Chapter 15 Review
Student: ___________________________________________________________________________
1.
Which is not a characteristic property of acids?
A. tastes sour
B. turns litmus from blue to red
C. reacts with metals to yield CO2 gas
D. neutralizes bases
E. reacts with carbonates to yield CO2 gas
2.
Which is the formula for the hydronium ion?
A. OHB. H2O
C. H3O+
D. H3OE. H2O+
3.
In the reaction H2CO3 + H2O
A. H2CO3 and H2O.
B. HCO3- and H2CO3.
C. H2O and H3O+.
D. H3O+ and H2CO3.
E. H2O and HCO3-.
4.
In the reaction HSO4-(aq) + OH-(aq)
HCO3- + H3O+, the Brønsted acids are
SO42-(aq) + H2O(l), the conjugate acid-base pairs
are
A. Row 1
B. Row 2
C. Row 3
D. Row 4
E. Row 5
5.
Identify the conjugate base of HPO42- in the reaction
HCO3- + HPO42A. H2O
B. HCO3C. H2CO3
D. PO43E. none of these
6.
Identify the conjugate base of HClO3 in the reaction
ClO3- + HSO4A. ClO3B. HSO4C. OHD. H3O+
E. SO42-
7.
H2CO3 + PO43-
HClO3 + SO42-
Identify the conjugate acid of SO42- in the reaction
CO32- + HSO4A. CO32B. HSO4C. OHD. H3O+
E. SO42-
HCO3- + SO42-
8.
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.
9.
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
10. 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.
11. 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
12. 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
13. 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
14. 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
15. 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
16. 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
17. 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
18. 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
19. 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
20. 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
21. Which one of these responses is true with regard to a 0.1 M solution of a weak acid HA?
A. [H+] > [A-]
B. pH = 1.0
C. [H+] < [A-]
D. pH > 1.0
E. [OH-] > [H+]
22. Acid strength decreases in the series HI > HSO4- > HF > HCN. Which of these anions is the weakest base?
A. IB. SO42C. FD. CN23. Acid strength increases in the series: HCN < HF < HSO4-. Which of these species is the strongest base?
A. H2SO4
B. SO42C. FD. CN E. HSO424. Acid strength decreases in the series: HNO3 > HF > CH3COOH. Which of these species is the strongest base?
A. NO3B. CH3COOC. FD. CH3COOH
25. Which of these acids is the strongest?
A. H2SeO3
B. H2TeO3
C. H2SO3
26. 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
27. 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
28. 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
29. Which one of these net ionic equations represents the reaction of a strong acid with a weak base?
A. H+(aq) + OH-(aq) → H O(aq)
2
B. H+(aq) + CH NH (aq) → CH NH +(aq)
3
2
3
3
C. OH-(aq) + HCN(aq) → H O(aq) + CN-(aq)
2
D. HCN(aq) + CH NH (aq) → CH NH + (aq)+ CN-(aq)
3
2
3
3
30. Which one of these net ionic equations represents the reaction of a strong acid with a strong base?
A. H+(aq) + OH-(aq) → H O(aq)
2
B. H+(aq) + CH NH (aq) → CH NH +(aq)
3
2
3
3
C. OH-(aq) + HCN(aq) → H O(aq) + CN-(aq)
2
D. HCN(aq) + CH NH (aq) → CH NH +(aq) + CN-(aq)
3
2
3
3
31. Which one of these equations represents the reaction of a weak acid with a weak base?
A. H+(aq) + OH-(aq) → H O(aq)
2
B. H+(aq) + CH NH (aq) → CH NH +(aq)
3
2
3
3
C. OH-(aq) + HCN(aq) → H O(aq) + CN-(aq)
2
D. HCN(aq) + CH NH (aq) → CH NH +(aq) + CN-(aq)
3
2
3
3
32. Which one of these equations represents the reaction of a weak acid with a strong base?
A. H+(aq) + OH-(aq) → H O(aq)
2
B. H+(aq) + CH NH (aq) → CH NH +(aq)
3
2
3
3
C. OH-(aq) + HCN(aq) → H O(aq) + CN-(aq)
2
D. HCN(aq) + CH NH (aq) → CH NH +(aq) + CN-(aq)
3
2
3
3
33. Predict the direction in which the equilibrium will lie for the reaction
H2CO3 + F-
HCO3- + HF.
