Question 1

Calculate the pH of a 1.8 M solution of HNO3.

Accepted Answer

A)  -0.59 
B)  -0.26 
C)  14.26 
D)  13.74 
E)  0.26 
A)  -0.59 
B)  -0.26 
C)  14.26 
D)  13.74 
E)  0.26

Question 2

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 3

​The pH of a 0.010 M weak acid solution is 5.28. Calculate Ka for this acid.

Accepted Answer

A)  1.9​×10-9 
B)  ​2.8×10-9 
C)  ​5.3×10-6 
D)  ​3.6×10-16 
E)  ​5.3×10-8 
A)  1.9​×10-9 
B)  ​2.8×10-9 
C)  ​5.3×10-6 
D)  ​3.6×10-16 
E)  ​5.3×10-8

Question 4

For a neutral solution, it must be true that

Accepted Answer

A)  pH = 7.00. 
B)  [H+] = [OH-]. 
C)  [H2O] = 1 × 10-14 
D)  [H+] = 0 M. 
E)  At least two of these must be true. 
A)  pH = 7.00. 
B)  [H+] = [OH-]. 
C)  [H2O] = 1 × 10-14 
D)  [H+] = 0 M. 
E)  At least two of these must be true.

Question 5

​Which of the following is true of Arrhenius concept of acids and bases?

Accepted Answer

A)  ​Acids produce hydroxide ions in aqueous solution and bases produce hydrogen ions. 
B)  ​Acids and bases are proton (H+) donors. 
C)  ​Acids are proton (H+) acceptors and bases are proton donors. 
D)  Acids produce hydrogen ions in aqueous solution and bases produce hydroxide ions. 
E)  ​Acids are electron donors and bases are electron acceptors. 
A)  ​Acids produce hydroxide ions in aqueous solution and bases produce hydrogen ions. 
B)  ​Acids and bases are proton (H+) donors. 
C)  ​Acids are proton (H+) acceptors and bases are proton donors. 
D)  Acids produce hydrogen ions in aqueous solution and bases produce hydroxide ions. 
E)  ​Acids are electron donors and bases are electron acceptors.

Question 6

If Ka for HCN is 6.2 × 10-10, what is Kb for CN-?

Accepted Answer

A)  6.2 × 10-24 
B)  6.2 × 104 
C)  1.6 × 10-5 
D)  1.6 × 1023 
E)  none of these 
A)  6.2 × 10-24 
B)  6.2 × 104 
C)  1.6 × 10-5 
D)  1.6 × 1023 
E)  none of these

Calculate the pH of a 1.8 M solution of HNO₃.

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

The pH of a 0.010 M weak acid solution is 5.28. Calculate K_a for this acid.

For a neutral solution, it must be true that

Which of the following is true of Arrhenius concept of acids and bases?

If K_a for HCN is 6.2 × 10^-10, what is K_b for CN^-?

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

Calculate the pH of a 1.8 M solution of HNO3.

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

​The pH of a 0.010 M weak acid solution is 5.28. Calculate Ka for this acid.

For a neutral solution, it must be true that

​Which of the following is true of Arrhenius concept of acids and bases?

If Ka for HCN is 6.2 × 10-10, what is Kb for CN-?

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 1.8 M solution of HNO₃.

The pH of a 0.010 M weak acid solution is 5.28. Calculate K_a for this acid.

Which of the following is true of Arrhenius concept of acids and bases?

If K_a for HCN is 6.2 × 10^-10, what is K_b for CN^-?