Question 1

List the following acids in order of increasing strength:
 H3PO4 &emsp; H2SO4 &emsp;  HClO4

Accepted Answer

A)  HClO4 3PO4 2SO4 
B)  H2SO4 43PO4 
C)  H2SO4 3PO4 4 
D)  H3PO4 2SO44 
E)  HClO4 2SO4 3PO4 
A)  HClO4 3PO4 2SO4 
B)  H2SO4 43PO4 
C)  H2SO4 3PO4 4 
D)  H3PO4 2SO44 
E)  HClO4 2SO4 3PO4

Question 2

In which of the following cases is water acting as a base under the Lewis definitions, but not under the Br∅nsted-Lowry definitions?

Accepted Answer

A)  H2O(l) + HF(g) ⇌ H3O+(aq) + F(aq) 
B)  H2O(l)+ CN-(aq) ⇌ OH-(aq) + HCN(aq) 
C)  H2O(l) + Cu2+(aq) ⇌ Cu(H2O)2+(aq) 
D)  H2O(l) + PO43-(aq) ⇌ 2OH-(aq) + H2PO4-(aq) 
E)  H2O(l) [electrolysis] ⇌ 2H2(g) + O2(g) 
A)  H2O(l) + HF(g) ⇌ H3O+(aq) + F(aq) 
B)  H2O(l)+ CN-(aq) ⇌ OH-(aq) + HCN(aq) 
C)  H2O(l) + Cu2+(aq) ⇌ Cu(H2O)2+(aq) 
D)  H2O(l) + PO43-(aq) ⇌ 2OH-(aq) + H2PO4-(aq) 
E)  H2O(l) [electrolysis] ⇌ 2H2(g) + O2(g)

Question 3

For the following compound, predict whether the solution is acidic, basic or neutral and why: NH4Cl.

Accepted Answer

A)  acidic because NH4Cl is a strong acid 
B)  basic because NH4Cl is a weak base 
C)  neutral because there is no hydrolysis 
D)  basic because NH4Cl is the salt of a weak acid 
E)  acidic because NH4Cl is the salt of a weak base 
A)  acidic because NH4Cl is a strong acid 
B)  basic because NH4Cl is a weak base 
C)  neutral because there is no hydrolysis 
D)  basic because NH4Cl is the salt of a weak acid 
E)  acidic because NH4Cl is the salt of a weak base

Question 4

Choose the Br∅nsted-Lowry acids and bases in the following equation: H2O + NH2- ⇌ NH3 + OH-

Accepted Answer

A)  acids H2O, OH- bases NH3, NH2- 
B)  acids NH2-, NH3 bases H2O, OH- 
C)  acids H2O, NH2- bases OH-, NH3 
D)  acids NH3, NH2- bases OH-, H2O 
E)  acids H2O, NH3 bases NH2-, OH- 
A)  acids H2O, OH- bases NH3, NH2- 
B)  acids NH2-, NH3 bases H2O, OH- 
C)  acids H2O, NH2- bases OH-, NH3 
D)  acids NH3, NH2- bases OH-, H2O 
E)  acids H2O, NH3 bases NH2-, OH-

Question 5

The Kb value for methylamine is 4.2 × 10-4. What is the pH of an aqueous solution for which the label reads "0.042 M CH3NH2"?

Accepted Answer

A)  2.4 
B)  4.8 
C)  9.2 
D)  11.6 
E)  12.3 
A)  2.4 
B)  4.8 
C)  9.2 
D)  11.6 
E)  12.3

Question 6

What is the pH of a 0.175 M solution of potassium benzoate? Ka (benzoic acid) = 6.3 × 10-5

Accepted Answer

A)  9.10 
B)  3.44 
C)  10.56 
D)  5.28 
E)  8.72 
A)  9.10 
B)  3.44 
C)  10.56 
D)  5.28 
E)  8.72

Question 7

Amine bases are known as strong bases

Accepted Answer

A) True 
 B)False

Question 8

Choose the Br∅nsted-Lowry acids and bases in the following equation: HCO3- + OH- ⇌ H2O + CO32-

