Deck 15: Acids and Bases

Question 1

The OH^- concentration in a 7.5 * 10^-3 M Ca(OH)₂ solution is

A) 7.5 * 10^-3 M.
B) 1.5 * 10^-2 M.
C) 1.3 * 10^-12 M.
D) 1.0 * 10^-7 M.
E) 1.0 * 10^-14 M.

Answer 1

1.5 * 10^-2 M.

Question 2

Which of the following is not a conjugate acid-base pair

A) H₃PO₄ and H₂PO₄^-
B) H₂PO₄^- and HPO₄^2-
C) H₃PO₄ and HPO₄^2-
D) HPO₄^2- and PO₄^3-
E) H₂O and H₃O⁺

Answer 2

H₃PO₄ and HPO₄^2-

Question 3

The hydronium ion and the hydroxide ion, in that order, are:

A) H₃O⁺, OH⁺
B) OH^-, H₃O^-
C) OH^-, H⁺
D) H₃O⁺, OH^-
E) H₃O^-, OH^-

Answer 3

H₃O⁺, OH^-

Question 4

Identify the conjugate base of HSO₄^-.

A) OH^-
B) H₂SO₄
C) H₂O
D) H₂SO₃
E) SO₄^2-

Question 5

What is the H⁺ ion concentration in a 4.8 * 10^-2 M KOH solution

A) 4.8 * 10^-2 M
B) 1.0 * 10^-7 M
C) 4.8 * 10^-11 M
D) 4.8 * 10^-12 M
E) 2.1 * 10^-13 M

Question 6

In the reaction: 2H₂O(l) $\leftrightharpoons$ H₃O⁺(aq) + OH^- (aq) the conjugate acid-base pairs are

A) pair 1: H₂O and H₂O; pair 2: H₃O⁺ and OH^-
B) pair 1: H₃O⁺ and OH^-; pair 2: H₃O⁺ and H₂O
C) pair 1: H₃O⁺ and OH^-; pair 2: OH^- and H₂O
D) pair 1: H₂O and OH^-; pair 2: H₂O and H₃O⁺
E) pair 1: H₃O⁺ and HO^-: pair 2: OH^- and H₃O⁺

Question 7

The OH^- concentration in a 1.0 * 10^-3 M Ba(OH)₂ solution is

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) 0.020 M.

Question 8

Which of the following does not fit the definition of a Brønsted Base

A) CO₃^2-
B) NH₃
C) H₂O
D) NH₄⁺
E) HCO₃^-

Question 9

The OH^- concentration in a 2.5 * 10^-3 M Ba(OH)₂ solution is

A) 4.0 * 10^-12 M.
B) 2.5 * 10^-3 M.
C) 5.0 * 10^-3 M.
D) 1.2 * 10^-2 M.
E) 0.025 M.

Question 10

Which of the following does not fit the definition of a Brønsted Acid

A) H₃PO₄
B) H₂PO₄^-
C) H₂O
D) NH₄⁺
E) CO₂

Question 11

Identify the conjugate acid of HCO₃^-.

A) H₂O
B) CO₃^2-
C) H₂CO₃
D) CO₂
E) H₃O⁺

Question 12

In the reaction: CH₃COOH(aq) + NH₂^- (aq) $\leftrightharpoons$ CH₃COO^- (aq) + NH₃(aq), the conjugate acid-base pairs are:

A) pair 1: CH₃COOH and CH₃COO^- ; pair 2: NH₂^- and NH₃
B) pair 1: CH₃COOH and NH₃; pair 2: NH₂^- and CH₃COO^-
C) pair 1: CH₃COOH and NH₂^- ; pair 2: NH₃ and CH₃OO^-
D) pair 1: CH₃COOH and CH₃COO^- ; pair 2: NH₄⁺ and NH₃
E) pair 1: CH₃COOH and CH₃COO^- ; pair 2: NH₂^- and NH₃⁺

Question 13

Which of the following is not a conjugate acid-base pair

A) H₂O and OH^-
B) H₂O and H₃O⁺
C) H₃O⁺ and OH^-
D) HO₂^- and H₂O₂
E) O₂^2- and HO₂^-

