Acids and Bases – Ch15 | Test Bank – Focused – 15th Ed - Test Bank | Foundations of College Chemistry 15e by Hein Arena by Hein Arena, Willard. DOCX document preview.
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Package Title: Hein Test Bank
Course Title: Hein 15e
Chapter Number: 15
Question Type: Multiple Choice
1) In the following reaction,
water behaves as:
a) an acid
b) a base
c) a salt
d) a conjugate base
Difficulty: medium
Learning Objective 1: Compare the definitions of acids and bases, including Arrhenius, Brønsted–lowry, and lewis acids and bases.
Section Reference 1: Section 15.1
2) Cl- is a conjugate base of which acid?
a) HCl
b) HOCl
c) HClO3
d) H3O+
Difficulty: medium
Learning Objective 1: Compare the definitions of acids and bases, including Arrhenius, Brønsted–lowry, and lewis acids and bases.
Section Reference 1: Section 15.1
3) In the following reaction,
the compound CH3NH2 behaves as:
a) an acid
b) a base
c) a salt
d) a conjugate acid
Difficulty: medium
Learning Objective 1: Compare the definitions of acids and bases, including Arrhenius, Brønsted–lowry, and lewis acids and bases.
Section Reference 1: Section 15.1
4) The conjugate acid of a strong base is a
a) strong acid
b) weak acid
c) strong base
d) weak base
Difficulty: medium
Learning Objective 1: Compare the definitions of acids and bases, including Arrhenius, Brønsted–lowry, and lewis acids and bases.
Section Reference 1: Section 15.1
5) The hydronium ion is responsible for the properties of
a) acids.
b) bases.
c) salts.
Difficulty: easy
Learning Objective 1: Compare the definitions of acids and bases, including Arrhenius, Brønsted–lowry, and lewis acids and bases.
Section Reference 1: Section 15.1
6) The hydroxide ion is responsible for the properties of
a) acids.
b) bases.
c) salts.
Difficulty: easy
Learning Objective 1: Compare the definitions of acids and bases, including Arrhenius, Brønsted–lowry, and lewis acids and bases.
Section Reference 1: Section 15.1
7) In the following reaction,
a) HClO4 is the conjugate acid of H2O
b) H2O is the conjugate acid of H3O+
c) H3O+ is the conjugate base of H2O
d) ClO4- is the conjugate base of HClO4
Difficulty: medium
Learning Objective 1: Compare the definitions of acids and bases, including Arrhenius, Brønsted–lowry, and lewis acids and bases.
Section Reference 1: Section 15.1
8) Which of the following species is an acid and also a conjugate base of another acid?
a) HSO4-
b) H2SO4
c) OH-
d) H3O+
Difficulty: medium
Learning Objective 1: Compare the definitions of acids and bases, including Arrhenius, Brønsted–lowry, and lewis acids and bases.
Section Reference 1: Section 15.1
9) In an acidic solution the
a) concentration of hydronium ion is greater than that of hydroxide ion.
b) concentration of hydroxide ion greater than that of hydronium ion.
c) concentration of hydronium ion and hydroxide ion are equal.
Difficulty: easy
Learning Objective 1: Calculate the pH of a solution from the hydrogen ion concentration.
Section Reference 1: Section 15.5
10) In a basic solution the
a) concentration of hydronium ion is greater than that of hydroxide ion.
b) concentration of hydroxide ion is greater than that of hydronium ion.
c) concentration of hydronium ion and hydroxide ion are equal.
Difficulty: easy
Learning Objective 1: Calculate the pH of a solution from the hydrogen ion concentration.
Section Reference 1: Section 15.5
11) In a neutral solution the
a) concentration of hydronium ion is greater than that of hydroxide ion.
b) concentration of hydroxide ion is greater than that of hydronium ion.
c) concentration of hydronium ion and hydroxide ion are equal.
Difficulty: easy
Learning Objective 1: Calculate the pH of a solution from the hydrogen ion concentration.
Section Reference 1: Section 15.5
12) A hydrogen ion consists of a(n)
a) electron.
b) proton.
c) neutron.
d) proton and electron.
Difficulty: easy
Learning Objective 1: Compare the definitions of acids and bases, including Arrhenius, Brønsted–lowry, and lewis acids and bases.
Section Reference 1: Section 15.1
13) Arrhenius defined an acid as a substance whose aqueous solution contains an excess of
a) sodium ion.
b) hydroxide ion.
c) chloride ion.
d) hydrogen ion.
Difficulty: easy
Learning Objective 1: Compare the definitions of acids and bases, including Arrhenius, Brønsted–lowry, and lewis acids and bases.
Section Reference 1: Section 15.1
14) Arrhenius defined base as a substance whose aqueous solution contains an excess of
a) sodium ion.
b) hydroxide ion.
c) chloride ion.
d) hydrogen ion.
Difficulty: easy
Learning Objective 1: Compare the definitions of acids and bases, including Arrhenius, Brønsted–lowry, and lewis acids and bases.
Section Reference 1: Section 15.1
15) Brønsted and Lowry defined an acid as a(n)
a) electron donor.
b) electron acceptor.
c) proton donor.
d) proton acceptor.
