Question 1

Which of the following is the strongest acid?

Accepted Answer

A) HNO2, Ka = 5.6 × 10−4 
B) HCN, Ka = 6.2 × 10−10 
C) NH4+, Ka = 5.6 × 10−10 
D) CH3CO2H, Ka = 1.8 × 10−5 
E) HCO2H, Ka = 1.8 × 10−4 
A) HNO2, Ka = 5.6 × 10−4 
B) HCN, Ka = 6.2 × 10−10 
C) NH4+, Ka = 5.6 × 10−10 
D) CH3CO2H, Ka = 1.8 × 10−5 
E) HCO2H, Ka = 1.8 × 10−4

Question 2

Calculate the pOH of a solution that has [H3O+] = 3.1 × 10-8 M.

Accepted Answer

A) pOH = 3.10 
B) pOH = 6.49 
C) pOH = 7.51 
D) pOH = 3.18 
E) pOH = 8.00 
A) pOH = 3.10 
B) pOH = 6.49 
C) pOH = 7.51 
D) pOH = 3.18 
E) pOH = 8.00

Question 3

Identify gastric juice, pH = 1.0, as acidic, basic, or neutral.

Accepted Answer

Gastric juice with a pH of 1.0 is highly

Question 4

Select the two Brønsted-Lowry acids in the following equation: NH3(aq)+ HF(aq)⇌ NH4+(aq)+ F−(aq)

Accepted Answer

A) NH3 and HF 
B) NH3 and F− 
C) HF and F− 
D) NH4+ and F- 
E) HF and NH4+ 
A) NH3 and HF 
B) NH3 and F− 
C) HF and F− 
D) NH4+ and F- 
E) HF and NH4+

Question 5

The indicator phenol red changes from yellow to red between pH 6.8 and pH 8.4. If phenol red is added to a solution, and the solution turns red, then

Accepted Answer

A) the solution is basic, and the pH must be at or below 7.0. 
B) the pH of the solution must be below 6.8, and the solution is basic. 
C) the pH of the solution must be below 6.8, and the solution is acidic. 
D) the pH of the solution must be above 8.4, and the solution is basic. 
E) the pH of the solution is above 8.4, and the solution is acidic. 
A) the solution is basic, and the pH must be at or below 7.0. 
B) the pH of the solution must be below 6.8, and the solution is basic. 
C) the pH of the solution must be below 6.8, and the solution is acidic. 
D) the pH of the solution must be above 8.4, and the solution is basic. 
E) the pH of the solution is above 8.4, and the solution is acidic.

Question 6

A solution of a strong acid will have a greater H3O+ concentration than a solution of a weak acid under any circumstances.

Accepted Answer

A) True 
 B)False

Question 7

Which of the following equations represents the behavior of H2PO4- as a base?

Accepted Answer

A) H2PO4-(aq)+ H3O+(aq)⇌ H3PO4(aq)+ H2O(l) 
B) H2PO4-(aq)+ F-(aq)⇌ HPO42-(aq)+ HF(aq) 
C) H2PO4-(aq)+ CN-(aq)⇌ HPO42-(aq)+ HCN(aq) 
D) H2PO4-(aq)+ OH-(aq)⇌ HPO42-(aq)+ H2O(l) 
E) H2PO4-(aq)+ H2O(l)⇌ H3PO4(aq)+ H3O+(aq) 
A) H2PO4-(aq)+ H3O+(aq)⇌ H3PO4(aq)+ H2O(l) 
B) H2PO4-(aq)+ F-(aq)⇌ HPO42-(aq)+ HF(aq) 
C) H2PO4-(aq)+ CN-(aq)⇌ HPO42-(aq)+ HCN(aq) 
D) H2PO4-(aq)+ OH-(aq)⇌ HPO42-(aq)+ H2O(l) 
E) H2PO4-(aq)+ H2O(l)⇌ H3PO4(aq)+ H3O+(aq)

Question 8

Select the strong acid from the following list.

