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AP Chemistry: Acid-Base Equilibria Practice

Total questions: 125

Worksheet time: 3hrs 32mins

Name
Class
Date
1.

Which of the following would be the SAME for equal volumes of 1.0 M HCl and

1.0 M HF?

a)

pH

b)

percent ionization

c)

conductivity

d)

moles of NaOH needed to neutralize acid sample

2.

Which species in the equation below are behaving as Bronsted-Lowry ACIDS?

NH3 + H2O ⇌ NH4+ + OH-

a)

NH₃ and H₂O

b)

H₂O and NH₄⁺

c)

NH₃ and OH⁻

d)

NH₄⁺ and OH⁻

3.

Which of the following gives the best estimate for the pH of a 1 × 10⁻⁵ M HClO₄ (aq) solution at 25°C?

a)

pH = 1.0, because HClO₄ is a strong acid

b)

pH = 5.0, because HClO₄ is a strong acid

c)

pH = 7.0, because HClO₄ is a strong base

d)

pH = 9.0, because HClO₄ is a strong base

4.

Which acid below has the WEAKEST conjugate base?

a)

Hydrofluoric acid, HF

(Ka = 7.2 x 10⁻⁴)

b)

Acetic Acid, CH₃COOH

(Ka = 1.8 x 10⁻⁵)

c)

Hydrocyanic acid, HCN

(Ka = 6.2 x 10⁻¹⁰)

d)

Formic acid, HCOOH

(Ka = 1.8 x 10 ⁻⁴)

5.

Which of the following is the correct mathematical relationship to use to calculate the pH of a 0.10 M aqueous HBr solution?

a)

pH = [H₃O⁺] = 0.10

b)

pH = ­-log (0.10)

c)

pH = 7.00 – (0.10)

d)

pH = 0.10

6.

Ammonia (NH₃) is a __________.

a)

weak base

b)

strong acid

c)

strong base

d)

weak acid

7.

Which of the following gives the best estimate for the pH of a 5 × 10⁻⁴ M Sr(OH)₂ (aq) solution at 25°C?

a)

pH = 3.0 because Sr(OH)₂ is a strong acid.

b)

pH = 5.0 because Sr(OH)₂ is a weak acid.

c)

pH = 9.0 because Sr(OH)₂ is a weak base.

d)

pH = 11.0 because Sr(OH)₂ is a strong base.

8.

Kw = [H₃O⁺] [OH⁻] = 1.0 x 10⁻¹⁴ at 25°C Based on this information, which of the following is true for a sample of pure water at 25°C?

a)

[H₃O⁺] = 7.0 M

b)

[OH⁻] = 1.0 x 10⁻¹⁴ M

c)

pH = 10⁻⁷

d)

pOH = 7.00

9.

The Ka of hypochlorous acid (HClO) is 3.0 x 10⁻⁸. What is the pH at 25°C of an aqueous solution that is 0.020 M in HClO?

a)

7.00

b)

2.45

c)

4.61

d)

9.22

10.

Which one of the following is the weakest acid?

a)

HF (Ka = 6.8 x 10⁻⁴)

b)

HC₂H₃O₂ (Ka = 1.8 x 10⁻⁵)

c)

HNO₂ (Ka = 4.5 x 10⁻⁴)

d)

HClO (Ka = 3.0 x 10⁻⁸)

11.

Of the following, __________ is a weak acid.

a)

CH₃NH₂

b)

HF

c)

HClO₄

d)

HCl

12.

Of the following, __________ is a weak base.

a)

CH₃NH₂

b)

HCl

c)

HNO₂

d)

KOH

13.

Sodium hydroxide is a strong base. This means that __________.

a)

aqueous solutions of NaOH contain equal concentrations of H⁺ (aq) and OH⁻ (aq)

b)

NaOH does not dissociate at all when it is dissolved in water

c)

NaOH dissociates completely to Na⁺(aq) and OH⁻(aq) when it dissolves in water

d)

NaOH cannot be neutralized by any strong or weak acid.

14.

