Deck 12: Acids and Bases

Question 1

Identify the major ions present in an aqueous LiOH solution.

A)Li²⁺, O⁻, H⁻
B)Li⁺, OH⁻
C)LiO⁻, H⁺
D)Li⁺, O²⁻, H⁺
E)Li⁻, OH⁺

Answer 1

Li⁺, OH⁻

Question 2

What is the name of a proton donor in an acid-base reaction?

A)Arrhenius acid
B)Arrhenius base
C)Brønsted acid
D)Brønsted base
E)Lewis base

Answer 2

Brønsted acid

Question 3

The substance (CH₃CH₂)₂NH is considered to be

A)a weak acid.
B)a weak base.
C)a strong acid.
D)a strong base.
E)neither acidic nor basic.

Answer 3

a weak base.

Question 4

Which is the strongest acid?

A)HBrO₄
B)HBr
C)HBrO₂
D)HBrO
E)HBrO₃

Question 5

Which is a strong base?

A)LiOH
B)CH₃COOH
C)NH₃
D)H₃PO₄
E)HClO₂

Question 6

Which is a strong acid?

A)Ba(OH)₂
B)H₃PO₄
C)HC₂H₃O₂
D)NaCl
E)HClO₄

Question 7

The substance HClO₄ is considered to be

A)a weak acid.
B)a weak base.
C)a strong acid.
D)a strong base.
E)neither acidic nor basic.

Question 8

Which is present in all aqueous Brønsted acid solutions?

A)H₂
B)H⁺
C)OH^-
D)H₂SO₄
E)Cl^-

Question 9

Which is a weak base?

A)NH₃
B)Ca(OH)₂
C)Ba(OH)₂
D)NaOH
E)CH₃COOH

Question 10

Which one of the following is a strong acid?

A)H₂CO₃
B)H₂SO₃
C)H₂SO₄
D)H₃PO₄
E)CH₃COOH

Question 11

Which of the following is a strong base?

A)NH₃
B)Ca(OH)₂
C)Al(OH)₃
D)B(OH)₃
E)CH₃OH

Question 12

Which is the strongest acid?

A)SO₄²⁻
B)H₂SO₃
C)H₂SO₄
D)HSO₄⁻
E)HSO₃⁻

Question 13

Which of the following is a weak acid?

A)H₂SO₄
B)HNO₃
C)HF
D)HBr
E)HCl

Question 14

Identify the major ions present in an aqueous HNO₃ solution.

A)HN²⁺, O²⁻
B)OH⁻, NO₃⁻
C)OH⁻, NO⁺
D)H⁺, N³⁻, O²⁻
E)H⁺, NO₃⁻

Question 15

The substance NH₃ is considered to be

A)a weak acid.
B)a weak base.
C)a strong acid.
D)a strong base.
E)neither acidic nor basic.

Question 16

Which of the following is a strong acid?

A)H₃PO₄
B)HNO₃
C)HF
D)CH₃COOH
E)H₂O

Question 17

Which is the strongest acid?

A)HBrO₃
B)HClO
C)HBrO₂
D)HBrO
E)HClO₃

Question 18

Which one of the following is a strong acid?

A)CH₃COOH
B)H₂SO₃
C)NH₃
D)H₃PO₄
E)HClO₃

Question 19

Complete the following reaction and identify the Brønsted acid.NaOH(aq) + HCl(aq) →

A)NaH(aq) + HOCl(aq); NaOH is the acid.
B)NaH(aq) + HOCl(aq); HCl is the acid.
C)NaCl(aq) + H₂O(l); NaOH is the acid.
D)NaCl(aq) + H₂O(l); HCl is the acid.
E)NaCl(aq) + H₂O(l); NaCl is the acid.

Question 20

What is the name of a proton acceptor in an acid-base reaction?

