Question 1

A 100 mL sample of 4.0 M H2SO4 could be neutralized by 100 mL of 4.0 M NH3.

Accepted Answer

A) True 
 B)False

Question 2

Which of the following acids is a monoprotic,strong acid?

Accepted Answer

A) sulfuric acid 
B) phosphoric acid 
C) hydrobromic acid 
D) carbonic acid 
E) none of the above 
A) sulfuric acid 
B) phosphoric acid 
C) hydrobromic acid 
D) carbonic acid 
E) none of the above

Question 3

The pH of a solution is 5.00.Which of the following is TRUE about the solution?

Accepted Answer

A) Its [H3O+] is 1.0 × 10-9 M 
B) Its [H3O+] is 1.0 × 10-5 M 
C) Its [H3O+] is 1.0 × 105 M 
D) It is more acidic than a solution whose pH is 4.00. 
E) none of the above 
A) Its [H3O+] is 1.0 × 10-9 M 
B) Its [H3O+] is 1.0 × 10-5 M 
C) Its [H3O+] is 1.0 × 105 M 
D) It is more acidic than a solution whose pH is 4.00. 
E) none of the above

Question 4

NH4+ and NH3 are considered a conjugate acid-base conjugate pair.

Accepted Answer

A) True 
 B)False

Question 5

What is the [OH-] in a solution that has a pOH of 9.65?

Accepted Answer

A) 4.5 ×   M 
B) 4.5 ×   M 
C) 9.8 ×   M 
D) 2.2 ×   M 
E) none of the above 
A) 4.5 ×   M 
B) 4.5 ×   M 
C) 9.8 ×   M 
D) 2.2 ×   M 
E) none of the above

Question 6

A substance that acts as an acid OR a base is called:

Accepted Answer

A) isoprotic. 
B) a salt. 
C) amphoteric. 
D) hydrophillic. 
E) none of the above 
A) isoprotic. 
B) a salt. 
C) amphoteric. 
D) hydrophillic. 
E) none of the above

Question 7

H2SO3 and H2SO4 are considered a conjugate acid-base pair.

Accepted Answer

A) True 
 B)False

Question 8

The Bronsted-Lowry definition of an acid is:

Accepted Answer

A) a proton donor. 
B) a proton acceptor. 
C) produces H⁺ in solution. 
D) produces OH⁻ in solution. 
E) none of the above 
A) a proton donor. 
B) a proton acceptor. 
C) produces H⁺ in solution. 
D) produces OH⁻ in solution. 
E) none of the above

Question 9

When an acid reacts with a metal,what is one of the usual products?

Accepted Answer

A) water 
B) salt 
C) carbon dioxide 
D) hydrogen gas 
E) none of the above 
A) water 
B) salt 
C) carbon dioxide 
D) hydrogen gas 
E) none of the above

Question 10

A neutralization reaction between an acid and sodium hydroxide formed water and the salt named sodium sulfate.What was the formula of the acid that was neutralized?

Accepted Answer

A) H2S 
B) H2SO4 
C) HCl 
D) Na2SO4 
E) none of the above 
A) H2S 
B) H2SO4 
C) HCl 
D) Na2SO4 
E) none of the above

Question 11

If the pH of an aqueous solution changed from 9.10 to 4.67,what happened to the hydronium ion concentration?

Accepted Answer

A) It decreased. 
B) It became zero. 
C) It became less than zero. 
D) It increased. 
E) none of the above 
A) It decreased. 
B) It became zero. 
C) It became less than zero. 
D) It increased. 
E) none of the above

Question 12

In a solution that has a pH = 7.0:

Accepted Answer

A) [H3O+] > [OH-] 
B) [H3O+] -] 
C) [H3O+] = [OH-] 
D) [H3O+] + [OH-] = Kw 
E) none of the above 
A) [H3O+] > [OH-] 
B) [H3O+] -] 
C) [H3O+] = [OH-] 
D) [H3O+] + [OH-] = Kw 
E) none of the above

Question 13

Which solution below would be considered the most acidic?

Accepted Answer

A) 2.9 × 10 -4 M HCl 
B) 4.5 × 10 -5 M HNO3 
C) 1.0 × 10 -7 M NaCl 
D) 1.5 × 10 -2 M KOH 
E) none of the above 
A) 2.9 × 10 -4 M HCl 
B) 4.5 × 10 -5 M HNO3 
C) 1.0 × 10 -7 M NaCl 
D) 1.5 × 10 -2 M KOH 
E) none of the above

Question 14

Substances that can act both as an acid and as a base are called:

Accepted Answer

A) neutral. 
B) buffers. 
C) indicators. 
D) amphoteric. 
E) none of these 
A) neutral. 
B) buffers. 
C) indicators. 
D) amphoteric. 
E) none of these

Question 15

The equation HCl (aq)+ H2O (l)↔ H3O+ (aq)+ Cl- (aq)properly depicts the behavior of hydrochloric acid in water.

Accepted Answer

A) True 
 B)False

Question 16

What is the pH of a solution that has a [ OH- ] = 0.0033 M?

Accepted Answer

A) 2.48 
B) 7.0033 
C) 11.52 
D) 3.3 
E) none of the above 
A) 2.48 
B) 7.0033 
C) 11.52 
D) 3.3 
E) none of the above

Question 17

A 35.0 mL sample of 0.225 M HBr was titrated with 42.3 mL of KOH.What is the concentration of the KOH?

