Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
|
|
1.
|
When an acid reacts with a base, what compounds are formed?
a.
|
a salt only
|
c.
|
metal oxides only
|
b.
|
water only
|
d.
|
a salt and water
|
|
|
|
|
|
|
2.
|
What is the formula for phosphoric acid?
a.
|
HPO
|
c.
|
HPO
|
b.
|
HPO
|
d.
|
HPO
|
|
|
|
|
|
|
3.
|
In a neutral solution, the [H] is ____.
a.
|
10M
|
c.
|
1 108M
|
b.
|
zero
|
d.
|
equal to [OH]
|
|
|
|
|
|
|
4.
|
What is the best description for a solution with a hydroxide-ion concentration of 1 10M?
a.
|
acidic
|
c.
|
neutral
|
b.
|
basic
|
d.
|
The answer cannot be determined.
|
|
|
|
|
|
|
5.
|
What is pH?
a.
|
the negative logarithm of the hydrogen ion concentration
|
b.
|
the positive logarithm of the hydrogen ion concentration
|
c.
|
the negative logarithm of the hydroxide ion concentration
|
d.
|
the positive logarithm of the hydroxide ion concentration
|
|
|
|
|
6.
|
Which type of solution is one with a pH of 8?
a.
|
acidic
|
b.
|
basic
|
c.
|
neutral
|
d.
|
The type varies, depending on the solution.
|
|
|
|
|
7.
|
Which of these solutions is the most basic?
|
|
8.
|
Bases make litmus paper turn
a.
|
blue.
|
c.
|
yellow.
|
b.
|
red.
|
d.
|
black.
|
|
|
|
|
|
|
9.
|
Which of the following is nitrous acid?
a.
|
HNO
|
c.
|
HNO3
|
b.
|
HNO2
|
d.
|
HNO4
|
|
|
|
|
|
|
10.
|
Which of the following is Nitric acid?
a.
|
HNO
|
c.
|
HNO3
|
b.
|
HNO2
|
d.
|
HNO4
|
|
|
|
|
|
|
11.
|
An acid having the suffix -ic produces an anion having the
a.
|
suffix -ate.
|
c.
|
prefix hydro-.
|
b.
|
suffix -ite.
|
d.
|
suffix -ous.
|
|
|
|
|
|
|
12.
|
According to the traditional definition, an acid contains
a.
|
hydrogen and does not ionize.
|
b.
|
hydrogen and ionizes to form hydrogen ions.
|
c.
|
oxygen and ionizes to form hydroxide ions.
|
d.
|
oxygen and ionizes to form oxygen ions.
|
|
|
|
|
13.
|
What is the product of H3O+ and OH– concentrations in water?
a.
|
10–28
|
c.
|
10–7
|
b.
|
10–14
|
d.
|
55.4
|
|
|
|
|
|
|
14.
|
The pH of an acidic solution is
a.
|
less than 0.
|
c.
|
greater than 7.
|
b.
|
less than 7.
|
d.
|
greater than 14.
|
|
|
|
|
|
|
15.
|
The pH of a basic solution is
a.
|
less than 0.
|
c.
|
greater than 7.
|
b.
|
less than 7.
|
d.
|
greater than 14.
|
|
|
|
|
|
|
16.
|
What is an acid according to Arrhenius?
a.
|
a substance that ionizes to yield protons in aqueous solution
|
b.
|
a substance that is a hydrogen ion donor
|
c.
|
a substance that accepts an electron pair
|
d.
|
a substance that is a hydrogen ion acceptor
|
|
|
|
|
17.
|
What is the charge on the hydronium ion?
|
|
18.
|
If the hydrogen ion concentration of a solution is 10M, is the solution acidic, alkaline, or neutral?
a.
|
acidic
|
c.
|
neutral
|
b.
|
alkaline
|
d.
|
The answer cannot be determined.
|
|
|
|
|
|
|
19.
|
Acids taste
a.
|
sweet.
|
c.
|
bitter.
|
b.
|
sour.
|
d.
|
salty.
|
|
|
|
|
|
|
20.
|
Acids react with
a.
|
bases to produce salts and water.
|
c.
|
water to produce bases and salts.
|
b.
|
salts to produce bases and water.
|
d.
|
neither bases, salts, nor water.
|
|
|
|
|
|
|
21.
|
Aqueous solutions of acids
a.
|
always have Faraday properties.
|
c.
|
have very high boiling points.
|
b.
|
conduct electricity.
|
d.
|
cannot be prepared.
|
|
|
|
|
|
|
22.
|
Bases taste
a.
|
soapy.
|
c.
|
sweet.
|
b.
|
sour.
|
d.
|
bitter.
|
|
|
|
|
|
|
23.
|
What is the concentration of H3O+ in pure water?
a.
|
10–7 M
|
c.
|
55.4 M
|
b.
|
0.7 M
|
d.
|
107 M
|
|
|
|
|
|
|
24.
|
If [H3O+] = 8.26 × 10–5 M, what is the pH of the solution?
a.
|
2.161
|
c.
|
4.083
|
b.
|
3.912
|
d.
|
8.024
|
|
|
|
|
|
|
25.
|
If [H3O+] of a solution is less than [OH–], the solution
a.
|
is always acidic.
|
c.
|
is always neutral.
|
b.
