Name: ________________________ Class: ___________________ Date: __________
fdd
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____
____
1. Acids taste
a. sweet.
b. sour.
c.
d.
bitter.
salty.
2. Acetic acid is found in
a. lemons.
b. vinegar.
c.
d.
sour milk.
apples.
____
3. Acids generally release H2 gas when they react with
a. nonmetals.
c. active metals.
b. semimetals.
d. inactive metals.
____
4. Acids react with
a. bases to produce salts and water.
b. salts to produce bases and water.
c.
d.
water to produce bases and salts.
neither bases, salts, nor water.
5. Aqueous solutions of acids
a. contain only two different elements.
b. carry electricity.
c.
d.
have very high boiling points.
cannot be prepared.
6. Bases taste
a. soapy.
b. sour.
c.
d.
sweet.
bitter.
7. Bases feel
a. rough.
b. moist.
c.
d.
slippery.
dry.
8. Bases react with
a. acids to produce salts and water.
b. salts to produce acids and water.
c.
d.
water to produce acids and salts.
neither acids, salts, nor water.
9. Aqueous solutions of bases
a. contain only two different elements.
b. carry electricity.
c.
d.
have very high boiling points.
cannot be prepared.
____ 10. A binary acid contains
a. two hydrogen atoms.
b. hydrogen and one other element.
c.
d.
hydrogen and two other elements.
hydrogen and three other elements.
____ 11. Which of the following is a binary acid?
a. H2SO4
b. CH3COOH
c.
d.
HBr
NaOH
____
____
____
____
____
1
ID: A
Name: ________________________
____ 12. The name of a binary acid
a. has no prefix.
b. begins with the prefix bi-.
ID: A
c.
d.
ends with the suffix -ous.
begins with the prefix hydro-.
____ 13. An oxyacid contains
a. oxygen and hydrogen only.
b. oxygen, hydrogen, and one other element.
c. oxygen, hydrogen, and two other elements.
d. oxygen and an element other than hydrogen.
____ 14. Which of the following is not an oxyacid?
a. H2O2
b. H2SO4
c.
d.
HClO4
HClO2
____ 15. Which of the following is perchloric acid?
a. HClO
b. HClO2
c.
d.
HClO3
HClO4
____ 16. Which of the following is chlorous acid?
a. HClO
b. HClO2
c.
d.
HClO3
HClO4
____ 17. Which of the following is chloric acid?
a. HClO
b. HClO2
c.
d.
HClO3
HClO4
____ 18. Compared with acids that have the suffix -ic, acids that have the suffix -ous contain
a. more hydrogen.
c. less oxygen.
b. more oxygen.
d. the same amount of oxygen.
____ 19. An acid ending with the suffix -ic produces an anion with the
a. suffix -ate.
c. prefix hydro-.
b. suffix -ite.
d. suffix -ous.
____ 20. Which acid is manufactured in largest quantity?
a. hydrochloric acid
c.
b. phosphoric acid
d.
nitric acid
sulfuric acid
____ 21. Which acid is used in batteries?
a. hydrochloric acid
b. phosphoric acid
nitric acid
sulfuric acid
c.
d.
____ 22. Which acid is used to make fertilizers and detergents and is a flavoring agent in beverages?
a. hydrochloric acid
c. nitric acid
b. phosphoric acid
d. sulfuric acid
____ 23. Which acid is used mainly in the manufacture of explosives, rubber, plastics, dyes, and drugs?
a. hydrochloric acid
c. nitric acid
b. phosphoric acid
d. sulfuric acid
2
Name: ________________________
____ 24. Which acid is produced in the stomach?
a. hydrochloric acid
b. phosphoric acid
ID: A
c.
d.
nitric acid
sulfuric acid
____ 25. Which acid is used to pickle metals, process food, and activate oil wells?
a. hydrochloric acid
c. nitric acid
b. phosphoric acid
d. sulfuric acid
____ 26. Which acid is found in vinegar?
a. acetic acid
b. nitric acid
c.
d.
phosphoric acid
hydrochloric acid
____ 27. Which acid turns yellowish on standing?
a. acetic acid
b. nitric acid
c.
d.
phosphoric acid
hydrochloric acid
____ 28. The traditional definition of acids is based on the observations of
a. Brønsted and Lowry.
c. Arrhenius.
b. Lewis.
d. Mendeleev.
