Question 1

What concentration of HF (Ka = 7.2 F1F1F1S1F1F1F10 10-4) has the same pH as that of 0.069 M HCl?

Accepted Answer

A)  6.6 M 
B)  5.0 F1F1F1S1F1F1F10 10-6 M 
C)  1.0 F1F1F1S1F1F1F10 10-2 M 
D)  0.069 M 
E)  0.15 M 
A)  6.6 M 
B)  5.0 F1F1F1S1F1F1F10 10-6 M 
C)  1.0 F1F1F1S1F1F1F10 10-2 M 
D)  0.069 M 
E)  0.15 M A

Question 2

The equilibrium constant for the reaction A- + H+   HA
Is called

Accepted Answer

A)  Kb 
B)    
C)  KwKa 
D)    
E)  Ka 
A)  Kb 
B)    
C)  KwKa 
D)    
E)  Ka D

Question 3

Calculate the pH of a 2.0 F1F1F1S1F1F1F10 10-3 M solution of KClO2. Ka for HClO2 = 1.2 F1F1F1S1F1F1F10 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 B

Question 4

If solid sodium cyanide (NaCN) is dissolved in pure water, will the solution be acidic, neutral, or basic?

Accepted Answer

A)  acidic 
B)  neutral 
C)  basic 
A)  acidic 
B)  neutral 
C)  basic

Question 5

Calculate the pH of a 0.02 M solution of KOH.

Accepted Answer

A)  1.7 
B)  We cannot calculate the answer unless a volume is given. 
C)  12.3 
D)  2.0 
E)  12.0 
A)  1.7 
B)  We cannot calculate the answer unless a volume is given. 
C)  12.3 
D)  2.0 
E)  12.0

Question 6

What is the equilibrium constant for the following reaction? NH4+ + OH-   NH3 + H2O

Accepted Answer

A)    
B)    
C)    
D)    
E)    
A)    
B)    
C)    
D)    
E)

Question 7

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 8

Which of the following is the equilibrium constant expression for the dissociation of the weak acid HOCl?

Accepted Answer

A)    
B)  K = [H+][OCl-] 
C)    
D)    
E)  none of these 
A)    
B)  K = [H+][OCl-] 
C)    
D)    
E)  none of these

Question 9

Consider two separate solutions of equal concentration. The first solution contains sodium hydroxide, and the second solution contains barium hydroxide. Which solution has the lower pH?

Accepted Answer

A)  The barium hydroxide solution. 
B)  The sodium hydroxide solution. 
C)  We need to know the concentrations to answer this question. 
D)  The pH's of the two solutions are equal. 
E)  We need to know the volumes to answer this question. 
A)  The barium hydroxide solution. 
B)  The sodium hydroxide solution. 
C)  We need to know the concentrations to answer this question. 
D)  The pH's of the two solutions are equal. 
E)  We need to know the volumes to answer this question.

Question 10

As water is heated, its pH decreases. This means that

Accepted Answer

A)  [OH-] > [H+]. 
B)  [H+] > [OH-]. 
C)  the water is no longer neutral. 
D)  Two of these are correct. 
E)  None of these is correct. 
A)  [OH-] > [H+]. 
B)  [H+] > [OH-]. 
C)  the water is no longer neutral. 
D)  Two of these are correct. 
E)  None of these is correct.

Question 11

Calculate the pH of a solution that is 7.22 F1F1F1S1F1F1F10 10-4 M C6H5NH2. Kb is 3.8 F1F1F1S1F1F1F10 10-10.

Accepted Answer

A)  6.28 
B)  7.72 
C)  6.50 
D)  7.50 
E)  none of these 
A)  6.28 
B)  7.72 
C)  6.50 
D)  7.50 
E)  none of these

Question 12

Provide an example of a salt that is acidic, a salt that is basic, and a salt that is neutral when dissolved in water. Provide chemical equations for each of these to support your answer.

Accepted Answer

See Sectio

Question 13

The pH of a 2.1 F1F1F1S1F1F1F10 10-3 M solution of a weak base is 9.87. Calculate Kb for this base.