Ka1( H2CO3) = 4.2 × 10-7; Ka(HF) = 7.1 × 10-4
A. to the right
B. to the left
C. in the middle
34. Predict the direction in which the equilibrium will lie for the reaction
H2SO4(aq).
H3PO4(aq) + HSO4-(aq)
H2PO4-(aq) +
H2SO3(aq) + HCO3- (aq)
HSO3-(aq) +
Ka1(H3PO4) = 7.5 × 10-3; Ka(H2SO4) = very large
A. to the right
B. to the left
C. in the middle
35. Predict the direction in which the equilibrium will lie for the reaction
H2CO3(aq).
Ka1(H2SO3) = 1 × 10-2; Ka1(H2CO3) = 4.2 × 10-7
A. to the right
B. to the left
C. in the middle
36. Which of the following yields a basic solution when dissolved in water?
A. NO2
B. P4O10
C. K2O
D. NaCl
E. SO2
37. Which of the following yields an acidic solution when dissolved in water?
A. NO2
B. LiOH
C. K2O
D. NaCl
E. Ca(OH)2
38. 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)
39. In the reaction CaO(s) + SO (g)
CaSO3(s),
2
A. O2- acts as a Lewis base, and SO2 acts as a Lewis acid.
B. Ca2+ acts as a Lewis base, and SO42- acts as a Lewis acid.
C. SO42- acts as a Lewis base, and SO2 acts as a Lewis acid.
D. SO2 acts as a Lewis base, and O2- acts as a Lewis acid.
E. SO2 acts as a Lewis base, and Ca2+ acts as a Lewis acid.
40. Which of these species will act as a Lewis acid?
A. NH3
B. NH4+
C. H2O
D. BF3
E. F41. Which of these species is a Lewis acid, but not a Brønsted acid?
A. HCN
B. CO32C. OHD. ClE. Al3+
42. Find the pH of a 0.135 M aqueous solution of periodic acid (HIO4), for which Ka = 2.3 × 10-2.
A. 1.25
B. 3.28
C. 1.17
D. 1.34
E. 1.64
43. For H3PO4, Ka1 = 7.3 × 10-3, Ka2 = 6.2 × 10-6, and Ka3 = 4.8 × 10-13. An aqueous solution of NaH2PO4 therefore would
be
A. neutral.
B. basic.
C. acidic.
44. For H3PO4, Ka1 = 7.3 × 10-3, Ka2 = 6.2 × 10-6, and Ka3 = 4.8 × 10-13. An aqueous solution of Na3PO4 therefore would be
A. neutral.
B. basic.
C. acidic.
45. An aqueous solution of KCl would be
A. neutral.
B. basic.
C. acidic.
46. Which one of these salts will form a neutral solution on dissolving in water?
A. NaCl
B. KNO2
C. NaCN
D. NH4NO3
E. FeCl3
47. Which one of these salts will form a basic solution on dissolving in water?
A. NaCl
B. KCN
C. NaNO3
D. NH4NO3
E. FeCl3
48. In 0.10 M KCN, the chemical species with the highest concentration (except H2O) is
A. Na+.
B. CN-.
C. H3O+(or H+).
D. OH-.
E. K+.
49. What is the pH of a 0.20 M solution of NH4Cl? [Kb(NH3) = 1.8 × 10-5]
A. 3.74
B. 4.98
C. 6.53
D. 9.02
E. 10.25
50. Consider the weak bases below and their Kb values:
Arrange the conjugate acids of these weak bases in order of increasing acid strength.
A. C5H5NH+ < C6H7OH < C2H5NH
B. C6H7OH < C5H5NH+ < C2H5NH
C. C5H5NH+ < C2H5NH3+ < C6H7OH
D. C6H7OH < C2H5NH3+< C5H5NH+
E. C2H5NH3+< C5H5NH+ < C6H7OH
51. Which response gives the products of hydrolysis of KF?
A. KOH + HF
B. OH- + HF
C. KOH + H+ + FD. KH + F- + OHE. No hydrolysis occurs.
52. Which one of these salts will form a basic solution upon dissolving in water?
A. NaCl
B. NaNO2
C. NH4NO3
D. KBr
E. AlCl3
53. Which one of the following salts will form an acidic solution on dissolving in water?
A. LiBr
B. NaF
C. KOH
D. FeCl3
E. NaCN
54. The equilibrium constant for the reaction
C6H5COOH(aq) + CH3COO-(aq)
C6H5COO-(aq) + CH3COOH(aq)
-5
is 3.6 at 25°C. If Ka for CH3COOH is 1.8 × 10 , what is the acid dissociation constant for C6H5COOH?
