Deck 15: Electrolytes, Acids, and Bases

Question 1

Which of the following acids does not produce two H₃O+ ion per molecule of acid when dissociated in water?

A) hydriodic acid
B) sulfurous acid
C) sulfuric acid
D) carbonic acid

Answer 1

hydriodic acid

Question 2

The compound HA is an acid that is soluble in water. Which of the "beakers" below shows HA behaving as a strong acid in water?

A)
B)
C)
D)

Answer 2

Question 3

Which of the following compounds is not a weak electrolyte when dissolved in distilled water?

A) ammonia
B) acetic acid (vinegar)
C) potassium chloride
D) hydrogen fluoride

Answer 3

potassium chloride

Question 4

Which of the following acids produces more than one H₃O+ ion per molecule of acid when dissociated in water?

A) hydrobromic acid
B) carbonic acid
C) hypochlorous acid
D) acetic acid

Question 5

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

A) sodium chloride
B) hydrochloric acid
C) sodium hydroxide
D) ethyl alcohol

Question 6

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

A) sodium chloride
B) sucrose
C) acetone (nail polish remover)
D) ethyl alcohol

Question 7

Which of the following acids can produce only one H₃O+ ion per molecule of acid when dissolved in water, although itself has other non-ionizable hydrogens?

A) hydrobromic acid
B) sulfurous acid
C) hypochlorous acid
D) acetic acid

Question 8

The compound HA is an acid that is soluble in water. Which of the "beakers" below shows HA behaving as a weak acid in water?

A)
B)
C)
D) Both A and C are weak acids in water.

Question 9

Which of the following acids is a strong acid?

A) acetic acid
B) hydrofluoric acid
C) phosphoric acid
D) hydrochloric acid

Question 10

Which of the following acids is the strongest acid?

A) acetic acid, Ka = 1.8 × 10^-5
B) nitrous acid, Ka = 4.5 × 10^-4
C) hydrogen peroxide, Ka = 2.4 × 10^-12
D) hypochlorous acid, Ka = 3.5 × 10^-8

Question 11

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

A) NaCl in water
B) CO in water
C) HCl in water
D) H₂SO₄ in water

Question 12

Which of the following compounds is an electrolyte when dissolved in distilled water?

A) ethyl alcohol
B) sucrose
C) sodium sulfate
D) oxygen

Question 13

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

A) phosphoric acid
B) nitric acid
C) potassium chloride
D) glucose

Question 14

Why is HF in water considered a weakly acidic solution, while HCl and HBr in water are considered strongly acidic solutions?

A) HF does not dissolve in water.
B) HF only partially dissociates into ions in water.
C) HF has a weak conjugate base, .
D) Both B and C are correct.

Question 15

What are the ions formed in glucose, C₆H₁₂O₆?

A) C₆H₁₁O₆- + H+
B) C₆H₁₁O₅₊ + OH-
C) CO₂ + H₂O
D) No ions are formed.

Question 16

Which of the following acids does not produce more than one H₃O+ ion per molecule of acid when dissociated in water?

A) carbonic acid
B) sulfurous acid
C) phosphoric acid
D) acetic acid

Question 17

Which of the following acids is a diprotic acid when dissolved in water?

A) hydrobromic acid
B) sulfuric acid
C) hypochlorous acid
D) phosphoric acid

Question 18

Which of the following compounds is not a strong electrolyte when dissolved in distilled water?

A) potassium chloride
B) sulfuric acid
C) acetic acid
D) potassium hydroxide

Question 19

Which of the following acids is a weak acid?

A) sulfuric acid
B) hydrochloric acid
C) nitric acid
D) carbonic acid

Question 20

Which of the following acids is a triprotic acid when dissolved in water?

A) hydrobromic acid
B) sulfuric acid
C) hypochlorous acid
D) phosphoric acid

Question 21

Which of the following bases is a strong base?

A) potassium hydroxide
B) ammonium hydroxide
C) aluminum hydroxide
D) fluoride ion

Question 22

Which of the following compounds is the weakest acid?