Question 14

What is the concentration of H⁺ in a 2.5 M HCl solution

A) 0
B) 1.3 M
C) 2.5 M
D) 5.0 M
E) 10. M

Question 15

In the reaction HSO₄^-(aq) + OH^-(aq) $\leftrightharpoons$ SO₄^2-(aq) + H₂O(l), the conjugate acid-base pairs are
$~~~~~~~~~\text { pair } 1 \quad~~~~~~~~~~~~~~~~~ \text { pair } 2$
A. $\mathrm{HSO}_{4}^{-}$ and $\mathrm{SO}_{4}{ }^{2-} ; \quad\mathrm{H}_{2} \mathrm{O}$ and $\mathrm{OH}^{-}$
B. $\mathrm{HSO}_{4}^{-}$ and $\mathrm{H}_{3} \mathrm{O}^{-} ; \quad\mathrm{SO}_{4}{ }^{2-}$ and $\mathrm{OH}^{-}$ .
C. $\mathrm{HSO}_{4}^{-}$ and $\mathrm{OH}^{-} ; \quad \mathrm{SO}_{4}^{2-}$ and $\mathrm{H}_{2} \mathrm{O}$ .
D. $\mathrm{HSO}_{4}{ }^{-}$ and $\mathrm{H}_{2} \mathrm{O}; \quad\mathrm{OH}^{-}$ and $\mathrm{SO}_{4}{ }^{2-}$
E. $\mathrm{HSO}_{4}^{-}$ and $\mathrm{OH}^{-} ; \quad \mathrm{SO}_{4}{ }^{2-}$ and $\mathrm{H}_{3} \mathrm{O}^{+}$

A) A
B) B
C) C
D) D
E) E

Question 16

Identify the conjugate base of HCO₃^-.

A) H₂CO₃
B) CO₃^2-
C) OH^-
D) CO₂
E) CO

Question 17

Identify the conjugate base of HPO₄^2-.

A) H₂O
B) H₂PO₄^-
C) H₃PO₄
D) PO₄^3-
E) OH^-

Question 18

Identify the conjugate acid of SO₄^2-.

A) H₂SO₄
B) HSO₄^-
C) H₂SO₃
D) H₃O⁺
E) SO₃^2-

Question 19

Which one of these statements about strong acids is true

A) All strong acids have H atoms bonded to electronegative oxygen atoms.
B) Strong acids are 100% ionized in water.
C) The conjugate base of a strong acid is itself a strong base.
D) Strong acids are very concentrated acids.
E) Strong acids produce solutions with a higher pH than weak acids.

Question 20

Identify the conjugate acid of CO₃^2-.

A) H₂CO₃
B) HCO₃^-
C) H₂O
D) H₃O⁺
E) CO₂

Question 21

Calculate the H⁺ ion concentration in lemon juice having a pH of 2.40.

A) 4.0 * 10^-2 M
B) 250 M
C) 0.38 M
D) 4.0 * 10^-3 M
E) 12 M

Question 22

Which of the following solutions is acidic

A) [OH^-] = 1.0 x 10^-7 M
B) [OH^-] > 1.0 x 10^-7 M
C) [OH^-] = 1.0 x 10^-10 M
D) [H₃O⁺] = 1.0 x 10^-10 M
E) [H₃O⁺] < 1.0 x 10^-7 M

Question 23

Calculate the pH of a 0.14 M HNO₂ solution that is 5.7% ionized.

A) 0.85
B) 1.70
C) 2.10
D) 11.90
E) 13.10

Question 24

What is the pH of 10.0 mL of 0.0020 M HCl

A) 0.70
B) 2.70
C) 3.70
D) 5.70
E) 10.0

Question 25

Determine the pH of a KOH solution made by mixing 0.251 g KOH with enough water to make 1.0 * 10² mL of solution.

A) 1.35
B) 2.35
C) 7.00
D) 11.65
E) 12.65

Question 26

A 0.10 M NH₃ solution is 1.3% ionized. Calculate the H⁺ ion concentration.NH₃ + H₂O $\leftrightharpoons$ NH₄⁺ + OH^-

A) 1.3 * 10^-3 M
B) 7.7 * 10^-2 M
C) 7.7 * 10^-12 M
D) 0.13 M
E) 0.10 M

Question 27

What is the OH^- ion concentration in a 5.2 * 10^-4 M HNO₃ solution

A) 1.9 * 10^-11 M
B) 1.0 * 10^-7 M
C) 5.2 * 10^-4 M
D) 0
E) 1.0 * 10^-4 M

Question 28

What is the pH of a 0.0055 M HA (weak acid) solution that is 8.2% ionized

A) 2.26
B) 3.35
C) 4.52
D) 8.21
E) 10.65

Question 29

Calculate the pH of a 6.7 * 10^-2 M NaOH solution.

