F3B:NH₃, BF₃ acts as:

What is the pH of a 0.052 M solution of sodium acetate? Ka (acetic acid)= 1.8 × 10^-5

In the equilibrium system described by: PO₄^3-(aq) + H₂O(l) ⇌ HPO₄^2-(aq) + OH-, Br nsted-Lowry theory would designate:

What is the pH of a 0.375 M solution of methylammonium chloride? Kb (CH₃NH₂) = 4.2 × 10^-4

Choose the Br∅nsted-Lowry acids and bases in the following equation: HCN + OH- ⇌ H₂O + CN-