Chapter 10 Acids and Bases
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Chapter 10 Acids and Bases
1) Which statement concerning Arrhenius acid-base theory is not correct?
A) An Arrhenius acid produces hydrogen ions in water solution.
B) An Arrhenius base produces hydroxide ions in water solution.
C) A neutralization reaction produces water plus a salt.
D) Acid-base reactions must take place in aqueous solution.
E) none of the above
Answer: E
Diff: 1
Section: 10.1
2) The H3O+ ion is called the ______ion.
A) hydroxide
B) hydronium
C) hydrogen
D) protium
E) water
Answer: B
Diff: 1
Section: 10.1
3) When acids and bases react the product other than water is a
A) hydrogen ion.
B) hydroxide ion.
C) hydronium ion.
D) metal.
E) salt.
Answer: E
Diff: 1
Section: 10.1
4) Which of the following compounds is a salt?
A) HBr
B) KNO3
C) H2SO4
D) NaOH
E) C6H12O6
Answer: B
Diff: 1
Section: 10.1
5) Which of the following compounds is a salt?
A) CH3CO2H
B) NH3
C) NH4NO3
D) Al(OH)3
E) C6H6
Answer: C
Diff: 1
Section: 10.1
6) Which compound is manufactured in larger quantities in the U.S. than any other industrial chemical?
A) HCl
B) HNO3
C) H3PO4
D) H2SO4
E) NaOH
Answer: D
Diff: 1
Section: 10.2
7) Which pair of compounds is used in the manufacture of fertilizers?
A) HCl and NaOH
B) HCl and H3PO4
C) HNO3 and HCl
D) H2SO4 and H3PO4
E) HNO3 and NaOH
Answer: D
Diff: 1
Section: 10.2
8) A Brønsted-Lowry acid is a substance which
A) produces hydrogen ions in aqueous solution.
B) produces hydroxide ions in aqueous solution.
C) donates protons to other substances.
D) accepts protons from other substances.
E) accepts hydronium ions from other substances.
Answer: C
Diff: 1
Section: 10.3
9) A Brønsted-Lowry base is a substance which
A) produces hydrogen ions in aqueous solution.
B) produces hydroxide ions in aqueous solution.
C) donates protons to other substances.
D) accepts protons from other substances.
E) accepts hydronium ions from other substances.
Answer: D
Diff: 1
Section: 10.3
10) A necessary requirement for a Brønsted base is
A) the presence of water as a reaction medium.
B) the presence of hydroxide in its formula.
C) a lone pair of electrons in its Lewis dot structure.
D) the production of hydronium ion upon reaction with water.
E) the presence of a metal ion in its formula.
Answer: C
Diff: 1
Section: 10.3
11) The base forms a new ______bond in a Brønsted-Lowry acid-base reaction.
A) covalent
B) aquo
C) hydrogen
D) ionic
E) metallic
Answer: A
Diff: 1
Section: 10.3
12) Which of the following is a diprotic acid?
A) acetic acid
B) hydrochloric acid
C) phosphoric acid
D) sulfuric acid
E) nitric acid
Answer: D
Diff: 1
Section: 10.3
13) What is the conjugate base of HSO4-?
A) SO42-
B) H2SO4
C) H3O+
D) OH-
E) H2SO3
Answer: A
Diff: 1
Section: 10.3
14) According to Brønsted-Lowry theory, acid-base reactions can be described as ______reactions.
A) electrolytic
B) electron transfer
C) gas phase
D) nuclear transfer
E) proton transfer
Answer: E
Diff: 2
Section: 10.3
15) C5H5N + H2CO3 C5H6 N+ + HCO3-
In the reaction shown, the conjugate acid of C5H5N is ______.
A) C5H5N
B) H2CO3
C) C5H6N+
D) HCO3-
E) H3O+
Answer: C
Diff: 2
Section: 10.3
16) CH3NH2 + HCl CH3NH3+ + Cl-
A conjugate acid-base pair in the reaction shown is ______and ______.
A) CH3NH2 and HCl
B) CH3NH2 and Cl-
C) CH3NH3+ and Cl-
D) HCl and Cl-
E) HCl and H3O+
Answer: D
Diff: 2
Section: 10.3
17) Consider the following reaction: NO2- + HCO3- CO3-2 + HNO2
Identify the acid, base, conjugate acid and conjugate base.
