Question 1

What is the hydroxide ion concentration of a lye solution that has a pH of 9.20?

Accepted Answer

A) 6.3 × 10-10 mol L-1 
B) 1.6 × 10-5 mol L-1 
C) 4.8 mol L-1 
D) 9.2 mol L-1 
A) 6.3 × 10-10 mol L-1 
B) 1.6 × 10-5 mol L-1 
C) 4.8 mol L-1 
D) 9.2 mol L-1

Question 2

The concept of an acid not limited to H+ or species containing one or more protons is inherent in:

Accepted Answer

A) only the Arrhenius theory 
B) both the Arrhenius and the Br∅nsted-Lowry theories 
C) only the Br∅nsted-Lowry theory 
D) both the Br∅nsted-Lowry and the Lewis theories 
E) only the Lewis theory 
A) only the Arrhenius theory 
B) both the Arrhenius and the Br∅nsted-Lowry theories 
C) only the Br∅nsted-Lowry theory 
D) both the Br∅nsted-Lowry and the Lewis theories 
E) only the Lewis theory

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-

Question 4

What is the hydroxide ion concentration and the pH for a hydrochloric acid solution that has a hydronium ion concentration of

Accepted Answer

A) 6.7 × 10-12 mol L-1,2.82 
B) 6.7 × 10-12 mol L-1,11.18 
C) 6.7 × 10-13 mol L-1,1.82 
D) 6.7 × 10-13 mol L-1,12.17 
A) 6.7 × 10-12 mol L-1,2.82 
B) 6.7 × 10-12 mol L-1,11.18 
C) 6.7 × 10-13 mol L-1,1.82 
D) 6.7 × 10-13 mol L-1,12.17

Question 5

When comparing binary acids of the elements in the same row of the periodic table,acid strength increases as the polarity of the element-hydrogen bond increases.

Accepted Answer

A) True 
 B)False

Question 6

What is the pH of a 0.570 M aqueous solution of aniline? 
Kb = 7.4 × 10-10

Accepted Answer

A) 11.4 
B) 2.6 
C) 9.8 
D) 4.7 
E) 9.3 
A) 11.4 
B) 2.6 
C) 9.8 
D) 4.7 
E) 9.3

Question 7

List the following acids in order of increasing strength:
H2SO4 H2SeO4 H2TeO4

Accepted Answer

A) H2SeO4 2TeO4 2SO4  
B) H2SeO4 2SO4 2TeO4  
C) H2SO4 2TeO4 2SeO4  
D) H2SO4 2SeO4 2TeO4  
E) H2TeO4 2SeO4 2SO4  
A) H2SeO4 2TeO4 2SO4  
B) H2SeO4 2SO4 2TeO4  
C) H2SO4 2TeO4 2SeO4  
D) H2SO4 2SeO4 2TeO4  
E) H2TeO4 2SeO4 2SO4

Question 8

What is the pH of a 0.380 M aqueous solution of ethylamine? 
Kb = 4.3 × 10-4

Accepted Answer

A) 12.1 
B) 1.9 
C) 10.2 
D) 5.5 
E) 8.5 
A) 12.1 
B) 1.9 
C) 10.2 
D) 5.5 
E) 8.5

Question 9

Calculate the pH of a 1.60 mol L-1 aqueous KBrO solution.Ka for hypobromous acid,HBrO,is

Accepted Answer

A) 2.55 
B) 4.25 
C) 9.75 
D) 11.45 
A) 2.55 
B) 4.25 
C) 9.75 
D) 11.45

Question 10

What is the pH of a 0.040 mol L-1 aqueous Ba(OH)2 solution?

