2302102 Acids and Bases Quiz
1.
(Points: 1)
In this reaction
NH3(aq) + H2O(l)  NH4+(aq) + OH (aq)
2.
1.
H2O acts as a base and NH4+ as an acid.
2.
H2O acts as an acid and NH4+ as a base.
3.
NH3 acts as a base and OH as an acid.
4.
NH3 acts as an acid and OH as a base.
5.
H2O acts as an acid and OH as a base.
(Points: 1)
In Bronsted-Lowry acid-base theory, an acid is defined as a substance which _____ and a base as one wh
_____.
3.
1.
donates a proton; accepts a proton
2.
generates OH in aqeous solution; generates H3O+ ion in aqueous solution
3.
generates H3O+ ions in aqueous solution; generates OH ions in aqeous solution
4.
generates H3O+ ions in aqueous solution; donates a proton
5.
accepts a proton; generates OH ions in aqueous solution
(Points: 1)
Which of the following can act as a Bronsted-Lowry base, but not as a Bronsted-Lowry acid?
1.
HSO4
2.
H2O
3.
NH4+
4.
HPO42
5.
PO43
4.
(Points: 1)
A Bronsted-Lowry acid is always
5.
1.
a weak acid
2.
a highly dissociated acid
3.
a donor of one or more hydrogen ions
4.
both an acceptor and donor of hydrogen ions
5.
a molecule or ion in which hydrogen is attached to an oxygen atom
(Points: 1)
Which of the following does not act as a Bronsted-Lowry base?
6.
1.
HSO4
2.
OH
3.
CH3NH2
4.
NH4+
5.
NH3
(Points: 1)
Which of the following does not act as a Bronsted-Lowry acid?
7.
1.
HPO42
2.
CH3NH3+
3.
H3O+
4.
HCOOH
5.
CH3COO
(Points: 1)
Which of the following is a conjugate acid-base pair?
1.
CH3COOH and CH3COO
2.
CH3COO and H2O
3.
CH3COOH and H3O+
4.
CH3COOH and OH
5.
H3O+ and OH
8.
(Points: 1)
Which of the following is not a conjugate acid-base pair?
9.
1.
HPO42 and PO43
2.
HCOOH and HCOO
3.
CH3NH3+ and CH3NH2
4.
CH3COOH and CH3COO
5.
H2SO3 and HSO4
(Points: 1)
Methylamine, CH3NH2, acts as a weak base in water. The products of the reaction are _____ and _____.
10.
1.
OH and CH3NH
2.
OH and CH3NH3+
3.
H3O+ and CH3NH3+
4.
H3O+ and CH3NH
5.
H3O+ and OH
(Points: 1)
Which reaction illustrates water acting as a base?
11.
1.
HSO4 + H2O  H3O+ + SO42
2.
HPO42 + H2O  OH + H3PO4
3.
NH3 + H2O  NH4+ + OH
4.
Cu(H2O)42+ + 4NH3  Cu(NH3)42+ 4H2O
5.
H2CO3  H2O + CO2
(Points: 1)
The conjugate base of NH3 is _____.
1.
NH2
2.
OH
3.
NH4OH
4.
NH4
5.
H2O
12.
(Points: 1)
Because water can act as a Bronsted-Lowry acid or base, it is said to be _____.
13.
1.
amphoteric
2.
amphihydrous
3.
amphiprotic
4.
amphiphilic
5.
amphiphobic
(Points: 1)
A Bronsted-Lowry base must have a(an) _____.
14.
1.
atom with an unshared pair of electrons
2.
nitrogen atom
3.
atom that does not obey the octet rule
4.
amphiprotic atom
5.
oxygen atom
(Points: 1)
In terms of acid strength, which of the following does not belong with the others?
15.
1.
HF
2.
HClO4
3.
HNO2
4.
HCOOH
5.
H2SO3
(Points: 1)
In terms of base strength, which of the following does not belong with the others?
1.
NaOH
2.
Sr(OH)2
3.
NH4OH
4.
Ba(OH)2
5.
LiOH
16.
(Points: 1)
Which of the following does not contribute to the acidity of the hydrogen atom in the carboxylic acid
functional group?
17.
1.
the attraction of the other atom of O for the electrons in the OH bond
2.
the electronegativity of the O that is bonded to the H
3.
resonance stabilization of the resulting anion
4.
the lack of polarity in the CH bonds in the rest of the molecule
5.
the electronegativity of the C atom
(Points: 1)
The reaction between acetic acid (CH3COOH) and water is written as
18.
1.
CH3COOH + H2O  CH3COO + H3O+
2.
CH3COOH + H2O  CH3COOH2+ + OH
3.
CH3COOH + H2O  CH3COO + OH
4.
CH3COOH + H2O  CH2COOH + H3O+
5.