Accepted Answer

A) H3PO4(aq) 
B) CH3CO2H(aq) 
C) H2S(aq) 
D) H2SO4(aq) 
E) HF(aq) 
A) H3PO4(aq) 
B) CH3CO2H(aq) 
C) H2S(aq) 
D) H2SO4(aq) 
E) HF(aq)

Question 9

Calculate the pH of a solution that has [H3O+] = 3.1 × 10-8 M.

Accepted Answer

A) pH = 7.51 
B) pH = 8.00 
C) pH = 3.10 
D) pH = 3.18 
E) pH = 6.49 
A) pH = 7.51 
B) pH = 8.00 
C) pH = 3.10 
D) pH = 3.18 
E) pH = 6.49

Question 10

When sodium hydroxide, NaOH, is dissolved in water, which species are present in addition to water?

Accepted Answer

A) NaOH(aq) 
B) Na+(aq)and OH−(aq) 
C) Na+(aq)and H3O−(aq) 
D) Na+(aq)and O2H22−(aq) 
E) NaO−(aq)and H3O+(aq) 
A) NaOH(aq) 
B) Na+(aq)and OH−(aq) 
C) Na+(aq)and H3O−(aq) 
D) Na+(aq)and O2H22−(aq) 
E) NaO−(aq)and H3O+(aq)

Question 11

If the pOH of a borax solution is 4.55, what is the H3O+ concentration in the borax solution?

Accepted Answer

A) 4.6 M 
B) 3.5 × 10-9 M 
C) 3.5 × 10-10 M 
D) 3.5 × 10-11 M 
E) 9.4 M 
A) 4.6 M 
B) 3.5 × 10-9 M 
C) 3.5 × 10-10 M 
D) 3.5 × 10-11 M 
E) 9.4 M

Question 12

Calculate the pH of a solution that has [OH-] = 1.0 × 10-6 M.

Accepted Answer

A) pH = 1.00 
B) pH = 7.00 
C) pH = 6.00 
D) pH = 8.00 
E) pH = 14.00 
A) pH = 1.00 
B) pH = 7.00 
C) pH = 6.00 
D) pH = 8.00 
E) pH = 14.00

Question 13

The indicator phenolphthalein changes from colorless to pink between pH 8.2 and pH 10. If phenolphthalein is added to a solution, and the solution remains colorless, then

Accepted Answer

A) the solution is acidic, and the pH must be at or below 7.0. 
B) the pH of the solution must be below 8.2, and the solution is basic. 
C) the pH of the solution must be below 8.2, but the solution could be either acidic or basic. 
D) the pH of the solution must be above 10, and the solution is basic. 
E) the pH of the solution is above 10, and the solution is acidic. 
A) the solution is acidic, and the pH must be at or below 7.0. 
B) the pH of the solution must be below 8.2, and the solution is basic. 
C) the pH of the solution must be below 8.2, but the solution could be either acidic or basic. 
D) the pH of the solution must be above 10, and the solution is basic. 
E) the pH of the solution is above 10, and the solution is acidic.

Question 14

What is the pH of a 0.015 M NaOH solution?

Accepted Answer

A) 0.015 
B) 1.82 
C) 7.00 
D) 12.18 
E) −1.82 
A) 0.015 
B) 1.82 
C) 7.00 
D) 12.18 
E) −1.82

Question 15

Which of the following bases is not commonly found in household products or antacids?

Accepted Answer

A) sodium hydroxide, NaOH 
B) ammonia, NH3 
C) calcium carbonate, CaCO3 
D) magnesium hydroxide, Mg(OH)2 
E) methyl amine, CH3NH2 
A) sodium hydroxide, NaOH 
B) ammonia, NH3 
C) calcium carbonate, CaCO3 
D) magnesium hydroxide, Mg(OH)2 
E) methyl amine, CH3NH2

Question 16

Select the solution below that is the most basic.