Accepted Answer

A) 1.10 
B) 1.40 
C) 12.60 
D) 12.90 
A) 1.10 
B) 1.40 
C) 12.60 
D) 12.90

Question 11

What is the [H2AsO4-] for an aqueous solution labeled "0.10 M arsenic acid (H3AsO4)"?
[Ka1 = 6 × 10-3,Ka2 = 1 × 10-7,Ka3 = 3 × 10-12]

Accepted Answer

A) 1 × 10-7 M 
B) 6 × 10-3 M  
C) 0.02 M 
D) 0.08 M 
E) 6 × 10-10 M 
A) 1 × 10-7 M 
B) 6 × 10-3 M  
C) 0.02 M 
D) 0.08 M 
E) 6 × 10-10 M

Question 12

In the equilibrium system described by: 
 
  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 13

In the reaction BF3 + NH3 → F3B:NH3,BF3 acts as a Br∅nsted acid.

Accepted Answer

A) True 
 B)False

Question 14

What is the pH of a 0.361 M aqueous solution of pyridinium bromide? Kb (pyridine)= 1.5 × 10-9

Accepted Answer

A) 8.38 
B) 5.62 
C) 4.63 
D) 2.81 
E) 11.19 
A) 8.38 
B) 5.62 
C) 4.63 
D) 2.81 
E) 11.19

Question 15

List the following acids in order of increasing strength:
HClO2 HClO3 HClO4

Accepted Answer

A) HClO2 4 3  
B) HClO4 3 2  
C) HClO4 2 3  
D) HClO3 2 4  
E) HClO2 3 4  
A) HClO2 4 3  
B) HClO4 3 2  
C) HClO4 2 3  
D) HClO3 2 4  
E) HClO2 3 4

Question 16

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 17

What is the pH of a 0.500 mol L-1 NH3 aqueous solution that has Kb = 1.8 × 10-5? 
The equation for the dissociation of NH3 is below:

Accepted Answer

A) 2.22 
B) 2.52 
C) 11.48 
D) 10.48 
A) 2.22 
B) 2.52 
C) 11.48 
D) 10.48

Question 18

What is the pH of a 0.052 M aqueous 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 19

A 0.505 g sample of a monoprotic base (mm = 45.09 g/mol)was dissolved in water to produce 100.0 mL of solution with a pH = 11.84.What is the ionization constant of this base?

Accepted Answer

A) 4.3 × 10-5 
B) 1.9 × 10-23 
C) 4.3 × 10-4 
D) 3.4 × 10-1 
E) 1.3 × 10-11 
A) 4.3 × 10-5 
B) 1.9 × 10-23 
C) 4.3 × 10-4 
D) 3.4 × 10-1 
E) 1.3 × 10-11

Question 20

What is the indication of the relative base strengths of the following bases?
CH3NH2 CHBr2NH2 CH2BrNH2

Accepted Answer

A) CH2BrNH2 > CHBr2NH2 > CH3NH2  
B) CHBr2NH2 > CH2BrNH2 > CH3NH2  
C) CHBr2NH2 > CH3NH2 > CH2BrNH2  
D) CH2BrNH2 > CH3NH2 > CHBr2NH2  
E) CH3NH2 > CH2BrNH2 > CHBr2NH2  
A) CH2BrNH2 > CHBr2NH2 > CH3NH2  
B) CHBr2NH2 > CH2BrNH2 > CH3NH2  
C) CHBr2NH2 > CH3NH2 > CH2BrNH2  
D) CH2BrNH2 > CH3NH2 > CHBr2NH2  
E) CH3NH2 > CH2BrNH2 > CHBr2NH2

Exam 16: Acids and Bases

What is the hydroxide ion concentration of a lye solution that has a pH of 9.20?

The concept of an acid not limited to H+ or species containing one or more protons is inherent in:

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

What is the hydroxide ion concentration and the pH for a hydrochloric acid solution that has a hydronium ion concentration of

When comparing binary acids of the elements in the same row of the periodic table,acid strength increases as the polarity of the element-hydrogen bond increases.