A) acetic acid, Ka = 1.8 × 10^-5
B) nitrous acid, Ka = 4.5 × 10^-4
C) hydrogen peroxide, Ka = 2.4 × 10^-12
D) hypochlorous acid, Ka = 3.5 × 10^-8

Question 23

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

A) potassium hydroxide
B) calcium hydroxide
C) aluminum hydroxide
D) ammonia

Question 24

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

A) NH₄+ and OH-
B) NH₂- and H+
C) NH₄+ and H-
D) NH₂+ and H-

Question 25

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

A) H₃O+ and OH-
B) H₂F- and H₃O+
C) H₃O+ and F-
D) H₂F+ and OH-

Question 26

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

A) HCl
B) CH₃COOH
C) KOH
D) HF

Question 27

Basic solutions ________.

A) have a higher concentration of hydronium ions than hydroxide ions
B) have a lower concentration of hydronium ions than hydroxide ions
C) turn blue litmus paper to pink
D) decolorize phenolphthalein solutions

Question 28

Which of the following compounds qualifies as a Bronsted-Lowry base?

A) CH₄
B) NH₃
C) SiH₄
D) H₂

Question 29

Which of the following bases is the weakest base?

A) ammonia, Kb = 1.7 × 10^-5
B) aniline, Kb = 4.2 × 10^-10
C) trimethylamine, Kb = 7.4 × 10^-5
D) methylamine, Kb = 4.4 × 10^-4

Question 30

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

A) CH₄
B) NH₃
C) PH₃
D) H₂O

Question 31

Which of the following bases is the strongest base?

A) ammonia, Kb = 1.7 × 10^-5
B) aniline, Kb = 4.2 × 10^-10
C) trimethylamine, Kb = 7.4 × 10^-5
D) methylamine, Kb = 4.4 × 10^-4

Question 32

Which of the following bases produces only one OH- ion per molecule of formula unit when dissolved in water?

A) potassium hydroxide
B) calcium hydroxide
C) aluminum hydroxide
D) barium hydroxide

Question 33

The base in the forward reaction is ________. NH₃ + H₂O → NH₄₊ + OH-

A) NH₄₊
B) H₂O
C) NH₃
D) OH-

Question 34

Which of the following bases is a weak base?

A) sodium hydroxide
B) ammonium hydroxide
C) lithium hydroxide
D) potassium hydroxide

Question 35

Which of the following acids could be considered an Arrhenius acid?

A) HCl
B) CH₃COOH
C) NH₄₊
D) All of the above are Arrhenius acids.

Question 36

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

A) HCO₃-
B) H₂O
C) H₂CO₃
D) OH-

Question 37

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

A) HF
B) H₂CO₃
C) H₂
D) H₂O

Question 38

Acidic solutions ________.

A) have a higher concentration of hydronium ions than hydroxide ions
B) have a lower concentration of hydronium ions than hydroxide ions
C) turn red litmus paper to blue
D) colorize phenolphthalein solutions

Question 39

Which of the following compounds or ions qualifies as a Bronsted-Lowry acid?

A) KOH
B) NH₃
C) Na⁺
D) NH₄+

Question 40

Which of the following compounds can behave both as a Bronsted-Lowry acid and a Bronsted-Lowry base?

A) CH₄
B) H₂O
C) SiH₄
D) H₂

Question 41

The conjugate acid of H₂PO₄- is ________.

A) H₃PO₄
B) HPO₄2-
C) PO₄-
D) H₄PO₄+

Question 42

The pH of an aqueous solution is 9.35. What is the pOH? (pH + pOH = 14 for aqueous acid/base systems).

A) 4.65
B) 0.971
C) -4.65
D) 0.668

Question 43

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

A) 4.72 × 10^-5 mol/L
B) 1.91 × 10^-14 mol/L
C) 5.25 × 10^-10 mol/L
D) 1.91 × 10^-5 mol/L

Question 44

The pH of natural rainwater is close to ________.