A) 12.83
B) 2.17
C) 11.82
D) 6.71
E) 1.17

Question 30

Calculate the pH of a carbonated beverage in which the hydrogen ion concentration is 3.4 * 10^-4 M.

A) 2.34
B) 3.47
C) 6.01
D) 7.99
E) 10.53

Question 31

Which of the following solutions is basic

A) [H₃O⁺] = 1.0 x 10^-10 M
B) [OH^-] = 1.0 x 10^-10 M
C) [H₃O⁺] > 1.0 x 10^-7 M
D) [OH^-] < 1.0 x 10^-10 M
E) [OH^-] = 1.0 x 10^-7 M

Question 32

Calculate the pH of a 3.5 * 10^-3 M HNO₃ solution.

A) -2.46
B) 0.54
C) 2.46
D) 3.00
E) 3.46

Question 33

Which of the following solutions is basic

A) [OH^-] = 1.0 x 10^-14 M
B) [OH-] = 1.0 x 10^-7 M
C) [H₃O⁺] = 1.0 x 10^-14 M
D) [H₃O⁺] > 1.0 x 10^-7 M
E) [OH^-] < 1.0 x 10^-7 M

Question 34

Calculate the pH of a 0.10 M HCN solution that is 0.0070% ionized.

A) 1.00
B) 0.00070
C) 3.15
D) 5.15
E) 7.00

Question 35

A 0.14 M HNO₂ solution is 5.7% ionized. Calculate the H⁺ ion concentration.

A) 8.0 * 10^-3 M
B) 0.057 M
C) 0.13 M
D) 0.14 M
E) 0.80 M

Question 36

Calculate the H⁺ ion concentration in a 8.8 * 10^-4 M Ca(OH)₂ solution.

A) 8.8 * 10^-4 M
B) 1.8 * 10^-3 M
C) 2.2 * 10^-11 M
D) 1.1 * 10^-11 M
E) 5.7 * 10^-12 M

Question 37

Which of the following solutions is acidic

A) [H₃O⁺] = 7.0 x 10^-7 M
B) [H₃O⁺] = 1.5 x 10^-10 M
C) [H₃O⁺] < 7.0 x 10^-7 M
D) [H₃O⁺] > 7.0 x 10^-7 M
E) [H₃O⁺] = 1.0 x 10^-14 M

Question 38

A 0.10 M HF solution is 8.4% ionized. Calculate the H⁺ ion concentration.

A) 0.84 M
B) 0.12 M
C) 0.10 M
D) 0.084 M
E) 8.4 * 10^-3 M

Question 39

Consider the weak acid CH₃COOH (acetic acid). If a 0.048 M CH₃COOH solution is 5.2% ionized, determine the [H₃O⁺] concentration at equilibrium.

A) 0.25 M
B) 9.2 * 10^-3 M
C) 0.048 M
D) 0.052 M
E) 2.5 * 10^-3 M

Question 40

Calculate the pH of 2.6 *10^-2 M KOH.

A) 12.41
B) 15.59
C) 2.06
D) 7.00
E) 1.59

Question 41

The pH of tomato juice is about 4.5. Calculate the concentration of hydrogen ions in this juice.

A) 3 * 10^-10 M
B) 3 * 10^-5 M
C) 5 * 10^-4 M
D) 4 M
E) 3 * 10¹⁰ M

Question 42

Calculate the hydrogen ion concentration in a solution having a pH of 4.60.

A) 4.0 * 10^-3 M
B) 4.0 * 10^-9 M
C) 4.0 * 10^-10 M
D) 2.5 * 10^-5 M
E) 2.5 * 10^-4 M

Question 43

The pOH of a solution is 10.40. Calculate the hydrogen ion concentration in the solution.