A)Arrhenius acid
B)Arrhenius base
C)Brønsted acid
D)Brønsted base
E)Lewis base

Question 21

Which is the net ionic equation for the reaction between aqueous solutions of lithium hydroxide and hydrobromic acid? LiOH(aq) + HBr(aq) → H₂O(l) + LiBr(aq)

A)LiOH(aq) → Li⁺(aq) + OH⁻(aq)
B)HBr(aq) → H⁺(aq) + Br⁻(aq)
C)H⁺(aq) + OH⁻(aq) → H₂O(l)
D)Li⁺(aq) + Br⁻(aq) → LiBr(aq)
E)Li⁺(aq) + OH⁻(aq)+ H⁺(aq) + Br⁻(aq) → H₂O(l) + LiBr(aq)

Question 22

Which solution is the most acidic?

A)3 × 10⁻⁴ M H⁺
B)5 × 10⁻⁵ M H⁺
C)6 × 10⁻³ M H⁺
D)1 × 10⁻⁶ M H⁺
E)5 × 10⁻² M H⁺

Question 23

What is the conjugate base of sulfuric acid?

A)HSO₄⁻
B)H₃O⁺
C)OH⁻
D)SO₄²⁻
E)H₃SO₄⁺

Question 24

Which solution is the most acidic?

A)pH = 1.00
B)pH = 10.00
C)pH = 5.00
D)pH = 3.00
E)pH = 4.00

Question 25

What is [OH⁻] for a solution at 25°C that has [H₃O⁺] = 2.35 × 10⁻³ M?

A)4.26 × 10⁻⁵ M
B)2.35 ×10⁻¹¹ M
C)4.26 × 10⁻¹² M
D)2.35 × 10⁻¹⁷ M
E)2.35 ×10⁻³ M

Question 26

What is the concentration of H⁺ in a 0.025 M HCl solution?

A)0
B)0.013 M
C)0.025 M
D)0.050 M
E)0.010 M

Question 27

What is the conjugate base of NH₃?

A)NH₂
B)NH₂⁺
C)NH₂⁻
D)NH₄
E)NH₄⁺

Question 28

What is the concentration of OH⁻ in a 0.083 M NaOH solution?

A)0.083 M
B)1.21 × 10⁻¹³ M
C)8.30 × 10⁻¹⁶ M
D)7 M
E)8.30 × 10¹² M

Question 29

Which solution is the most acidic?

A)1 × 10⁻⁴ M H⁺
B)1 × 10⁻⁹ M H⁺
C)1 × 10⁻³ M H⁺
D)1 × 10⁻⁷ M H⁺
E)1 × 10⁻¹⁰ M H⁺

Question 30

What is the name given to a substance that can act as a Brønsted acid or as a Brønsted base according to what it is reacting with?

A)hydrophilic
B)hydrophobic
C)amphoteric
D)isoprotic
E)isoelectronic

Question 31

A solution with a pH of 8.15 is

A)slightly acidic.
B)very basic.
C)neutral.
D)very acidic.
E)slightly basic.

Question 32

Complete the following reaction and identify the Brønsted base: NaOH(aq) + HCl(aq) →

A)Na(aq) + HOCl(aq); NaOH is the base.
B)NaCl(aq) + OH⁻(aq); HCl is the base.
C)NaCl(aq) + OH⁻(aq); NaOH is the base.
D)H₂O(l) + NaCl(aq); HCl is the base.
E)NaCl(aq)+ H₂O(l); NaOH is the base.

Question 33

What is the conjugate base of water?

A)H₃O⁺
B)OH⁻
C)H₃O
D)OH
E)H₂O₂

Question 34

What is the pH of a 0.056 M HNO₃ solution?

A)0.056
B)1.25
C)12.75
D)2.88
E)11.11

Question 35

Which one of these responses is with regard to a 0.1 M solution of a weak acid HA?

A)[H⁺] > 0.1 M.
B)pH = 1.0
C)[H⁺] < [A^-]
D)pH > 1.0
E)[OH^-] > [H⁺]

Question 36

What is [OH⁻] for a solution at 25°C that has [H₃O⁺] = 8.23 × 10⁻² M?