Difficulty: easy
Learning Objective 1: Compare the definitions of acids and bases, including Arrhenius, Brønsted–lowry, and lewis acids and bases.
Section Reference 1: Section 15.1
16) Brønsted and Lowry defined a base as a(n)
a) electron donor.
b) electron acceptor.
c) proton donor.
d) proton acceptor.
Difficulty: easy
Learning Objective 1: Compare the definitions of acids and bases, including Arrhenius, Brønsted–lowry, and lewis acids and bases.
Section Reference 1: Section 15.1
17) What is the total concentration of ions in a 0.10 M solution of barium chloride?
a) 0.10 M
b) 0.20 M
c) 0.30 M
d) 0.40 M
Difficulty: medium
Learning Objective 1: Describe properties, ionization, dissociation, and strength of electrolytes and compare them to nonelectrolytes
Section Reference 1: Section 15.4
18) Acids react with carbonates to produce the gas
a) hydrogen.
b) carbon dioxide.
c) nitrogen.
d) oxygen.
Difficulty: easy
Learning Objective 1: Describe the general reactions of acids and bases.
Section Reference 1: Section 15.2
19) Which of the following is a strong electrolyte?
a) sulfuric acid
b) sulfurous acid
c) ammonia
d) acetic acid
Difficulty: easy
Learning Objective 1: Describe properties, ionization, dissociation, and strength of electrolytes and compare them to nonelectrolytes.
Section Reference 1: Section 15.4
20) Which of the following is a strong electrolyte?
a) methanol, CH3OH
b) water
c) hydrosulfuric acid
d) hydrochloric acid
Difficulty: easy
Learning Objective 1: Describe properties, ionization, dissociation, and strength of electrolytes and compare them to nonelectrolytes.
Section Reference 1: Section 15.4
21) Which of the following is a strong electrolyte?
a) sodium hydroxide
b) aluminum hydroxide
c) ammonia
d) magnesium hydroxide
Difficulty: easy
Learning Objective 1: Describe properties, ionization, dissociation, and strength of electrolytes and compare them to nonelectrolytes.
Section Reference 1: Section 15.4
22) Which of the following is a nonelectrolyte?
a) methanol, CH3OH
b) acetic acid
c) sodium hydroxide
d) potassium chloride
Difficulty: easy
Learning Objective 1: Describe properties, ionization, dissociation, and strength of electrolytes and compare them to nonelectrolytes.
Section Reference 1: Section 15.4
23) Which of the following is a nonelectrolyte?
a) sugar
b) hypochlorous acid
c) sodium hydroxide
d) hydrosulfuric acid
Difficulty: easy
Learning Objective 1: Describe properties, ionization, dissociation, and strength of electrolytes and compare them to nonelectrolytes.
Section Reference 1: Section 15.4
24) An amphoteric substance is one that
a) may react as an acid or a conjugate acid.
b) may react as a salt.
c) may react as a base or a conjugate base.
d) may react as an acid or a base.
Difficulty: easy
Learning Objective 1: Describe the general reactions of acids and bases.
Section Reference 1: Section 15.2
25) Which of the following is the hydronium ion?
a) H +
b) H3O+
c) OH –
d) a proton
Difficulty: easy
Learning Objective 1: Compare the definitions of acids and bases, including Arrhenius, Brønsted–lowry, and lewis acids and bases
Section Reference 1: Section 15.1
26) The concentration of an aqueous solution of iron(II) chloride is 0.0550 M. What is the molarity of each ion in this solution?
a) 0.0550 M for both the iron(II) and chloride ions.
b) 0.0550 M for the iron(II) ion and 0.110 M for the chloride ion.
c) 0.110 M for the iron(II) ion and 0.0550 M for the chloride ion.
d) not enough information is given to determine each molarity.
Difficulty: medium
Learning Objective 1: Describe properties, ionization, dissociation, and strength of electrolytes and compare them to nonelectrolytes.
Section Reference 1: Section 15.4
27) In a 0.25 M aqueous solution of sodium phosphate, what is the total concentration of all ions?
a) 0.25 M
b) 0.50 M
c) 0.75 M
d) 1.0 M
Difficulty: medium
Learning Objective 1: Describe properties, ionization, dissociation, and strength of electrolytes and compare them to nonelectrolytes.
Section Reference 1: Section 15.4
28) In which of the following combinations will the acid and base combine to form calcium sulfate?
a) CaOH and H2SO3
b) CaOH and H2SO4
c) Ca(OH)2 and H2SO3
d) Ca(OH)2 and H2SO4
Difficulty: medium
Learning Objective 1: Describe the general reactions of acids and bases.
Learning Objective 2: Describe a neutralization reaction and do calculations, involving titrations.
Section Reference 1: Section 15.2 and 15.6
29) In which of the following combinations will the acid and base combine to form sodium sulfite?
a) NaOH and H2SO3
b) NaOH and H2SO4
c) Na(OH)2 and H2SO3
d) Na(OH)2 and H2SO4
Difficulty: medium
Learning Objective 1: Describe the general reactions of acids and bases.
Learning Objective 2: Describe a neutralization reaction and do calculations, involving titrations.