A) 4.0 * 10^-11 M
B) 3.6 M
C) 4.0 * 10^-10 M
D) 2.5 * 10^-4 M
E) 1.8 * 10^-4 M

Question 44

If the pH of an acid rain storm is approximately 3.0, how many times greater is the [H⁺] in the rain than in a cup of coffee having a pH of 5.0

A) 1000
B) 100
C) 20
D) 1.7
E) 0.60

Question 45

A 5.5 L sample of a 0.25 M HNO₃ solution is mixed with 1.2 L of a 0.34 M HCl solution. What is the pH of the mixture

A) 0.23
B) 0.57
C) 1.07
D) 0.50
E) 0.84

Question 46

What is the pH of a solution prepared by mixing 10.0 mL of a strong acid solution with pH = 2.0 and 10.0 mL of a strong acid solution with pH = 6.0

A) 2.0
B) 2.3
C) 4.0
D) 6.0
E) 8.0

Question 47

Diet cola drinks have a pH of about 3.0, while milk has a pH of about 7.0. How many times greater is the H₃O⁺ concentration in diet cola than in milk

A) 2.3 times higher in diet cola than in milk
B) 400 times higher in diet cola than in milk
C) 0.43 times higher in diet cola than in milk
D) 1,000 times higher in diet cola than in milk
E) 10,000 times higher in diet cola than in milk

Question 48

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. M

Question 49

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 50

A 1.5 L sample of a 0.44 M HBr solution is mixed with 2.2 L of a 0.080 M HClO₄ solution. What is the pH of the mixture

A) 0.28
B) 0.36
C) 1.45
D) 0.73
E) 0.65

Question 51

What is the pH of a 0.001 M Ca(OH)₂ solution

A) 3.0
B) 11.0
C) 2.7
D) 17.0
E) 11.3

Question 52

The pOH of a solution is 9.60. Calculate the hydrogen ion concentration in this solution.

A) 2.5 * 10^-10 M
B) 6.0 * 10^-9 M
C) 4.0 * 10^-5 M
D) 2.4 * 10^-4 M
E) 1.0 * 10^-14 M

Question 53

A 2.1 L sample of a 0.23 M NaOH solution is mixed with 1.9 L of a 0.021 M KOH solution. What is the pH of the mixture

A) 13.40
B) 13.12
C) 11.68
D) 12.84
E) 13.04

Question 54

The pH of coffee is approximately 5.0. How many times greater is the [H⁺] in coffee than in neutral water

A) 200
B) 100
C) 5.0
D) 1.4
E) 0.01

Question 55

Calculate the hydrogen ion concentration in a solution of iced tea with lemon having a pH of 2.87.

A) 2.9 * 10^-2 M
B) 5.7 * 10^-2 M
C) 1.3 * 10^-3 M
D) 2.9 * 10^-3 M
E) 5.7 * 10^-4 M

Question 56

Calculate the pOH for a solution with [H₃O⁺] = 2.5 x 10^-5 M

A) 4.60
B) 9.40
C) 4.0 x 10^-10
D) 2.50
E) 11.50

Question 57

Calculate the pH of a 1.6 M KOH solution.

A) 1.60
B) -0.20
C) 0.20
D) 14.20
E) 13.80

Question 58

A 5.2 L sample of a 1.1 M KOH solution is mixed with 2.3 L of a 0.20 M Sc(OH)₃ solution. What is the pH of the mixture

A) 13.67
B) 13.89
C) 14.11
D) 14.23
E) 13.98

Question 59

Calculate the hydrogen ion concentration in a solution of fruit juice having a pH of 4.25.

A) 1.0 * 10^-14 M
B) 5.6 * 10^-5 M
C) 4.0 * 10^-25 M
D) 2.5 * 10^-4 M
E) 5.6 * 10^-4 M

Question 60

The pH of coffee is approximately 5.0. How many times greater is the [H₃O⁺] in coffee than in tap water having a pH of 8.0

A) 0.62
B) 1.6
C) 30
D) 1,000
E) 1.0 * 10⁴

Question 61

Which one of these net ionic equations represents the reaction of a strong acid with a weak base

A)H⁺(aq) + OH^-(aq) $\rarr$ H₂O(aq)
B)H⁺(aq) + CH₃NH₂(aq) $\rarr$ CH₃NH₃⁺(aq)
C)OH^-(aq) + HCN(aq) $\rarr$ H₂O(aq) + CN^-(aq)
D)HCN(aq) + CH₃NH₂(aq) $\rarr$ CH₃NH₃⁺ (aq)+ CN^-(aq)

Question 62

The equilibrium expression for the ionization of a weak monoprotic acid, HA, in water is:

A) K_a = [HA]/[OH^-][H₃O⁺]
B) K_a = [OH^-][H₃O⁺]/[HA]
C) K_a = [H₃O⁺][HA]/[A^-]
D) K_a = [H₃O⁺][A^-]/[HA]
E) K_a = [HA]/[H₃O⁺][A^-]