Accepted Answer

A) [H3O+] = 1.0 × 10-4 M 
B) [H3O+] = 1.0 × 10-6 M 
C) [H3O+] = 1.0 × 10-7 M 
D) [H3O+] = 1.0 × 10-8 M 
E) [H3O+] = 1.0 × 10-10 M 
A) [H3O+] = 1.0 × 10-4 M 
B) [H3O+] = 1.0 × 10-6 M 
C) [H3O+] = 1.0 × 10-7 M 
D) [H3O+] = 1.0 × 10-8 M 
E) [H3O+] = 1.0 × 10-10 M

Question 17

List the acid, base, conjugate acid, and conjugate base, in that order, for the following reaction: HOCl(aq)+ H2O(l)⇌ OCl−(aq)+ H3O+(aq)

Accepted Answer

A) HOCl, H2O, OCl−, H3O+ 
B) H2O, HOCl, OCl−, H3O+ 
C) HOCl, H2O, H3O+, OCl− 
D) H2O, HOCl, H3O+, OCl− 
E) OCl−, H3O+, H2O, HOCl 
A) HOCl, H2O, OCl−, H3O+ 
B) H2O, HOCl, OCl−, H3O+ 
C) HOCl, H2O, H3O+, OCl− 
D) H2O, HOCl, H3O+, OCl− 
E) OCl−, H3O+, H2O, HOCl

Question 18

Calculate the pOH of a solution that has [OH-] = 5.9 × 10-5 M.

Accepted Answer

A) pOH = 5.90 
B) pOH = 5.00 
C) pOH = 4.23 
D) pOH = 5.59 
E) pOH = 9.77 
A) pOH = 5.90 
B) pOH = 5.00 
C) pOH = 4.23 
D) pOH = 5.59 
E) pOH = 9.77

Question 19

Which of the following ions is amphoteric?

Accepted Answer

A) Cl− 
B) OH− 
C) H+ 
D) NO3- 
E) HCO3- 
A) Cl− 
B) OH− 
C) H+ 
D) NO3- 
E) HCO3-

Question 20

Select the two Brønsted-Lowry acids in the following equation: HF(aq)+ H2O(l)⇌ F−(aq)+ H3O+(aq)

Accepted Answer

A) HF and H2O 
B) HF and F− 
C) H2O and F− 
D) HF and H3O+ 
E) H3O+ and F− 
A) HF and H2O 
B) HF and F− 
C) H2O and F− 
D) HF and H3O+ 
E) H3O+ and F−

Which of the following is the strongest acid?

Calculate the pOH of a solution that has [H₃O⁺] = 3.1 × 10^-8 M.

Identify gastric juice, pH = 1.0, as acidic, basic, or neutral.

Select the two Brønsted-Lowry acids in the following equation: NH₃(aq)+ HF(aq)⇌ NH₄⁺(aq)+ F⁻(aq)

The indicator phenol red changes from yellow to red between pH 6.8 and pH 8.4. If phenol red is added to a solution, and the solution turns red, then

A solution of a strong acid will have a greater H₃O⁺ concentration than a solution of a weak acid under any circumstances.

Which of the following equations represents the behavior of H₂PO₄^- as a base?

Select the strong acid from the following list.

Calculate the pH of a solution that has [H₃O⁺] = 3.1 × 10^-8 M.

When sodium hydroxide, NaOH, is dissolved in water, which species are present in addition to water?

If the pOH of a borax solution is 4.55, what is the H₃O⁺ concentration in the borax solution?

Calculate the pH of a solution that has [OH^-] = 1.0 × 10^-6 M.

The indicator phenolphthalein changes from colorless to pink between pH 8.2 and pH 10. If phenolphthalein is added to a solution, and the solution remains colorless, then

What is the pH of a 0.015 M NaOH solution?

Which of the following bases is not commonly found in household products or antacids?

Select the solution below that is the most basic.

List the acid, base, conjugate acid, and conjugate base, in that order, for the following reaction: HOCl(aq)+ H₂O(l)⇌ OCl⁻(aq)+ H₃O⁺(aq)

Calculate the pOH of a solution that has [OH^-] = 5.9 × 10^-5 M.

Which of the following ions is amphoteric?