A. 5.0 × 10-6
B. 6.5 × 10-5
C. 2.3 × 10-4
D. 8.3 × 10-5
E. 5.6 ×10-6
Chapter 15 Review Key
1.
Which is not a characteristic property of acids?
A. tastes sour
B. turns litmus from blue to red
C. reacts with metals to yield CO2 gas
D. neutralizes bases
E. reacts with carbonates to yield CO2 gas
Difficulty: Easy
Raymond - 015 Acids... #1
2.
Which is the formula for the hydronium ion?
A. OHB. H2O
C. H3O+
D. H3OE. H2O+
Difficulty: Easy
Raymond - 015 Acids... #2
3.
In the reaction H2CO3 + H2O
A. H2CO3 and H2O.
B. HCO3- and H2CO3.
C. H2O and H3O+.
D. H3O+ and H2CO3.
E. H2O and HCO3-.
HCO3- + H3O+, the Brønsted acids are
Difficulty: Easy
Raymond - 015 Acids... #3
4.
In the reaction HSO4-(aq) + OH-(aq)
are
A.
B.
C.
D.
E.
5.
SO42-(aq) + H2O(l), the conjugate acid-base pairs
Row 1
Row 2
Row 3
Row 4
Row 5
Identify the conjugate base of HPO42- in the reaction
A.
B.
C.
D.
E.
HCO3- + HPO42H2O
HCO3H2CO3
PO43none of these
Difficulty: Medium
Raymond - 015 Acids... #4
H2CO3 + PO43-
Difficulty: Medium
Raymond - 015 Acids... #5
6.
Identify the conjugate base of HClO3 in the reaction
A.
B.
C.
D.
E.
ClO3- + HSO4ClO3HSO4OHH3O+
SO42-
HClO3 + SO42-
Difficulty: Medium
Raymond - 015 Acids... #9
7.
Identify the conjugate acid of SO42- in the reaction
A.
B.
C.
D.
E.
CO32- + HSO4CO32HSO4OHH3O+
SO42-
HCO3- + SO42-
Difficulty: Medium
Raymond - 015 Acids... #10
8.
9.
10.
11.
12.
13.
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.
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
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.
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
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
Determine the pH of a KOH solution made by mixing 0.251 g KOH with enough water to make
solution.
A. 1.35
B. 2.35
C. 7.00
D. 11.65
E. 12.65
Difficulty: Medium
Raymond - 015 Acids... #13
Difficulty: Easy
Raymond - 015 Acids... #16
Difficulty: Medium
Raymond - 015 Acids... #17
Difficulty: Medium
Raymond - 015 Acids... #20
Difficulty: Medium
Raymond - 015 Acids... #22
1.00 × 102 mL of
Difficulty: Medium
Raymond - 015 Acids... #28
14.
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
Difficulty: Medium
Raymond - 015 Acids... #29
15.
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
Difficulty: Medium
Raymond - 015 Acids... #37
16.
17.
18.
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
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
Diet cola drinks have a pH of about 3.0, while milk has a pH of about 7.0. How many times
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
Difficulty: Medium
Raymond - 015 Acids... #40
Difficulty: Medium
Raymond - 015 Acids... #46
greater is the H3O+
Difficulty: Medium
Raymond - 015 Acids... #47
19.
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
Difficulty: Medium
Raymond - 015 Acids... #52
20.
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
Difficulty: Medium
Raymond - 015 Acids... #54
21.
Which one of these responses is true with regard to a 0.1 M solution of a weak acid HA?
A. [H+] > [A-]
B. pH = 1.0
C. [H+] < [A-]
D. pH > 1.0
E. [OH-] > [H+]
Difficulty: Medium
Raymond - 015 Acids... #55
22.
23.
Acid strength decreases in the series HI > HSO4- > HF > HCN. Which of these anions is the weakest base?
A. IB. SO42C. FD. CN-
-.
Difficulty: Medium
Raymond - 015 Acids... #56
Acid strength increases in the series: HCN < HF < HSO4 Which of these species is the strongest base?
A. H2SO4
B. SO42C. FD. CN E. HSO4Difficulty: Medium
Raymond - 015 Acids... #58
24.
Acid strength decreases in the series: HNO3 > HF > CH3COOH. Which of these species is the strongest base?
A. NO3B. CH3COOC. FD. CH3COOH
Difficulty: Medium
Raymond - 015 Acids... #60
25.