Answer: Acid: HCO3- ; Conjugate Base: CO3-2 ; Base: NO2- ; Conjugate Acid: HNO2
Diff: 2
Section: 10.3 and 10.12
18) Consider the reaction: H2SO3 + HCO3- H2CO3 + HSO3-
a) Identify the acid, base, conjugate acid and conjugate base
b) Identify two substances from the reaction which could be used to prepare a buffer.
Answer: a) Acid: H2SO3; Conjugate Base: HSO3-; Base: HCO3- ; Conjugate Acid: H2CO3
b) Buffers: either conjugate acid base pair
Diff: 2
Section: 10.3 and 10.12
19) Which of the following cannot act as a Brønsted base?
A) HCO3-
B) CO32-
C) NH3
D) NH2-
E) NH4+
Answer: E
Diff: 2
Section: 10.3
20) In the following equation, which of the following is acting as the Bronsted acid?
HClO4 + H2O --> ClO4- + H3O+
A) HClO4
B) H2O
C) ClO4-
D) H3O+
Answer: A
Diff: 1
Section: 10.3
21) Which of the following is a triprotic acid?
A) H3PO4
B) CH3COOH
C) HNO3
D) NH3
E) Al(OH)3
Answer: A
Diff: 3
Section: 10.3
22) Ammonia reacts with acids because
A) it contains the hydroxide group.
B) it is neutral.
C) it is itself an acid.
D) it is a salt.
E) it contains a lone pair of electrons.
Answer: E
Diff: 3
Section: 10.3
23) What is the conjugate acid of HSO4-?
A) SO42-
B) H2SO4
C) H3O+
D) OH-
E) H2SO3
Answer: B
Diff: 3
Section: 10.3
24) Water and HSO4- can either accept protons or donate protons. Such substances are said to be
A) amphoteric.
B) conjugate.
C) diprotic.
D) monoprotic.
E) triprotic.
Answer: A
Diff: 2
Section: 10.3
25) Which statement is correct for pure water?
A) Pure water contains equal amounts of hydroxide, [OH-], and hydronium, [H3O+], ions.
B) Pure water contains larger amounts of hydroxide, [OH-], ions than hydronium, [H3O+], ions.
C) Pure water contains larger amounts of hydronium, [H3O+], ions than hydroxide,
[OH-], ions.
D) Pure water is an electrolyte.
E) Pure water contains no ions.
Answer: A
Diff: 3
Section: 10.3
26) Acetic acid is a weak acid in water because it is
A) dilute.
B) only slightly soluble.
C) unable to hold onto its hydrogen ion.
D) only slightly dissociated into ions.
E) completely dissociated into hydronium ions and acetate ions.
Answer: D
Diff: 1
Section: 10.4
27) The classification of an acid or a base as weak or strong is determined by
A) the solubility of the acid or base.
B) the extent of dissociation of the dissolved acid or base.
C) the concentrations of the acid or base.
D) more than one choice is correct.
Answer: B
Diff: 1
Section: 10.4
28) Hydrogen cyanide, HCN, is a weak acid. Which equation best represents its aqueous chemistry?
A) HCN (aq) + H2O (l) CN- (aq) + H3O+ (aq)
B) HCN (aq) + H2O (l) H2CN+ (aq) + OH- (aq)
C) HCN (aq) H+ (aq) + CN- (aq)
D) HCN (aq) H- (aq) + CN+ (aq)
E) H2O (l) H+ (aq) + OH- (aq)
Answer: A
Diff: 1
Section: 10.4
29) Which of the following is a strong acid?
A) HNO3
B) H3PO4
C) NH4+
D) HCO3-
E) H2O
Answer: A
Diff: 2
Section: 10.4
30) Which of the following is a weak acid?
A) HNO3
B) H3PO4
C) NH3
D) HCl
E) OH-
Answer: B
Diff: 3
Section: 10.4
31) Which reaction best illustrates the behavior of the weak base H2PO4- in aqueous solution?