What is the pH of a 0.015-M aqueous solution of barium hydroxide?

a)

12.48

b)

1.52

c)

12.18

d)

1.82

15.

Which solution below has the highest concentration of hydroxide ions?

a)

pH = 3.21

b)

pH = 9.82

c)

pH = 7.93

d)

pH = 12.59

16.

How would you calculate Kb for the formate ion (HCO2–), given that the Ka for formic acid (HCHO2) is 1.8 × 10–4?

a)

Kb = Ka × Kw

b)

Kb = Kw / Ka

c)

Kb = Ka / Kw

d)

Kb = Kw + Ka

17.

The magnitude of Kw indicates that ______________.

a)

water autoionizes very slowly

b)

water autoionizes very quickly

c)

water autoionizes only to a very small extent

d)

the autoionization of water is exothermic

18.

Consider the reaction of an acid in water:

HA(aq) + H2O ⇌ H3O+(aq) + A-(aq)

If A- is a stronger base than H2O, which of the following describes the system at equilibrium?

a)

reactants are favored at equilibrium

b)

products are favored at equilibrium

c)

more information is needed

19.

If the solid ammonium nitrate is dissolved in water, will the resulting solution be acidic, basic or neutral?

a)

acidic

b)

basic

c)

neutral

20.

In which of the following aqueous solutions does the weak acid exhibit the highest percent ionization?

a)

.01 M HC2H3O2

(Ka 1.8 x 10-5)

b)

.01 M HNO2

(Ka =4.5 x 10-4)

c)

.01 M HClO

(Ka= 3.0 x 10-8)

d)

.01 M HF

(Ka = 6.8 x 10-4)

21.

Of the following, which is the strongest acid?

a)

HClO

b)

HClO2

c)

HClO3

d)

HClO4

22.

HA is a weak acid. Which equilibrium reaction corresponds to the equilibrium constant Kb for A-?

a)

HA (aq) + H2O (l) ⇌ H2A+ (aq) + OH-(aq)

b)

A- (aq) + H3O+ (aq) ⇌ HA (aq) + H2O (l)

c)

HA (aq) + OH- (aq) ⇌ H2O (l) + H+ (aq)

d)

A- (aq) + H2O (l) ⇌ HA (aq) + OH- (aq)

e)

A- (aq) + OH- (aq) ⇌ HOA2- (aq)

23.

A- is a weak base. Which equilibrium corresponds to the equilibrium constant Ka for HA?

a)

HA (aq) + H2O (l) ⇌ H2A+ (aq) + OH- (aq)

b)

A- (aq) + H3O+ (aq) ⇌ HA (aq) + H2O (l)

c)

HA (aq) + H2O (l) ⇌ H3O+ (aq) + A- (aq)

d)

A- (aq) + H2O (l) ⇌ HA (aq) + OH- (aq)

e)

A- (aq) + OH- (aq) ⇌ HOA2- (aq)

24.

Using the data in the table, which of the conjugate bases below is the weakest base?

a)

OAc-

b)

C7H5O2-

c)

NO2-

d)

F-

e)

OAc- and C7H5O2-

25.

Using the data in the table, which of the conjugate bases below is the strongest base?

a)

OAc-

b)

CHO2-

c)

ClO-

d)

F-

e)

OAc- and CHO2-

26.

Using the data in the table, which of the conjugate acids below is the strongest acid?

a)

HClO

b)

HCO3-

c)

H2S

d)

NH3CH3+

e)

H2S and HClO

27.

Using the data in the table, which of the conjugate acids below is the weakest acid?

a)

HClO

b)

HCO3-

c)

H2S

d)

NH3CH3+

e)

H2S and HClO

28.

Z- is a weak base. An aqueous solution of NaZ is prepared by dissolving 0.350 mol of NaZ in sufficient water to yield 1.0 L of solution. The pH of the solution was 8.93 at 25.0 0C. What is the Kb of the solution?

a)

1.2 x 10-5

b)

6.9 x 10-9

c)

2.1 x 10-10

d)

2.8 x 10-12

29.
Which of the following is a conjugate acid/base pair?
a)
HCl/OCl-
b)
H2SO4/SO42-
c)
NH4+/NH3
d)
H3O+/OH-
30.

Acetic cid (HC2H3O2) is a weak monoprotic acid. Calculate the pH of a 0.20 M acetic acid solution. Ka = 1.8x10-5 for acetic acid.

a)

.698

b)

2.72

c)

11.28

d)

None of the answers are correct

31.