CH3COOH + H2O  CH3COOH + H3O+
(Points: 1)
In an acidic solution at 25C, which of the following is not true?
1.
[H3O+] > [OH]
2.
[H3O+][OH] > 1.0  107
3.
[OH] < 1.0  107
4.
[H3O+] > 1.0  107
5.
[H3O+][OH] < 1.0  107
19.
(Points: 1)
One water molecule can donate a proton to another in a process called _____; the equilibrium constant
expression for this reaction is _____.
20.
1.
protonation; [H3O+][OH]
[H2O]
2.
neutralization; [H3O+][OH]
[H2O]
3.
autoionization; [H3O+][OH]
4.
autoionization; [H3O+][OH]
[H2O]
5.
hydrolysis; [H3O+][OH]
[H2O]
(Points: 1)
Kw for water
21.
1.
increases as the temperature increases
2.
none of these choices are correct
3.
decreases as the temperature increases
4.
is equal to 1.0  1014 at all temperatures
5.
is equal to 1.0  1014 at all temperatures
(Points: 1)
A solution is not neutral. Which one of these statements is true?
1.
[H3O+] = 1.0  107 M
2.
[H3O+][OH] = 1.0  107
3.
[OH] = 1.0  107 M
4.
[H3O+][OH] = 1.0  1014
5.
[H3O+] = [OH]
22.
(Points: 1)
In a basic solution at 25C,
23.
1.
[H3O+][OH] < 1.0  1014.
2.
[OH] > 1.0  107.
3.
[H3O+][OH] > 1.0  1014.
4.
[H3O+] > 1.0  107.
5.
[H3O+] > [OH].
(Points: 1)
In a 1.2 M solution of KOH, a strong base, [H3O+] = _____, and [OH] = _____.
24.
1.
8.3  1015 M; 1.2 M
2.
8.3  1015 M; 1.0  1014 M
3.
1.0  107 M; 1.0  107 M
4.
1.2 M; 1.2 M
5.
1.2 M; 8.3  1015 M
(Points: 1)
In a 1.2 M solution of HClO4, a strong acid, [H3O+] = _____, and [OH] = _____.
1.
1.2 M; 1.2 M
2.
1.2 M; 8.3  1015 M
3.
1.0  107 M; 1.0  107 M
4.
8.3  1015 M; 1.2 M
5.
8.3  1015 M; 1.0  1014 M
25.
(Points: 1)
An acidic solution is diluted until [H3O+] is exactly half as much as before. The pH of the solution is now
_____ than before.
1.
0.69 higher
2.
2.00 higher
3.
0.30 higher
4.
2.00 lower
5.
0.30 lower
26.
(Points: 1)
If the hydrogen ion concentration of a solution is increased by a factor of 4, the pH is
27.
1.
raised by 4 pH units
2.
raised by 0.3 pH units
3.
lowered by 0.25 pH units
4.
lowered by 0.6 pH units
5.
lowered by 2 pH units
(Points: 1)
If the pH of a solution is raised from 6.27 to 7.57
28.
1.
[OH] has increased by a factor of 20
2.
[H3O+] has decreased by a factor of 20
3.
all of these choices
4.
the new [H3O+] = 2.7  108
5.
the solution has gone from acidic to basic
(Points: 1)
Which of the following represents the most acidic solution?
1.
pH = 3.6
2.
pOH = 14.7
3.
[H3O+] = 1.0 M
4.
[H+] = 1.0  1014 M
5.
[OH] = 1.0  1014 M
29.
(Points: 1)
Calculate the pH of a solution where [OH] = 4.6  104. Is this solution acidic or basic?
30.
1.
10.66; basic
2.
9.40; basic
3.
3.34; acidic
4.
10.66; acidic
5.
3.34; basic
(Points: 1)
Arrange the solutions in order of increasing acidity:
a solution with [H3O+] = 4.2  106 M
lemonade, pH = 2.65
0.25 M nitric acid
pickle juice, pH = 3.10
I.
II.
III.
IV.
31.
1.
IIIIIIIV
2.
IIVIIIII
3.
IIIVIIII
4.
IIIIIIVI
5.
IVIIIIII
(Points: 1)
A wine sample had a pH of 3.52. This corresponds to [H3O+] =
1.
5.2  104 M.
2.
3.3  1011 M.
3.
3.3  103 M.
4.
3.0  104 M.
5.
5.2  103 M.
32.
(Points: 1)
As the pH of a solution rises, [H3O+] _____, pOH _____, and [OH] _____.
33.
1.
falls, falls, falls
2.
falls; falls; rises
3.
rises; falls; falls
4.
falls; rises; falls
5.
rises; falls; rises
(Points: 1)
Phenolphthalein is an acid-base indicator that is colorless in its acid form and pink in its basic form,
changing at pH = 8.5. Bromcresol green is yellow in its acidic form and blue in its basic form, changi
at pH = 4.8. A solution is colorless in phenolphthalein and blue in bromcresol green. Therefore we ca
conclude that the pH of the solution is _____.