|
is always basic.
|
d.
|
might be acidic, basic, or neutral.
|
|
|
|
|
|
|
26.
|
Which expression represents the pH of a solution?
a.
|
log[H3O+]
|
c.
|
log[OH–]
|
b.
|
–log[H3O+]
|
d.
|
–log[OH–]
|
|
|
|
|
|
|
27.
|
A water solution whose pH is 7
a.
|
is always neutral.
|
c.
|
is always acidic.
|
b.
|
is always basic.
|
d.
|
might be neutral, basic, or acidic.
|
|
|
|
|
|
|
28.
|
What is the pH of a 10–4 M HCl solution?
|
|
29.
|
What is the pH of a solution whose hydronium ion concentration is 5.03 × 10–1 M?
a.
|
0.2984
|
c.
|
1.542
|
b.
|
0.5133
|
d.
|
5.031
|
|
|
|
|
|
|
30.
|
What is the pH of a 0.001 62 M NaOH solution?
a.
|
3.841
|
c.
|
9.923
|
b.
|
5.332
|
d.
|
11.210
|
|
|
|
|
|
|
31.
|
What is the hydronium ion concentration of a solution whose pH is 7.30?
a.
|
1.4 × 10–11 M
|
c.
|
5.0 × 10–8 M
|
b.
|
3.8 × 10–8 M
|
d.
|
7.1 × 10–6 M
|
|
|
|
|
|
|
32.
|
What is the hydroxide ion concentration of a solution whose pH is 12.40?
a.
|
2.5 × 10–2 M
|
c.
|
8.9 × 10–2 M
|
b.
|
4.4 × 10–2 M
|
d.
|
1.0 × 10–1 M
|
|
|
|
|
|
|
33.
|
Dyes with pH-sensitive colors are used as
a.
|
primary standards.
|
c.
|
titrants.
|
b.
|
indicators.
|
d.
|
None of the above
|
|
|
|
|
|
|
34.
|
An acid-base titration involves a
a.
|
composition reaction.
|
c.
|
single-replacement reaction.
|
b.
|
neutralization reaction.
|
d.
|
decomposition reaction.
|
|
|
|
|
|
|
35.
|
Which quantity is directly measured in a titration?
a.
|
mass
|
c.
|
volume
|
b.
|
concentration
|
d.
|
density
|
|
|
|
|
|
|
36.
|
What unknown quantity can be calculated after performing a titration?
a.
|
volume
|
c.
|
mass
|
b.
|
concentration
|
d.
|
density
|
|
|
|
|
|
|
37.
|
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.
|
|
|
|
|
|
|
38.
|
Which of the following is a triprotic acid?
a.
|
H2SO4
|
c.
|
HCl
|
b.
|
CH3COOH
|
d.
|
H3PO4
|
|
|
|
|
|
|
39.
|
Which of the following is a strong base?
a.
|
NH3
|
c.
|
NaOH
|
b.
|
aniline
|
d.
|
acetate ion
|
|
|
|
|
|
|
40.
|
Which of the following is a weak base?
a.
|
KOH
|
c.
|
NH3
|
b.
|
Ca(OH)2
|
d.
|
HCl
|
|
|
|
|
|
|
41.
|
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
|
|
|
|
|
|
|
42.
|
A Brønsted-Lowry base is a(n)
a.
|
producer of OH– ions.
|
c.
|
electron-pair donor.
|
b.
|
proton acceptor.
|
d.
|
electron-pair acceptor.
|
|
|
|
|
|
|
43.
|
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 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.
|
|
|
|
|
44.
|
What are the acids in the following equilibrium reaction?
|
|
45.
|
An indicator is what type of compound?
a.
|
oxidizing agent
|
c.
|
strong base or acid
|
b.
|
weak base or acid
|
d.
|
salt
|
|
|
|
|
|
|
46.
|
What characterizes a strong acid or base?
a.
|
polar covalent bonding
|
b.
|
complete ionization in water
|
c.
|
ionic bonding
|
d.
|
presence of a hydroxide or hydrogen ion
|
|
|
|
|
47.
|
What is the molarity of an HCl solution if 50.0 mL is neutralized in a titration by 40.0 mL of 0.400 M NaOH?
a.
|
0.200 M
|
c.
|
0.320 M
|
b.
|
0.280 M
|
d.
|
0.500 M
|
|
|
|
|
|
|
48.
|
What is the molarity of an HCl solution if 125 mL is neutralized in a titration by 76.0 mL of 1.22 M KOH?
a.
|
0.371 M
|
c.
|
0.617 M
|
b.
|
0.455 M
|
d.
|
0.742 M
|
|
|
|
|
|
|
49.
|
What is the molarity of an H2SO4 solution if 49.0 mL is completely titrated by 68.4 mL of an NaOH solution whose concentration is 0.333 M?
a.
|
0.116 M
|
c.
|
0.465 M
|
b.
|
0.232 M
|
d.
|
0.880 M
|
|
|
|
|
|
|
50.
|
What is the molarity of a Ba(OH)2 solution if 93.9 mL is completely titrated by 15.3 mL of 0.247 M H2SO4?
a.
|
0.0101 M
|
c.
|
0.0402 M
|
b.
|
0.0201 M
|
d.
|
0.0805 M
|
|
|
|
|
|