Question 1

What is the pH of a 4.9 M solution of HClO4?

Accepted Answer

A)  14.69 
B)  0.69 
C)  -0.69 
D)  13.31 
E)  minus infinity 
A)  14.69 
B)  0.69 
C)  -0.69 
D)  13.31 
E)  minus infinity C

Question 2

Choose the case that is not a Bronsted conjugate acid-base pair.

Accepted Answer

A)  CH3NH3+, CH3NH2 
B)  HCN, CN- 
C)  HClO2, ClO2- 
D)  HCO2H, HCOH 
E)  H3BO3, H2BO3- 
A)  CH3NH3+, CH3NH2 
B)  HCN, CN- 
C)  HClO2, ClO2- 
D)  HCO2H, HCOH 
E)  H3BO3, H2BO3- D

Question 3

A solution where [H+] = 10-13 M is ______________.

Accepted Answer

A)  basic 
B)  neutral 
C)  acidic 
D)  strongly acidic 
E)  two of these 
A)  basic 
B)  neutral 
C)  acidic 
D)  strongly acidic 
E)  two of these A

Question 4

Which of the following statements is/are correct?

Accepted Answer

A)  In an acidic solution, [H+] > [OH-]. 
B)  In a basic solution, [OH-] > [H+]. 
C)  In a neutral solution, [H+] = [OH-]. 
D)  None of the above statements (a-c) are correct. 
E)  All of the above statements (a-c) are correct. 
A)  In an acidic solution, [H+] > [OH-]. 
B)  In a basic solution, [OH-] > [H+]. 
C)  In a neutral solution, [H+] = [OH-]. 
D)  None of the above statements (a-c) are correct. 
E)  All of the above statements (a-c) are correct.

Question 5

Calculate the [H+] in a solution that has a pH of 5.15.

Accepted Answer

A)    M 
B)    M 
C)  8.85 M 
D)  5.15 M 
E)  none of these 
A)    M 
B)    M 
C)  8.85 M 
D)  5.15 M 
E)  none of these

Question 6

A solution with a pH of 2 is how many times more acidic as a solution with a pH of 6?

Accepted Answer

A)  3 
B)  0.3 
C)  100000 
D)  10000 
E)  8 
A)  3 
B)  0.3 
C)  100000 
D)  10000 
E)  8

Question 7

Calculate the [OH-] in a solution that has a pH of 3.76.

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 8

A solution has a pH of 4.42. The [H+] in this solution is

Accepted Answer

A)  2.6 * 10-10 M 
B)  3.8 * 10-5 M 
C)  9.58 
D)  4.42 
E)  none of these 
A)  2.6 * 10-10 M 
B)  3.8 * 10-5 M 
C)  9.58 
D)  4.42 
E)  none of these

Question 9

A solution has [OH-] = 3.0 *10-7 M. The [H+] in this solution is

Accepted Answer

A)  1.0 M 
B)    M 
C)    M 
D)    M 
E)  none of these 
A)  1.0 M 
B)    M 
C)    M 
D)    M 
E)  none of these

Question 10

How many moles of pure NaOH must be used to prepare 1.0 L of a solution that has pH = 12.26?

Accepted Answer

A)  8.2 * 10-16 mol 
B)  0.018 mol 
C)  5.5 * 10-13 mol 
D)  1.74 mol 
E)  none of these 
A)  8.2 * 10-16 mol 
B)  0.018 mol 
C)  5.5 * 10-13 mol 
D)  1.74 mol 
E)  none of these

Question 11

Calculate the [H+] in a solution that has a pH of 9.16.

Accepted Answer

A)    M 
B)    M 
C)  4.84 M 
D)  9.16 M 
E)  none of these 
A)    M 
B)    M 
C)  4.84 M 
D)  9.16 M 
E)  none of these

Question 12

Identify the Bronsted acids and bases in the following equation (A = Bronsted acid, B = Bronsted base): HSO3-  + CN-$\rightarrow$ HCN + SO32-

Accepted Answer

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

Question 13

A solution has [H+] = 5.0 *10-8 M. The pH of this solution is

Accepted Answer

A)  6.70 
B)  5.98 
C)  7.30 
D)  9.77 
E)  none of these 
A)  6.70 
B)  5.98 
C)  7.30 
D)  9.77 
E)  none of these

Question 14

A buffered solution contains HNO2. It also contains

Accepted Answer

A)  KCl 
B)  HNO3 
C)  KOH 
D)  KNO2 
E)  NaCl 
A)  KCl 
B)  HNO3 
C)  KOH 
D)  KNO2 
E)  NaCl

Question 15

A solution has [H+] = 4.3 *10-8 M. The pOH of this solution is

Accepted Answer

A)  7.37 
B)  6.63 
C)  9.37 
D)  3.28 
E)  none of these 
A)  7.37 
B)  6.63 
C)  9.37 
D)  3.28 
E)  none of these

Question 16

Which statement is true for a strong base solution with a concentration greater than 1.0 M?