A) H2PO4- (aq) + H2O (l) HPO42- (aq) + H3O+ (aq)
B) H2PO4- (aq) + H2O (l) H3PO4 (aq) + OH- (aq)
C) H2PO4- (aq) 2H+ (aq) + PO43- (aq)
D) H2PO4- (aq) H+ (aq) + HPO42- (aq)
E) H2PO4- (aq) + H+ (aq) H3PO4 (aq)
Answer: B
Diff: 3
Section: 10.4
32) Which one of the following is the weakest acid?
A) HCN(Ka = 4.9 × 10-10)
B) HClO(Ka = 3.0 × 10-8)
C) HNO2(Ka = 4.5 × 10-4)
D) HF(Ka = 6.8 × 10-4)
Answer: A
Diff: 2
Section: 10.5
33) Which one of the following is the strongest weak acid?
A) HCN(Ka = 4.9 × 10-10)
B) HClO(Ka = 3.0 × 10-8)
C) HNO2(Ka = 4.5 × 10-4)
D) HF(Ka = 6.8 × 10-4)
Answer: D
Diff: 3
Section: 10.5
34) Which compound has a very large value of Ka in aqueous solution?
A) NaCl
B) HNO3
C) H3PO4
D) KOH
E) NH3
Answer: B
Diff: 2
Section: 10.5
35) Which compound has a value of Ka that is close to 10-5?
A) NaCl
B) HNO3
C) CH3CH2CO2H
D) KOH
E) NH3
Answer: C
Diff: 2
Section: 10.5
36) At 25°C, the value of Kw is ______.
A) 1.00
B) 1.00 × 10-7
C) 1.00 × 10-14
D) 1.00 × 107
E) 1.00 × 1014
Answer: C
Diff: 2
Section: 10.6
37) What is the conjugate base of water?
A) H2O (l)
B) H3O+ (aq)
C) OH- (aq)
D) H+ (aq)
E) O2- (aq)
Answer: C
Diff: 2
Section: 10.6
38) What is the conjugate acid of water?
A) H2O (l)
B) H3O+ (aq)
C) OH- (aq)
D) H+ (aq)
E) O2- (aq)
Answer: B
Diff: 2
Section: 10.6
39) Which solution is basic?
A) [H3O+] = 1.0 × 10-4
B) [H3O+] = 1.0 × 10-7
C) [H3O+] = 1.0 × 10-10
D) [OH-] = 1.0 × 10-7
E) [OH-] = 1.0 × 10-10
Answer: C
Diff: 1
Section: 10.7
40) In an aqueous solution that is basic, [H3O+] is ______than 1.0 × 10-7 and ______than [OH-].
A) greater; less
B) less; greater
C) greater; greater
D) less; less
E) none of the above
Answer: D
Diff: 1
Section: 10.7
41) Which example is not acidic?
A) orange juice
B) soil for azaleas with pH of 4.8
C) a solution of NH4NO3 with pH < 7.00
D) lake water that turns blue litmus to red
E) a solution in which [H3O+] = 1.00 × 10-7
Answer: E
Diff: 1
Section: 10.7
42) An increase in solution pH corresponds to
A) an increase in hydronium ion concentration.
B) a decrease in hydronium ion concentration.
C) no change in hydronium ion concentration.
D) a decrease in hydroxide ion concentration.
Answer: B
Diff: 1
Section: 10.7
43) Which example is not basic?
A) shampoo
B) vinegar
C) window cleaner
D) limewater
E) Mg(OH)2, used in remedies for upset stomach
Answer: B
Diff: 1
Section: 10.7
44) If the concentration of OH- in an aqueous solution is 1.4 × 10-7 M, the concentration of H3O+ is ______.
A) 7.1 × 10+6 M
B) 1.0 × 10-7 M
C) 1.4 × 10-7 M
D) 7.1 × 10-8 M
E) 1.3 × 10-8 M
Answer: D
Diff: 2
Section: 10.8
45) If the concentration of H3O+ in an aqueous solution is 7.6 × 10-9 M, the concentration of OH- is ______.
A) 7.6 × 10-23 M
B) 1.3 × 10+8 M
C) 6.4 × 10-5 M
D) 1.3 × 10-6 M
E) 7.6 × 10-9 M
Answer: D
Diff: 2
Section: 10.8
46) In an aqueous solution that is acidic, [H3O+] is ______than 1.0 × 10-7 and ______than [OH-].