____ 29. An Arrhenius acid contains
a. hydrogen that does not ionize.
b. hydrogen that ionizes to form hydrogen ions.
c. oxygen that ionizes to form hydroxide ions.
d. oxygen that ionizes to form oxygen ions.
____ 30. Which of the following did Arrhenius theorize?
a. An acid increases the concentration of OH– ions in solution.
b. A base increases the concentration of H+ ions in solution.
c. Acids and bases contain nonpolar molecules.
d. Because acids and bases carry electric current, they must produce ions in solution.
____ 31. Arrhenius theorized that an acid is a chemical compound that
a. increases the concentration of hydrogen ions when dissolved in water.
b. increases the concentration of hydroxide ions when dissolved in water.
c. decreases the concentration of hydrogen ions when dissolved in water.
d. decreases the concentration of hydroxide ions when dissolved in water.
____ 32. Arrhenius theorized that a base is a chemical compound that
a. increases the concentration of hydrogen ions when dissolved in water.
b. increases the concentration of hydroxide ions when dissolved in water.
c. decreases the concentration of hydrogen ions when dissolved in water.
d. decreases the concentration of hydroxide ions when dissolved in water.
____ 33. Which statement about Arrhenius acids is false?
a. Their water solutions are called aqueous acids.
b. They are molecular compounds with ionizable hydrogen atoms.
c. Their pure aqueous solutions are electrolytes.
d. They increase the concentration of hydroxide ions in aqueous solution.
3
Name: ________________________
ID: A
____ 34. Which statement about Arrhenius bases is false?
a. Some are ionic hydroxides.
b. They dissociate in solution to release hydroxide ions into the solution.
c. They increase the concentration of hydrogen ions in aqueous solution.
d. Some react with water and remove a hydrogen ion, leaving hydroxide ions.
____ 35. A substance that ionizes nearly completely in aqueous solutions and produces H3O+ is a
a. weak base.
c. weak acid.
b. strong base.
d. strong acid.
____ 36. Which of the following is not a strong acid?
a. HNO3
b. CH3COOH
c.
d.
H2SO4
HCl
____ 37. Which of the following is a strong acid?
a. HSO 4
b. H2SO4
c.
d.
CH3COOH
H3PO4
____ 38. The dilute aqueous solution of a weak base contains
a. hydronium ions.
c. acid molecules.
b. anions.
d. all of the above
____ 39. In water, hydroxides of Group 2 metals
a. are all strong bases.
b. are all weak bases.
c.
d.
are all acids.
are nonelectrolytes.
____ 40. Which of the following is a weak base?
a. NH3
b. KOH
c.
d.
NaOH
Ba(OH)2
____ 41. Which of the following is a strong base?
a. KOH
b. H2
c.
d.
NH3
HCl
____ 42. Many organic compounds, such as codeine, that contain nitrogen are
a. strong bases.
c. strong acids.
b. weak bases.
d. weak acids.
____ 43. Which of the following is a triprotic acid?
a. H2SO4
b. CH3COOH
c.
d.
HCl
H3PO4
____ 44. Which of the following is a diprotic acid?
a. H2SO4
b. CH3COOH
c.
d.
HCl
H3PO4
____ 45. Whose definition of acids and bases emphasizes the role of protons?
a. Brønsted and Lowry
c. Arrhenius
b. Lewis
d. Bohr
4
Name: ________________________
____ 46. A Brønsted-Lowry acid is a(n)
a. electron-pair acceptor.
b. electron-pair donor.
ID: A
c.
d.
proton acceptor.
proton donor.
____ 47. In the equation HCl(g) + H2O(l)  H3O+(aq) + Cl–(aq), which species is a Brønsted-Lowry acid?
a. HCl
c. Cl–
b. H2O
d. None of the above
____ 48. A Brønsted-Lowry base is a(n)
a. producer of OH– ions.
b. proton acceptor.
c.
d.
electron-pair donor.
electron-pair acceptor.