Section Reference 1: Section 15.2 and 15.6
30) Which type of compound is a nonelectrolyte?
a) alcohol
b) acid
c) base
d) salt
Difficulty: easy
Learning Objective 1: Describe properties, ionization, dissociation, and strength of electrolytes and compare them to nonelectrolytes.
Section Reference 1: Section 15.4
31) Combining sodium hydroxide and hydrochloric acid will produce water and
a) sodium chloride.
b) sodium chlorite.
c) sodium chlorate.
d) sodium hypochlorite.
Difficulty: easy
Learning Objective 1: Describe the general reactions of acids and bases.
Learning Objective 2: Describe a neutralization reaction and do calculations, involving titrations.
Section Reference 1: Section 15.2 and 15.6
32) Combining potassium hydroxide and sulfuric acid will produce water and
a) potassium sulfide.
b) potassium sulfate.
c) potassium sulfite.
d) potassium hypersulfate.
Difficulty: easy
Learning Objective 1: Describe the general reactions of acids and bases.
Learning Objective 2: Describe a neutralization reaction and do calculations, involving titrations.
Section Reference 1: Section 15.2 and 15.6
33) Which of the following will dissociate when placed in water?
a) CH3OH
b) HCl
c) NaCl
d) HClO4
e) All of these choices except CH3OH dissociate in water.
Difficulty: medium
Learning Objective 1: Describe properties, ionization, dissociation, and strength of electrolytes and compare them to nonelectrolytes.
Section Reference 1: Section 15.4
34) Which of the following will ionize when placed in water?
a) KOH
b) HCl
c) KCl
d) LiCl
e) All will ionize when placed in water.
Difficulty: medium
Learning Objective 1: Describe properties, ionization, dissociation, and strength of electrolytes and compare them to nonelectrolytes.
Section Reference 1: Section 15.4
35) Which of the following is a strong acid?
a) HNO3
b) HNO2
c) HClO
d) HClO2
Difficulty: easy
Learning Objective 1: Describe properties, ionization, dissociation, and strength of electrolytes and compare them to nonelectrolytes.
Section Reference 1: Section 15.4
36) Which of the following is a strong acid?
a) HClO3
b) HClO2
c) H2SO3
d) H2SO4
Difficulty: easy
Learning Objective 1: Describe properties, ionization, dissociation, and strength of electrolytes and compare them to nonelectrolytes.
Section Reference 1: Section 15.4
37) Which of the following is a strong base?
a) NH4OH
b) Ca(OH)2
c) HNO2
d) HNO3
Difficulty: easy
Learning Objective 1: Describe properties, ionization, dissociation, and strength of electrolytes and compare them to nonelectrolytes.
Section Reference 1: Section 15.4
38) Which of the following is a strong base?
a) NH3
b) HCl
c) KOH
d) CH3OH
Difficulty: easy
Learning Objective 1: Describe properties, ionization, dissociation, and strength of electrolytes and compare them to nonelectrolytes.
Section Reference 1: Section 15.4
39) The pH of distilled water is
- 0
- 14
- 7
- 9
Difficulty: easy
Learning Objective 1: Describe a neutralization reaction and do calculations, involving titrations.
Section Reference 1: Section 15.6
40) Which pH listed below is most acidic?
a) 3
b) 7
c) 9
d) 14
Difficulty: easy
Learning Objective 1: Describe a neutralization reaction and do calculations, involving titrations.
Section Reference 1: Section 15.6
41) Which pH listed below is most alkaline (basic)?
a) 1
b) 5
c) 7
d) 12
Difficulty: easy
Learning Objective 1: Describe a neutralization reaction and do calculations, involving titrations
Section Reference 1: Section 15.6
42) Which pH listed below represents a neutral solution?
a) 2
b) 4
c) 5
d) 7
Difficulty: easy
Learning Objective 1: Describe a neutralization reaction and do calculations, involving titrations.
Section Reference 1: Section 15.6
43) An aqueous solution whose pH=0 is
- acidic
- basic
- neutral
- amphoteric
Difficulty: easy
Learning Objective 1: Describe a neutralization reaction and do calculations, involving titrations.
Section Reference 1: Section 15.6
44) Which of the following is the pH of a solution in which the concentration of hydrogen ion is greater than the concentration of hydroxide ion?
a) 12
b) 9
c) 7
d) 3
Difficulty: easy
Learning Objective 1: Describe a neutralization reaction and do calculations, involving titrations.
Section Reference 1: Section 15.6
45) Which of the following is the pH of a solution in which the concentration of hydroxide ion is greater than the concentration of hydrogen ion?
a) 7
b) 2
c) 6
d) 13
Difficulty: easy
Learning Objective 1: Describe a neutralization reaction and do calculations, involving titrations.
Section Reference 1: Section 15.6
46) Which of the following is the pH of a solution in which the concentration of hydrogen ion is equal to the concentration of hydroxide ion?
a) 7
b) 9
c) 12
d) 4
Difficulty: easy
Learning Objective 1: Describe a neutralization reaction and do calculations, involving titrations.