A)8.23 × 10⁻² M
B)1.22 × 10⁻⁶ M
C)8.23 × 10⁻¹² M
D)1.22 × 10⁻¹³ M
E)8.23 × 10⁻¹⁶ M

Question 37

What is the H⁺ ion concentration in a 2.1 × 10⁻⁴ M Ca(OH)₂ solution?

A)7.3 × 10⁻⁴ M
B)4.2 × 10⁻⁴ M
C)2.1 × 10⁻⁴ M
D)2.4 × 10⁻¹¹ M
E)4.8 × 10⁻¹¹ M

Question 38

What is the conjugate acid of the acetate ion?

A)CH₃O²⁻
B)COOH
C)HC₂H₃O₂
D)H₂O
E)CH₄

Question 39

Which solution is basic?

A)pH = 1.00
B)pH = 10.00
C)pH = 5.00
D)pH = 3.00
E)pH = 4.00

Question 40

What is the concentration of OH⁻ in a 1.0 × 10⁻³ M Ba(OH)₂ solution?

A)0.50 × 10⁻³ M
B)1.0 × 10⁻³ M
C)2.0 × 10⁻³ M
D)1.0 × 10⁻² M
E)3.3 × 10⁻⁴ M

Question 41

What is the conjugate acid of CO₃²⁻ in the reaction below? CO₃²⁻ + HSO₄⁻ HCO₃⁻ + SO₄²⁻

A)HCO₃⁻
B)HSO₄⁻
C)OH⁻
D)H₃O⁺
E)SO₄²⁻

Question 42

What is the pH of a solution in which [H⁺] is 1.22 × 10⁻⁴ M?

A)−3.914
B)1.220
C)3.914
D)4.000
E)4.086

Question 43

The pH of a Ba(OH)₂ solution is 10.00.What is the H⁺ ion concentration of this solution?

A)4.0 × 10⁻¹¹ M
B)1.6 × 10⁻¹⁰ M
C)1.3 × 10⁻⁵ M
D)1.0 × 10⁻¹⁰ M
E)10.00 M

Question 44

Automobile batteries use 3.0 M H₂SO₄ as an electrolyte.How much 1.20 M NaOH will be needed to neutralize 225 mL of battery acid? H₂SO₄(aq) + 2NaOH(aq) → 2H₂O(l) + Na₂SO₄(aq)

A)0.045 L
B)0.28 L
C)0.56 L
D)0.90 L
E)1.1 L

Question 45

What volume of a 0.442 M NaOH solution is needed to neutralize 65.0 mL of a 0.296 M solution of HNO₃?

A)8.71 mL
B)21.8 mL
C)43.5 mL
D)87.1 mL
E)174 mL

Question 46

What volume of a 0.452 M NaOH solution is needed to neutralize 85.0 mL of a 0.176 M solution of H₂SO₄?

A)218.3 mL
B)66.2 mL
C)38.4 mL
D)436.6 mL
E)33.1 mL

Question 47

In the reaction, HSO₄
, the conjugate acid-base pairs are

A)HSO ⁻ and SO ²⁻; H O and OH⁻.4 4
2
B)HSO₄⁻ and H₃O⁺; SO₄^{2 −} and OH⁻.
C)HSO₄⁻ and OH⁻; SO₄^{2 −} and H₂O.
D)HSO₄⁻ and H₂O; OH ⁻ and SO₄²⁻.
E)HSO₄⁻ and OH⁻; SO₄^{2 −} and H₃O⁺.

Question 48

What is the pH of a 0.050 M LiOH solution?

A)1.30
B)3.00
C)11.00
D)12.39
E)12.70

Question 49

What is the conjugate base of HSO₄⁻ in the reaction below? CO₃²⁻ + HSO₄⁻ HCO₃⁻ + SO₄²⁻

A)HSO₄⁻
B)CO₃²⁻
C)OH⁻
D)H O⁺
3
E)SO₄²⁻

Question 50

What is the [H₃O⁺] for a solution at 25°C that has pOH = 5.640?