____ 49. In the reaction represented by the equation NH 3  H 2 O  NH 4  OH  , H2O is a(n)
a. Brønsted-Lowry acid.
c. Brønsted-Lowry base.
b. Lewis base.
d. Arrhenius.
____ 50. A Lewis acid is
a. an electron-pair acceptor.
b. an electron-pair donor.
c.
d.
a proton acceptor.
a proton donor.
____ 51. Whose acid definition is the broadest?
a. Arrhenius
b. Lewis
c.
d.
Brønsted-Lowry
Faraday
____ 52. A Lewis base is a(n)
a. producer of OH– ions.
b. proton acceptor.
c.
d.
electron-pair donor.
electron-pair acceptor.
____ 53. An electron-pair donor is a
a. Arrhenius acid.
b. Brønsted-Lowry acid.
c.
d.
Brønsted-Lowry base.
Lewis base.
____ 54. Whenever ammonia donates an electron pair to form a covalent bond, it acts as a(n)
a. Brønsted-Lowry base.
c. Lewis base.
b. Lewis acid.
d. Arrhenius acid.
____ 55. An electron-pair acceptor is a(n)
a. Brønsted-Lowry base.
b. Lewis acid.
c.
d.
Lewis base.
Arrhenius acid.
____ 56. Which is a Lewis acid but not a Brønsted-Lowry acid?
a. HCl
c. BF3
b. NH3
d. None of the above
____ 57. In the reaction represented by the equation Ni2  + nH 2 O [Ni(H 2 O) n ] 2  H2O is a
a. Brønsted-Lowry acid.
c. Lewis acid.
b. Brønsted-Lowry base.
d. Lewis base.
5
Name: ________________________
ID: A
____ 58. The reaction represented by the equation Ag+(aq) + 2NH3(aq)  [Ag(NH3)2]+(aq) is a(n)
a. traditional acid-base reaction.
c. Brønsted-Lowry acid-base reaction.
b. Lewis acid-base reaction.
d. None of the above
____ 59. In the reaction represented by the equation Ag+(aq) + 2NH3(aq)  [Ag(NH3)2]+(aq), Ag+ is a
a. Brønsted-Lowry acid.
c. Brønsted-Lowry base.
b. Lewis acid.
d. Arrhenius base.
____ 60. A conjugate acid is the species that
a. remains after a base has given up a proton.
b. is formed by the addition of a proton to a base.
c. is formed by the addition of a proton to an acid.
d. remains after an acid has given up a proton.
____ 61. A species that remains when an acid has lost a proton is a
a. conjugate base.
c. strong base.
b. conjugate acid.
d. strong acid.
____ 62. A species that is formed when a base gains a proton is a
a. conjugate base.
c. strong base.
b. conjugate acid.
d. strong acid.
____ 63. How many conjugate acid-base pairs participate in a Brønsted-Lowry acid-base reaction?
a. none
c. two
b. one
d. four
____ 64. The members of a conjugate acid-base pair
a. appear on the same side of the chemical equation.
b. appear on opposite sides of the chemical equation.
c. might appear on the same side or on opposite sides of the equation.
d. are not included in the chemical equation.
____ 65. In a conjugate acid-base pair, the acid typically has
a. one more proton than the base.
b. one fewer proton than the base.
c. two fewer protons than the base.
d. the same number of protons as the base.
____ 66. Whose theory of acids and bases do conjugate acids and bases belong to?
a. Arrhenius
c. Brønsted-Lowry
b. Lewis
d. None of the above
____ 67. The two members of a conjugate acid-base pair differ by a
a. water molecule.
c. hydronium ion.
b. hydroxide ion.
d. proton.
H 3 O + + F  , a conjugate acid-base pair is
____ 68. In the reaction represented by the equation HF + H 2 O
a. HF and H2O.
c. H3O+ and H2O.
–
+
b. F and H3O .
d. HF and H3O+.
