Question 1

Identify the hydronium ion among the following ions.

Accepted Answer

A)  H3O+ 
B)  H3O- 
C)  H2O2+ 
D)  H2O2- 
E)  H3O2+ 
A)  H3O+ 
B)  H3O- 
C)  H2O2+ 
D)  H2O2- 
E)  H3O2+

Question 2

Calculate the pH of a 2.0 × 10-3 M solution of KClO2. Ka for HClO2 = 1.2 × 10-2

Accepted Answer

A)  7.24 
B)  7.03 
C)  6.97 
D)  7.39 
E)  6.61 
A)  7.24 
B)  7.03 
C)  6.97 
D)  7.39 
E)  6.61

Question 3

The following acids are listed in order of decreasing acid strength in water.HI > HNO2 > CH3COOH > HClO > HCN
According to Brønsted-Lowry theory, which of the following ions is the weakest base?

Accepted Answer

A)  ClO- 
B)  NO2- 
C)  CH3COO- 
D)  I- 
E)  CN- 
A)  ClO- 
B)  NO2- 
C)  CH3COO- 
D)  I- 
E)  CN-

Question 4

Which of the following is a conjugate acid-base pair?

Accepted Answer

A)  H3O+/OH- 
B)  N2H5+/N2H4 
C)  Mg2+/Mg(OH)2 
D)  HCl/OCl- 
E)  H2SO4/SO42- 
A)  H3O+/OH- 
B)  N2H5+/N2H4 
C)  Mg2+/Mg(OH)2 
D)  HCl/OCl- 
E)  H2SO4/SO42-

Question 5

​Determine the pH of a 7.5 M H3PO4 (   ) solution.

Accepted Answer

A)  0.63 
B)  1.02 
C)  0.89 
D)  0.41 
E)  1.84 
A)  0.63 
B)  1.02 
C)  0.89 
D)  0.41 
E)  1.84

Question 6

What is the pH of a 0.2 M solution of NH4Cl? Kb for NH3 is 1.8 × 10-5.

Accepted Answer

A)  5.0 
B)  11.3 
C)  2.7 
D)  7.0 
E)  9.0 
A)  5.0 
B)  11.3 
C)  2.7 
D)  7.0 
E)  9.0

Question 7

The pH of a 0.124 M solution of a weak base is 10.89 at 25°C. Calculate the pH of a 0.0470 M solution of the base at 25°C.

Accepted Answer

A)  10.68 
B)  11.31 
C)  4.13 
D)  3.32 
E)  10.47 
A)  10.68 
B)  11.31 
C)  4.13 
D)  3.32 
E)  10.47

Question 8

Calculate the pH of the following aqueous solutions. Choose your answer from the given pH ranges.
-1.0 M NaHSO4 (pKa for HSO4- = 1.92)

Accepted Answer

A)  pH 9.00-10.99 
B)  pH 3.00-5.99 
C)  pH 6.00-8.99 
D)  pH 11.00-14.00 
E)  pH 0.00-2.99 
A)  pH 9.00-10.99 
B)  pH 3.00-5.99 
C)  pH 6.00-8.99 
D)  pH 11.00-14.00 
E)  pH 0.00-2.99

Question 9

Calculate the pH of a 2.0 × 10-7 M solution of Ca(OH)2.

Accepted Answer

A)  6.62 
B)  7.30 
C)  6.37 
D)  7.38 
E)  7.63 
A)  6.62 
B)  7.30 
C)  6.37 
D)  7.38 
E)  7.63

Question 10

The pH of a 2.1 × 10-3 M solution of a weak base is 9.87. Calculate Kb for this base.

Accepted Answer

A)  2.6 × 10-6 
B)  1.2 × 10-4 
C)  6.4 × 10-8 
D)  8.7 × 10-18 
E)  none of these 
A)  2.6 × 10-6 
B)  1.2 × 10-4 
C)  6.4 × 10-8 
D)  8.7 × 10-18 
E)  none of these

Question 11

Calculate the [H+] in a 2.0 × 10-6 M solution of NaC2H3O2.(Ka for HC2H3O2 = 1.8 × 10-5)

Accepted Answer

A)  6.0 × 10-6 M 
B)  1.7 × 10-9 M 
C)  3.4 × 10-8 M 
D)  1.1 × 10-7 M 
E)  9.6 × 10-8 M 
A)  6.0 × 10-6 M 
B)  1.7 × 10-9 M 
C)  3.4 × 10-8 M 
D)  1.1 × 10-7 M 
E)  9.6 × 10-8 M

Question 12

In which of the following are the species listed in order of increasing pH? (Ka for HC2H3O2 is 1.80 × 10-5, and Ka for NH4+ is 5.56 × 10-10).