What is the [OH-] if the [H+] is 1.0 x 10-3M?

a)

1.0 x 10-3 M

b)

6.02 x 10-23 M

c)

1.0 x 10-14 M

d)

1.0 x 10-11 M

32.

Which of the following would be a weak base?

a)
b)
c)
d)
33.

In which of the following reactions does H2PO4- act as an acid?

a)

H3PO4 + H2O ⇌ H3O+ + H2PO4-

b)

H2PO4- + H2O ⇌ H3O+ + HPO42-

c)

H2PO4- + OH- ⇌ H3PO4 + O2-

d)

The ion cannot act as an acid

34.
What is the hydrogen ion concentration in a solution with pOH = 3.3?
a)
10.7 M
b)

0.0005 M

c)

0.00003 M

d)

2 x 10-11 M

35.

What is the conjugate acid of NH3?

a)

NH4+

b)

NH2-

c)

NH4OH

d)

NH4

36.

What is the conjugate base of HSO4-

a)

H2SO4

b)

SO42-

c)

H2SO4+

d)

HSO42-

37.

Calculate the pH of a 0.500 M NH3 solution. The Kb of ammonia is 1.77x 10-5.

a)

12.58

b)

2.98

c)

11.47

d)

10.69

38.

The Ka for gallic acid is 4.57 x 10-3. What is the Kb for gallate ion (its conjugate base)?

a)

4.57 x 10-3

b)

5.43 x 10-5

c)

2.19 x 10-12

d)

7.81 x 10-6

39.

The Ka for HF is 7.0 x 10-4. What is the Kb for F-?

a)

1.4 x 10-11

b)

2.0 x 10-8

c)

7.0 x 10-18

d)

7.0 x 10-4

e)

1.4 x 103

40.

An Arrhenius acid

a)

donates an H+

b)

increases the concentration of H+

c)

accepts a pair of electrons

d)

reacts with the solvent to form a cation

41.

Which of the following are weak acids?

a)

nitrous acid

b)

hydrofluoric acid

c)

hydrochloric acid

d)

hydroiodic acid

42.

True or False? The stronger the acid, the larger the value of the Ka.

a)

True

b)

False

43.

Select ALL of the strong acids.

a)

HClO4

b)

HNO2

c)

HF

d)

HI

e)

HNO3

44.

What is the conjugate acid of HCO31-?

a)

CO3

b)

H2CO3

c)

CO32-

d)

H2CO32-

45.

Estimate the pH of a 1.5 x 10-6 M solution of HCl.

a)

5.82

b)

7.85

c)

8.15

d)

9.5

46.

Estimate the pH of a barium hydroxide solution with a concentration of 2.5 x 10-2 M. Assume complete dissociation.

a)

12.7

b)

1.75

c)

1.3

d)

8.5

47.

Which of the following is closest to the pKa for an acid, HA, with Ka = 4.5 x 10-11 M.

a)

11.45

b)

4.5

c)

10.55

d)

15.5

48.

If a weak acid, HA, has a Ka = 2.9 x 10-5, what is the Kb for its conjugate base, A-?

a)

3.8 x 10-8

b)

3.4 x 10-10

c)

1.4 x 10-7

d)

1.4 x 10-9

49.

Which two species are acting as Bronsted-Lowry bases in the reaction shown below?

HF(aq) + NH3(aq) ⇌ F-(aq) + NH4+(aq)

a)

HF and F-

b)

NH3 and F-

c)

NH3 and NH4+

d)

NH4+ and F-

50.

Which of these is the strongest Bronsted base?

a)

F-

b)

Cl-

c)

Br-

d)

I-

51.

Which of these would be the strongest acid?

a)
b)
c)
d)
52.