6
Name: ________________________
ID: A
H 3 O + + F  , a conjugate acid-base pair is
____ 69. In the reaction represented by the equation HF + H 2 O
a. F– and H2O.
c. H3O+ and HF.
–
b. HF and F .
d. HF and H2O.
____ 70. In the reaction represented by the equation HClO 3 + NH 3
NH 4 + ClO 3 the conjugate acid of NH3 is
a.
HClO3.
c.
NH 4 .
b.
ClO 3 .
d.
not shown.
____ 71. In the reaction represented by the equation HClO 3  NH 3
a.
b.
ClO 3 .
NH3.
c.
d.
NH 4  ClO 3 , the conjugate base of HClO3 is
NH 4 .
not shown.
____ 72. In the reaction represented by the equation CH 3 COOH  H 2 O
of CH3COO– is
a. H2O.
c. H3O+.
b. CH3COOH.
d. not shown.
H 3 O +  CH 3 COO – , the conjugate acid
____ 73. In the reaction represented by the equation CH 3 COOH  H 2 O
of H3O+ is
a. H2O.
c. CH3COO–.
b. CH3COOH.
d. not shown.
H 3 O +  CH 3 COO – , the conjugate base
____ 74. The conjugate of a strong base is a
a. strong acid.
b. weak acid.
c.
d.
strong base.
weak base.
____ 75. The conjugate of a strong acid is a
a. strong acid.
b. weak acid.
c.
d.
strong base.
weak base.
____ 76. The conjugate of a weak base is a
a. strong acid.
b. weak acid.
c.
d.
strong base.
weak base.
____ 77. The conjugate of a weak acid is a
a. strong acid.
b. weak acid.
c.
d.
strong base.
weak base.
____ 78. A base is weak if its tendency to
a. attract a proton is great.
b. attract a proton is slight.
c.
d.
donate a proton is great.
donate a proton is slight.
____ 79. If a substance has a great tendency to give up protons, its conjugate has a
a. great tendency to give up protons.
c. slight tendency to give up protons.
b. great tendency to attract protons.
d. slight tendency to attract protons.
7
Name: ________________________
ID: A
____ 80. In the equation HI + H2O  H3O+ + I–, HI is a strong acid and I– is a
a. strong acid.
c. weak acid.
b. strong base.
d. weak base.
H 3 O +  CH 3 COO – , H2O is a weak base and H3O+ is a
c. weak acid.
d. weak base.
____ 81. In the equation CH 3 COOH  H 2 O
a. strong acid.
b. strong base.
____ 82. In the equation HClO 4  NH 3
a. strong acid.
b. strong base.
NH 4  ClO 4 , ClO 4 is a weak base and HClO4 is a
c. weak acid.
d. weak base.
____ 83. An amphoteric species is one that reacts as a(n)
a. acid only.
c.
b. base only.
d.
acid or base.
None of the above
____ 84. A species that can react as either an acid or a base is a(n)
a. Lewis acid.
c. oxyacid.
b. amphoteric substance.
d. salt.
____ 85. Which of the following is amphoteric?
a. H2SO4
b. SO 24 
c.
d.
H+
HSO 4
____ 86. Which of the following is amphoteric?
a. H3PO4
c.
HPO 24 
d.
PO 34 
c.
d.
H+
O2–
b.
H+
____ 87. Which of the following is amphoteric?
a. H2O
b. H3O+
____ 88. In the reaction represented by the equation H 2 SO 4 + H 2 O
H 3 O + + HSO 4 , the ion HSO 4 acts as a(n)
a. acid.
c. spectator species.
b. base.
d. salt.
H 3 O + + SO 24  , the ion HSO 4 acts as a(n)
____ 89. In the reaction represented by the equation HSO 4  H 2 O
a. acid.
c. spectator species.
b. base.
d. salt.
____ 90. In the reaction represented by the equation H 3 PO 4  H 2 O
H 3 O + + H 2 PO 4 , the ion H 2 PO 4 acts as a(n)
a. acid.
c. spectator species.
b. base.
d. salt.
8
Name: ________________________
ID: A
H 3 O + + H 2 PO 4 , the molecule H 2 O acts as
____ 91. In the reaction represented by the equation H 3 PO 4  H 2 O
a(n)
a. acid.
c. spectator species.
b. base.
d. salt.