Section Reference 1: Section 15.6
47) How many times more concentrated is the hydrogen ion concentration in a solution with a pH of 3 than that with a pH of 5?
a) 2 times
b) 10 times
c) 100 times
d) 1000 times
Difficulty: medium
Learning Objective 1: Describe a neutralization reaction and do calculations, involving titrations.
Section Reference 1: Section 15.6
48) A solution of a strong acid has a pH of 3.0. The concentration of hydronium ions in this solution is
a) 0.001 M.
b) 3 M.
c) 0.3 M.
d) 0.003 M.
Difficulty: easy
Learning Objective 1: Describe a neutralization reaction and do calculations, involving titrations.
Section Reference 1: Section 15.6
49) A solution of a strong base has a pH of 11.0. The concentration of hydronium ions in this solution is
a) 11 M.
b) 
.
c) 
.
d) 
.
Difficulty: easy
Learning Objective 1: Describe a neutralization reaction and do calculations, involving titrations.
Section Reference 1: Section 15.6
50) Which of the following aqueous solutions will have the lowest boiling point?
a) 0.06 m NaCl
b) 0.10 m ethanol (ethyl alcohol)
c) 0.05 m MgCl2
d) 0.10 m NaOH
Difficulty: medium
Learning Objective 1: Describe properties, ionization, dissociation, and strength of electrolytes and compare them to nonelectrolytes.
Section Reference 1: Section 15.4
51) An acid solution of pH 6 is diluted hundred times. The pH of solution becomes
a) 7
b) 2
c) 4
d) 0
Difficulty: easy
Learning Objective 1: Describe a neutralization reaction and do calculations, involving titrations.
Section Reference 1: Section 15.6
52) The pH of a solution can be calculated from which of the following expressions?
a) pH = –log [OH –]
b) pH = log [OH–]
c) pH = –log [H +]
d) pH = log [H +]
Difficulty: easy
Learning Objective 1: Describe a neutralization reaction and do calculations, involving titrations.
Section Reference 1: Section 15.6
53) What are the spectator ions when hydrochloric acid reacts with sodium hydroxide?
a) Na + and H +
b) Cl – and OH –
c) H + and OH –
d) Na + and Cl –
Difficulty: medium
Learning Objective 1: Write net ionic equations using the stated rules.
Section Reference 1: Section 15.7
54) What is the net ionic equation when hydrobromic acid reacts with potassium hydroxide?
a) H +1 + OH– → H2O
b) H + + Br-- → HBr
c) K + + OH – → KOH
d) K + + H–→ KH
Difficulty: medium
Learning Objective 1: Write net ionic equations using the stated rules.
Section Reference 1: Section 15.7
55) Which are the two Brønsted-Lowry bases in the following equation?
NH3 + H2O 
NH4 + + OH –
a) NH3 and H2O
b) NH3 and NH4 +
c) NH3 and OH –
d) NH4 + and H2O
Difficulty: medium
Learning Objective 1: Compare the definitions of acids and bases, including Arrhenius, Brønsted–lowry, and lewis acids and bases.
Section Reference 1: Section 15.1
56) Which are the two Brønsted-Lowry acids in the following equation?
NH3 + H2O 
NH2 – + H3O +
a) H2O and NH2 –
b) NH3 and H2O
c) H3O + and NH3
d) NH2 – and H3O +
Difficulty: medium
Learning Objective 1: Compare the definitions of acids and bases, including Arrhenius, Brønsted–lowry, and lewis acids and bases.
Section Reference 1: Section 15.1
57) What is the conjugate acid of HS– in the following equation?
H2S + H2O 
HS – + H3O +
a) HS –
b) H2S
c) H3O +
d) H2O
Difficulty: easy
Learning Objective 1: Compare the definitions of acids and bases, including Arrhenius, Brønsted–lowry, and lewis acids and bases.
Section Reference 1: Section 15.1
58) What is the conjugate acid of H2O in the following equation?
HNO2 + H2O 
H3O + + NO2 –
a) H3O +
b) H2O
c) HNO2
d) NO2 –
Difficulty: medium
Learning Objective 1: Compare the definitions of acids and bases, including Arrhenius, Brønsted–lowry, and lewis acids and bases.
Section Reference 1: Section 15.1
59) Which of the following is a conjugate acid-base pair in the following equation?
H3PO4 + H2O 
H3O + + H2PO4 –
a) H3PO4 and H2O
b) H3O + and H2PO4 –
c) H2O and H3O +
d) H3PO4 and H3O +
Difficulty: easy
Learning Objective 1: Compare the definitions of acids and bases, including Arrhenius, Brønsted–lowry, and lewis acids and bases.
Section Reference 1: Section 15.1
60) Which of the following is a conjugate acid-base pair in the following equation?
HS – + H2O 
S 2– + H3O +
a) HS – and H3O +
b) HS – and S 2–
c) H3O + and S 2–
d) HS – and H2O
Difficulty: easy
Learning Objective 1: Compare the definitions of acids and bases, including Arrhenius, Brønsted–lowry, and lewis acids and bases.
Section Reference 1: Section 15.1
61) Which of the following is a conjugate acid base pair in the following equation?