Question 63

Given the following K_a values, which anion is the strongest base $\begin{array}{|l|l|}\hline \text { Acid } & \mathrm{K}_{\mathrm{a}} \\\hline \mathrm{HF} & 7.1 \times 10^{-4} \\\hline \mathrm{HCOOH} & 1.7 \times 10^{-4} \\\hline \mathrm{HCN} & 4.9 \times 10^{-10} \\\hline \mathrm{HNO}_{2} & 4.5 \times 10^{-4} \\\hline \mathrm{CH}_{3} \mathrm{COOH} & 1.8 \times 10^{-5} \\\hline\end{array}$

A) F^-
B) HCOO^-
C) CN^-
D) NO₂^-
E) CH₃COO^-

Question 64

Arrange the acids HOCl, HClO₃, and HClO₂ in order of increasing acid strength.

A) HOCl < HClO₃ < HClO₂
B) HOCl < HClO₂ < HClO₃
C) HClO₂ < HOCl < HClO₃
D) HClO₃ < HOCl < HClO₂
E) HClO₃ < HClO₂ < HOCl

Question 65

Which one of these equations represents the reaction of a weak acid with a weak base

A)H⁺(aq) + OH^-(aq) $\rarr$ H₂O(aq)
B)H⁺(aq) + CH₃NH₂(aq) $\rarr$ CH₃NH₃⁺(aq)
C)OH^-(aq) + HCN(aq) $\rarr$ H₂O(aq) + CN^-(aq)
D)HCN(aq) + CH₃NH₂(aq) $\rarr$ CH₃NH₃⁺(aq) + CN^-(aq)

Question 66

Arrange the acids HBr, H₂Se, and H₃As in order of increasing acid strength.

A) HBr < H₂Se < H₃As
B) HBr < H₃As < H₂Se
C) H₂Se < H₃As < HBr
D) H₃As < H₂Se < HBr
E) H₃As < HBr < H₂Se

Question 67

Which one of the following equations represents the ionization of a weak base in water

A) NH₃(aq) + H₂O(l) $\leftrightharpoons$ NH₂⁺(aq) + H₃O⁺(aq)
B) NH₃(aq) + H₂O(l) $\leftrightharpoons$ NH₄⁺(aq) + OH^-(aq)
C) NH₃(aq) + H₂O(l) $\leftrightharpoons$ NH₄^- (aq) + OH⁺(aq)
D) NH₃(aq) + OH^-(aq) $\leftrightharpoons$ NH₂^- (aq) + H₂O(l)
E) NH₃(aq) + H₃O⁺(aq) $\leftrightharpoons$ NH $_4^+$ (aq) + H $_2$ O(l)

Question 68

Arrange the acids HOBr, HBrO₃, and HBrO₂ in order of increasing acid strength.

A) HOBr < HBrO₃ < HBrO₂
B) HOBr < HBrO₂ < HBrO₃
C) HBrO₂ < HOBr < HBrO₃
D) HBrO₃ < HOBr < HBrO₂
E) HBrO₃ < HBrO₂ < HOBr

Question 69

Given the following K_a values, which anion is the strongest base $\begin{array}{|l|l|}\hline \text { Acid } & \mathrm{K}_{3} \\\hline \mathrm{H}_{2} \mathrm{CO}_{3} & 4.2 \times 10^{-7} \\\hline \mathrm{HCO}_{3}^{-} & 4.8 \times 10^{-11} \\\hline \mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4} & 6.5 \times 10^{-2} \\\hline \mathrm{HC}_{2} \mathrm{O}_{4}^{-} & 6.1 \times 10^{-5} \\\hline \mathrm{H}_{2} \mathrm{PO}_{4}^{-} & 6.2 \times 10^{-8} \\\hline\end{array}$

A) HCO₃^-
B) CO₃^2-
C) HC₂O₄^-
D) C₂O₄^2-
E) HPO₄^2-

Question 70

Arrange the acids H₂Se, H₂Te, and H₂S in order of increasing acid strength.

A) H₂S < H₂Se < H₂Te
B) H₂S < H₂Te < H₂Se
C) H₂Te < H₂S < H₂Se
D) H₂Se < H₂S < H₂Te
E) H₂Se < H₂Te < H₂S

Question 71

Calculate the pOH for a solution with [H₃O⁺] = 3.1 x 10^-9 M.