Which of these acids is the strongest?
A. H2SeO3
B. H2TeO3
C. H2SO3
Difficulty: Medium
Raymond - 015 Acids... #61
26.
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
Difficulty: Medium
Raymond - 015 Acids... #62
27.
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
Difficulty: Medium
Raymond - 015 Acids... #64
28.
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
Difficulty: Medium
Raymond - 015 Acids... #66
29.
Which one of these net ionic equations represents the reaction of a strong acid with a weak base?
A. H+(aq) + OH-(aq) → H O(aq)
2
B. H+(aq) + CH NH (aq) → CH NH +(aq)
3
2
3
3
C. OH-(aq) + HCN(aq) → H O(aq) + CN-(aq)
2
D. HCN(aq) + CH NH (aq) → CH NH + (aq)+ CN-(aq)
3
2
3
3
Difficulty: Medium
Raymond - 015 Acids... #67
30.
Which one of these net ionic equations represents the reaction of a strong acid with a strong base?
A. H+(aq) + OH-(aq) → H O(aq)
2
B. H+(aq) + CH NH (aq) → CH NH +(aq)
3
2
3
3
C. OH-(aq) + HCN(aq) → H O(aq) + CN-(aq)
2
D. HCN(aq) + CH NH (aq) → CH NH +(aq) + CN-(aq)
3
2
3
3
Difficulty: Medium
Raymond - 015 Acids... #68
31.
Which one of these equations represents the reaction of a weak acid with a weak base?
A. H+(aq) + OH-(aq) → H O(aq)
2
B. H+(aq) + CH NH (aq) → CH NH +(aq)
3
2
3
3
C. OH-(aq) + HCN(aq) → H O(aq) + CN-(aq)
2
D. HCN(aq) + CH NH (aq) → CH NH +(aq) + CN-(aq)
3
2
3
3
Difficulty: Medium
Raymond - 015 Acids... #69
32.
Which one of these equations represents the reaction of a weak acid with a strong base?
A. H+(aq) + OH-(aq) → H O(aq)
2
B. H+(aq) + CH NH (aq) → CH NH +(aq)
3
2
3
3
C. OH-(aq) + HCN(aq) → H O(aq) + CN-(aq)
2
D. HCN(aq) + CH NH (aq) → CH NH +(aq) + CN-(aq)
3
2
3
3
33.
Predict the direction in which the equilibrium will lie for the reaction
H2CO3 + F-
Difficulty: Medium
Raymond - 015 Acids... #70
HCO3- + HF.
Ka1( H2CO3) = 4.2 × 10-7; Ka(HF) = 7.1 × 10-4
A. to the right
B. to the left
C. in the middle
34.
Predict the direction in which the equilibrium will lie for the reaction
H2SO4(aq).
H3PO4(aq) +
Difficulty: Medium
Raymond - 015 Acids... #71
HSO4-(aq)
H2PO4-(aq) +
H2SO3(aq) +
Difficulty: Medium
Raymond - 015 Acids... #72
HCO3- (aq)
HSO3-(aq) +
Ka1(H3PO4) = 7.5 × 10-3; Ka(H2SO4) = very large
A. to the right
B. to the left
C. in the middle
35.
Predict the direction in which the equilibrium will lie for the reaction
H2CO3(aq).
Ka1(H2SO3) = 1 × 10-2; Ka1(H2CO3) = 4.2 × 10-7
A. to the right
B. to the left
C. in the middle
Difficulty: Medium
Raymond - 015 Acids... #73
36.
Which of the following yields a basic solution when dissolved in water?
A. NO2
B. P4O10
C. K2O
D. NaCl
E. SO2
Difficulty: Medium
Raymond - 015 Acids... #76
37.
Which of the following yields an acidic solution when dissolved in water?
A. NO2
B. LiOH
C. K2O
D. NaCl
E. Ca(OH)2
Difficulty: Medium
Raymond - 015 Acids... #77
38.
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)
Difficulty: Medium
Raymond - 015 Acids... #78
39.
In the reaction CaO(s) + SO2(g)
CaSO3(s),
A. O2- acts as a Lewis base, and SO2 acts as a Lewis acid.
B. Ca2+ acts as a Lewis base, and SO42- acts as a Lewis acid.
C. SO42- acts as a Lewis base, and SO2 acts as a Lewis acid.
D. SO2 acts as a Lewis base, and O2- acts as a Lewis acid.
E. SO2 acts as a Lewis base, and Ca2+ acts as a Lewis acid.
Difficulty: Medium
Raymond - 015 Acids... #80
40.
