General Chemistry, 10e Cdn (Petrucci)
Chapter 16 Acids and Bases
1) According to the Arrhenius theory, a neutralization reaction involves the combination of an acid with a base to make only water.
Answer: FALSE
Diff: 1 Type: TF
Reference: Section 16-1
2) According to the Arrhenius theory, a neutralization reaction involves the combination of hydrogen ions and hydroxide ions to form water.
Answer: TRUE
Diff: 1 Type: TF
Reference: Section 16-1
3) Br∅nsted and Lowry suggested that bases be defined as proton acceptors.
Answer: TRUE
Diff: 1 Type: TF
Reference: Section 16-2
4) The term pH = -ln [H+].
Answer: FALSE
Diff: 1 Type: TF
Reference: Section 16-3
5) Amine bases are known as strong bases
Answer: FALSE
Diff: 1 Type: TF
Reference: Section 16-5
6) HNO3 is a strong acid.
Answer: TRUE
Diff: 1 Type: TF
Reference: Section 16-5
7) The first ionization step is approximately 100% for H2SO3.
Answer: FALSE
Diff: 2 Type: TF
Reference: Section 16-6
8) H2SO4 is a weaker acid than H2SO3.
Answer: FALSE
Diff: 2 Type: TF
Reference: Section 16-8
9) When comparing binary acids of the elements in the same row of the periodic table, acid strength increases as the polarity of the element-hydrogen bond increases.
Answer: TRUE
Diff: 2 Type: TF
Reference: Section 16-8
10) In the reaction BF3 + NH3 → F3B:NH3, BF3 acts as a Br∅nsted acid.
Answer: FALSE
Diff: 1 Type: TF
Reference: Section 16-9
11) The definition of a neutralization reaction as a reaction in which an acid reacts with a base to produce water and a salt is inherent in:
A) only the Arrhenius theory
B) both the Arrhenius and the Br∅nsted-Lowry theories
C) only the Br∅nsted-Lowry theory
D) both the Br∅nsted-Lowry and the Lewis theories
E) only the Lewis theory
Answer: A
Diff: 1 Type: MC
Reference: Section 16-1
12) According to the Arrhenius theory, a neutralization reaction involves:
A) the combination of hydrogen ions and hydroxide ions to form water.
B) the dissociation of a strong acid to hydrogen ions and an anion.
C) the dissociation of a strong base into hydroxide ions and a cation.
D) the addition of water to ammonia to make ammonium hydroxide.
E) the combination of an acid with a base to make only water.
Answer: A
Diff: 1 Type: MC
Reference: Section 16-1
13) Proton acceptor is an abbreviated definition of:
A) Br∅nsted-Lowry base
B) Br∅nsted-Lowry acid
C) Lewis base
D) Lewis acid
E) Arrhenius acid
Answer: A
Diff: 1 Type: MC
Reference: Section 16-2
14) In the equilibrium system described by: PO43-(aq) + H2O(l) ⇌ HPO42-(aq) + OH-, Br∅nsted-Lowry theory would designate:
A) PO43- and H2O as the bases
B) H2O and OH- as a conjugate pair
C) HPO42- and OH- as the acids
D) HPO42- and H2O as a conjugate pair
E) PO43- as amphiprotic
Answer: B
Diff: 1 Type: MC
Reference: Section 16-2
15) Choose the strongest acid.
A) HF
B) H2CO3
C) HCN
D) HC2H3O2
E) HClO4
Answer: E
Diff: 1 Type: MC
Reference: Section 16-2
16) Choose the INCORRECT statement.
A) H2SO4, HCl, and HNO3 all form H3O+ when reacted with H2O.
B) Neutralization takes place when the hydronium ion reacts with the hydroxide ion to form water.
C) Br∅nsted and Lowry suggested that bases be defined as proton acceptors.
D) The odor that is noticeable when the stopper is removed from a bottle of aqueous ammonia is good evidence of the strength of the substance as a base.
