Question 1

A solution has [OH-]= 5.0 *10-4 M. The pH of this solution is

Accepted Answer

A)  3.30 
B)  2.00 * 10-11 
C)  5.35 
D)  10.70 
E)  none of these 
A)  3.30 
B)  2.00 * 10-11 
C)  5.35 
D)  10.70 
E)  none of these

Question 2

Calculate the pH of 0.056 M HClO4.

Accepted Answer

A)  0.056 
B)  7.00 
C)  1.25 
D)  12.75 
E)  none of these 
A)  0.056 
B)  7.00 
C)  1.25 
D)  12.75 
E)  none of these

Question 3

The pH of a solution at 25oC in which [OH-] = 3.5 *10-5 M is

Accepted Answer

A)  4.46 
B)  4.77 
C)  9.54 
D)  11.04 
E)  none of these 
A)  4.46 
B)  4.77 
C)  9.54 
D)  11.04 
E)  none of these

Question 4

A solution with a pH of 2.17 is

Accepted Answer

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

Question 5

Calculate the pH of an acid solution containing 0.044 M HNO3.

Accepted Answer

A)  12.64 
B)  2.81 
C)  1.36 
D)  0.044 
E)  none of these 
A)  12.64 
B)  2.81 
C)  1.36 
D)  0.044 
E)  none of these

Question 6

A solution with a pH of 3 is how many times as acidic as a solution with a pH of 5? (Ignore significant figures for this problem.)

Accepted Answer

A)  0.6 times as acidic 
B)  2 times as acidic 
C)  100 times as acidic 
D)  15 times as acidic 
E)  8 times as acidic 
A)  0.6 times as acidic 
B)  2 times as acidic 
C)  100 times as acidic 
D)  15 times as acidic 
E)  8 times as acidic

Question 7

Which of the following is true for a buffered solution?

Accepted Answer

A)  The solution resists any change in its [H+]. 
B)  The solution will not change its pH very much even if a concentrated acid is added. 
C)  The solution will not change its pH very much even if a strong base is added. 
D)  Any H+ ions added will react with a conjugate base of a weak acid already in solution. 
E)  all of these 
A)  The solution resists any change in its [H+]. 
B)  The solution will not change its pH very much even if a concentrated acid is added. 
C)  The solution will not change its pH very much even if a strong base is added. 
D)  Any H+ ions added will react with a conjugate base of a weak acid already in solution. 
E)  all of these

Question 8

As water is heated, its [H+] increases. This means that

Accepted Answer

A)  the water is no longer neutral 
B)  [H+] > [OH-] 
C)  [OH-] > [H+] 
D)  a and b are correct 
E)  none of these 
A)  the water is no longer neutral 
B)  [H+] > [OH-] 
C)  [OH-] > [H+] 
D)  a and b are correct 
E)  none of these

Question 9

Arrhenius postulated that acids produce hydrogen ions in aqueous solution, whereas bases produce hydroxide ions.

Accepted Answer

A) True 
 B)False

Question 10

A solution is prepared by dissolving 111.9 g HCl(g) in enough water to make 160.0 L of solution. The pH of this solution is

Accepted Answer

A)  1.72 
B)  12.28 
C)  0.155 
D)  3.07 
E)  none of these 
A)  1.72 
B)  12.28 
C)  0.155 
D)  3.07 
E)  none of these

Question 11

Calculate the [H+] in a solution that has a pH of 8.82.

Accepted Answer

A)    M 
B)    M 
C)    M 
D)    M 
E)  none of these 
A)    M 
B)    M 
C)    M 
D)    M 
E)  none of these

Question 12

What is the pH of a solution prepared by dissolving 96.1 g NaOH in enough water to make 3.2 L of solution?

Accepted Answer

A)  13.88 
B)  0.12 
C)  14.12 
D)  10.28 
E)  none of these 
A)  13.88 
B)  0.12 
C)  14.12 
D)  10.28 
E)  none of these

Question 13

A strong acid is one for which the forward reaction predominates.

Accepted Answer

A) True 
 B)False

Question 14

A NaCl(aq) solution is automatically buffered.

