Question 1

Calculate the molarity of hydroxide ion in an aqueous solution that has a pOH of 3.24.

Accepted Answer

A)  5.8 × 10-4 
B)  10.76 
C)  1.7 × 10-11 
D)  3.2 × 10-14 
E)  1.1 × 10-13 
A)  5.8 × 10-4 
B)  10.76 
C)  1.7 × 10-11 
D)  3.2 × 10-14 
E)  1.1 × 10-13 A

Question 2

What does the term amphoteric mean?

Accepted Answer

A substance is amphoteric if it can behave as an acid or a base,depending on the environment.

Question 3

Determine the [OH⁻] concentration in a 0.235 M LiOH solution.

Accepted Answer

A)  4.25 × 10-14 M 
B)  0.470 M 
C)  2.13 × 10-14 M 
D)  0.118 M 
E)  0.235 M 
A)  4.25 × 10-14 M 
B)  0.470 M 
C)  2.13 × 10-14 M 
D)  0.118 M 
E)  0.235 M E

Question 4

Which of the following is a triprotic acid?

Accepted Answer

A)  HCl 
B)  H2SO4 
C)  H3PO4 
D)  CF4 
E)  HC2H3O2 
A)  HCl 
B)  H2SO4 
C)  H3PO4 
D)  CF4 
E)  HC2H3O2

Question 5

Calculate the concentration of H3O⁺ in a solution that contains 6.25 × 10-9 M OH⁻ at 25°C.Identify the solution as acidic,basic,or neutral.

Accepted Answer

A)  6.38 × 10-9 M, basic 
B)  1.60 × 10-6 M, acidic 
C)  7.94 × 10-11 M, acidic 
D)  7.38 × 10-3 M, basic 
E)  4.92× 10-5 M, acidic 
A)  6.38 × 10-9 M, basic 
B)  1.60 × 10-6 M, acidic 
C)  7.94 × 10-11 M, acidic 
D)  7.38 × 10-3 M, basic 
E)  4.92× 10-5 M, acidic

Question 6

Which of the following bases is the strongest? The base is followed by its Kb.

Accepted Answer

A)  (CH3CH2)2NH, 8.6 × 10-4 
B)  CH3NH2, 4.4 × 10-4 
C)  C6H5NH2, 4.0 × 10-10 
D)  NH3, 1.76 × 10-5 
E)  C5H5N, 1.7 × 10-9 
A)  (CH3CH2)2NH, 8.6 × 10-4 
B)  CH3NH2, 4.4 × 10-4 
C)  C6H5NH2, 4.0 × 10-10 
D)  NH3, 1.76 × 10-5 
E)  C5H5N, 1.7 × 10-9

Question 7

Calculate the pH of a solution that contains 2.4 × 10-8 M H3O⁺ at 25°C.

Accepted Answer

A)  2.40 
B)  6.38 
C)  7.62 
D)  5.38 
E)  8.62 
A)  2.40 
B)  6.38 
C)  7.62 
D)  5.38 
E)  8.62

Question 8

Which of the following acids is the weakest? The acid is followed by its Ka value.

Accepted Answer

A)  HF, 3.5 × 10-4 
B)  HIO, 2.3 × 10-11 
C)  HNO2, 4.6 × 10-4 
D)  H5COOH, 6.5 × 10-5 
E)  HClO2, 1.1 × 10-2 
A)  HF, 3.5 × 10-4 
B)  HIO, 2.3 × 10-11 
C)  HNO2, 4.6 × 10-4 
D)  H5COOH, 6.5 × 10-5 
E)  HClO2, 1.1 × 10-2

Question 9

Determine the pH of a 0.18 M H2CO3 solution.Carbonic acid is a diprotic acid whose Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

Accepted Answer

A)  11.00 
B)  10.44 
C)  5.50 
D)  4.31 
E)  3.56 
A)  11.00 
B)  10.44 
C)  5.50 
D)  4.31 
E)  3.56

Question 10

Describe a molecule that can be a Lewis acid.

Accepted Answer

A molecule with an i

Question 11

Determine the pH of a 0.00598 M HClO4 solution.

Accepted Answer

A)  11.777 
B)  6.434 
C)  7.566 
D)  2.223 
E)  3.558 
A)  11.777 
B)  6.434 
C)  7.566 
D)  2.223 
E)  3.558

Question 12

A Lewis base

Accepted Answer

A)  donates electrons. 
B)  accepts electrons. 
C)  donates a proton. 
D)  accepts a proton. 
E)  donates more than one proton. 
A)  donates electrons. 
B)  accepts electrons. 
C)  donates a proton. 
D)  accepts a proton. 
E)  donates more than one proton.

Question 13

Calculate the pOH of a solution that contains 2.4 × 10-8 M H3O⁺ at 25°C.

Accepted Answer

A)  2.40 
B)  6.38 
C)  7.62 
D)  5.38 
E)  8.62 
A)  2.40 
B)  6.38 
C)  7.62 
D)  5.38 
E)  8.62

Question 14

Determine the pH of a 0.023 M HNO3 solution.

Accepted Answer

A)  12.36 
B)  3.68 
C)  1.64 
D)  2.30 
E)  2.49 
A)  12.36 
B)  3.68 
C)  1.64 
D)  2.30 
E)  2.49

Question 15

What is the pOH of a 0.0020 M HNO3 solution?