Accepted Answer

A)  HNO3, NH4Cl, KCl, NaC2H3O2, KOH 
B)  NH4Cl, HNO3, KCl, KOH, NaC2H3O2 
C)  KCl, NH4Cl, HNO3, KOH, NaC2H3O2 
D)  HNO3, KCl, NH4Cl, KOH, NaC2H3O2 
E)  none of these 
A)  HNO3, NH4Cl, KCl, NaC2H3O2, KOH 
B)  NH4Cl, HNO3, KCl, KOH, NaC2H3O2 
C)  KCl, NH4Cl, HNO3, KOH, NaC2H3O2 
D)  HNO3, KCl, NH4Cl, KOH, NaC2H3O2 
E)  none of these

Question 13

If an acid, HA, is 10.0% dissociated in a 1.0 M solution, what is Ka for this acid?

Accepted Answer

A)  6.3 × 10-2 
B)  9.1 × 10-2 
C)  8.1 × 10-1 
D)  1.1 × 10-2 
E)  none of these 
A)  6.3 × 10-2 
B)  9.1 × 10-2 
C)  8.1 × 10-1 
D)  1.1 × 10-2 
E)  none of these

Question 14

At a particular temperature, the ion-product constant of water, Kw, is 1.7 ×10-14. What is the pH of pure water at this temperature?

Accepted Answer

A)  6.73 
B)  7.00 
C)  7.12 
D)  6.77 
E)  6.88 
A)  6.73 
B)  7.00 
C)  7.12 
D)  6.77 
E)  6.88

Question 15

What concentration of HF (Ka = 7.2 × 10-4) has the same pH as that of 0.070 M HCl?

Accepted Answer

A)  6.8 M 
B)  5.0× 10-6 M 
C)  1.0 × 10-2 M 
D)  0.070 M 
E)  0.15 M 
A)  6.8 M 
B)  5.0× 10-6 M 
C)  1.0 × 10-2 M 
D)  0.070 M 
E)  0.15 M

Question 16

Calcium carbonate is used in many antacid tablets because it reacts with HCl, the primary acid in the stomach, to produce water, calcium chloride, and carbon dioxide. At 37°C and 760 torr, what volume of CO2 is produced when a person consumes an antacid tablet containing 500.0 mg of CaCO3 to eliminate excess stomach acid? Assume acid is in excess of the carbonate. (R = 0.08206 L.atm/K. mol)

Accepted Answer

A)  17 ml 
B)  30 ml 
C)  1300 ml 
D)  130 ml 
E)  150 ml 
A)  17 ml 
B)  30 ml 
C)  1300 ml 
D)  130 ml 
E)  150 ml

Question 17

The dihydrogenphosphate ion, H2PO4-, has both a conjugate acid and a conjugate base. These are, respectively,

Accepted Answer

A)  H2PO4- and HPO42- 
B)  HPO42- and H3PO4 
C)  HPO42- and PO43- 
D)  H3PO4 and PO43- 
E)  H3PO4 and HPO42- 
A)  H2PO4- and HPO42- 
B)  HPO42- and H3PO4 
C)  HPO42- and PO43- 
D)  H3PO4 and PO43- 
E)  H3PO4 and HPO42-

Question 18

How much water should be added to 10.0 mL of 12.0 M HCl so that it has the same pH as 0.90 M acetic acid (Ka = 1.8 × 10-5)? (Assume the volumes are additive.)

Accepted Answer

A)  30 mL 
B)  3 L 
C)  30 L 
D)  300 L 
E)  300 mL 
A)  30 mL 
B)  3 L 
C)  30 L 
D)  300 L 
E)  300 mL

Question 19

Calculate the pH of a 0.005 M solution of potassium oxide, K2O.