Accepted Answer

A)  2.6 F1F1F1S1F1F1F10 10-6 
B)  1.2 F1F1F1S1F1F1F10 10-4 
C)  6.4 F1F1F1S1F1F1F10 10-8 
D)  8.7 F1F1F1S1F1F1F10F1F1F1S1F1F1F1010-18 
E)  none of these 
A)  2.6 F1F1F1S1F1F1F10 10-6 
B)  1.2 F1F1F1S1F1F1F10 10-4 
C)  6.4 F1F1F1S1F1F1F10 10-8 
D)  8.7 F1F1F1S1F1F1F10F1F1F1S1F1F1F1010-18 
E)  none of these

Question 14

Calculate the pH of a 0.23 M solution of NaA (Ka for HA is 2.5 F1F1F1S1F1F1F10 10-4) at 25°C.

Accepted Answer

A)  11.88 
B)  5.52 
C)  8.48 
D)  2.96 
E)  2.12 
A)  11.88 
B)  5.52 
C)  8.48 
D)  2.96 
E)  2.12

Question 15

In which of the following are the species listed in order of increasing pH? (Ka for HC2H3O2 is 1.80 F1F1F1S1F1F1F10 10-5, and Ka for NH4+ is 5.56 F1F1F1S1F1F1F10 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 16

The strong acid HA is added to water. Which of the following is the strongest base in the system?

Accepted Answer

A)  A- 
B)  HA 
C)  H3O+ 
D)  H2A- 
E)  H2O 
A)  A- 
B)  HA 
C)  H3O+ 
D)  H2A- 
E)  H2O

Question 17

Calculate the pH of a 0.048 M solution of KOH.

Accepted Answer

A)  12.68 
B)  11.32 
C)  1.32 
D)  2.68 
E)  none of these 
A)  12.68 
B)  11.32 
C)  1.32 
D)  2.68 
E)  none of these

Question 18

What is the [H3O+] of a 0.13 M solution of NH4Cl in H2O at 25°C? (Kb for NH3 = 1.8 F1F1F1S1F1F1F10 10-5)

Accepted Answer

A)  1.2 F1F1F1S1F1F1F10 10-9 M 
B)  8.5 F1F1F1S1F1F1F10 10-6 M 
C)  2.3 F1F1F1S1F1F1F10 10-6 M 
D)  7.2F1F1F1S1F1F1F10F1F1F1S1F1F1F10 10-9 M 
E)  1.5 F1F1F1S1F1F1F10 10-3 M 
A)  1.2 F1F1F1S1F1F1F10 10-9 M 
B)  8.5 F1F1F1S1F1F1F10 10-6 M 
C)  2.3 F1F1F1S1F1F1F10 10-6 M 
D)  7.2F1F1F1S1F1F1F10F1F1F1S1F1F1F10 10-9 M 
E)  1.5 F1F1F1S1F1F1F10 10-3 M

Question 19

Calculate the pH of a 5.0 M solution of aniline (C6H5NH2; Kb = 3.8 F1F1F1S1F1F1F10 10-10).

Accepted Answer

A)  9.64 
B)  9.30 
C)  4.36 
D)  -0.070 
E)  none of these 
A)  9.64 
B)  9.30 
C)  4.36 
D)  -0.070 
E)  none of these

Question 20

The pH of a 0.6 M solution of a weak acid is 4.0. What percent of the acid has ionized?

Accepted Answer

A)  0.02% 
B)  7% 
C)  4% 
D)  0.06% 
E)  2% 
A)  0.02% 
B)  7% 
C)  4% 
D)  0.06% 
E)  2%

What concentration of HF (K_a = 7.2  10^-⁴) has the same pH as that of 0.069 M HCl?

The equilibrium constant for the reaction A^- + H⁺ HA Is called

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

If solid sodium cyanide (NaCN) is dissolved in pure water, will the solution be acidic, neutral, or basic?