Which of these species will act as a Lewis acid?
A. NH3
B. NH4+
C. H2O
D. BF3
E. FDifficulty: Medium
Raymond - 015 Acids... #81
41.
42.
Which of these species is a Lewis acid, but not a Brønsted acid?
A. HCN
B. CO32C. OHD. ClE. Al3+
Find the pH of a 0.135 M aqueous solution of periodic acid (HIO4), for which Ka = 2.3 × 10-2.
A. 1.25
B. 3.28
C. 1.17
D. 1.34
E. 1.64
Difficulty: Medium
Raymond - 015 Acids... #82
Difficulty: Medium
Raymond - 015 Acids... #83
43.
For H3PO4, Ka1 = 7.3 × 10-3, Ka2 = 6.2 × 10-6, and Ka3 = 4.8 × 10-13. An aqueous solution of NaH2PO4 therefore would
be
A. neutral.
B. basic.
C. acidic.
Difficulty: Medium
Raymond - 015 Acids... #90
44.
For H3PO4, Ka1 = 7.3 × 10-3, Ka2 = 6.2 × 10-6, and Ka3 = 4.8 × 10-13. An aqueous solution of Na3PO4 therefore would
be
A. neutral.
B. basic.
C. acidic.
Difficulty: Medium
Raymond - 015 Acids... #91
45.
An aqueous solution of KCl would be
A. neutral.
B. basic.
C. acidic.
Difficulty: Medium
Raymond - 015 Acids... #92
46.
Which one of these salts will form a neutral solution on dissolving in water?
A. NaCl
B. KNO2
C. NaCN
D. NH4NO3
E. FeCl3
Difficulty: Medium
Raymond - 015 Acids... #93
47.
Which one of these salts will form a basic solution on dissolving in water?
A. NaCl
B. KCN
C. NaNO3
D. NH4NO3
E. FeCl3
Difficulty: Medium
Raymond - 015 Acids... #94
48.
49.
In 0.10 M KCN, the chemical species with the highest concentration (except H2O) is
A. Na+.
B. CN-.
C. H3O+(or H+).
D. OH-.
E. K+.
What is the pH of a 0.20 M solution of NH4Cl? [Kb(NH3) = 1.8 × 10-5]
A. 3.74
B. 4.98
C. 6.53
D. 9.02
E. 10.25
Difficulty: Medium
Raymond - 015 Acids... #95
Difficulty: Medium
Raymond - 015 Acids... #96
50.
Consider the weak bases below and their Kb values:
Arrange the conjugate acids of these weak bases in order of increasing acid strength.
A. C5H5NH+ < C6H7OH < C2H5NH
B. C6H7OH < C5H5NH+ < C2H5NH
C. C5H5NH+ < C2H5NH3+ < C6H7OH
D. C6H7OH < C2H5NH3+< C5H5NH+
E. C2H5NH3+< C5H5NH+ < C6H7OH
Difficulty: Medium
Raymond - 015 Acids... #98
51.
Which response gives the products of hydrolysis of KF?
A. KOH + HF
B. OH- + HF
C. KOH + H+ + FD. KH + F- + OHE. No hydrolysis occurs.
Difficulty: Medium
Raymond - 015 Acids... #100
52.
Which one of these salts will form a basic solution upon dissolving in water?
A. NaCl
B. NaNO2
C. NH4NO3
D. KBr
E. AlCl3
Difficulty: Medium
Raymond - 015 Acids... #101
53.
54.
Which one of the following salts will form an acidic solution on dissolving in water?
A. LiBr
B. NaF
C. KOH
D. FeCl3
E. NaCN
The equilibrium constant for the reaction
C6H5COOH(aq) + CH3COO-(aq)
-5
is 3.6 at 25°C. If Ka for CH3COOH is 1.8 × 10 , what is the acid dissociation constant
A. 5.0 × 10-6
B. 6.5 × 10-5
C. 2.3 × 10-4
D. 8.3 × 10-5
E. 5.6 ×10-6
Difficulty: Medium
Raymond - 015 Acids... #104
C6H5COO-(aq) + CH3COOH(aq)
for C6H5COOH?
Difficulty: Medium
Raymond - 015 Acids... #110
Chapter 15 Review Summary
Category
Difficulty: Easy
Difficulty: Medium
Raymond - 015 Acids...
# of Questions
4
50
54