Accepted Answer

A)  acids HCO3-, H2O bases OH-, CO32- 
B)  acids OH-, CO32- bases HCO3-, H2O 
C)  acids H2O, OH- bases HCO3-, CO32- 
D)  acids HCO3-, OH- bases CO32-, H2O 
E)  acids H2O, CO32- bases HCO3-, OH- 
A)  acids HCO3-, H2O bases OH-, CO32- 
B)  acids OH-, CO32- bases HCO3-, H2O 
C)  acids H2O, OH- bases HCO3-, CO32- 
D)  acids HCO3-, OH- bases CO32-, H2O 
E)  acids H2O, CO32- bases HCO3-, OH-

Question 9

A certain acid, HA, has a Ka given by: HA + H2O ⇌ H3O+ + A- Ka = 6.80 × 10-6
What is the pH of a 0.247 M solution of the acid's potassium salt, KA, which undergoes the hydrolysis reaction?
A- + H2O ⇌ OH- + HA

Accepted Answer

A)  4.72 
B)  9.28 
C)  4.11 
D)  9.89 
E)  9.44 
A)  4.72 
B)  9.28 
C)  4.11 
D)  9.89 
E)  9.44

Question 10

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 11

According to the Arrhenius theory, a neutralization reaction involves the combination of an acid with a base to make only water.

Accepted Answer

A) True 
 B)False

Question 12

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 13

What is the pH of a 0.380 M 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 14

What is the pH of a solution labeled "0.50 M Sodium Fluoride" if the ionization constant of hydrofluoric acid is 6.0 × 10-4?

Accepted Answer

A)  10.8 
B)  8.5 
C)  7.1 
D)  6.9 
E)  5.5 
A)  10.8 
B)  8.5 
C)  7.1 
D)  6.9 
E)  5.5

Question 15

What is the pH of a 0.530 M solution of hypochlorus acid? Ka = 2.9 × 10-8

Accepted Answer

A)  10.6 
B)  3.4 
C)  10.1 
D)  3.9 
E)  0.28 
A)  10.6 
B)  3.4 
C)  10.1 
D)  3.9 
E)  0.28

Question 16

What is the indication of the relative base strengths of the following bases? 
CH3NH2   &emsp;  CHBr2NH2   &emsp;  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

Question 17

The definition of a neutralization reaction as a reaction in which an acid reacts with a base to produce water and a salt 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 18

What is the pH of a 0.470 M solution of pyridine? Kb = 1.5 × 10-9

Accepted Answer

A)  9.6 
B)  11.2 
C)  2.8 
D)  9.4 
E)  4.6 
A)  9.6 
B)  11.2 
C)  2.8 
D)  9.4 
E)  4.6

Question 19

0.375 g of a monoprotic acid (mm = 245 g/mol) is dissolved in water to produce 25.0 mL of a solution with pH = 3.28. Determine the ionization constant of the acid.

Accepted Answer

A)  8.56 × 10-3 
B)  4.5 × 10-6 
C)  7.4 × 10-5 
D)  4.5 × 10-3 
E)  2.3 × 10-2 
A)  8.56 × 10-3 
B)  4.5 × 10-6 
C)  7.4 × 10-5 
D)  4.5 × 10-3 
E)  2.3 × 10-2

Question 20

pOH = 3.14 is equivalent to:

Accepted Answer

A)  pH = 11. 
B)  [H+] = 1.4 × 10-10 M 
C)  [OH-] = 7.2 × 10-4 M 
D)  [H+} = 7.0 × 10-4 M 
E)  [OH-] = 3.14 × 10-7 M 
A)  pH = 11. 
B)  [H+] = 1.4 × 10-10 M 
C)  [OH-] = 7.2 × 10-4 M 
D)  [H+} = 7.0 × 10-4 M 
E)  [OH-] = 3.14 × 10-7 M

Exam 16: Acids and Bases

List the following acids in order of increasing strength: H3PO4 H2SO4 HClO4

In which of the following cases is water acting as a base under the Lewis definitions, but not under the Br∅nsted-Lowry definitions?