Calculate the pH of a 0.02 M solution of KOH.

What is the equilibrium constant for the following reaction? NH₄⁺ + OH^- NH₃ + H₂O

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 the equilibrium constant expression for the dissociation of the weak acid HOCl?

Consider two separate solutions of equal concentration. The first solution contains sodium hydroxide, and the second solution contains barium hydroxide. Which solution has the lower pH?

As water is heated, its pH decreases. This means that

Calculate the pH of a solution that is 7.22  10^-⁴ M C₆H₅NH₂. K_b is 3.8  10^-¹⁰.

Provide an example of a salt that is acidic, a salt that is basic, and a salt that is neutral when dissolved in water. Provide chemical equations for each of these to support your answer.

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 pH of a 0.23 M solution of NaA (K_a for HA is 2.5  10^-⁴) at 25°C.

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).

The strong acid HA is added to water. Which of the following is the strongest base in the system?

Calculate the pH of a 0.048 M solution of KOH.

What is the [H₃O⁺] of a 0.13 M solution of NH₄Cl in H₂O at 25°C? (K_b for NH₃ = 1.8  10^-⁵)

Calculate the pH of a 5.0 M solution of aniline (C₆H₅NH₂; K_b = 3.8  10^-¹⁰).

The pH of a 0.6 M solution of a weak acid is 4.0. What percent of the acid has ionized?

Atoms, Molecules, and Ions

Stoichiometry

Chemical Reactions and Solutions 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

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Exam 7: Acids and Bases

What concentration of HF (Ka = 7.2  10-4) has the same pH as that of 0.069 M HCl?

The equilibrium constant for the reaction A- + H+ HA Is called

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

If solid sodium cyanide (NaCN) is dissolved in pure water, will the solution be acidic, neutral, or basic?

Calculate the pH of a 0.02 M solution of KOH.

What is the equilibrium constant for the following reaction? NH4+ + OH- NH3 + H2O

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 the equilibrium constant expression for the dissociation of the weak acid HOCl?

Consider two separate solutions of equal concentration. The first solution contains sodium hydroxide, and the second solution contains barium hydroxide. Which solution has the lower pH?

As water is heated, its pH decreases. This means that

Calculate the pH of a solution that is 7.22  10-4 M C6H5NH2. Kb is 3.8  10-10.

Provide an example of a salt that is acidic, a salt that is basic, and a salt that is neutral when dissolved in water. Provide chemical equations for each of these to support your answer.

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

Calculate the pH of a 0.23 M solution of NaA (Ka for HA is 2.5  10-4) at 25°C.

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).

The strong acid HA is added to water. Which of the following is the strongest base in the system?

Calculate the pH of a 0.048 M solution of KOH.

What is the [H3O+] of a 0.13 M solution of NH4Cl in H2O at 25°C? (Kb for NH3 = 1.8  10-5)

Calculate the pH of a 5.0 M solution of aniline (C6H5NH2; Kb = 3.8  10-10).

The pH of a 0.6 M solution of a weak acid is 4.0. What percent of the acid has ionized?

Atoms, Molecules, and Ions

Stoichiometry

Chemical Reactions and Solutions 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

What concentration of HF (K_a = 7.2  10^-⁴) has the same pH as that of 0.069 M HCl?

The equilibrium constant for the reaction A^- + H⁺ HA Is called

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

What is the equilibrium constant for the following reaction? NH₄⁺ + OH^- NH₃ + H₂O

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?

Calculate the pH of a solution that is 7.22  10^-⁴ M C₆H₅NH₂. K_b is 3.8  10^-¹⁰.

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 pH of a 0.23 M solution of NaA (K_a for HA is 2.5  10^-⁴) at 25°C.

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).

What is the [H₃O⁺] of a 0.13 M solution of NH₄Cl in H₂O at 25°C? (K_b for NH₃ = 1.8  10^-⁵)

Calculate the pH of a 5.0 M solution of aniline (C₆H₅NH₂; K_b = 3.8  10^-¹⁰).