A) greater; less
B) less; greater
C) greater; greater
D) less; less
E) none of the above
Answer: C
Diff: 2
Section: 10.8
47) Which of the following statements is correct?
A) In an acidic solution, [H3O+] < 10-7; [OH-] < 10-7.
B) In an acidic solution, [H3O+] > 10-7; [OH-] > 10-7.
C) In an acidic solution, [H3O+] > 10-7; [OH-] < 10-7.
D) In an acidic solution, [H3O+] < 10-7; [OH-] > 10-7.
E) In an acidic solution, [H3O+] > 10-7; [OH-] = 10-7.
Answer: C
Diff: 2
Section: 10.8
48) If the [H+] of a water sample is 1 × 10-4 M, the [OH-] is
A) 1 × 10-4 M.
B) 1 × 10-14 M.
C) 1 × 104 M.
D) 1 × 10-10 M.
E) none of the above
Answer: D
Diff: 2
Section: 10.8
49) If the concentration of OH- is 1 × 10-2 M, the concentration of H3O+ is ______M.
A) 1 × 100
B) 1 × 10-2
C) 1 × 10-7
D) 1 × 10-12
E) 1 × 10-14
Answer: D
Diff: 3
Section: 10.8
50) If the concentration of H3O+ is 3.5 × 10-3 M, the concentration of OH- is ______M.
A) 2.9 × 10-12
B) 1.0 × 10-12
C) 1.0 × 10-7
D) 3.5 × 10-11
E) 10.5 × 10-3
Answer: A
Diff: 3
Section: 10.8
51) Which of the following statements is correct?
A) In a basic solution, [H3O+] < 10-7; [OH-] < 10-7.
B) In a basic solution, [H3O+] > 10-7; [OH-] > 10-7.
C) In a basic solution, [H3O+] > 10-7; [OH-] < 10-7.
D) In a basic solution, [H3O+] < 10-7; [OH-] > 10-7.
E) In a basic solution, [H3O+] > 10-7; [OH-] = 10-7.
Answer: D
Diff: 3
Section: 10.8
52) The pH of a cup of coffee is measured as 5.45. Express this measurement as [H+], using the correct number of significant figures.
A) 3.548 × 10-6 M
B) 3.55 × 10-6 M
C) 3.5 × 10-6 M
D) 4 × 10-6 M
E) 2.82 × 105 M
Answer: C
Diff: 1
Section: 10.8
53) What is the value of [H3O+] in a solution with pH = 10.82?
A) 6.6 × 10-4 M
B) 1.5 × 10-11 M
C) 1.03 M
D) 10.82 M
E) 3.18 M
Answer: B
Diff: 2
Section: 10.8
54) The pH of a solution with [H3O+] = 5.9 × 10-3 M, to the correct number of significant figures, is ______.
A) 5.9 × 10-3
B) 2.2
C) 2.23
D) 1.01
E) 2.229
Answer: C
Diff: 2
Section: 10.8
55) If the [H3O+] of a water sample is 1 × 10-4 M, the pH of the sample is ______, and the sample is ______.
A) -4; acidic
B) 4; acidic
C) 4; basic
D) 10; basic
E) -10; basic
Answer: B
Diff: 3
Section: 10.8
56) What is the pH of a solution in which [H3O+] = 1.2 × 10-3 M?
A) 1.20
B) 2.92
C) 11.08
D) 12.80
E) 8.33 × 10-12
Answer: B
Diff: 3
Section: 10.8
57) What is the pH of a solution in which [H3O+] = 3.8 × 10-8 M?
A) 7.42
B) 6.58
C) 3.80
D) 1.0 × 10-8
E) 2.6 × 10-7
Answer: A
Diff: 3
Section: 10.8
58) What is the pH of a solution in which the hydrogen ion concentration is 5.1 × 10-8 M?
A) 6.71
B) 1.96 × 10-7
C) 8.90
D) 5.10
E) 7.29
Answer: E
Diff: 3
Section: 10.8
59) What is the pH of a solution in which [H3O+] = 4.1 × 10-2 M?
A) 12.61
B) 1.39
C) 1.10
D) 12.90
E) 4.10
Answer: B
Diff: 3
Section: 10.8
60) What is the hydrogen ion concentration in a solution with pH = 2.34?