H2SO4 + H2O 
HSO4 – + H3O +
a) H2SO4 and HSO4 –
b) H2SO4 and H2O
c) HSO4 – and H3O +
d) H3O + and H2SO4
Difficulty: easy
Learning Objective 1: Compare the definitions of acids and bases, including Arrhenius, Brønsted–lowry, and lewis acids and bases.
Section Reference 1: Section 15.1
62) Which of the following is a conjugate acid base pair in the following equation?
HF + H2O 
H3O + + F –
a) HF and H3O +
b) HF and H2O
c) H3O + and F –
d) HF and F –
Difficulty: easy
Learning Objective 1: Compare the definitions of acids and bases, including Arrhenius, Brønsted–lowry, and lewis acids and bases.
Section Reference 1: Section 15.1
63) What is the conjugate acid of OH –?
a) O2–
b) H +
c) O2H
d) HOH
Difficulty: easy
Learning Objective 1: Compare the definitions of acids and bases, including Arrhenius, Brønsted–lowry, and lewis acids and bases.
Section Reference 1: Section 15.1
64) What is the conjugate base of H2O?
a) OH–
b) H +
c) O2H
d) HOH
Difficulty: easy
Learning Objective 1: Compare the definitions of acids and bases, including Arrhenius, Brønsted–lowry, and lewis acids and bases.
Section Reference 1: Section 15.1
65) Which the conjugate base of OH– ?
a) O2–
b) H +
c) O2H
d) HOH
Difficulty: medium
Learning Objective 1: Compare the definitions of acids and bases, including Arrhenius, Brønsted–lowry, and lewis acids and bases.
Section Reference 1: Section 15.1
66) What is the conjugate acid of NH3?
a) N3–
b) NH4 +
c) NH2 –
d) NH 2–
Difficulty: easy
Learning Objective 1: Compare the definitions of acids and bases, including Arrhenius, Brønsted–lowry, and lewis acids and bases.
Section Reference 1: Section 15.1
67) What is the conjugate base of NH3?
a) NH2 –
b) NH 2–
c) NH4 +
d) H +
Difficulty: easy
Learning Objective 1: Compare the definitions of acids and bases, including Arrhenius, Brønsted–lowry, and lewis acids and bases.
Section Reference 1: Section 15.1
68) What is the conjugate base of HS –?
a) H2S
b) S 2–
c) H +
d) OH –
Difficulty: easy
Learning Objective 1: Compare the definitions of acids and bases, including Arrhenius, Brønsted–lowry, and lewis acids and bases.
Section Reference 1: Section 15.1
69) What is the conjugate acid of HS –?
a) H2S
b) S 2–
c) H +
d) OH –
Difficulty: easy
Learning Objective 1: Compare the definitions of acids and bases, including Arrhenius, Brønsted–lowry, and lewis acids and bases.
Section Reference 1: Section 15.1
70) What is the concentration of chloride ion in a 2.0 M solution of calcium chloride?
a) 1.0 M
b) 2.0 M
c) 3.0 M
d) 4.0 M
Difficulty: easy
Learning Objective 1: Describe properties, ionization, dissociation, and strength of electrolytes and compare them to nonelectrolytes.
Section Reference 1: Section 15.4
71) What is the concentration of potassium ion in a 2.0 M solution of potassium sulfide?
a) 1.0 M
b) 2.0 M
c) 3.0 M
d) 4.0 M
Difficulty: easy
Learning Objective 1: Describe properties, ionization, dissociation, and strength of electrolytes and compare them to nonelectrolytes.
Section Reference 1: Section 15.4
72) What is the boiling point of a 2.0 m aqueous solution of sodium chloride? (The boiling point elevation constant for water is 0.512 °C kg solvent/mol solute.)
a) 101.02 °C
b) 1.02 °C
c) 2.05 °C
d) 102.05 °C
Difficulty: hard
Learning Objective 1: Describe properties, ionization, dissociation, and strength of electrolytes and compare them to nonelectrolytes.
Section Reference 1: Section 15.4
73) What is the boiling point of a 0.50 m aqueous solution of aluminum nitrate? (The boiling point elevation constant for water is 0.512 °C kg solvent/mol solute.)
a) 100.51 °C
b) 101.02 °C
c) 102.05 °C
d) 106.60 °C
Difficulty: hard
Learning Objective 1: Describe properties, ionization, dissociation, and strength of electrolytes and compare them to nonelectrolytes.
Section Reference 1: Section 15.4
74) Which one has the highest boiling point?
a) 1% glucose
b) 1% sucrose
c) 1% NaCl
d) 1% CaCl2
Difficulty: hard
Learning Objective 1: Describe properties, ionization, dissociation, and strength of electrolytes and compare them to nonelectrolytes.
Section Reference 1: Section 15.4
75) What is the freezing point of a 1.0 m aqueous solution of CaCl2? (The freezing point depression constant for water is 1.86 °C kg solvent/mol solute.)
a) –1.86 °C
b) 1.86 °C
c) –3.72 °C
d) –5.58 °C
Difficulty: hard
Learning Objective 1: Describe properties, ionization, dissociation, and strength of electrolytes and compare them to nonelectrolytes.