Accepted Answer

A) True 
 B)False

Question 15

What is the pH of a 2.1 M solution of HNO3?

Accepted Answer

A)  -0.32 
B)  0.32 
C)  14.32 
D)  13.68 
E)  none of these 
A)  -0.32 
B)  0.32 
C)  14.32 
D)  13.68 
E)  none of these

Question 16

Calculate the pH of a 0.045 M HCl solution.

Accepted Answer

A)  1.23 
B)  1.35 
C)  12.65 
D)  12.29 
E)  none of these 
A)  1.23 
B)  1.35 
C)  12.65 
D)  12.29 
E)  none of these

Question 17

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

Accepted Answer

A)  HNO3-, H2NO3 
B)  HNH4, NH4+ 
C)  H2F, HF- 
D)  HPO42-, PO43- 
E)  H2CN, CN- 
A)  HNO3-, H2NO3 
B)  HNH4, NH4+ 
C)  H2F, HF- 
D)  HPO42-, PO43- 
E)  H2CN, CN-

Question 18

A solution has a pH of 3.16. The pOH of this solution is

Accepted Answer

A)  3.26 
B)  10.74 
C)  3.16 
D)  10.84 
E)  none of these 
A)  3.26 
B)  10.74 
C)  3.16 
D)  10.84 
E)  none of these

Question 19

The conjugate acid of a weak base is a strong acid.

Accepted Answer

A) True 
 B)False

Question 20

What is the pH of a 0.25 M nitric acid (HNO3) solution?

Accepted Answer

A)  0.60 
B)  2.50 
C)  2.49 
D)  13.40 
E)  none of these 
A)  0.60 
B)  2.50 
C)  2.49 
D)  13.40 
E)  none of these

Exam 16: Acids and Bases

A solution has [OH-]= 5.0 *10-4 M. The pH of this solution is

Calculate the pH of 0.056 M HClO4.

The pH of a solution at 25oC in which [OH-] = 3.5 *10-5 M is

A solution with a pH of 2.17 is

Calculate the pH of an acid solution containing 0.044 M HNO3.

A solution with a pH of 3 is how many times as acidic as a solution with a pH of 5? (Ignore significant figures for this problem.)

Which of the following is true for a buffered solution?

As water is heated, its [H+] increases. This means that

Arrhenius postulated that acids produce hydrogen ions in aqueous solution, whereas bases produce hydroxide ions.

A solution is prepared by dissolving 111.9 g HCl(g) in enough water to make 160.0 L of solution. The pH of this solution is

Calculate the [H+] in a solution that has a pH of 8.82.

What is the pH of a solution prepared by dissolving 96.1 g NaOH in enough water to make 3.2 L of solution?

A strong acid is one for which the forward reaction predominates.

A NaCl(aq) solution is automatically buffered.

What is the pH of a 2.1 M solution of HNO3?

Calculate the pH of a 0.045 M HCl solution.

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

A solution has a pH of 3.16. The pOH of this solution is

The conjugate acid of a weak base is a strong acid.

What is the pH of a 0.25 M nitric acid (HNO3) solution?

Chemistry: an Introduction

Measurements and Calculations

Matter

Chemical Foundations: Elements, Atoms, and Ions

Nomenclature

Chemical Reactions: an Introduction

Reactions in Aqueous Solutions

Chemical Composition

Chemical Quantities

Energy

Modern Atomic Theory

Chemical Bonding

Gases

Liquids and Solids

Solutions

Equilibrium

Oxidation-Reduction Reactions and Electrochemistry

Radioactivity and Nuclear Energy

Organic Chemistry

Biochemistry

Filters

A solution has [OH^-]= 5.0 *10^-⁴ M. The pH of this solution is

Calculate the pH of 0.056 M HClO₄.

The pH of a solution at 25^oC in which [OH^-] = 3.5 *10^-⁵ M is

Calculate the pH of an acid solution containing 0.044 M HNO₃.

As water is heated, its [H⁺] increases. This means that

Calculate the [H⁺] in a solution that has a pH of 8.82.

What is the pH of a 2.1 M solution of HNO₃?

What is the pH of a 0.25 M nitric acid (HNO₃) solution?