A) 4.57 × 10-3 M
B) 2.34 × 10-3 M
C) 2.19 × 10-12 M
D) 1.17 × 101 M
E) 4.27 × 10-12 M
Answer: A
Diff: 3
Section: 10.8
61) Calculate the hydrogen ion concentration in a solution with pH = 6.35.
A) 7.65 M
B) 6.35 M
C) 4.5 × 10-7 M
D) 0.80 M
E) 2.2 × 10-8 M
Answer: C
Diff: 3
Section: 10.8
62) What is the [H3O+] in a solution with pH = 11.61?
A) 1.16 × 10+1 M
B) 2.39 × 10+1 M
C) 4.07 × 10-3 M
D) 1.00 × 10-14 M
E) 2.45 × 10-12 M
Answer: E
Diff: 3
Section: 10.8
63) The [OH-] and the pH of 0.035 M KOH at 25°C are, respectively,
A) 0.035 M and +1.46.
B) 0.035 M and -1.46.
C) 2.9 × 10-13 M and -12.54.
D) 0.035 and +12.54.
E) 2.9 × 10-13 M and +12.54.
Answer: D
Diff: 3
Section: 10.8
64) Which of the following pH's corresponds to a strongly basic solution?
A) 11.5
B) 2.7
C) 6.9
D) 7.4
E) 4.3
Answer: A
Diff: 1
Section: 10.8
65) Which of the following pH's corresponds to a neutral solution?
A) 7.0
B) 1.8
C) 6.2
D) 8.5
E) 14.0
Answer: A
Diff: 3
Section: 10.8
66) Which of the following pH's corresponds to a weakly acidic solution?
A) 5.3
B) 1.4
C) 7.8
D) 9.2
E) 11.5
Answer: A
Diff: 3
Section: 10.8
67) To prepare a buffer using sodium phosphate, which of the following would also be needed?
A) hydrochloric acid
B) ammonium hydroxide
C) ammonium phosphate
D) phosphoric acid
E) sodium hydroxide
Answer: D
Diff: 1
Section: 10.10
68) A buffer solution
A) is a salt solution.
B) maintains pH at 7.00.
C) is a strong base.
D) neutralizes only acids.
E) closely maintains its original pH.
Answer: E
Diff: 2
Section: 10.10
69) The pH of a 250. mL sample of a buffer solution is 9.85. If 1.0 mL of 6 M HCl is added, the pH of the resulting mixture is closest to ______.
A) 0.00
B) 1.65
C) 7.00
D) 9.70
E) 10.00
Answer: D
Diff: 3
Section: 10.10
70) Which of the following solutions is a buffer?
A) a solution of acetic acid and sodium acetate
B) a solution of acetic acid and sodium sulfate
C) a solution of hydrochloric acid and sodium sulfate
D) a solution of hydrochloric acid and sodium acetate
E) a solution of sulfuric acid and sodium sulfate
Answer: A
Diff: 3
Section: 10.10
71) All of the following species are involved in the blood buffer system except ______.
A) CO2
B) H2CO3
C) HCO3-
D) CO32-
E) none of the above
Answer: E
Diff: 1
Section: 10.10
72) Which of these, if dissolved in 1.0 L of pure water, would produce a buffer solution?
A) 0.1 mol NaCl + 0.1 mol KCl
B) 0.1 mol H3O+ + 0.1 OH-
C) 0.1 mol NaH2PO4 + 0.1 mol Na2HPO4
D) 0.1 mol HCl + 0.1 mol NaOH
E) 0.1 mol H3O+ + 0.1 mol Cl-
Answer: C
Diff: 2
Section: 10.10
73) All of the statements regarding equivalents of acids and bases are true except
A) equivalents are the same as moles.
B) equivalents of acid are based on the number of hydrogen ions produced per formula unit of acid.
C) equivalents are used to determine normality of solutions.
D) the equivalent weight of a base is the weight that produces one mole of hydroxide ions.
E) one equivalent of any acid will neutralize one equivalent of any base.
Answer: A
Diff: 2
Section: 10.11
74) What is the normality of a solution containing 49 g of H2SO4 in enough water to make 400 mL of solution?
A) 2.5 N
B) 5.0 N
C) 1.0 N
D) 10 N
E) 0.20 N
Answer: A
Diff: 2
Section: 10.11
75) The normality of a solution prepared by dissolving 25.0 g of Ca(OH)2 in water to make 250. mL solution is ______N.