Section Reference 1: Section 15.4
76) What is the freezing point of a 0.05 m solution of a non-electrolyte? (The freezing point depression constant for water is 1.86 °C kg solvent/mol solute.)
a) –1.86 °C
b) -0.93 °C
c) –0.093 °C
d) 0.93 °C
Difficulty: hard
Learning Objective 1: Describe properties, ionization, dissociation, and strength of electrolytes and compare them to nonelectrolytes.
Section Reference 1: Section 15.4
77) What is the freezing point of a 3.0 m aqueous solution of NaCl? (The freezing point depression constant for water is 1.86 °C kg solvent/mol solute.)
a) 5.6 °C
b) –5.6 °C
c) 11 °C
d) –11 °C
Difficulty: hard
Learning Objective 1: Describe properties, ionization, dissociation, and strength of electrolytes and compare them to nonelectrolytes.
Section Reference 1: Section 15.4
78) What is the pH of a 0.01 M solution of HCl?
a) 0.01
b) 1
c) –2
d) none of these choices
Difficulty: easy
Learning Objective 1: Calculate the pH of a solution from the hydrogen ion concentration.
Section Reference 1: Section 15.5
79) What is the pH of a 1.0 M solution of perchloric acid?
a) 0
b) 1
c) –1
d) 4
Difficulty: easy
Learning Objective 1: Calculate the pH of a solution from the hydrogen ion concentration.
Section Reference 1: Section 15.5
80) What is the pH of a solution whose H3O + concentration is 1 
10 –9?
a) 1
b) 9
c) –9
d) –1
Difficulty: easy
Learning Objective 1: Calculate the pH of a solution from the hydrogen ion concentration.
Section Reference 1: Section 15.5
81) What is the pH of a 0.034 M hydrochloric acid solution?
a) -2.00
b) 3.40
c) -1.47
d) 1.47
Difficulty: easy
Learning Objective 1: Calculate the pH of a solution from the hydrogen ion concentration.
Section Reference 1: Section 15.5
82) What is the pH of a solution whose H + concentration is 4.0 
10 –9?
a) 4.00
b) 8.40
c) 3.60
d) 9.00
Difficulty: easy
Learning Objective 1: Calculate the pH of a solution from the hydrogen ion concentration.
Section Reference 1: Section 15.5
83) What is the pH of a 0.02 M hydrobromic acid solution?
a) 0.02
b) -2.0
c) 1.7
d) 4.0
Difficulty: easy
Learning Objective 1: Calculate the pH of a solution from the hydrogen ion concentration.
Section Reference 1: Section 15.5
84) The pH of a 0.005 M aqueous solution of sulfuric acid is
a) 0.005
b) 2
c) 1
d) 0.01
Difficulty: easy
Learning Objective 1: Calculate the pH of a solution from the hydrogen ion concentration.
Section Reference 1: Section 15.5
85) What is the concentration of an HCl solution if 25.0 mL of the solution is neutralized completely by 40.0 mL of a 0.30 M KOH solution?
a) 0.19 M
b) 300 M
c) 46.9 M
d) 0.48 M
Difficulty: easy
Learning Objective 1: Describe a neutralization reaction and do calculations, involving titrations.
Section Reference 1: Section 15.6
86) An aqueous solution of magnesium chloride has a boiling point of 102.oC. What is the concentration (molality, m) of this solution? The Kb for water is 0.512°C kg solvent/mol solute.
a) 0.67 m
b) 1.30 m
c) 3.91 m
d) 1.95 m
Difficulty: hard
Learning Objective 1: Describe properties, ionization, dissociation, and strength of electrolytes and compare them to nonelectrolytes.
Section Reference 1: Section 15.4
87) What is the concentration of an HBr solution if 12.0 mL of the solution is neutralized by 15.0 mL of a 0.25 M KOH solution?
a) 0.75 M
b) 0.31 M
c) 0.40 M
d) 0.20 M
Difficulty: easy
Learning Objective 1: Calculate the pH of a solution from the hydrogen ion concentration.
Section Reference 1: Section 15.5
88) What is the concentration of a HCl solution if 20.0 mL of the solution is neutralized by 15.0 mL of a 0.10 M Ca(OH)2 solution?
a) 0.075 M
b) 0.038 M
c) 0.15 M
d) 0.13 M
Difficulty: medium
Learning Objective 1: Calculate the pH of a solution from the hydrogen ion concentration.
Section Reference 1: Section 15.5
89) The volume of 0.025M H3PO4 required to neutralize 25 mL of 0.030M Ca(OH)2 is
- 20. mL
- 25 mL
- 40. mL
- 50. mL
Difficulty: medium
Learning Objective 1: Calculate the pH of a solution from the hydrogen ion concentration.
Section Reference 1: Section 15.5
90) What is the concentration of a H2SO4 solution if 10.0 mL of the solution is neutralized by 7.8 mL of a 0.20 M NaOH solution?
a) 0.0026 M
b) 0.078 M
c) 0.156 M
d) 0.31 M
Difficulty: medium
Learning Objective 1: Calculate the pH of a solution from the hydrogen ion concentration.