____ 92. The substances produced when KOH(aq) neutralizes HCl(aq) are
a. HClO(aq) and KH(aq).
c. H2O(l) and KCl(aq).
b. KH2O+(aq) and Cl–(aq).
d. H3O+(aq) and KCl(aq).
____ 93. A salt is not
a. an ionic compound composed of a metal cation from a base.
b. an ionic compound composed of an anion from an acid.
c. a product of neutralization.
d. a proton donor.
____ 94. Which of the following is not a reactant in a neutralization reaction?
a. H3O+ ion
b. OH– ion
c. an acid and a base in an aqueous solution
d. a salt
____ 95. Which compound is produced by a neutralization?
a. H2O(l)
c. Ca(OH)2(s)
b. HNO3(aq)
d. H3PO4(aq)
____ 96. Which of the following gases does not dissolve in atmospheric water to produce acidic solutions?
a. NO
c. O2
b. NO2
d. CO2
Choose the best answer from the options that follow each question.
____ 97. Which of the properties listed below is not characteristic of an acid?
a. a sour taste
b. a slippery feel
c. the ability to conduct an electric current
d. reactivity with metals
____ 98. Which is an example of a weak acid?
a. HCl
b. H2SO4
c. H3PO4
d. HNO3
____ 99. Acetic acid is found in
a. vinegar.
b. the stomach.
c. antacids.
d. oranges.
9
Name: ________________________
ID: A
____ 100. A characteristic of an Arrhenius base is that it
a. is an electrolyte.
b. tastes bitter.
c. dissociates to form OH  ions.
d. All of the above
____ 101. Which of the following is a Brønsted-Lowry base?
a. HCl
b. HCO 3
c. H3O+
d. H3PO4
____ 102. In the reaction represented by the equation
H2C2O4(aq) + CH3NH2(aq)  HC2O4(aq) + CH3NH 3 (aq),
which of these is a conjugate acid-base pair?
a. H2C2O4(aq) and CH3NH2(aq)
b. H2C2O4(aq) and CH3NH 3 (aq)
c.
CH3NH2(aq) and CH3NH 3 (aq)
d.
HC2O 4 (aq) and CH3NH 3 (aq)
____ 103. What is the correct formula for hydrosulfuric acid?
a. H2SO4
b. H2S
c. H2SO3
d. SO 24 
____ 104. What is the correct acid name for an aqueous solution of HClO4?
a. hypochlorous acid
b. chlorous acid
c. chloric acid
d. perchloric acid
____ 105. A substance that increases the concentration of OH  ions in an aqueous solution is known as a(n)
a. Arrhenius acid.
b. Arrhenius base.
c. Lewis acid.
d. Lewis base.
____ 106. An Arrhenius acid in an aqueous solution
a. attracts negatively charged anions.
b. attracts positively charged cations.
c. gives up one or more of its hydrogen ions to water molecules.
d. forms ionic bonds with water molecules.
10
Name: ________________________
ID: A
____ 107. Which of the following is an indication of acid strength?
a. the number of hydrogen atoms in the formula of the acid
b. how strongly an aqueous solution of the acid conducts an electric current
c. how quickly the acid dissolves in water
d. the number of total atoms in one molecule of the acid
____ 108. Which of the following is an organic acid?
a. CH3COOH
b. H2SO4
c. HI
d. HClO3
____ 109. The neutralization of any strong acid and strong base produces mostly
a. H2O molecules.
b. H3O+ and OH  ions.
c. H3O+ ions.
d. OH  ions.
____ 110. A strong base in an aqueous solution
a. is a weak electrolyte.
b. produces many H+ ions.
c. will not dissolve.
d. completely dissociates into ions.