What is the conjugate base of HClO4?

a)

H+

b)

Cl-

c)

ClO3-

d)

ClO4-

53.

What is the pH of a solution with [OH-] = 4.0 x 10-9?

a)

9.00

b)

5.60

c)

8.30

d)

4.30

54.

Which acid produces the strongest conjugate base?

a)

HClO4 (Ka= 1.0 x 107)

b)

HCN (Ka= 4.0 x 10-10)

c)

H3PO4 (Ka= 7.5 x 10-3)

d)

H2CO3 (Ka = 4.2 x 10-7)

55.

Which represents an acid with the smallest Ka value?

a)
b)
c)
56.

What is the closest pH to a solution with a [H+] = 2.5 x 10-10?

a)

2.5

b)

3.0

c)

4

d)

9

57.

If the [OH-] = 4.0 x 10-9, what is the pH of the solution?

a)

9.0

b)

5.7

c)

8.3

d)

4.3

58.

Which salt will form an acidic solution?

a)

NH4Cl

b)

NaCl

c)

NaHCO3

d)

BaCl2

59.

Which relationship relates Ka, Kb and Kw?

a)

Kw = Ka + Kb

b)

Kw = Kb/Ka

c)

Ka = Kw + Kb

d)

Kb = Kw/Ka

60.

Which of the following are the conjugate bases of HSO4–, CH3OH, and H3O+, respectively?

a)

SO42–, CH2OH–, and OH–

b)

CH3O–, SO42–, and H2O

c)

SO42–, CH3O–, and H2O

d)

SO42–, CH2OH–, and H2O

61.

Select any species that is acting as a Bronsted-Lowry base in the following reaction

OH– + NH4+ ⇌ H2O + NH3

a)

OH–

b)

NH4+

c)

H2O

d)

NH3

62.

Which of the following is not a strong base?

a)

Ca(OH)2

b)

Fe(OH)3

c)

KOH

d)

NaOH

63.

What is the pH of a solution that has an [H+] of 2.5 × 10–5?

a)

4.60

b)

5.0

c)

2.5

d)

7

64.

What is the [H+] if the pH is 4.0?

a)

1.0 × 10–10 M

b)

1.0 × 10–4 M

c)

1.0 × 10–14 M

d)

1.0 × 10–7 M

65.

What is the pOH of a solution where the [OH–] is 7.3 × 10–2 M?

a)

-1.14

b)

2.0

c)

1.14

d)

7.3

66.

What is the pOH of a solution where the [H+] is 2.5 × 10–12 M?

a)

11.6

b)

2.40

c)

12

d)

2.5

67.

Which of the following is the strongest weak acid?

a)

CH3COOH (Ka = 1.8 × 10–5)

b)

HF (Ka = 6.5 × 10–4)

c)

HCN (Ka = 6.3 × 10–10)

d)

HClO (Ka = 3.0 × 10–8)

68.

Which of the following produces the strongest conjugate base?

a)

CH3COOH (Ka = 1.8 × 10–5)

b)

HF (Ka = 6.5 × 10–4)

c)

HCN (Ka = 6.3 × 10–10)

d)

HClO (Ka = 3.0 × 10–8)

69.

Which of the following is the strongest weak acid?

a)

HF (pKa = 3.17)

b)

HCO3– (pKa = 10.32)

c)

H2PO4– (pKa = 7.18)

d)

NH4+ (pKa = 9.20)

70.

The value of Ka for HSO4– is 1 × 10–2. What is the value of Kb for SO42–?

a)

1 × 10–12

b)

1 × 10–8

c)

1 × 10–2

d)

1 × 102

71.

A 1-molar solution of a very weak monoprotic acid has a pH of 5. What is the value of Ka for the acid?

a)

1 × 10–10

b)

1 × 10–7

c)

1 × 10–5

d)

1 × 10–2

72.