Section Reference 1: Section 15.5
91) What is the concentration of a H2SO4 solution if 15.0 mL of the solution is neutralized by 3.60 mL of a 0.65 M Ca(OH)2 solution?
a) 0.078 M
b) 0.16 M
c) 0.31 M
d) 2.7 M
Difficulty: medium
Learning Objective 1: Calculate the pH of a solution from the hydrogen ion concentration.
Section Reference 1: Section 15.5
92) How many mL of 1.0 M H2SO4 solution will be neutralized by 10. mL of 1.0 M NaOH is
- 10. mL
- 20. mL
- 2.5 mL
- 5.0 mL
Difficulty: medium
Learning Objective 1: Calculate the pH of a solution from the hydrogen ion concentration.
Section Reference 1: Section 15.5
93) What mass of sodium chloride should be added to 500.0 g of water in order to decrease its freezing point to –1.0 °C? The Kf for water is 1.86°C kg solvent/mol solute. Consider if the solute is an electrolyte or a nonelectrolyte.
a) 0.269 g
b) 134 g
c) 15.7 g
d) 7.85 g
Difficulty: hard
Learning Objective 1: Describe properties, ionization, dissociation, and strength of electrolytes and compare them to nonelectrolytes.
Section Reference 1: Section 15.4
94) What mass of ethanol, C2H5OH, should be added to 200.0 g of water in order to increase its boiling point to 102.5°C? The Kb for water is 0.512°C kg solvent/mol solute. Consider if the solute is an electrolyte or a nonelectrolyte.
a) 4.9 g
b) 0.98 g
c) 45 g
d) 90. g
Difficulty: hard
Learning Objective 1: Describe properties, ionization, dissociation, and strength of electrolytes and compare them to nonelectrolytes.
Section Reference 1: Section 15.4
95) A solution is prepared by adding 0.1000 moles of sugar to 200.0 g of water. What is the boiling point of the solution? The Kb for water is 0.512°C kg solvent/mol solute. Consider if the solute is an electrolyte or a nonelectrolyte.
a) 100.5°C
b) 100.05°C
c) 100.3°C
d) 101.03°C
Difficulty: hard
Learning Objective 1: Describe properties, ionization, dissociation, and strength of electrolytes and compare them to nonelectrolytes.
Section Reference 1: Section 15.4
96) A solution is prepared by adding 35.5 mL of ethylene glycol, C2H6O2, to 250.0 g of water. What is the freezing point of this solution? The Kf for water is 1.86°C kg solvent/mol solute and the density of ethylene glycol is 1.1135 g/mL. Consider if the solute is an electrolyte or a nonelectrolyte.
a) −0.29°C
b) −4.74°C
c) −0.01°C
d) 0.00°C
Difficulty: hard
Learning Objective 1: Calculate the pH of a solution from the hydrogen ion concentration.
Section Reference 1: Section 15.5
97) An aqueous solution is 18.7% by mass Na3PO4. What is the boiling point of this solution? The Kb for water is 0.512°C kg solvent/mol solute. Consider if the solute is an electrolyte or a nonelectrolyte.
a) 102.89°C
b) 100.72°C
c) 101.44°C
d) 100.00 °C
Difficulty: hard
Learning Objective 1: Describe properties, ionization, dissociation, and strength of electrolytes and compare them to nonelectrolytes.
Section Reference 1: Section 15.4
98) Which of the following solutions is a strong electrolyte?
a) AgCl
b) PbI2
c) NH4Cl
d) BaSO4
Difficulty: easy
Learning Objective 1: Describe properties, ionization, dissociation, and strength of electrolytes and compare them to nonelectrolytes.
Section Reference 1: Section 15.4
Question Type: True/False
99) Boron trifluoride is a Lewis acid.
Difficulty: easy
Learning Objective 1: Compare the definitions of acids and bases, including Arrhenius, Brønsted–lowry, and lewis acids and bases
Section Reference 1: Section 15.1
100) A 0.1 M HNO3 solution and a 0.1 M HNO2 solution have the same pH.
Difficulty: medium
Learning Objective 1: Describe properties, ionization, dissociation, and strength of electrolytes and compare them to nonelectrolytes.
Learning Objective 2: Calculate the pH of a solution from the hydrogen ion concentration.
Section Reference 1: Section 15.4 and 15.5
101) Strong acids are strong electrolytes.
Difficulty: easy
Learning Objective 1: Describe properties, ionization, dissociation, and strength of electrolytes and compare them to nonelectrolytes.
Section Reference 1: Section 15.4
102) Weak bases are nonelectrolytes.
Difficulty: easy
Learning Objective 1: Describe properties, ionization, dissociation, and strength of electrolytes and compare them to nonelectrolytes.
Section Reference 1: Section 15.4
103) According to the Lewis acid definition, an acid is a substance that is able to donate a pair of electrons.
Difficulty: easy
Learning Objective 1: Compare the definitions of acids and bases, including Arrhenius, Brønsted–lowry, and lewis acids and bases.
Section Reference 1: Section 15.1
104) A hydronium ion is a hydrated proton.
Difficulty: easy
Learning Objective 1: Compare the definitions of acids and bases, including Arrhenius, Brønsted–lowry, and lewis acids and bases.