____ 111. In a Brønsted-Lowry acid-base reaction, what are transferred from one reactant to another?
a. electrons
b. water molecules
c. protons
d. OH  ions
____ 112. How many protons per molecule can a monoprotic acid donate?
a. one
b. two
c. three
d. zero
____ 113. How many stages of ionization does phosphoric acid go through?
a. one
b. two
c. three
d. four
____ 114. Which substance is a Lewis acid in the reaction shown by the equation below?
BF3(aq) + F  (aq)  BF 4 4 (aq)
a. BF3
b. F 
c. BF 4
d. None of the above
11
Name: ________________________
ID: A
____ 115. What is the conjugate acid of water?
a. OH 
b. H3O+
c. H2O2
d. HOH
____ 116. HCl is a strong acid. When it combines with water, the conjugate of HCl will be a
a. weak base.
b. weak acid.
c. strong base.
d. strong acid.
____ 117. Which is the stronger base in the reaction represented by the following equation?
CH3COOH(aq) + H2O(l)  H3O+(aq) + CH3COO  (aq)
a. CH3COOH
b. CH3COO 
c. H3O+
d. H2O
____ 118. Consider the reaction represented by the equation below.
HClO4(aq) + H2O(l)  H3O+(aq) + ClO 4 (aq)
Which substances are present in the greatest concentrations?
a. HClO4 and H2O
b. HClO4 and ClO 4
c.
d.
H3O+ and ClO 4
H2O and H3O+
____ 119. Consider the two equations below.
H2SO4(aq) + H2O(l)  H3O+(aq) + HSO 4 (aq)
NH3(g) + H2O(l)  NH 4 (aq) + OH  (aq)
They illustrate that water is
a. an acid in both reactions.
b. a base in both reactions.
c. amphoteric.
d. a weak electrolyte.
____ 120. What is the correct net ionic equation for the neutralization reaction between the substances below?
HNO3(aq) + KOH(aq)
a. NO 3 (aq) + K+(aq)  KNO3(aq)
b.
c.
d.
H3O+(aq) + OH  (aq)  2H2O(l)
H3O+(aq) + NO 3 (aq) + K+(aq) + OH  (aq)  NO 3 (aq) + K+(aq) + 2H2O(l)
HNO3(aq) + KOH(aq)  KNO3(aq) + H2O(l)
12
Name: ________________________
ID: A
____ 121. Sulfur trioxide gas dissolves in atmospheric water. The product of the reaction, which falls to the ground as a
component of acid rain or snow, is
a. H2SO4(aq).
b. HS(aq).
c. H3O+(aq).
d. SO 24  (aq).
PART I Choose the best answer from the options that follow each question.
____ 122. Which of the following is an oxyacid?
a. HCl
b. H2O
c. H2S
d. H2SO4
____ 123. Which acid is produced in the stomach?
a. HNO3
b. CH3COOH
c. H2SO4
d. HCl
____ 124. Which of the following is a strong base?
a. NH3
b. aniline
c. NaOH
d. acetate ion
____ 125. In the reaction represented by the equation HF(aq) + H2O(l)  H3O+(aq) + F  (aq), a conjugate acid-base pair
is
a. F  and H2O.
b. H3O+ and HF.
c. HF and F  .
d. HF and H2O.
____ 126. If H2O in the reaction represented by the equation H2O + C2H3COOH  H3O+ + C2H3COO  is considered to
be a weaker base, then H3O is a
a. stronger acid.
b. stronger base.
c. weaker acid.
d. weaker base.
____ 127. Proton-transfer reactions favor production of the
a. stronger acid and stronger base.
b. weaker acid and weaker base.
c. stronger acid and weaker base.
d. weaker acid and stronger base.
13
Name: ________________________
ID: A
____ 128. Aqueous solutions of most bases contain
a. hydroxide ions and cations.
b. hydroxide ions and anions.
c. hydrogen ions and anions.
d. hydrogen ions and cations.
____ 129. Acid strength increases with
a. increasing polarity and increasing bond strength.
b. increasing polarity and decreasing bond strength.
c. decreasing polarity and increasing bond strength.
d. decreasing polarity and decreasing bond strength.
Choose the best answer from the options that follow each question.