E) Br∅nsted and Lowry suggested that acids be defined as proton donors.
Answer: D
Diff: 1 Type: MC
Reference: Section 16-2
17) Which of the following are Br∅nsted-Lowry acid?
I) CH3COOH
II) [Cu(H2O)4]2+
III) H2O
IV) CH3NH2
V) H3O+
A) I), II) and III)
B) II), III), and IV)
C) I), II), III) and IV)
D) I), II), III), and V)
E) II), III) and V)
Answer: D
Diff: 2 Type: MC
Reference: Section 16-2
18) Which of the following is the strongest base?
A) Cl-
B) ClO4-
C) F-
D) NO3-
E) H2O
Answer: C
Diff: 2 Type: MC
Reference: Section 16-2
19) pOH = 3.14 is equivalent to:
A) pH = 11.
B) [H+] = 1.4 × 10-10 M
C) [OH-] = 7.2 × 10-4 M
D) [H+} = 7.0 × 10-4 M
E) [OH-] = 3.14 × 10-7 M
Answer: C
Diff: 1 Type: MC
Reference: Section 16-3
20) Choose the Br∅nsted-Lowry acids and bases in the following equation:
HCN + OH- ⇌ H2O + CN-
A) acids HCN, CN- bases OH-, H2O
B) acids CN-, OH- bases HCN, H2O
C) acids HCN, H2O bases OH-, CN-
D) acids OH-, H2O bases CN-, HCN
E) acids HCN, OH- bases H2O, CN-
Answer: C
Diff: 2 Type: MC
Reference: Section 16-2
21) Choose the Br∅nsted-Lowry acids and bases in the following equation:
NH4+ + OH- ⇌ H2O + NH3
A) acids NH4+, OH- bases H2O, NH3
B) acids OH-, H2O bases NH3, NH4+
C) acids NH4+, OH- bases NH4+, H2O
D) acids NH4+, H2O bases OH-, NH3
E) acids NH4+, NH3 bases OH-, H2O
Answer: D
Diff: 2 Type: MC
Reference: Section 16-2
22) Choose the Br∅nsted-Lowry acids and bases in the following equation:
H2O + NH2- ⇌ NH3 + OH-
A) acids H2O, OH- bases NH3, NH2-
B) acids NH2-, NH3 bases H2O, OH-
C) acids H2O, NH2- bases OH-, NH3
D) acids NH3, NH2- bases OH-, H2O
E) acids H2O, NH3 bases NH2-, OH-
Answer: E
Diff: 2 Type: MC
Reference: Section 16-2
23) Choose the Br∅nsted-Lowry acids and bases in the following equation:
HCO3- + OH- ⇌ H2O + CO32-
A) acids HCO3-, H2O bases OH-, CO32-
B) acids OH-, CO32- bases HCO3-, H2O
C) acids H2O, OH- bases HCO3-, CO32-
D) acids HCO3-, OH- bases CO32-, H2O
E) acids H2O, CO32- bases HCO3-, OH-
Answer: A
Diff: 2 Type: MC
Reference: Section 16-2
24) Choose the Br∅nsted-Lowry acids and bases in the following equation:
HSO4- + C2H3O2- ⇌ HC2H3O2 + SO42-
A) acids HSO4-, SO42- bases HC2H3O2, C2H3O2-
B) acids HSO4-, HC2H3O2 bases SO42-, C2H3O2-
C) acids SO42-, HC2H3O2 bases HSO4-, C2H3O2-
D) acids SO42-, C2H3O2- bases HSO4-, HC2H3O2
E) acids HSO4-, C2H3O2- bases HC2H3O2, SO42-
Answer: B
Diff: 2 Type: MC
Reference: Section 16-2
25) Consider the reaction:
HC2H3O2 + H2O ⇌ H3O+ + C2H3O2-
Choose the pair of substances that are both bases in the reaction.