Accepted Answer

A)  2.3 
B)  11.7 
C)  7.0 
D)  12.0 
E)  2.0 
A)  2.3 
B)  11.7 
C)  7.0 
D)  12.0 
E)  2.0

Question 20

Calculate the pH of a 0.10 M solution of HOCl, Ka = 3.5 × 10-8.

Accepted Answer

A)  8.46 
B)  4.23 
C)  1.00 
D)  3.73 
E)  3.23 
A)  8.46 
B)  4.23 
C)  1.00 
D)  3.73 
E)  3.23

Identify the hydronium ion among the following ions.

Calculate the pH of a 2.0 × 10^-3 M solution of KClO₂. K_a for HClO₂ = 1.2 × 10^-2

The following acids are listed in order of decreasing acid strength in water.HI > HNO₂ > CH₃COOH > HClO > HCN According to Brønsted-Lowry theory, which of the following ions is the weakest base?

Which of the following is a conjugate acid-base pair?

Determine the pH of a 7.5 M H₃PO₄ ( ) solution.

What is the pH of a 0.2 M solution of NH₄Cl? K_b for NH₃ is 1.8 × 10^-5.

The pH of a 0.124 M solution of a weak base is 10.89 at 25°C. Calculate the pH of a 0.0470 M solution of the base at 25°C.

Calculate the pH of the following aqueous solutions. Choose your answer from the given pH ranges. -1.0 M NaHSO₄ (pK_a for HSO₄^- = 1.92)

Calculate the pH of a 2.0 × 10^-7 M solution of Ca(OH)₂.

The pH of a 2.1 × 10^-3 M solution of a weak base is 9.87. Calculate K_b for this base.

Calculate the [H⁺] in a 2.0 × 10^-6 M solution of NaC₂H₃O₂.(K_a for HC₂H₃O₂ = 1.8 × 10^-5)

In which of the following are the species listed in order of increasing pH? (K_a for HC₂H₃O₂ is 1.80 × 10^-5, and K_a for NH₄⁺ is 5.56 × 10^-10).

If an acid, HA, is 10.0% dissociated in a 1.0 M solution, what is K_a for this acid?

At a particular temperature, the ion-product constant of water, K_w, is 1.7 ×10^-14. What is the pH of pure water at this temperature?

What concentration of HF (K_a = 7.2 × 10^-4) has the same pH as that of 0.070 M HCl?

The dihydrogenphosphate ion, H₂PO₄^-, has both a conjugate acid and a conjugate base. These are, respectively,

How much water should be added to 10.0 mL of 12.0 M HCl so that it has the same pH as 0.90 M acetic acid (K_a = 1.8 × 10^-5)? (Assume the volumes are additive.)

Calculate the pH of a 0.005 M solution of potassium oxide, K₂O.

Calculate the pH of a 0.10 M solution of HOCl, K_a = 3.5 × 10^-8.

Atoms, Molecules, and Ions

Stoichiometry

Types of Chemical Reactions and Solution Stoichiometry

Gases

Chemical Equilibrium

Applications of Aqueous Equilibria

Energy, Enthalpy, and Thermochemistry

Spontaneity, Entropy, and Free Energy

Electrochemistry

Quantum Mechanics and Atomic Theory

Bonding: General Concepts

Covalent Bonding: Orbitals

Chemical Kinetics

Liquids and Solids

Properties of Solutions

The Representative Elements

Transition Metals and Coordination Chemistry

The Nucleus: a Chemists View

Organic and Biochemical Molecules

Filters

Exam 7: Acids and Bases

Identify the hydronium ion among the following ions.

Calculate the pH of a 2.0 × 10-3 M solution of KClO2. Ka for HClO2 = 1.2 × 10-2

The following acids are listed in order of decreasing acid strength in water.HI > HNO2 > CH3COOH > HClO > HCN According to Brønsted-Lowry theory, which of the following ions is the weakest base?

Which of the following is a conjugate acid-base pair?

​Determine the pH of a 7.5 M H3PO4 ( ) solution.

What is the pH of a 0.2 M solution of NH4Cl? Kb for NH3 is 1.8 × 10-5.

The pH of a 0.124 M solution of a weak base is 10.89 at 25°C. Calculate the pH of a 0.0470 M solution of the base at 25°C.