Accepted Answer

A) 0.157 M 
B) 0.303 M 
C) 0.272 M 
D) 0.186 M 
E) none of the above 
A) 0.157 M 
B) 0.303 M 
C) 0.272 M 
D) 0.186 M 
E) none of the above

Question 18

A weak acid is a dilute acid that is not very powerful.

Accepted Answer

A) True 
 B)False

Question 19

What is the [H⁺] in a solution that has a pH of 3.35?

Accepted Answer

A) 1 ×   M 
B) 2.2 ×   M 
C) 4.5 ×   M 
D) 3.35 ×   M 
E) none of the above 
A) 1 ×   M 
B) 2.2 ×   M 
C) 4.5 ×   M 
D) 3.35 ×   M 
E) none of the above

Question 20

Which of the following acids is a diprotic,weak acid?

Accepted Answer

A) sulfuric acid 
B) phosphoric acid 
C) hydrobromic acid 
D) carbonic acid 
E) none of the above 
A) sulfuric acid 
B) phosphoric acid 
C) hydrobromic acid 
D) carbonic acid 
E) none of the above

A 100 mL sample of 4.0 M H₂SO₄ could be neutralized by 100 mL of 4.0 M NH₃.

Which of the following acids is a monoprotic,strong acid?

The pH of a solution is 5.00.Which of the following is TRUE about the solution?

NH₄⁺ and NH₃ are considered a conjugate acid-base conjugate pair.

What is the [OH^-] in a solution that has a pOH of 9.65?

A substance that acts as an acid OR a base is called:

H₂SO₃ and H₂SO₄ are considered a conjugate acid-base pair.

The Bronsted-Lowry definition of an acid is:

When an acid reacts with a metal,what is one of the usual products?

A neutralization reaction between an acid and sodium hydroxide formed water and the salt named sodium sulfate.What was the formula of the acid that was neutralized?

If the pH of an aqueous solution changed from 9.10 to 4.67,what happened to the hydronium ion concentration?

In a solution that has a pH = 7.0:

Which solution below would be considered the most acidic?

Substances that can act both as an acid and as a base are called:

The equation HCl (aq)+ H₂O (l)↔ H₃O⁺ (aq)+ Cl^-(aq)properly depicts the behavior of hydrochloric acid in water.

What is the pH of a solution that has a [ OH^- ] = 0.0033 M?

A 35.0 mL sample of 0.225 M HBr was titrated with 42.3 mL of KOH.What is the concentration of the KOH?

A weak acid is a dilute acid that is not very powerful.

What is the [H⁺] in a solution that has a pH of 3.35?

Which of the following acids is a diprotic,weak acid?

The Chemical World

Measurement and Problem Solving

Matter and Energy

Atoms and Elements

Molecules and Compounds

Chemical Composition

Chemical Reactions

Quantities in Chemical Reactions

Electrons in Atoms and the Periodic Table

Chemical Bonding

Gases

Liquids, solids, and Intermolecular Forces

Solutions

Chemical Equilibrium

Oxidation and Reduction

Radioactivity and Nuclear Chemistry

Organic Chemistry

Biochemistry

Filters

Exam 14: Acids and Bases

A 100 mL sample of 4.0 M H2SO4 could be neutralized by 100 mL of 4.0 M NH3.

Which of the following acids is a monoprotic,strong acid?

The pH of a solution is 5.00.Which of the following is TRUE about the solution?

NH4+ and NH3 are considered a conjugate acid-base conjugate pair.

What is the [OH-] in a solution that has a pOH of 9.65?

A substance that acts as an acid OR a base is called:

H2SO3 and H2SO4 are considered a conjugate acid-base pair.

The Bronsted-Lowry definition of an acid is:

When an acid reacts with a metal,what is one of the usual products?

A neutralization reaction between an acid and sodium hydroxide formed water and the salt named sodium sulfate.What was the formula of the acid that was neutralized?

If the pH of an aqueous solution changed from 9.10 to 4.67,what happened to the hydronium ion concentration?

In a solution that has a pH = 7.0:

Which solution below would be considered the most acidic?

Substances that can act both as an acid and as a base are called:

The equation HCl (aq)+ H2O (l)↔ H3O+ (aq)+ Cl- (aq)properly depicts the behavior of hydrochloric acid in water.

What is the pH of a solution that has a [ OH- ] = 0.0033 M?

A 35.0 mL sample of 0.225 M HBr was titrated with 42.3 mL of KOH.What is the concentration of the KOH?

A weak acid is a dilute acid that is not very powerful.

What is the [H⁺] in a solution that has a pH of 3.35?

Which of the following acids is a diprotic,weak acid?

The Chemical World

Measurement and Problem Solving

Matter and Energy

Atoms and Elements

Molecules and Compounds

Chemical Composition

Chemical Reactions

Quantities in Chemical Reactions

Electrons in Atoms and the Periodic Table

Chemical Bonding

Gases

Liquids, solids, and Intermolecular Forces

Solutions

Chemical Equilibrium

Oxidation and Reduction

Radioactivity and Nuclear Chemistry

Organic Chemistry

Biochemistry

Filters

A 100 mL sample of 4.0 M H₂SO₄ could be neutralized by 100 mL of 4.0 M NH₃.

NH₄⁺ and NH₃ are considered a conjugate acid-base conjugate pair.

What is the [OH^-] in a solution that has a pOH of 9.65?

H₂SO₃ and H₂SO₄ are considered a conjugate acid-base pair.

The equation HCl (aq)+ H₂O (l)↔ H₃O⁺ (aq)+ Cl^-(aq)properly depicts the behavior of hydrochloric acid in water.

What is the pH of a solution that has a [ OH^- ] = 0.0033 M?