Select the two Brønsted-Lowry acids in the following equation: HF(aq)+ H₂O(l)⇌ F⁻(aq)+ H₃O⁺(aq)

Matter and Energy

Atoms, Ions, and the Periodic Table

Chemical Compounds

Chemical Composition

Chemical Reactions and Equations

Quantities in Chemical Reactions

Electron Structure of the Atom

Chemical Bonding

The Gaseous State

The Liquid and Solid States

Solutions

Reaction Rates and Chemical Equilibrium

Oxidation-Reduction Reactions

Nuclear Chemistry

Organic Chemistry

Biochemistry

Filters

Exam 13: Acids and Bases

Which of the following is the strongest acid?

Calculate the pOH of a solution that has [H3O+] = 3.1 × 10-8 M.

Identify gastric juice, pH = 1.0, as acidic, basic, or neutral.

Select the two Brønsted-Lowry acids in the following equation: NH3(aq)+ HF(aq)⇌ NH4+(aq)+ F−(aq)

The indicator phenol red changes from yellow to red between pH 6.8 and pH 8.4. If phenol red is added to a solution, and the solution turns red, then

A solution of a strong acid will have a greater H3O+ concentration than a solution of a weak acid under any circumstances.

Which of the following equations represents the behavior of H2PO4- as a base?

Select the strong acid from the following list.

Calculate the pH of a solution that has [H3O+] = 3.1 × 10-8 M.

When sodium hydroxide, NaOH, is dissolved in water, which species are present in addition to water?

If the pOH of a borax solution is 4.55, what is the H3O+ concentration in the borax solution?

Calculate the pH of a solution that has [OH-] = 1.0 × 10-6 M.

The indicator phenolphthalein changes from colorless to pink between pH 8.2 and pH 10. If phenolphthalein is added to a solution, and the solution remains colorless, then

What is the pH of a 0.015 M NaOH solution?

Which of the following bases is not commonly found in household products or antacids?

Select the solution below that is the most basic.

List the acid, base, conjugate acid, and conjugate base, in that order, for the following reaction: HOCl(aq)+ H2O(l)⇌ OCl−(aq)+ H3O+(aq)

Calculate the pOH of a solution that has [OH-] = 5.9 × 10-5 M.

Which of the following ions is amphoteric?

Select the two Brønsted-Lowry acids in the following equation: HF(aq)+ H2O(l)⇌ F−(aq)+ H3O+(aq)

Matter and Energy

Atoms, Ions, and the Periodic Table

Chemical Compounds

Chemical Composition

Chemical Reactions and Equations

Quantities in Chemical Reactions

Electron Structure of the Atom

Chemical Bonding

The Gaseous State

The Liquid and Solid States

Solutions

Reaction Rates and Chemical Equilibrium

Oxidation-Reduction Reactions

Nuclear Chemistry

Organic Chemistry

Biochemistry

Filters

Calculate the pOH of a solution that has [H₃O⁺] = 3.1 × 10^-8 M.

Select the two Brønsted-Lowry acids in the following equation: NH₃(aq)+ HF(aq)⇌ NH₄⁺(aq)+ F⁻(aq)

A solution of a strong acid will have a greater H₃O⁺ concentration than a solution of a weak acid under any circumstances.

Which of the following equations represents the behavior of H₂PO₄^- as a base?

Calculate the pH of a solution that has [H₃O⁺] = 3.1 × 10^-8 M.

If the pOH of a borax solution is 4.55, what is the H₃O⁺ concentration in the borax solution?

Calculate the pH of a solution that has [OH^-] = 1.0 × 10^-6 M.

List the acid, base, conjugate acid, and conjugate base, in that order, for the following reaction: HOCl(aq)+ H₂O(l)⇌ OCl⁻(aq)+ H₃O⁺(aq)

Calculate the pOH of a solution that has [OH^-] = 5.9 × 10^-5 M.

Select the two Brønsted-Lowry acids in the following equation: HF(aq)+ H₂O(l)⇌ F⁻(aq)+ H₃O⁺(aq)