Accepted Answer

A) pOH > pH B) pH > pOH C) pH < 0 D) pH<14 E) Two of these (a-d) are true. A) pOH > pH B) pH > pOH C) pH < 0 D) pH<14 E) Two of these (a-d) are true.

Question 17

Solid calcium hydroxide is dissolved in water until the pH of the solution is 10.39. The hydroxide ion concentration [OH-] of the solution is

Accepted Answer

A)    M 
B)  3.61 M 
C)    M 
D)    M 
E)  none of these 
A)    M 
B)  3.61 M 
C)    M 
D)    M 
E)  none of these

Question 18

Consider the reaction HC2H3O2(aq) + H2O(l) $\rightarrow$H3O+(aq) + C2H3O2-(aq). Which species is the conjugate acid?

Accepted Answer

A)  HC2H3O2(aq) 
B)  H2O(l) 
C)  H3O+(aq) 
D)    
E)  two of these 
A)  HC2H3O2(aq) 
B)  H2O(l) 
C)  H3O+(aq) 
D)    
E)  two of these

Question 19

What is the pH of a solution that has [OH-] =   .

Accepted Answer

A)  4.93 M 
B)  9.07 M 
C)  2.46 M 
D)  7.14 M 
E)  none of these 
A)  4.93 M 
B)  9.07 M 
C)  2.46 M 
D)  7.14 M 
E)  none of these

Question 20

Calculate the [H+] in a solution that has a pH of 5.54.

Accepted Answer

A)  8.46 
B)    M 
C)  5.54 
D)    M 
E)  none of these 
A)  8.46 
B)    M 
C)  5.54 
D)    M 
E)  none of these

Exam 16: Acids and Bases

What is the pH of a 4.9 M solution of HClO4?

Choose the case that is not a Bronsted conjugate acid-base pair.

A solution where [H+] = 10-13 M is ______________.

Which of the following statements is/are correct?

Calculate the [H+] in a solution that has a pH of 5.15.

A solution with a pH of 2 is how many times more acidic as a solution with a pH of 6?

Calculate the [OH-] in a solution that has a pH of 3.76.

A solution has a pH of 4.42. The [H+] in this solution is

A solution has [OH-] = 3.0 *10-7 M. The [H+] in this solution is

How many moles of pure NaOH must be used to prepare 1.0 L of a solution that has pH = 12.26?

Calculate the [H+] in a solution that has a pH of 9.16.

Identify the Bronsted acids and bases in the following equation (A = Bronsted acid, B = Bronsted base): HSO3- + CN- →\rightarrow→ HCN + SO32-

A solution has [H+] = 5.0 *10-8 M. The pH of this solution is

A buffered solution contains HNO2. It also contains

A solution has [H+] = 4.3 *10-8 M. The pOH of this solution is

Which statement is true for a strong base solution with a concentration greater than 1.0 M?

Solid calcium hydroxide is dissolved in water until the pH of the solution is 10.39. The hydroxide ion concentration [OH-] of the solution is

Consider the reaction HC2H3O2(aq) + H2O(l) →\rightarrow→ H3O+(aq) + C2H3O2-(aq). Which species is the conjugate acid?

What is the pH of a solution that has [OH-] = .

Calculate the [H+] in a solution that has a pH of 5.54.

Chemistry: an Introduction

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Chemical Foundations: Elements, Atoms, and Ions

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Chemical Reactions: an Introduction

Reactions in Aqueous Solutions

Chemical Composition

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Modern Atomic Theory

Chemical Bonding

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Filters

What is the pH of a 4.9 M solution of HClO₄?

A solution where [H⁺] = 10^-13 M is ______________.

Calculate the [H⁺] in a solution that has a pH of 5.15.

Calculate the [OH^-] in a solution that has a pH of 3.76.

A solution has a pH of 4.42. The [H⁺] in this solution is

A solution has [OH^-] = 3.0 *10^-⁷ M. The [H⁺] in this solution is

Calculate the [H⁺] in a solution that has a pH of 9.16.

Identify the Bronsted acids and bases in the following equation (A = Bronsted acid, B = Bronsted base): HSO₃^- + CN^- $\rightarrow$ HCN + SO₃²^-

A solution has [H⁺] = 5.0 *10^-⁸ M. The pH of this solution is

A buffered solution contains HNO₂. It also contains

A solution has [H⁺] = 4.3 *10^-⁸ M. The pOH of this solution is

Solid calcium hydroxide is dissolved in water until the pH of the solution is 10.39. The hydroxide ion concentration [OH^-] of the solution is

Consider the reaction HC₂H₃O₂(aq) + H₂O(l) $\rightarrow$ H₃O⁺(aq) + C₂H₃O₂^-(aq). Which species is the conjugate acid?

What is the pH of a solution that has [OH^-] = .

Calculate the [H⁺] in a solution that has a pH of 5.54.