A) 2.70
B) 1.35
C) 0.675
D) 3.51
E) 1.75
Answer: A
Diff: 2
Section: 10.11
76) The normality of a solution prepared by dissolving 50.0 g of Ca(OH)2 in water to make 250. mL solution is ______N.
A) 1.35
B) 2.70
C) 3.51
D) 5.40
E) 7.02
Answer: D
Diff: 2
Section: 10.11
77) Explain the term "amphoteric." Use the hydrogen carbonate ion, HCO3- to illustrate amphoteric behavior.
Answer: An amphoteric compound or ion is one that can behave either as an acid or a base in solution, depending on the chemical environment. In reaction (1), it acts as an acid by donating a hydrogen ion. In reaction (2), it acts as a base by accepting the hydrogen ion.
(1) HCO3- (aq) + H2O (l) HCO+ (aq) + CO32- (aq)
(2) HCO3- (aq) + H2O (l) H2CO3 (aq) + OH- (aq)
Diff: 3
Section: 10.12
78) What is the normality of a solution containing 100. g HNO3 in 500. mL of solution?
A) 1.26 N
B) 1.59 N
C) 3.17 N
D) 0.500 N
E) 0.630 N
Answer: C
Diff: 3
Section: 10.11
79) What is the normality of a solution prepared by dissolving 75.0 g citric acid, a triprotic acid with molar mass of 192.14 g, in water to make 250. mL solution?
A) 0.173 N
B) 0.0576 N
C) 0.293 N
D) 4.68 N
E) 1.56 N
Answer: D
Diff: 3
Section: 10.11
80) What is the normality of a solution prepared by dissolving 37.5 g citric acid, a triprotic acid with molar mass of 192.14 g, in water to make 250. mL solution?
A) 2.34 N
B) 0.780 N
C) 0.147 N
D) 0.0865 N
E) 0.288 N
Answer: A
Diff: 3
Section: 10.11
81) Which net ionic equation correctly represents the neutralization of a solution of barium hydroxide by a solution of nitric acid?
A) Ba2+ + 2 NO3- → Ba(NO3)2
B) H+ + NO3- → HNO3
C) Ba2+ + 2 OH- → Ba(OH)2
D) H+ + OH- → H2O
E) Ba(NO3)2 + H2O → Ba2+ + 2 NO3-
Answer: D
Diff: 2
Section: 10.12
82) Which substance produces carbon dioxide and water upon reaction with an acid?
A) NaCH3CO2
B) NH4NO3
C) MgCO3
D) H2C2O4
E) C8H18
Answer: C
Diff: 3
Section: 10.12
83) Which equation correctly represents the neutralization of aluminum hydroxide by sulfuric acid?
A) 2 Al(OH)3 + 3 H2SO4 → Al2(SO4)3 + 3 H2O
B) Al(OH)3 + H3SO4 → AlSO4 + 3 H2O
C) Al(OH)2 + H2SO4 → AlSO4 + 2 H2O
D) 2 Al(OH)3 + 3 H2SO4 → Al2(SO4)3 + 6 H2O
E) 3 Al(OH)3 + 2 H3SO4 → Al3(SO4)2 + 6 H2O
Answer: D
Diff: 3
Section: 10.12
84) The net ionic equation for the reaction of formic acid, a weak acid, with potassium hydroxide, a strong base, is:
A) HCO2H (aq) + KOH (aq) → KHCO2 (aq) + H2O (l)
B) HCO2H (aq) + K+ (aq) + OH- (aq) → K+ (aq) + HCO2- (aq) + H2O (l)
C) HCO2H (aq) + OH- (aq) → HCO2- (aq) + H2O (l)
D) HCO2- (aq) + KOH (aq) → KHCO2 (aq) + OH- (aq)
E) H+ (aq) + HCO2- (aq) + K+ (aq) + OH- (aq) → K+ (aq) + HCO2- (aq) + H2O (l)
Answer: C
Diff: 3
Section: 10.12
85) What is the concentration of a weak base solution if a 25.0 mL sample is neutralized by 48.3 mL of 0.105 M H3PO4?