A) HC2H3O2 and H3O+
B) H2O and C2H3O2-
C) H2O and H3O+
D) HC2H3O2 and C2H3O2-
E) H3O+ and HC2H3O2
Answer: B
Diff: 1 Type: MC
Reference: Section 16-2
26) A solution has pOH of -0.47. This means that:
A) the solution has a pH of 13.53
B) the solution has an [OH-] = 0.34 M
C) the solution has an [OH-] greater than 10.0 M
D) the solution has an [OH-] = 2.95 M
E) The solution has an [H+] = 2.95 M
Answer: D
Diff: 1 Type: MC
Reference: Section 16-3
27) At 25°C, the pH of pure water is:
A) 0
B) >0, <7
C) 7
D) >7, <14
E) 14
Answer: C
Diff: 1 Type: MC
Reference: Section 16-3
28) Choose the INCORRECT statement. The term pH:
A) refers to the "potential" of hydrogen ion
B) = -ln [H+]
C) = 14 - pOH
D) is more convenient than exponential notation
E) = -log [H3O+]
Answer: B
Diff: 1 Type: MC
Reference: Section 16-3
29) A saturated aqueous solution of calcium hydroxide has a pH of 12.25. What is the [Ca2+] of such a solution?
A) 0.018
B) 5.6 × 10-13
C) 2.3 × 10-5
D) 0.035
E) 8.9 × 10-3
Answer: E
Diff: 3 Type: MC
Reference: Section 16-4
30) 0.272 g of a monoprotic acid (Mw = 189 g/mol) is dissolved in water to produce 25.0 mL of a solution with pH = 4.93. Determine the ionization constant of the acid.
A) 4.1 × 10-8
B) 1.4 × 10-10
C) 2.1 × 10-4
D) 2.8 × 10-7
E) 2.4 × 10-9
Answer: E
Diff: 2 Type: MC
Reference: Section 16-5
31) 0.375 g of a monoprotic acid (mm = 245 g/mol) is dissolved in water to produce 25.0 mL of a solution with pH = 3.28. Determine the ionization constant of the acid.
A) 8.56 × 10-3
B) 4.5 × 10-6
C) 7.4 × 10-5
D) 4.5 × 10-3
E) 2.3 × 10-2
Answer: B
Diff: 2 Type: MC
Reference: Section 16-5
32) 0.653 g of a monoprotic acid (mm = 157 g/mol) is dissolved in water to produce 50.0 mL of a solution with pH = 2.13. Determine the ionization constant of the acid.
A) 7.9 × 10-3
B) 8.9 × 10-2
C) 6.6 × 10-4
D) 3.9 × 10-2
E) 3.6 × 10-6
Answer: C
Diff: 2 Type: MC
Reference: Section 16-5
33) A 0.632 M solution of a monoprotic base has a pH of 11.53. What is the ionization constant of this base?
A) 1.8 × 10-5
B) 2.1 × 10-3
C) 1.6 × 10-23
D) 5.0 × 10-12
E) 5.3 × 10-3
Answer: A
Diff: 2 Type: MC
Reference: Section 16-5
34) A 0.214 M solution of a monoprotic base has a pH of 11.48. What is the ionization constant of this base?
A) 1.4 × 10-2
B) 4.3 × 10-5
C) 1.5 × 10-11
D) 5.1 × 10-23
E) 2.0 × 10-6
Answer: B
Diff: 2 Type: MC
Reference: Section 16-5
35) A 0.505 g sample of a monoprotic base (mm = 45.09 g/mol) was dissolved in water to produce 100.0 mL of solution with a pH = 11.84. What is the ionization constant of this base?
A) 4.3 × 10-5
B) 1.9 × 10-23
C) 4.3 × 10-4
D) 3.4 × 10-1
E) 1.3 × 10-11
Answer: C
Diff: 2 Type: MC
Reference: Section 16-5
36) A 0.0925 g sample of a monoprotic base (mm = 17.03 g/mol) was dissolved in water to produce 100 mL of solution with a pH = 11.00. What is the ionization constant of this base?