For the following compound, predict whether the solution is acidic, basic or neutral and why: NH4Cl.

Choose the Br∅nsted-Lowry acids and bases in the following equation: H2O + NH2- ⇌ NH3 + OH-

The Kb value for methylamine is 4.2 × 10-4. What is the pH of an aqueous solution for which the label reads "0.042 M CH3NH2"?

What is the pH of a 0.175 M solution of potassium benzoate? Ka (benzoic acid) = 6.3 × 10-5

Amine bases are known as strong bases

Choose the Br∅nsted-Lowry acids and bases in the following equation: HCO3- + OH- ⇌ H2O + CO32-

A certain acid, HA, has a Ka given by: HA + H2O ⇌ H3O+ + A- Ka = 6.80 × 10-6 What is the pH of a 0.247 M solution of the acid's potassium salt, KA, which undergoes the hydrolysis reaction? A- + H2O ⇌ OH- + HA

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.

According to the Arrhenius theory, a neutralization reaction involves the combination of an acid with a base to make only water.

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

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

What is the pH of a solution labeled "0.50 M Sodium Fluoride" if the ionization constant of hydrofluoric acid is 6.0 × 10-4?

What is the pH of a 0.530 M solution of hypochlorus acid? Ka = 2.9 × 10-8

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

The definition of a neutralization reaction as a reaction in which an acid reacts with a base to produce water and a salt is inherent in:

What is the pH of a 0.470 M solution of pyridine? Kb = 1.5 × 10-9

0.375 g of a monoprotic acid (mm = 245 g/mol) is dissolved in water to produce 25.0 mL of a solution with pH = 3.28. Determine the ionization constant of the acid.

pOH = 3.14 is equivalent to:

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: Additional Aspects

Intermolecular Forces: Liquids and Solids

Solutions and Their Physical Properties

Chemical Kinetics

Principles of Chemical Equilibrium

Additional Aspects of Acid-Base Equilibria

Solubility and Complex-Ion Equilibria

Spontaneous Change: Entropy and Free Energy

Electrochemistry

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

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

The Transition Elements

Complex Ions and Coordination Compounds

Nuclear Chemistry 1-41

Structures of Organic Compounds

Reactions of Organic Compounds

Chemistry of the Living State

Filters

List the following acids in order of increasing strength: H₃PO₄ H₂SO₄ HClO₄

For the following compound, predict whether the solution is acidic, basic or neutral and why: NH₄Cl.

Choose the Br∅nsted-Lowry acids and bases in the following equation: H₂O + NH₂^- ⇌ NH₃ + OH-

The Kb value for methylamine is 4.2 × 10^-4. What is the pH of an aqueous solution for which the label reads "0.042 M CH₃NH₂"?

What is the pH of a 0.175 M solution of potassium benzoate? Ka (benzoic acid) = 6.3 × 10^-5

Choose the Br∅nsted-Lowry acids and bases in the following equation: HCO₃^- + OH- ⇌ H₂O + CO₃^2-

A certain acid, HA, has a Ka given by: HA + H₂O ⇌ H₃O⁺ + A- Ka = 6.80 × 10^-6 What is the pH of a 0.247 M solution of the acid's potassium salt, KA, which undergoes the hydrolysis reaction? A- + H₂O ⇌ OH- + HA

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

What is the pH of a solution labeled "0.50 M Sodium Fluoride" if the ionization constant of hydrofluoric acid is 6.0 × 10^-4?

What is the pH of a 0.530 M solution of hypochlorus acid? Ka = 2.9 × 10^-8

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

What is the pH of a 0.470 M solution of pyridine? Kb = 1.5 × 10^-9