Section Reference 1: Section 15.1
105) The following substances are Lewis bases: ammonia, water, and methanol, CH3OH.
Difficulty: easy
Learning Objective 1: Compare the definitions of acids and bases, including Arrhenius, Brønsted–lowry, and lewis acids and bases.
Section Reference 1: Section 15.1
106) An electrolyte is a substance whose aqueous solution conducts an electric current.
Difficulty: easy
Learning Objective 1: Describe properties, ionization, dissociation, and strength of electrolytes and compare them to nonelectrolytes.
Section Reference 1: Section 15.4
107) At 25 °C the concentration of H + in pure water is 1 
10 –7 M.
Difficulty: easy
Learning Objective 1: Describe properties, ionization, dissociation, and strength of electrolytes and compare them to nonelectrolytes.
Section Reference 1: Section 15.4
108) Water can act both as an acid and a base.
Difficulty: easy
Learning Objective 1: Describe properties, ionization, dissociation, and strength of electrolytes and compare them to nonelectrolytes.
Section Reference 1: Section 15.4
109) The net ionic equation for the neutralization of sulfuric acid by magnesium hydroxide is 
.
Difficulty: medium
Learning Objective 1: Write net ionic equations using the stated rules.
Section Reference 1: Section 15.7
Question Type: Essay
110) For the following neutralization reaction:
hydrochloric acid plus barium hydroxide yields barium chloride plus water
a) Write the balanced formula equation.
b) Write the total ionic equation.
c) Write the net ionic equation.
Difficulty: hard
Learning Objective 1: Describe a neutralization reaction and do calculations, involving titrations.
Learning Objective 2: Write net ionic equations using the stated rules.
Section Reference 1: Section 15.6 and 15.7
111) For the following neutralization reaction:
sulfuric acid plus potassium hydroxide yields potassium sulfate plus water
a) Write the balanced formula equation.
b) Write the total ionic equation.
c) Write the net ionic equation.
Difficulty: hard
Learning Objective 1: Describe a neutralization reaction and do calculations, involving titrations.
Learning Objective 2: Write net ionic equations using the stated rules.
Section Reference 1: Section 15.6 and 15.7
112) Calculate the pH of the following solutions:
a) 0.034 M HCl
b) 0.31 M HNO3
c) 0.0034 M HI
Difficulty: easy
Learning Objective 1: Calculate the pH of a solution from the hydrogen ion concentration.
Section Reference 1: Section 15.5
113) The pH of an aqueous solution of hydrobromic acid solution is 1.2. How many mL of water should be added to 250. mL of this solution to increase the pH to 1.7? Assume that volumes are additive.
Difficulty: hard
Learning Objective 1: Calculate the pH of a solution from the hydrogen ion concentration.
Section Reference 1: Section 15.5
114) A 40.0 mL sample of sulfuric acid is titrated to a neutral end point by the addition of 15.6 mL of a 0.250 M potassium hydroxide solution.
a) Write the balanced formula equation for this reaction.
b) What is the molarity of the sulfuric acid solution in this question?
Difficulty: medium
Learning Objective 1: Describe a neutralization reaction and do calculations, involving titrations.
Section Reference 1: Section 15.6
115) A 20.0 mL sample of nitric acid is titrated to the end point by the addition of 3.60 mL of a 0.80 M solution of barium hydroxide.
a) Write a balanced formula equation for this reaction.
b) What is the molarity of the nitric acid solution in this question?
Difficulty: medium
Learning Objective 1: Describe a neutralization reaction and do calculations, involving titrations.
Section Reference 1: Section 15.6
116) A 400. g sample of aluminum sulfate is dissolved in 3000. mL of solution.
a) What is the molarity of the solution?
b) What is the molarity of aluminum ion in the solution?
c) What is the molarity of the sulfate ion in the solution?
Difficulty: hard
Learning Objective 1: Describe properties, ionization, dissociation, and strength of electrolytes and compare them to nonelectrolytes.
Section Reference 1: Section 15.4
117) A 50.0 mL aliquot of a 1.0 M aqueous nitric acid solution is added to a solution prepared from 0.50 g of sodium hydroxide dissolved in enough water to make 500.0 mL of solution. Will the resulting solution be acidic or basic? Support your answer by showing the appropriate calculations.
Difficulty: medium
Learning Objective 1: Describe a neutralization reaction and do calculations, involving titrations.
Section Reference 1: Section 15.6
118) A solution of an acid, with a general formula HA, contains 0.400 moles of H +1. The acid solution is neutralized by 43.4 mL of sodium hydroxide. What is the molarity of the sodium hydroxide solution?
Difficulty: easy
Learning Objective 1: Describe a neutralization reaction and do calculations, involving titrations.
Section Reference 1: Section 15.6
119) A base solution contains 0.400 mol of OH –. The base solution is neutralized by 43.4 mL of sulfuric acid. What is the molarity of the sulfuric acid solution?
Difficulty: medium
Learning Objective 1: Describe a neutralization reaction and do calculations, involving titrations.
Section Reference 1: Section 15.6
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Test Bank | Foundations of College Chemistry 15e by Hein Arena
By Hein Arena, Willard