If [H3O+] in an aqueous solution is 7.5 × 10–9 M, what is the [OH–]?

a)

6.4 × 10–5 M

b)

3.8 × 10–5 M

c)

7.5 × 10–5 M

d)

1.3 × 10–5 M

73.
Accepts a proton (H+ hydrogen ion) 
a)

Arrhenius acid

b)

Arrhenius base

c)

Bronstead Lowry base

d)

Arrhenius acid

74.

What is the conjugate acid in the following equation?

PO43- + HNO3 ⇌ NO3- + HPO42-

a)
PO43- 
b)
HNO3 
c)
NO3- 
d)
HPO42-
75.

What is the conjugate base in the following reaction?

HCO3- + HCl ⇌ H2CO3 + Cl-

a)
HCO3- 
b)
HCl
c)
 H2CO3 
d)

Cl-

76.
A compound that donates H+ ions is 
a)

a Bronsted-Lowry acid

b)

an Arrhenius Acid

c)

a Bronsted-Lowry base

d)

an Arrhenius base

77.
A substance that remains when a base has accepted an H+ ion is
a)

an acid

b)

a base

c)

a conjugate acid

d)

a conjugate base

78.

Which of these pKa values corresponds to the strongest acid?

a)

1.2

b)

1.4

c)

1.6

d)

1.8

79.

Which of these pKa values corresponds to the weakest (least strong) acid?

a)

5.6

b)

5.2

c)

4.8

d)

4.4

80.

Which of these Ka values corresponds to the weakest acid?

a)

4 x 10-4

b)

5 x 10-4

c)

6 x 10-4

d)

7 x 10-4

81.

Which of these Ka values corresponds to the strongest acid?

a)

4 x 10-4

b)

5 x 10-4

c)

6 x 10-4

d)

7 x 10-4

82.

The initial concentration of a weak monoprotic acid HA is 0.20M and the equilibrium concentration of H+ ions is 0.0019M. Calculate the Ka value for the weak acid.

a)

1.8x10-5

b)

1.8x10-15

c)

0.0019

d)

5.56x10-10

83.

Formic acid is a weak monoprotic acid. Calculate the Ka value if the initial acid concentration is 0.10M and the equilibrium concentration of H+ ions is 0.0042M.

a)

0.150

b)

12.56 x 10-6

c)

1.8 x 10-4

d)

0.042

e)

2.37

84.

Isobutlyamine is a weak base. If the initial concentration is 0.55M and the equilibrium concentration of OH- ions is 0.0040M, calculate the Kb value for isobutylamine.

a)

.055

b)

4.0x10-3

c)

1.6x10-5

d)

3.1x10-4

e)

2.9 x 10-5

85.

Uric acid is a weak monoprotic acid. Calculate the final concentration of uric acid if the initial concentration is 0.110M and the equilibrium concentration of H+ ions is 0.034M.

a)

.011

b)

.034

c)

.076

d)

1.47

86.

Calcuate the pH of a 0.30 M acetic acid solution. Acetic acid is a weak monoprotic acid with Ka = 1.8x10-5.

a)

5.26

b)

2.63

c)

11.37

d)

2.37

e)

None of these options are correct.

87.

Ammonia is a weak base. Calculate the pH of a solution with concentration is 0.150M. Kb = 1.7x10-5

a)

2.80

b)

11.20

c)

2.37

d)

5.59

e)

8.41

88.

Is the salt NaNO3 acidic, basic, or neutral?

a)

Acidic

b)

Basic

c)

Neutral

89.

Is the salt NaNO2 acidic, basic, or neutral?

a)

Acidic

b)

Basic

c)

Neutral

90.

Is the salt C5H5NHClO4 acidic, basic, or neutral?

a)

Acidic

b)

Basic

c)

Neutral

91.

Is the salt KOCl acidic, basic, or neutral?

a)

Acidic

b)

Basic

c)

Neutral

92.
Which of the following is a conjugate acid/base pair?
a)
HCl/OCl-
b)
H2SO4/SO42-
c)
NH4+/NH3
d)
H3O+/OH-
93.
Calculate the [H+] in a solution that has a pH of 2.73.
a)
5.4 x 10-12 M
b)
1.9 x 10-3 M
c)
2.7 M
d)
11.3 M
94.