Accepted Answer

A)  0.0020 
B)  0.0040 
C)  2.70 
D)  11.30 
A)  0.0020 
B)  0.0040 
C)  2.70 
D)  11.30

Question 16

Determine the Ka of an acid whose 0.294 M solution has a pH of 2.80.

Accepted Answer

A)  1.2 × 10-5 
B)  8.5 × 10-6 
C)  2.7 
D)  4.9 × 10-7 
E)  5.4 × 10-3 
A)  1.2 × 10-5 
B)  8.5 × 10-6 
C)  2.7 
D)  4.9 × 10-7 
E)  5.4 × 10-3

Question 17

Calculate the hydronium ion concentration in an aqueous solution with a pH of 9.85 at 25°C.

Accepted Answer

A)  7.1 × 10-5 M 
B)  4.2 × 10-10 M 
C)  8.7 × 10-10 M 
D)  6.5 × 10-5 M 
E)  1.4 × 10-10 M 
A)  7.1 × 10-5 M 
B)  4.2 × 10-10 M 
C)  8.7 × 10-10 M 
D)  6.5 × 10-5 M 
E)  1.4 × 10-10 M

Question 18

An aqueous solution at 25.0°C contains [H+] = 0.090 M.What is the pH of the solution?

Accepted Answer

A)  1.05 
B)  -1.05 
C)  13.0 
D)  0.0900 
E)  1.10 × 10-13 
A)  1.05 
B)  -1.05 
C)  13.0 
D)  0.0900 
E)  1.10 × 10-13

Question 19

Calculate the pOH in an aqueous solution with a pH of 7.85 at 25°C.

Accepted Answer

A)  4.15 
B)  5.15 
C)  6.15 
D)  7.15 
E)  8.15 
A)  4.15 
B)  5.15 
C)  6.15 
D)  7.15 
E)  8.15

Question 20

Which of the following is a Lewis acid?

Accepted Answer

A)  BCl3 
B)  CI4 
C)  NH3 
D)  CHI3 
E)  None of the above are Lewis acids. 
A)  BCl3 
B)  CI4 
C)  NH3 
D)  CHI3 
E)  None of the above are Lewis acids.

Exam 17: Acids and Bases

Calculate the molarity of hydroxide ion in an aqueous solution that has a pOH of 3.24.

What does the term amphoteric mean?

Determine the [OH⁻] concentration in a 0.235 M LiOH solution.

Which of the following is a triprotic acid?

Calculate the concentration of H3O⁺ in a solution that contains 6.25 × 10-9 M OH⁻ at 25°C.Identify the solution as acidic,basic,or neutral.

Which of the following bases is the strongest? The base is followed by its Kb.

Calculate the pH of a solution that contains 2.4 × 10-8 M H3O⁺ at 25°C.

Which of the following acids is the weakest? The acid is followed by its Ka value.

Determine the pH of a 0.18 M H2CO3 solution.Carbonic acid is a diprotic acid whose Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

Describe a molecule that can be a Lewis acid.

Determine the pH of a 0.00598 M HClO4 solution.

A Lewis base

Calculate the pOH of a solution that contains 2.4 × 10-8 M H3O⁺ at 25°C.

Determine the pH of a 0.023 M HNO3 solution.

What is the pOH of a 0.0020 M HNO3 solution?

Determine the Ka of an acid whose 0.294 M solution has a pH of 2.80.

Calculate the hydronium ion concentration in an aqueous solution with a pH of 9.85 at 25°C.

An aqueous solution at 25.0°C contains [H+] = 0.090 M.What is the pH of the solution?

Calculate the pOH in an aqueous solution with a pH of 7.85 at 25°C.

Which of the following is a Lewis acid?

Essentials: Units, Measurements, and Problem Solving

Atoms

The Quantum Mechanical Model of the Atom

Periodic Properties of the Elements

Molecules and Compounds

Chemical Bonding I

Chemical Bonding Ii

Chemical Reactions and Chemical Quantities

Introduction to Solutions and Aqueous Reactions

Thermochemistry

Gases

Liquids, Solids, and Intermolecular Forces

Crystalline Solids and Modern Materials

Solutions

Chemical Kinetics

Chemical Equilibrium

Aqueous Ionic Equilibrium

Free Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry

Transition Metals and Coordination Compounds

Filters

Calculate the concentration of H₃O⁺ in a solution that contains 6.25 × 10^-9 M OH⁻ at 25°C.Identify the solution as acidic,basic,or neutral.

Which of the following bases is the strongest? The base is followed by its K_b.

Calculate the pH of a solution that contains 2.4 × 10^-⁸ M H₃O⁺ at 25°C.

Which of the following acids is the weakest? The acid is followed by its K_a value.

Determine the pH of a 0.18 M H₂CO₃ solution.Carbonic acid is a diprotic acid whose K_a1 = 4.3 × 10^-7 and K_a2 = 5.6 × 10^-11.

Determine the pH of a 0.00598 M HClO₄ solution.

Calculate the pOH of a solution that contains 2.4 × 10^-⁸ M H₃O⁺ at 25°C.

Determine the pH of a 0.023 M HNO₃ solution.

What is the pOH of a 0.0020 M HNO₃ solution?

Determine the K_a of an acid whose 0.294 M solution has a pH of 2.80.

An aqueous solution at 25.0°C contains [H⁺] = 0.090 M.What is the pH of the solution?