Calculate the pH of the following aqueous solutions. Choose your answer from the given pH ranges. -1.0 M NaHSO4 (pKa for HSO4- = 1.92)

Calculate the pH of a 2.0 × 10-7 M solution of Ca(OH)2.

The pH of a 2.1 × 10-3 M solution of a weak base is 9.87. Calculate Kb for this base.

Calculate the [H+] in a 2.0 × 10-6 M solution of NaC2H3O2.(Ka for HC2H3O2 = 1.8 × 10-5)

In which of the following are the species listed in order of increasing pH? (Ka for HC2H3O2 is 1.80 × 10-5, and Ka for NH4+ is 5.56 × 10-10).

If an acid, HA, is 10.0% dissociated in a 1.0 M solution, what is Ka for this acid?

At a particular temperature, the ion-product constant of water, Kw, is 1.7 ×10-14. What is the pH of pure water at this temperature?

What concentration of HF (Ka = 7.2 × 10-4) has the same pH as that of 0.070 M HCl?

The dihydrogenphosphate ion, H2PO4-, has both a conjugate acid and a conjugate base. These are, respectively,

How much water should be added to 10.0 mL of 12.0 M HCl so that it has the same pH as 0.90 M acetic acid (Ka = 1.8 × 10-5)? (Assume the volumes are additive.)

Calculate the pH of a 0.005 M solution of potassium oxide, K2O.

Calculate the pH of a 0.10 M solution of HOCl, Ka = 3.5 × 10-8.

Atoms, Molecules, and Ions

Stoichiometry

Types of Chemical Reactions and Solution Stoichiometry

Gases

Chemical Equilibrium

Applications of Aqueous Equilibria

Energy, Enthalpy, and Thermochemistry

Spontaneity, Entropy, and Free Energy

Electrochemistry

Quantum Mechanics and Atomic Theory

Bonding: General Concepts

Covalent Bonding: Orbitals

Chemical Kinetics

Liquids and Solids

Properties of Solutions

The Representative Elements

Transition Metals and Coordination Chemistry

The Nucleus: a Chemists View

Organic and Biochemical Molecules

Filters

Calculate the pH of a 2.0 × 10^-3 M solution of KClO₂. K_a for HClO₂ = 1.2 × 10^-2

The following acids are listed in order of decreasing acid strength in water.HI > HNO₂ > CH₃COOH > HClO > HCN According to Brønsted-Lowry theory, which of the following ions is the weakest base?

Determine the pH of a 7.5 M H₃PO₄ ( ) solution.

What is the pH of a 0.2 M solution of NH₄Cl? K_b for NH₃ is 1.8 × 10^-5.

Calculate the pH of the following aqueous solutions. Choose your answer from the given pH ranges. -1.0 M NaHSO₄ (pK_a for HSO₄^- = 1.92)

Calculate the pH of a 2.0 × 10^-7 M solution of Ca(OH)₂.

The pH of a 2.1 × 10^-3 M solution of a weak base is 9.87. Calculate K_b for this base.

Calculate the [H⁺] in a 2.0 × 10^-6 M solution of NaC₂H₃O₂.(K_a for HC₂H₃O₂ = 1.8 × 10^-5)

In which of the following are the species listed in order of increasing pH? (K_a for HC₂H₃O₂ is 1.80 × 10^-5, and K_a for NH₄⁺ is 5.56 × 10^-10).

If an acid, HA, is 10.0% dissociated in a 1.0 M solution, what is K_a for this acid?

At a particular temperature, the ion-product constant of water, K_w, is 1.7 ×10^-14. What is the pH of pure water at this temperature?

What concentration of HF (K_a = 7.2 × 10^-4) has the same pH as that of 0.070 M HCl?

The dihydrogenphosphate ion, H₂PO₄^-, has both a conjugate acid and a conjugate base. These are, respectively,

How much water should be added to 10.0 mL of 12.0 M HCl so that it has the same pH as 0.90 M acetic acid (K_a = 1.8 × 10^-5)? (Assume the volumes are additive.)

Calculate the pH of a 0.005 M solution of potassium oxide, K₂O.

Calculate the pH of a 0.10 M solution of HOCl, K_a = 3.5 × 10^-8.