A)2.34 × 10⁻⁴ M
B)2.29 × 10⁻⁶ M
C)4.37 × 10⁻⁹ M
D)4.27 × 10⁻¹¹ M
E)8.360 M

Question 51

Identify the conjugate base of HPO₄²⁻ in the reaction HCO₃⁻ + HPO₄²⁻ H₂CO₃ + PO₄³⁻

A)H₂O
B)HCO₃⁻
C)H₂CO₃
D)PO₄³⁻
E)None of these

Question 52

During a titration, it is found that 53.5 mL of a solution of NaOH is needed to neutralize a solution that contains 1.86 g of HCl.What is the concentration of the NaOH solution?

A)0.051 M
B)0.686 M
C)1.05 M
D)0.035 M
E)0.953 M

Question 53

What is the pH of a 0.056 M HNO₃ solution?

A)0.056
B)1.25
C)12.75
D)2.88
E)11.11

Question 54

What is the [H⁺] in a solution with a pH of 5.63?

A)2.344 × 10⁻⁶ M H⁺
B)2.344 × 10⁻⁵ M H⁺
C)5.63 M H⁺
D)2.3 × 10⁻⁶ M H⁺
E)2.3 × 10⁻⁵ M H⁺

Question 55

A standard solution of 0.243 M NaOH was used to determine the concentration of a hydrochloric acid solution.If 46.33 mL of NaOH is needed to neutralize 10.00 mL of the acid, what is the molar concentration of the acid in the original solution?

A)0.243 M
B)0.200 M
C)1.13 M
D)0.563 M
E)0.0313 M

Question 56

A 34.62-mL of 0.1510 M NaOH was needed to neutralize 50.0 mL of an H₂SO₄ solution.What is the concentration of the original sulfuric acid solution?

A)0.0229 M
B)0.218 M
C)0.0523 M
D)0.209 M
E)0.105 M

Question 57

Vinegar is a solution of acetic acid, HC₂H₃O₂ , dissolved in water.A 5.54-g sample of vinegar was neutralized by 30.10 mL of 0.100 M NaOH.What is the percent by weight of acetic acid in the vinegar?

A)0.0543%
B)1.08%
C)3.26%
D)5.43%
E)9.23%

Question 58

What is the pOH of a 0.0085 M KOH solution?

A)2.07
B)4.85
C)9.15
D)11.93
E)0.0085

Question 59

What is the pH of a 0.014 M Ca(OH)₂ solution?

A)1.85
B)1.55
C)12.15
D)12.45
E)15.85

Question 60

What is the pOH of a 0.025 M HI solution?

A)0.025
B)0.94
C)1.60
D)12.40
E)10.31

Question 61

Which one of these salts will form an acidic solution upon dissolving in water?

A)LiBr
B)NaF
C)NH₄Br
D)KOH
E)NaCN

Question 62

Which one of these salts will form a basic solution upon dissolving in water?

A)NaCl
B)NaNO₂
C)NH₄NO₃
D)KBr
E)AlCl₃

Question 63

Which pair of substances could form a buffered aqueous solution?

A)HCl, NaCl
B)HNO₃, NaNO₃
C)H₃PO₄, NaH₂PO₄
D)H₂SO₄, CH₃COOH
E)NH₃, NaOH

Question 64

Which pair of substances is capable of forming a buffer in aqueous solution?

A)H₃PO₄, Na₃PO₃
B)HNO₃, NaNO₃
C)HCl, NaCl
D)H₂CO₃, NaNO₂
E)CH₃COOH, CH₃COONa

Question 65

Which pair of substances cannot form a buffered aqueous solution?

A)HCN and KCN
B)NH₃ and (NH₄)₂SO₄
C)HNO₃ and NaNO₃
D)HF and NaF
E)HNO₂ and NaNO₂