What is the pH of a 0.570 M aqueous solution of aniline? Kb = 7.4 × 10-10

List the following acids in order of increasing strength: H2SO4 H2SeO4 H2TeO4

What is the pH of a 0.380 M aqueous solution of ethylamine? Kb = 4.3 × 10-4

Calculate the pH of a 1.60 mol L-1 aqueous KBrO solution.Ka for hypobromous acid,HBrO,is

What is the pH of a 0.040 mol L-1 aqueous Ba(OH)2 solution?

What is the [H2AsO4-] for an aqueous solution labeled "0.10 M arsenic acid (H3AsO4)"? [Ka1 = 6 × 10-3,Ka2 = 1 × 10-7,Ka3 = 3 × 10-12]

In the equilibrium system described by: Theory would designate:

In the reaction BF3 + NH3 → F3B:NH3,BF3 acts as a Br∅nsted acid.

What is the pH of a 0.361 M aqueous solution of pyridinium bromide? Kb (pyridine)= 1.5 × 10-9

List the following acids in order of increasing strength: HClO2 HClO3 HClO4

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

What is the pH of a 0.500 mol L-1 NH3 aqueous solution that has Kb = 1.8 × 10-5? The equation for the dissociation of NH3 is below:

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

A 0.505 g sample of a monoprotic base (mm = 45.09 g/mol)was dissolved in water to produce 100.0 mL of solution with a pH = 11.84.What is the ionization constant of this base?

What is the indication of the relative base strengths of the following bases? CH3NH2 CHBr2NH2 CH2BrNH2

Matter: Its Properties and Measurement

Atoms and the Atomic Theory

Chemical Compounds

Chemical Reactions

Introduction to Reactions in Aqueous Solutions

Gases

Thermochemistry

Electrons in Atoms

The Periodic Table and Some Atomic Properties

Chemical Bonding I: Basic Concepts

Chemical Bonding Ii: Valence Bond and Molecular Orbital Theories

Intermolecular Forces: Liquids and Solids

Spontaneous Change: Entropy and Gibbs Energy

Solutions and Their Physical Properties

Principles of Chemical Equilibrium

Additional Aspects of Acidbase Equilibria

Solubility and Complex-Ion Equilibria

Electrochemistry

Chemical Kinetics

Chemistry of the Main-Group Elements I: Groups 1,2,13,and 14

Chemistry of the Main-Group Elements Ii: Groups 18,17,16,15,and Hydrogen

The Transition Elements

Complex Ions and Coordination Compounds

Nuclear Chemistry

Structures of Organic Compounds

Reactions of Organic Compounds

Chemistry of the Living State

Filters

The concept of an acid not limited to H⁺ or species containing one or more protons is inherent in:

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

What is the pH of a 0.570 M aqueous solution of aniline? K_b = 7.4 × 10^-10

List the following acids in order of increasing strength: H₂SO₄ H₂SeO₄ H₂TeO₄

What is the pH of a 0.380 M aqueous solution of ethylamine? K_b = 4.3 × 10^-4

Calculate the pH of a 1.60 mol L^-1 aqueous KBrO solution.K_a for hypobromous acid,HBrO,is

What is the pH of a 0.040 mol L^-1 aqueous Ba(OH)₂ solution?

What is the [H₂AsO₄^-] for an aqueous solution labeled "0.10 M arsenic acid (H₃AsO₄)"? [K_a1 = 6 × 10^-3,K_a2 = 1 × 10^-7,K_a3 = 3 × 10^-12]

In the reaction BF₃ + NH₃ → F₃B:NH₃,BF₃ acts as a Br∅nsted acid.

What is the pH of a 0.361 M aqueous solution of pyridinium bromide? K_b (pyridine)= 1.5 × 10^-9

List the following acids in order of increasing strength: HClO₂ HClO₃ HClO₄

What is the pH of a 0.500 mol L^-1 NH₃ aqueous solution that has K_b = 1.8 × 10^-5? The equation for the dissociation of NH₃ is below:

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

What is the indication of the relative base strengths of the following bases? CH₃NH₂ CHBr₂NH₂ CH₂BrNH₂