Phenol, C6H5OH, has a Ka =1.0 x 10-10. What is the approximate pH of a 0.010 M solution of phenol?

a)

between 3-7

b)

10

c)

2

d)

between 7-10

e)

7

95.

What are the major species in an aqueous solution of HCl?

a)

H2O, H+, Cl-, OH-

b)

H+, Cl-, OH-

c)

H+, Cl-

d)

H2O, H+, Cl-

e)

H2O, H+

96.

HA, a weak acid, is partially dissociated in water into hydrogen ions and A- . Which of the following equation represents dissociation of HA, a weak acid, in water?

a)

HA(aq) ⇌ H- (aq) + A+ (aq)

b)

H- (aq) + A+ (aq) ⇌ HA(aq)

c)

HA(aq) ⇌ H+ (aq) + A- (aq)

d)

H+ (aq) + A- (aq) ⇌ HA(aq)

97.

B, a weak base, can react with water in equilibrium to form hydroxide ions and BH+. Which of the following equation represents dissociation of B, a weak base, in water?

a)

B(aq) + H2O(l) ⇌ BH+(aq) + OH- (aq)

b)

B(aq) + H2O(l) ⇌ BH+(aq) + H3O+ (aq)

c)

B(aq) + H3O+(aq) ⇌ BH+(aq) + H2O(l)

d)

B(aq) + OH-(aq) ⇌ BH+(aq) + O2-(aq)

98.

the following equation represents the equilibrium reaction between weak base, B, with water :


B(aq) + H2O(l) ⇌ BH+(aq) + OH-(aq)


The equilibrium constant for this reaction is represented by Kb . Which of the following equation represents expression of equilibrium constant, Kb?

a)
b)
c)
d)
99.
Rank the following in order of conjugate base strength.
   i.   H2CO3       Ka = 4.3 x 10-7
   ii.  NH4+          Ka = 5.6 x 10-10
   iii. HCNO        Ka = 3.5 x 10-4
a)
CO3-2 > NH3 > CNO-
b)
NH3 > CO3-2 > CNO-
c)
CNO- > CO3-2 > NH3
d)
CNO- > NH3 > CO3-2
100.

Which acid produces the strongest conjugate base?

a)

HClO4 (Ka= 1.0 x 107)

b)

HCN (Ka= 4.0 x 10-10)

c)

H3PO4 (Ka= 7.5 x 10-3)

d)

H2CO3 (Ka = 4.2 x 10-7)

101.

Which acid produces the strongest conjugate base?

a)

HClO4 (Ka= 1.0 x 107)

b)

HCN (Ka= 4.0 x 10-10)

c)

H3PO4

(Ka= 7.5 x 10-3)

d)

H2CO3

(Ka = 4.2 x 10-7)

102.

Which order lists the bases from the weakest to the strongest?

(Hint: strong acids = weak conjugate bases)

a)

BrO−, BrO2−, BrO3− , BrO4−

b)

BrO4−, BrO3− , BrO−, BrO2−

c)

BrO−, BrO2−, BrO4−, BrO3− ,

d)

BrO4−, BrO3− , BrO2−, BrO−

103.
What is the conjugate base of HCO3-?
a)
HCO3-
b)
H2CO3-
c)
H2CO3
d)
CO32-
104.
If a solution has a [H+] of 1.2 x 10-4M what is the [OH-]?
a)
8.3 x 10-4M 
b)
8.3 x 10-11M 
c)
1.2 x 1010M 
d)
1.2 x 10-4M 
105.
Which of the following is a conjugate acid/base pair?
a)
HCl/OCl-
b)
H2SO4/SO42-
c)
NH4+/NH3
d)
H3O+/OH-
106.

Ammonia, NH3, behaves as a base when placed in water according to the following equilibrium:

NH3(aq) + H2O(l) ⥨ NH4+(aq) + OH-(aq)

Calculate the pH of a 0.47M NH3 solution. (Kb = 1.8 x 10-5)

a)

2.54

b)

8.93

c)

5.07

d)

11.46

107.

