Deck 15: Acids and Bases

Question 1

Identify the conjugate base of HCO₃^- in the reaction CO₃^2- + HSO₄^- HCO₃^- + SO₄^2-

A)HSO₄^-
B)CO₃^2-
C)OH^-
D)H₃O⁺
E)SO₄^2-

Answer 1

CO₃^2-

Question 2

Identify the conjugate acid of HCO₃^- in the reaction HCO₃^- + HPO₄^2- H₂CO₃ + PO₄^3-

A)H₂O
B)HCO₃^-
C)H₂CO₃
D)PO₄^3-
E)HPO₄^2-

Answer 2

H₂CO₃

Question 3

Identify the conjugate acid of SO₄^2- in the reaction CO₃^2- + HSO₄^- HCO₃^- + SO₄^2-

A)CO₃^2-
B)HSO₄^-
C)OH^-
D)H₃O⁺
E)SO₄^2-

Answer 3

HSO₄^-

Question 4

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 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 HSO₄^-(aq)+ OH^-(aq) SO₄^2-(aq)+ H₂O(l), the conjugate acid-base pairs are

Question 7

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 8

What is the pH of an aqueous solution that contains 2.7 *10²⁰ H₃O⁺ ions per liter of solution?

A)2.70
B)3.35
C)6.02
D)10.65
E)11.30

Question 9

Identify the conjugate base of HSO₄ ^- in the reaction H₂PO₄^- + HSO₄^- H₃PO₄ + SO₄^2-

A)H₂PO₄^-
B)H₂SO₄
C)H₂O
D)H₃PO₄
E)SO₄^2-

Question 10

Identify the conjugate base of HPO₄^2- in the reaction HCO₃^- + HPO₄^2- H₂CO₃ + PO₄^3-

A)H₂O
B)HCO₃^-
C)H₂CO₃
D)PO₄^3-
E)None of these.

Question 11

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 12

Which is not a characteristic property of acids?

A)neutralizes bases
B)turns litmus from blue to red
C)reacts with active metals to produce H₂(g)
D)reacts with CO₂(g)to form carbonates
E)All of the above are characteristic properties of acids.

Question 13

In the reaction H₂CO₃ + H₂O HCO₃^- + H₃O⁺, the Brønsted acids are

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

Question 14

Identify the conjugate acid of CO₃^2- in the reaction CO₃^2- + H₂PO₄^- HCO₃^- + HPO₄^2-

A)H₂CO₃
B)HCO₃^-
C)H₂O
D)HPO₄^2-
E)H₂PO₄^-

Question 15

Identify the conjugate base of HClO₃ in the reaction ClO₃^- + HSO₄^- HClO₃ + SO₄^2-

A)ClO₃^-
B)HSO₄^-
C)OH^-
D)H₃O⁺
E)SO₄^2-

Question 16

Which is the formula for the hydronium ion?

A)OH^-
B)H₂O
C)H₃O⁺
D)H₃O^-
E)H₂O⁺

Question 17

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 18

Identify the conjugate base of CH₃COOH in the reaction CH₃COOH + HSO₄^- H₂SO₄ + CH₃COO^-

A)HSO₄^-
B)SO₄^2-
C)CH₃COO^-
D)H₂SO₄
E)OH^-

Question 19

What is the pH of an aqueous solution that contains 5.3 *10¹⁷ OH^- ions per liter of solution?

A)5.30
B)6.06
C)7.94
D)8.70
E)11.3

Question 20

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.

Question 21

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 22

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 23

Calculate the pH of a 6.71 * 10^-2 M NaOH solution.

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

Question 24

Calculate the H⁺ ion concentration in lemon juice having a pH of 2.4.

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

Question 25

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 26

Determine the pH of a KOH solution made by mixing 0.251 g KOH with enough water to make 1.00 * 10² mL of solution.

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

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)zero
E)1.0 * 10^-4 M

Question 28

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 29

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 30

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 31

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 32

A 0.10 M NH₃ solution is 1.3% ionized. Calculate the H⁺ ion concentration. NH₃ + H₂O 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 33

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 34

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 35

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 36

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 37

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 38

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 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

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 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

The pH of a certain solution is 3.0. How many H⁺(aq)ions are there in 1.0 L of the solution?

A)0.001 ions
B)1,000 ions
C)6.* 10²⁰ ions
D)3 ions
E)6.* 10²⁶ ions

Question 43

Acid strength decreases in the series: HNO₃ > HF > CH₃COOH. Which of these species is the strongest base?