A) 1.8 × 10-6
B) 1.8 × 10-11
C) 1.8 × 10-21
D) 1.9 × 10-5
E) 1.1 × 10-6
Answer: D
Diff: 2 Type: MC
Reference: Section 16-5
37) Which of the following statements is NOT true?
A) In liquid ammonia, the strongest possible base is the NH2- ion.
B) Ammonium hydroxide and acetic acid have equal ionization constants in water at 25 °C because of the leveling effect.
C) The second ionization constant of a diprotic acid is always smaller than the first ionization constant.
D) A Br∅nsted base may be any substance that can act as a proton acceptor.
E) Bases neutralize acids to form salts plus water.
Answer: B
Diff: 1 Type: MC
Reference: Section 16-6
38) For which of the following polyprotic acids is the first ionization step approximately 100%?
A) H2S
B) H2SO3
C) H2CO3
D) H2SO4
E) H3PO4
Answer: D
Diff: 2 Type: MC
Reference: Section 16-6
39) What is the [HPO4-2] of a solution labeled "0.10 M Phosphoric Acid"?
[Ka1 = 7.1 × 10-3; Ka2 = 6.3 × 10-8; Ka3 = 4.2 × 10-13]
A) 4.2 × 10-13 M
B) 6.3 × 10-8 M
C) 7.1 × 10-3 M
D) 1.6 × 10-9 M
E) 1.6 × 10-16 M
Answer: B
Diff: 3 Type: MC
Reference: Section 16-6
40) What is the [AsO43-] for a solution labeled 0.10 M arsenic acid (H3AsO4)?
[Ka1 = 6 × 10-3, Ka2 = 1 × 10-7, Ka3 = 3 × 10-12]
A) 1 × 10-7 M
B) 1 × 10-17 M
C) 3 × 10-12 M
D) 3 × 10-19 M
E) 6 × 10-10 M
Answer: B
Diff: 3 Type: MC
Reference: Section 16-6
41) Which of the following is a logical inference from the fact that a 0.10 molar solution of potassium acetate, KC2H3O2, is less alkaline than a 0.10 molar solution of potassium cyanide, KCN?
A) Hydrocyanic acid is a weaker acid than acetic acid.
B) Cyanides are less soluble than acetates.
C) Hydrocyanic acid is less soluble in water than acetic acid.
D) Acetic acid is a weaker acid than hydrocyanic acid.
E) 0.10 M potassium acetate is more concentrated than 0.10 M potassium cyanide.
Answer: A
Diff: 2 Type: MC
Reference: Section 16-7
42) Determine the pH of 263 ml of solution which has [NH4I] = 0.300 M. Kb = 1.74 × 10-5 for NH3(aq).
A) 2.6
B) 11.4
C) 4.9
D) 9.1
E) 4.6
Answer: C
Diff: 2 Type: BI
Reference: Section 16-7
43) The pH of a solution of NH4C2H3O2 is approximately 7. The best explanation is:
A) This salt does not react with water.
B) Ammonium acetate is a weak electrolyte.
C) All salts of weak acids and weak bases are neutral.
D) Aqueous ammonia and acetic acid have approximately equal ionization constants.
E) The salt is a product of a strong acid and a strong base.
Answer: D
Diff: 2 Type: MC
Reference: Section 16-7
44) Which indication of relative acid strengths is INCORRECT?
A) HCl > HF
B) HClO2 > HClO
C) H2SO4 > H2SO3
D) H2SO3 > HNO3
E) CH3CO2H > CH3CH2OH
Answer: D
Diff: 2 Type: MC
Reference: Section 16-8
45) Which of the following statements concerning aqueous solutions of salts is FALSE?
A) For any salt of a strong acid and a strong base, the pH will be about 7.
B) For any salt of a strong acid and a weak base, the pH will be <7.
C) For any salt of a weak acid and a strong base, the pH will be >7.