Question 1

What is the pOH of an aqueous solution having a hydrogen-ion concentration of 6.83 × 10-3 mol/L?

Accepted Answer

A)   16.17
B)   11.83
C)   2.17
D)   1.03E) None of the above
F) A) and B)

Question 2

Which of the following compounds could be considered an Arrhenius base?

Accepted Answer

A)   HCl
B)   CH3COOH
C)   KOH
D)   HFE) B) and C)
F) C) and D)

Question 3

A sodium sulfate solution will not conduct an electric current.

Accepted Answer

A) True 
 B)False

Question 4

Which of the following bases produces two OH- ions per formula unit of base when dissolved in water?

Accepted Answer

A)   potassium hydroxide
B)   calcium hydroxide
C)   aluminum hydroxide
D)   ammoniaE) B) and C)
F) None of the above

Question 5

Identify each of the acids as a strong acid or a weak acid.
-acetic acid

Accepted Answer

A)  weak acid
B)  strong acidC) A) and B)
D) undefined

Question 6

Which of the following solutions would you expect not to conduct electricity?

Accepted Answer

A)   NaCl in water
B)   CO in water
C)   HCl in water
D)   H2SO4 in waterE) A) and B)
F) A) and C)

Question 7

Identify each [H?O+] / [OH-] / pH / pOH  as acidic or basic.
-pH = 10.24

Accepted Answer

A)  Basic
B)  AcidicC) A) and B)
D) undefined

Question 8

What is the hydrogen-ion concentration of an aqueous solution having a pH of 4.72?

Accepted Answer

A)   4.72 × 10-5 mol/L
B)   4.72 mol/L
C)   0.67 mol/L
D)   1.91 × 10-5 mol/LE) None of the above
F) B) and C)

Question 9

Which of the following compounds does not qualify as a Bronsted-Lowry acid?

Accepted Answer

A)   HF
B)   H₂CO₃
C)   H₂
D)   H₂OE) B) and C)
F) A) and B)

Question 10

An electrolyte is a substance that, when dissolved in water, yields a solution that conducts electric current.

Accepted Answer

A) True 
 B)False

Question 11

Identify the household products as acidic or basic.
-Household ammonia

Accepted Answer

A)  Acidic
B)  BasicC) A) and B)
D) undefined

Question 12

Arrhenius' definition of a base is an electrolyte that contains a metal and hydroxide ions that dissociate when placed in water.

Accepted Answer

A) True 
 B)False

Question 13

The acid in the forward reaction is ________. HCO₃- + H₂O → H₂CO₃ + OH-

Accepted Answer

A)   HCO₃-
B)   H₂O
C)   H₂CO₃
D)   OH-E) B) and C)
F) C) and D)

Question 14

Water can serve both as a Bronsted-Lowry acid and Bronsted-Lowry base.

Accepted Answer

A) True 
 B)False

Question 15

Match each of the acids with the maximum number of H?O+ produced per molecule of acid.
-hydrochloric acid

Accepted Answer

A)  3
B)  1
C)  2D) A) and B)
E) All of the above

Question 16

Which of the following compounds is a non-electrolyte when dissolved in distilled water?

Accepted Answer

A)   sodium chloride
B)   hydrochloric acid
C)   sodium hydroxide
D)   ethyl alcoholE) A) and B)
F) A) and C)

Question 17

Identify each of the acids as a strong acid or a weak acid.
-hydrobromic acid

Accepted Answer

A)  weak acid
B)  strong acidC) A) and B)
D) undefined

Question 18

Identify each of the substances as an electrolyte or non-electrolyte.
-aqueous sulfuric acid solution

Accepted Answer

A)  non-electrolyte
B)  electrolyteC) A) and B)
D) undefined

Question 19

When ammonia is dissolved in water, the ionized species are ________.

Accepted Answer

A)   NH₄+ and OH-
B)   NH₂- and H+
C)   NH₄+ and H-
D)   NH₂+ and H-E) None of the above
F) B) and D)

Question 20

Identify each [H?O+] / [OH-] / pH / pOH  as acidic or basic.
-[OH-] = 1.2 × 10-8

Accepted Answer

A)  Basic
B)  AcidicC) A) and B)
D) undefined

Exam 15: Electrolytes, Acids, and Bases

Which of the following compounds does not qualify as a Bronsted-Lowry acid?

Correct AnswerverifiedShow Answer

Which of the following compounds is a non-electrolyte when dissolved in distilled water?

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What is the pOH of an aqueous solution having a hydrogen-ion concentration of 6.83 × 10-3 mol/L?

Correct AnswerverifiedShow Answer

Identify each [H?O+] / [OH-] / pH / pOH as acidic or basic. -pH = 10.24

Correct AnswerverifiedShow Answer

Identify each of the substances as an electrolyte or non-electrolyte. -aqueous sulfuric acid solution

Correct AnswerverifiedShow Answer

Which of the following solutions would you expect not to conduct electricity?

Correct AnswerverifiedShow Answer

Water can serve both as a Bronsted-Lowry acid and Bronsted-Lowry base.

Correct AnswerverifiedShow Answer

The acid in the forward reaction is ________. HCO₃- + H₂O → H₂CO₃ + OH-

Correct AnswerverifiedShow Answer

Identify each of the acids as a strong acid or a weak acid. -acetic acid

Correct AnswerverifiedShow Answer

What is the hydrogen-ion concentration of an aqueous solution having a pH of 4.72?

Correct AnswerverifiedShow Answer

Match each of the acids with the maximum number of H?O+ produced per molecule of acid. -hydrochloric acid

Correct AnswerverifiedShow Answer

Arrhenius' definition of a base is an electrolyte that contains a metal and hydroxide ions that dissociate when placed in water.

Correct AnswerverifiedShow Answer

Identify each of the acids as a strong acid or a weak acid. -hydrobromic acid

Correct AnswerverifiedShow Answer

When ammonia is dissolved in water, the ionized species are ________.

Correct AnswerverifiedShow Answer

Which of the following bases produces two OH- ions per formula unit of base when dissolved in water?

Correct AnswerverifiedShow Answer

A sodium sulfate solution will not conduct an electric current.

Correct AnswerverifiedShow Answer

Identify the household products as acidic or basic. -Household ammonia

Correct AnswerverifiedShow Answer

Identify each [H?O+] / [OH-] / pH / pOH as acidic or basic. -[OH-] = 1.2 × 10-8

Correct AnswerverifiedShow Answer

An electrolyte is a substance that, when dissolved in water, yields a solution that conducts electric current.

Correct AnswerverifiedShow Answer

Which of the following compounds could be considered an Arrhenius base?

Correct AnswerverifiedShow Answer

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What is the pOH of an aqueous solution having a hydrogen-ion concentration of 6.83 × 10^-3 mol/L?

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Identify each [H?O+] / [OH-] / pH / pOH as acidic or basic. -[OH-] = 1.2 × 10^-8

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