____ 130. A strong acid
a. ionizes completely in solution.
b. produces hydronium ions in solution.
c. reacts with metals that are more active than hydrogen.
d. All of the above
____ 131. When a solution of hydrochloric acid, HCl, reacts with zinc, which of the following substances is a reactant?
a. Clb. H+
c. H3O+
d. H2O
____ 132. Which of the following characteristics describes a base?
a. reacts with oils in the skin and converts them to acids
b. forms alkaline solutions
c. is a nonelectrolyte
d. None of the above
____ 133. Which of the following substances is a weak base?
a. NH3
b. KOH
c. K2O
d. NaOH
____ 134. Strong acids are
a. strong electrolytes.
b. weak electrolytes.
c. nonelectrolytes.
d. nonionized.
____ 135. Hydroxides of Group 1 metals
a. are all strong bases.
b. are all weak bases.
c. are all acids.
d. do not dissociate in solution.
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Name: ________________________
ID: A
____ 136. Strong bases are
a. strong electrolytes.
b. weak electrolytes.
c. nonelectrolytes.
d. also strong acids.
____ 137. Which of the following is not a strong acid?
a. HCl
b. H2SO4
c. CH3COOH
d. HBr
____ 138. A highly polar molecule that contains a weak bond between a hydrogen atom and another element would be
a. a weak acid.
b. unable to ionize completely.
c. a nonelectrolyte.
d. a strong acid.
____ 139. An Arrhenius acid is a chemical compound that
a. does not conduct electricity.
b. increases the concentration of H+ ions in solution.
c. reacts with water to remove H+ ions.
d. dissociates to release OH- ions in solution.
Choose the best answer from the options that follow each question.
____ 140. All Brønsted-Lowry acids
a. are aqueous solutions.
b. can act as Arrhenius acids.
c. donate protons.
d. All of the above
____ 141. Which of the following substances is both a Brønsted-Lowry base and an Arrhenius base?
a. NH3(s)
b. NH3(aq)
c. HCl(g)
d. HCl(aq)
____ 142. .In the following reaction, which substance acts as a Brønsted-Lowry acid?
HCl + NH3  NH 4 + Cl 
a.
b.
c.
HCl
NH3
NH 4
d.
Cl 
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Name: ________________________
ID: A
____ 143. In the following reaction, which substance acts as a Brønsted-Lowry base?
HCl + NH3  NH 4 + Cl 
a.
b.
c.
HCl
NH3
NH 4
d.
Cl 
____ 144. Which of the following is a polyprotic acid?
a. HCl
b. H2SO4
c. HNO3
d. HF
____ 145. Which stage of ionization of H3PO4 produces the most ions in solution?
a. H3PO4(aq) + H2O(l) H3O+(aq) + H2PO 4 (aq)
b.
H2PO 4 (aq) + H2O(l) H3O+(aq) + HPO 24  (aq)
c.
d.
HPO 24  (aq) + H2O(l) H3O+(aq) + PO 34  (aq)
All stages produce the same number of ions in solution.
____ 146. Which of the following can act as a Lewis acid?
a. NH3(aq)
b. Cl  (aq)
c.
d.
BF 4 (aq)
Ag+(aq)
____ 147. A Lewis acid
a. is an anion.
b. donates an electron pair to form a covalent bond.
c. can be a substance that does not contain a hydrogen atom.
d. All of the above
____ 148. Which of the following substances can act as an Arrhenius base, a Brønsted-Lowry base, and a Lewis base?
a. F  (aq)
b.
c.
d.
NH3(aq)
H+(aq)
NaOH(aq)
____ 149. Which of the following will be present in an aqueous solution of H2SO4?
a. H3O+(aq)
b. HSO 4 (aq)
c.
d.
SO 24  (aq)
All of the above
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Name: ________________________
ID: A
Choose the best answer from the options that follow each question.
____ 150. What is the conjugate base of the hydronium ion, H3O+?
a. OH 
b.
c.
d.
H+
H2O
H3O2+
____ 151. The conjugate acid of the chloride ion, Cl  , is
a.
b.
c.
d.
Cl2.
H+.
HCl.
ClO.
____ 152. A conjugate acid is an acid that forms when
a. the acid gains a proton.
b. a base loses a proton.
c. a base gains a proton.
d. an atom accepts an electron pair.