A) 3.10
B) 10.90
C) 8.51
D) 5.49
E) 3.2 x 10^-6

Question 72

Which one of the following equations represents the ionization of a weak monoprotic acid in water

A) HNO₂(aq) + OH^- (aq) $\leftrightharpoons$ H₂O(l) + NO₂^-(aq)
B) HNO₂(aq) + NH₃(aq) $\leftrightharpoons$ NH₄NO₂(aq)
C) HNO₂(aq) + H₂O(l) $\leftrightharpoons$ H₃O⁺(aq) + NO₂^-(aq)
D) HNO₃(aq) + OH^-(aq) $\leftrightharpoons$ H₂O(l) + NO₃^-(aq)
E) NO₂^- (aq) + H₂O(aq) $\leftrightharpoons$ HNO $_2$ (aq) + OH $^-$ (aq)

Question 73

When comparing acid strength of binary acids HX, as X varies within a particular group of the periodic table, which one of these factors dominates in affecting the acid strength

A) bond strength
B) electron withdrawing effects
C) percent ionic character of the H-X bond
D) solubility
E) Le Châtelier's principle

Question 74

Given the following K_b values, which cation is the strongest acid $\begin{array}{|l|l|}\hline \text { Base } & \mathrm{K}_{\mathrm{b}} \\\hline \mathrm{NH}_{3} & 1.8 \times 10^{-5} \\\hline \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{NH}_{2} & 5.6 \times 10^{-4} \\\hline \mathrm{C}_{5} \mathrm{H}_{5} \mathrm{~N} & 1.7 \times 10^{-9} \\\hline \mathrm{C}_{8} \mathrm{H}_{10} \mathrm{~N}_{4} \mathrm{O}_{2} & 5.3 \times 10^{-14} \\\hline\left(\mathrm{NH}_{2}\right)_{2} \mathrm{CO} & 1.5 \times 10^{-14} \\\hline\end{array}$

A) NH₄⁺
B) C₂H₅NH₃⁺
C) C₅H₆N⁺
D) [C₈H₁₁N₄O₂]⁺
E) [NH₂NH₃CO]⁺

Question 75

Which solution will have the lowest pH

A) 0.25 M HClO
B) 0.25 M HClO₂
C) 0.25 M HClO₃
D) 0.25 M HClO₄
E) 0.25 M NaClO₄

Question 76

Which one of the following equations represents the ionization of a weak monoprotic acid in water

A) HCN(aq) + H₂O(l) $\leftrightharpoons$ H₃O⁺(aq) + CN^-(aq)
B) HCN(aq) + OH^-(aq) $\leftrightharpoons$ H₂O(l) + CN⁺(aq)
C) CN^- (aq) + H₂O(aq) $\leftrightharpoons$ HCN(aq) + OH^-(aq)
D) HCN(aq) + OH^- (aq) $\leftrightharpoons$ H₂O(l) + CN^-(aq)
E) HCN(aq) + NH₃(aq) $\leftrightharpoons$ NH $_4$ CN(aq)

Question 77

Which one of the following statements is true for a 0.1 M solution of a weak acid HA

A) The concentration of H⁺ is slightly greater than the concentration of A^-.
B) The pH equals 1.0.
C) The concentration of H⁺ is exactly equal to the concentration of A^-.
D) The pH is less than 1.0.
E) The concentration of H⁺ is slightly less than the concentration of A^-.

Question 78

Which one of these net ionic equations represents the reaction of a strong acid with a strong base

A)H⁺(aq) + OH^-(aq) $\rarr$ H₂O(aq)
B)H⁺(aq) + CH₃NH₂(aq) $\rarr$ CH₃NH₃⁺(aq)
C)OH^-(aq) + HCN(aq) $\rarr$ H₂O(aq) + CN^-(aq)
D)HCN(aq) + CH₃NH₂(aq) $\rarr$ CH₃NH₃⁺(aq) + CN^-(aq)

Question 79

Which one of these equations represents the reaction of a weak acid with a strong base

A)H⁺(aq) + OH^-(aq) $\rarr$ H₂O(aq)
B)H⁺(aq) + CH₃NH₂(aq) $\rarr$ CH₃NH₃⁺(aq)
C)OH^-(aq) + HCN(aq) $\rarr$ H₂O(aq) + CN^-(aq)
D)HCN(aq) + CH₃NH₂(aq) $\rarr$ CH₃NH₃⁺(aq) + CN^-(aq)

Question 80

Which solution will have the lowest pH

A) 0.10 M HCN
B) 0.10 M HNO₃
C) 0.10 M NaCl
D) 0.10 M H₂CO₃
E) 0.10 M NaOH