A) 0.0543 M
B) 0.0676 M
C) 0.163 M
D) 0.203 M
E) 0.609 M
Answer: E
Diff: 2
Section: 10.13
86) How many mL of 0.100 M NaOH are needed to neutralize 24.0 mL of 0.150 M HCl?
A) 12.0 mL
B) 18.0 mL
C) 24.0 mL
D) 36.0 mL
E) 48.0 mL
Answer: D
Diff: 3
Section: 10.13
87) How many mL of 0.100 M NaOH are needed to neutralize 50.00 mL of a 0.150 M solution of CH3CO2H, a monoprotic acid?
A) 25.00 mL
B) 37.50 mL
C) 50.00 mL
D) 75.00 mL
E) 100.00 mL
Answer: D
Diff: 3
Section: 10.13
88) What is the concentration of a solution of HCl in which a 10.0 mL sample of acid required 50.0 mL of 0.150 M NaOH for neutralization?
A) 0.0300 M
B) 0.150 M
C) 0.600 M
D) 0.750 M
E) 7.50 M
Answer: D
Diff: 3
Section: 10.13
89) What is the concentration of a nitric acid solution if a 10.00 mL sample of the acid requires 31.25 mL of 0.135 M KOH for neutralization?
A) 0.422 M
B) 0.0432 M
C) 0.844 M
D) 0.135 M
E) 0.211 M
Answer: A
Diff: 3
Section: 10.13
90) What is the concentration of an acetic acid solution if a 10.0 mL sample required 26.4 mL of 0.950 M KOH for neutralization?
A) 0.379 M
B) 0.399 M
C) 0.950 M
D) 2.51 M
E) 2.78 M
Answer: D
Diff: 3
Section: 10.13
91) What is the concentration of a phosphoric acid solution of a 25.00 mL sample of the acid requires 42.24 mL of 0.135 M NaOH for neutralization?
A) 0.228 M
B) 0.684 M
C) 0.0760 M
D) 0.0266 M
E) 0.0799 M
Answer: C
Diff: 3
Section: 10.13
92) How many mL of 0.360 M HNO3 are needed to neutralize a 22.5 mL sample of 0.240 M KOH?
A) 5.40 mL
B) 15.0 mL
C) 22.5 mL
D) 33.8 mL
E) 62.5 mL
Answer: B
Diff: 3
Section: 10.13
93) How many mL of 0.150 M NaOH are needed to neutralize 50.00 mL of a 0.120 M solution of H2SO4?
A) 40.0 mL
B) 50.0 mL
C) 80.0 mL
D) 120.0 mL
E) 160.0 mL
Answer: C
Diff: 3
Section: 10.13
94) How many mL of 0.241 M H2SO4 will be needed to neutralize a 50.0 mL sample of 0.191 M KOH?
A) 19.8 mL
B) 31.5 mL
C) 39.6 mL
D) 79.3 mL
E) 126 mL
Answer: A
Diff: 3
Section: 10.13
95) Which compound produces an acidic solution when dissolved in water?
A) NH4Cl
B) NaF
C) K2SO4
D) KCl
E) Ca(NO3)2
Answer: A
Diff: 2
Section: 10.14
96) Which compound produces a basic solution when dissolved in water?
A) NH4Cl
B) NaF
C) KClO4
D) KCl
E) Ca(NO3)2
Answer: B
Diff: 2
Section: 10.14
97) Of the following four substances, which would form a basic solution when dissolved in water:
NH4ClCu(NO3)2K2CO3NaF
A) NH4Cl, Cu(NO3)2
B) K2CO3, NH4Cl
C) NaF, K2CO3
D) NaF only
E) none of them
Answer: C
Diff: 2
Section: 10.14
Match the following.
A) an acid-base theory that bases reactions on hydrogen and hydroxide ions
B) the species that results when a base accepts a proton
C) a substance which can behave as either an acid or a base
D) the species that results when an acid donates a proton
E) a theory that treats acid-base reactions as proton-transfer reactions
98) Arrhenius theory
Diff: 1
Section: 10.1
99) conjugate base
Diff: 1
Section: 10.3
100) Bronsted-Lowry theory
Diff: 1
Section: 10.3
101) conjugate acid
Diff: 1
Section: 10.3
102) amphoteric
Diff: 1
Section: 10.4
Answers: 98) A 99) D 100) E 101) B 102) C
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