____ 153. Ions that are present before and after a neutralization reaction are
a. nonelectrolytes.
b. metal ions.
c. neutral ions.
d. spectator ions.
____ 154. In an acid-base reaction, the conjugate base of the weaker acid is the
a. stronger acid.
b. stronger base.
c. weaker base.
d. None of the above
____ 155. An amphoteric species is one that reacts at 25°C as a(n)
a. acid only.
b. base only.
c. acid or base.
d. None of the above
____ 156. A conjugate base is the species that
a. remains after a base has given up a proton.
b. is formed by the addition of a proton.
c. is formed by the addition of a proton to a base.
d. remains after an acid has given up a proton.
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Name: ________________________
ID: A
____ 157. In the following reaction, which substance is the conjugate base of HClO4?
HClO4(aq) + H2O(l)  H3O+(aq) + ClO 4 (aq)
a. H2O(l)
b. H3O+(aq)
c. ClO 4
d. Both (a) and (b)
____ 158. Water is amphoteric. If it reacts with a compound that is a stronger acid than itself, water acts as a
a. weak base.
b. strong base.
c. weak acid.
d. hydroxide ion.
____ 159. Which of the following is most acidic?
a. H2CrO4
b. Cr(OH)3
c. Cr(OH)2
d. Cr
Short Answer
1. What determines the behavior of an amphoteric compound?
2. Explain how industrial processes create acid rain.
3. Use the following equation to explain acid rain: SO3(g) + H2O(l)  H2SO4(aq)
PART III
Write the name of each of the following acids in the space provided.
4. HNO2
5. HCl
6. H2CO3
7. H2SO4
8. HI
9. HBrO
Write the formula for each of the following acids in the space provided.
10. hydrosulfuric acid
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Name: ________________________
ID: A
11. nitric acid
12. phosphorous acid
13. perchloric acid
Refer to the equation below to answer the following questions.
HCl(g) + NH3(l)  NH  (aq) + Cl  (aq)
4
14. List the conjugate acid-base pairs.
15. Identify each reactant and product as acidic or basic.
Refer to the equation below to answer the following questions.
H2O(l) + NH3(g)  NH 4 (aq) + OH  (aq)
16. List the conjugate acid-base pairs.
17. Identify each reactant and product as a proton donor or a proton acceptor.
Refer to the following statement to answer the following questions:
Dilute HCl(aq) and NaOH(aq) are mixed in chemically equivalent quantities
18. Write the chemical equation for the reaction.
19. Write the overall ionic equation for the reaction.
20. Write the net ionic equation.
Use the following three acids to answer the following questions.
iodic acid
hypoiodous acid
periodic acid
21. Give the formulas for these three acids.
22. List the acids in order of increasing acid strength.
PART IV Write the answers to the following questions in the space provided.
23. Explain the difference between strong acids and weak acids.
24. Explain how the production of sulfur trioxide, SO3, in industrial processes can result in acid rain. Write an
equation for the reaction.
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Name: ________________________
ID: A
25. List five properties of aqueous acids.
26. Write the balanced equations that describe the three-stage ionization of phosphoric acid in a dilute aqueous
solution.
Essay
1. Is the reaction to the left or the reaction to the right more favorable in the following reaction? Explain your
answer in terms of acid and base strengths.
CH3COOH(aq) + H2O(l)
H3O+(aq) + CH3COO–(aq)
Completion
Complete each statement.
PART II Write the correct term (or terms) in the space provided.
1. A substance that ionizes almost completely in aqueous solutions, producing H3O+ ions, is a(n)
____________________ acid.
2. An acid that contains hydrogen and only one other element is called a(n) ____________________ acid.
3. The species that forms when an acid has given up a proton is called the acid’s ____________________.
4. An acid that can donate two protons per molecule is called a(n) ____________________ acid.
5. Bases are said to be neutralized when they react with ____________________ to yield
____________________ and a(n) ____________________.
6. Any species that can react as either an acid or a base is described as ____________________.
7. Barium carbonate will react with hydrochloric acid to produce ____________________,
____________________, and ____________________.
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