A)NO₃^-
B)CH₃COO^-
C)F^-
D)CH₃COOH

Question 44

What is the pH of a solution prepared by mixing 10.0 mL of a strong acid solution with pH = 2.00 and 10.0 mL of a strong acid solution with pH = 6.00?

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

Question 45

Acid strength decreases in the series: strongest HSO₄^- > HF > HCN. Which of these species is the weakest base?

A)HF
B)SO₄^2-
C)F^-
D)CN^-

Question 46

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 47

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 48

Acid strength decreases in the series: HCl > HSO₄^- > HCN. Which of these species is the strongest base?

A)CN^-
B)SO₄^2-
C)HCN
D)Cl^-

Question 49

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 50

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 51

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 52

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 53

Acid strength increases in the series: HCN < HF < HSO₄^-. Which of these species is the strongest base?

A)H₂SO₄
B)SO₄^2-
C)F^-
D)CN ^-
E)HSO₄^-

Question 54

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 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

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 57

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 58

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

Question 59

Acid strength decreases in the series HI > HSO₄^- > HF > HCN. Which of these anions is the weakest base?

A)I^-
B)SO₄^2-
C)F^-
D)CN^-

Question 60

The pH of a certain solution is 2.0. How many H⁺(aq)ions are there in 1.0 L of the solution?

A)0.01 ions
B)100 ions
C)2 ions
D)6.* 10²¹ ions
E)6.* 10²³ ions

Question 61

Which of the following yields a basic solution when dissolved in water?

A)NO₂
B)P₄O₁₀
C)K₂O
D)NaCl
E)SO₂

Question 62

Hard water deposits (calcium carbonate)have built up around your bathroom sink. Which one of these substances would be most effective in dissolving the deposits?

A)ammonia
B)bleach (sodium hypochlorite)
C)lye (sodium hydroxide)
D)vinegar (acetic acid)

Question 63

Predict the direction in which the equilibrium will lie for the reaction C₆H₅COO^- + HF C₆H₅COOH + F^- .
K_a(C₆H₅COOH)= 6.5 *10^-5; K_a(HF)= 7.1 *10^-4

A)to the right
B)to the left
C)in the middle

Question 64

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 65

Predict the direction in which the equilibrium will lie for the reaction H₃PO₄(aq)+ HSO₄^-(aq) H₂PO₄^-(aq) + H₂SO₄(aq).
K_a1(H₃PO₄)= 7.5 * 10^-3; K_a(H₂SO₄)= very large

A)to the right
B)to the left
C)in the middle

Question 66

Predict the direction in which the equilibrium will lie for the reaction H₃PO₄ + NO₃^- H₂PO₄^- + HNO₃ K_a(H₃PO₄)= 7.5 * 10^-3

A)to the right
B)to the left
C)in the middle

Question 67

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 68

P₄O₁₀ is classified as an acidic oxide because it

A)reacts with acids to produce a salt.
B)is insoluble in water.
C)reacts with water to produce OH^-.
D)gives a solution of phosphoric acid, H₃PO₄, on dissolving in water.
E)can act as a Lewis base by donating electron pairs.

Question 69

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 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

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 72

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 73

Which of the following yields an acidic solution when dissolved in water?

A)NO₂
B)LiOH
C)K₂O
D)NaCl
E)Ca(OH)₂

Question 74

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 75

In the reaction CaO(s)+ SO₂(g) CaSO₃(s),

A)O^2- acts as a Lewis base, and SO₂ acts as a Lewis acid.
B)Ca²⁺ acts as a Lewis base, and SO₄^2- acts as a Lewis acid.
C)SO₄^2- acts as a Lewis base, and SO₂ acts as a Lewis acid.
D)SO₂ acts as a Lewis base, and O^2- acts as a Lewis acid.
E)SO₂ acts as a Lewis base, and Ca²⁺ acts as a Lewis acid.

Question 76

Predict the direction in which the equilibrium will lie for the reaction H₂SO₃(aq)+ HCO₃^- (aq) HSO₃^-(aq)+ H₂CO₃(aq).
K_a1(H₂SO₃)= 1 * 10^-2; K_a1(H₂CO₃)= 4.2 * 10^-7

A)to the right
B)to the left
C)in the middle

Question 77

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 78

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 79

Which of these acids is the strongest?

A)H₂SO₃
B)H₂SeO₃
C)H₂TeO₃

Question 80

Predict the direction in which the equilibrium will lie for the reaction H₂CO₃ + F^-
HCO₃^- + HF. K_a1( H₂CO₃)= 4.2 * 10^-7; K_a(HF)= 7.1 * 10^-4

A)to the right
B)to the left
C)in the middle