A) 5.6
B) 6.3
C) 7.0
D) 8.2

Question 45

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

A) 16.17
B) 11.83
C) 2.17
D) 1.03

Question 46

What is the hydroxide-ion concentration of an aqueous solution having a hydrogen-ion concentration of 4.75 × 10^-5 mol/L?

A) 2.10 × 10^-10 mol/L
B) 5.25 × 10^-10 mol/L
C) 4.75 × 10^-5 mol/L
D) -4.75 × 10^-5 mol/L

Question 47

Stomach juices have a pH close to ________.

A) 1.5
B) 2.8
C) 4.5
D) 7.0

Question 48

The pH of diabetic patients can be as low as ________.

A) 3.2
B) 5.8
C) 6.8
D) 7.0

Question 49

The pH of blood is approximately ________.

A) 5.2
B) 7.0
C) 7.4
D) 9.1

Question 50

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

A) 6.83
B) 0.83
C) 2.17
D) 1.03

Question 51

A change in pH from 10 to 7 ________.

A) increases the acidity 1000×
B) reduces the acidity 3000×
C) increases the acidity 3×
D) increases the acidity 3000×

Question 52

The conjugate base of H₂PO₄- is ________.

A) H₃PO₄
B) HPO₄2-
C) PO₄-
D) H₄PO₄+

Question 53

The conjugate base of HCO₃- is ________.

A) H₂CO₃
B) CO₃2-
C) CO₂2-
D) H₃CO₃+

Question 54

A drop of a full unit in the pH scale ________.

A) reduces the acidity 10×
B) increases the acidity 10×
C) reduces the acidity 2×
D) increases the acidity 2×

Question 55

Which solution is the most basic solution?

A) a solution whose [H+] = 10⁰
B) a solution whose [OH-] = 10^-14
C) a solution whose pH = 0
D) All of the above have the same degree of basicity.

Question 56

The conjugate acid of HCO₃- is ________.

A) H₂CO₃
B) CO₃2-
C) CO₂2-
D) H₃CO₃-

Question 57

Which substance is the most basic?

A) blood
B) milk
C) household ammonia
D) milk of magnesia

Question 58

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

A) 4.72 × 10^-5 mol/L
B) 4.72 mol/L
C) 0.67 mol/L
D) 1.91 × 10^-5 mol/L

Question 59

Which substance is the most acidic?

A) coffee
B) milk
C) oven cleaner
D) baking soda

Question 60

Which solution is the most acidic solution?

A) a solution whose [H+] = 10^-1
B) a solution whose [OH-] = 10^-10
C) a solution whose pH = 0
D) All of the above have the same degree of acidity.

Question 61

A sodium hydroxide solution is a non-electrolyte.

Question 62

A sodium sulfate solution will not conduct an electric current.

Question 63

A concentrated solution of a non-electrolyte such as glucose can be made to conduct electricity.

Question 64

Sucrose (table sugar) is a strong electrolyte.

Question 65

CH₃CO₂H has four acidic hydrogens.

Question 66

Sodium chloride (NaCl) is considered an electrolyte because it dissolves in water into positive and negative ions.

Question 67

Sulfuric acid is a diprotic acid.

Question 68

The compound HCl is considered a Bronsted-Lowry base because it increases the concentration of when it dissociates in water.

Question 69

A baking soda solution is a strong electrolyte.

Question 70

An aqueous solution of HCl is called hydrochloric acid.

Question 71

Deionized water can conduct electricity.

Question 72

Acetic acid is a diprotic acid.

Question 73

Carbonic acid, phosphoric acid, and sulfuric acid can produce two H₃O+ ions per molecule of acid when dissolved in water.

Question 74

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

Question 75

The conjugate base of ammonia is ________.

A) NH₂-
B) NH-
C) N3-
D) NH₄+

Question 76

Solid sodium chloride is a strong electrolyte.

Question 77

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

Question 78

Which of the following conjugate pairs would form a good buffer?

A) HCl/
B) / O
C) / +
D) / -

Question 79

Hydrochloric, hypochlorous and hydrobromic acids produce only one H₃O+ ion per molecule of acid when dissolved in water.

Question 80

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