Listed below are weak acids with their Ka values. Which of the following is the strongest acid?

a)

CH3COOH (Ka = 1.8 × 10–5)

b)

HF (Ka = 6.5 × 10–4)

c)

HCN (Ka = 6.3 × 10–10)

d)

HClO (Ka = 3.0 × 10–8)

108.

Listed below are weak acids along with the pKa. Which of the acids is the strongest?

a)

HF (pKa = 3.17)

b)

HCO3– (pKa = 10.32)

c)

H2PO4– (pKa = 7.18)

d)

NH4+ (pKa = 9.20)

109.

A 1.0 molar solution of a very weak monoprotic acid (HA) has a pH of 5. What is the value of Ka for the acid?

a)

1 × 10–10

b)

1 × 10–7

c)

1 × 10–5

d)

1 × 10–2

110.

Equal moles of the indicated acids are dissolved in the amounts of water shown in the beakers below. In which solution will the percent ionization of the acid be the lowest?

a)

Beaker A

b)

Beaker B

c)

Beaker C

d)

Impossible to tell from the information given.

111.

Which represents an acid with the smallest Ka value?

a)

HX

b)

HY

c)

HZ

112.

What is the pH of a 0.053 M solution of potassium hydroxide?

a)

6.91

b)

12.72

c)

7.33

d)

1.28

113.

Which of the following ions will act as a weak base in water?

a)

OH-1

b)

Cl-1

c)

NO3-1

d)

ClO-1

114.

A .1 M solution of ______ will have a pH of 7.00.

a)

NaNO3

b)

KF

c)

Na2S

d)

NaF

115.

Of the following, which is the strongest acid?

a)

HClO

b)

HClO2

c)

HClO3

d)

HClO4

116.

What is the conjugate acid of CO3-2?

a)

CO2-2

b)

HCO22-2

c)

H2CO3

d)

HCO3-1

117.

Z-1 is a weak base. An aqueous solution of Naz is prepared by dissolving 0.350 mol of NaZ in sufficient water to yield 1.0 L of solution. The pH of the solution was 8.93 at 25.0 0C. What is the Kb of the solution?

a)

1.2 x 10-5

b)

6.9 x 10-9

c)

2.1 x 10-10

d)

2.8 x 10-12

118.

What is the [H+] if the pH is 4.0?

a)

1.0 x 10-10 M

b)

1.0 x 10-4 M

c)

1.0 x 10-14 M

d)

1.0 x 10-7 M

119.
What is the pOH of a solution that has a pH of 2?
a)
10
b)
12
c)
14
d)
1
120.

A solution contains 0.040 M of a weak acid. Calculate the pH of the solution knowing that the Ka for the acid is 1.6 x 10-7

a)

It is not possible to solve if the identity of the acid is not known

b)

4.10

c)

4.90

d)

Because the Ka is very small, the pH is close to neutral (about 6)

121.
The Kw constant is:
a)
1.0 x 10-14
b)
1.0 x 1014
c)
6.022 x 1023
d)
6.0634 x 10-34
122.

What is the pKa of hydrocyanic acid, if its Ka is 4.9 x 10-10?

a)

6.50

b)

9.10

c)

9.31 

d)

5.40

123.

Given 0.10 M solutions of the four weak acids below all with 0.10 M concentration, which will have the greatest percent ionization?

HF (Ka = 7.2 x 10-4)

HNO2 (Ka = 4.0 x 10-4)

HCO2H (Ka = 1.8 x 10-4)

HC3H5O3 (Ka = 1.4 x 10-4)

a)

HF because its Ka is the largest.

b)

HF because its molar mass is the smallest.

c)

HC3H5O3 because its Ka is the smallest.

d)

HC3H5O3 because its molar mass is the greatest.

124.

Which of the following represents an acid with the lowest pH? Assume the solutions are the same concentration.

a)
b)
c)
125.

What are the major species in an aqueous solution of HNO2?

a)

H2O, H+, NO2-

b)

H+, NO2-, OH-

c)

H+, NO2-

d)

H2O, HNO2

e)

H2O, H+

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