34.
1.
less than 4.8
2.
between 4.8 and 8.5
3.
between 7.0 and 8.5
4.
greater than 8.5
5.
exactly 7.0
(Points: 1)
The larger the value of Ka
35.
1.
the less highly dissociated the acid and the stronger the acid
2.
the less highly dissociated the acid and the weaker the acid
3.
none of these choices are correct
4.
the more highly dissociated the acid and the stronger the acid
5.
the more highly dissociated the acid and the weaker the acid
(Points: 1)
For the dissociation of a very weak acid, HA, in water
33.
1.
Ka = [H3O+][ A]
2.
Ka = [H3O+][ A] / [HA]
3.
Ka = [H3O+][ A] / [H2O]
4.
Ka = [HA][H3O+][ A]
5.
Ka = [HA] / [A][H3O+]
(Points: 1)
Write the acid ionization constant expression for the ionization of the hydrogen sulfate ion, HSO4- , in
aqueous solution.
34.
1.
Ka = [HSO4-][H2O]
[SO42-][H3O+]
2.
Ka = [SO42-][H3O+]
[HSO4-]
3.
Ka = [HSO4-][H2O]
[H2SO4][H3O+]
4.
Ka = [H2SO4][ OH-]
[HSO4-]
5.
Ka = [H2SO4][H3O+]
[HSO4-]
(Points: 1)
Consider a 0.50 M solution of HNO2, a weak acid with Ka = 4.5  104. Which statement is true?
1.
pH = 3.35.
2.
pH > 0.32.
3.
The acid is mostly ionized.
4.
pH = 0.32.
5.
[H3O+] > 0.50 M.
35.
(Points: 1)
Two common polyprotic acids are
36.
1.
nitric acid and phosphoric acid
2.
sulfuric acid and perchloric acid
3.
sulfuric acid and phosphoric acid
4.
perchloric acid and nitric acid
5.
sulfuric acid and nitric acid
(Points: 1)
In a neutral polyprotic acid, the value of Ka2 will be _____ the value of Ka1 because _____.
1.
larger than; it is more difficult to remove a hydrogen ion from an anion than from a neutral mole
2. smaller than; it is more difficult to remove a hydrogen ion from a cation than from a neutral
molecule
3.
larger than; it is more difficult to remove a hydrogen ion from a cation than from a neutral molec
4. smaller than; it is more difficult to remove a hydrogen ion from an anion than from a neutral
molecule
5.
37.
the same as; both hydrogen ions are bonded to the same anion
(Points: 1)
Typically, for a weak acid and its conjugate base
1.
Ka  Kb = 1.0
2.
Ka / Kb = 1.0
3.
Ka  Kb = 1.0  1014
4.
Ka / Kb = 1.0  1014
5.
Ka  Kb = 14
38.
(Points: 1)
The pH of a 0.50 M solution of the weak acid HA is 4.76. The value of Ka is
39.
1.
7.6  104
2.
6.0  1010
3.
9.24
4.
3.5  105
5.
1.7  105
(Points: 1)
The pH of a solution of a 0.15 M solution of HOCl is 4.14. What is the Ka for HOCl?
40.
1.
8.8  103
2.
3.5  108
3.
7.2  105
4.
5.7  102
5.
4.8  104
(Points: 1)
The value of the ionization constant for a weak acid HA is 4.2  107. What is the pH of a 0.35 M solut
of this acid?
1.
2.96
2.
3.19
3.
6.83
4.
3.42
5.
6.38
41.
(Points: 1)
The poison strychnine is a weakly basic compound with Kb = 1.8  106. What is the pH of a 0.058 M
solution of strychnine?
42.
1.
7.30
2.
12.76
3.
3.49
4.
10.51
5.
8.26
(Points: 1)
The pH of a 0.172 M solution of benzoic acid (pKa = 4.20) is
43.
1.
2.48.
2.
4.37.
3.
5.63.
4.
4.96.
5.
3.44.
(Points: 1)
Ammonia is a weak base and perchloric acid is a strong acid. Which statement is true of a solution of
ammonium perchlorate?
1.
We cannot predict its acid-base properties without more information.
2.
It is weakly basic.
3.
It is weakly acidic.
4.
It is strongly acidic.
5.
It is neutral.
44.
(Points: 1)
Ammonia is a weak base and acetic acid is a weak acid. Which statement is true of a solution of
ammonium acetate?
45.
1.
It is strongly acidic.
2.
We cannot predict its acid-base properties without more information.
3.
It is weakly acidic.
4.
It is weakly basic.
5.
It is neutral.
(Points: 1)
The reaction between the ion of a weak acid or a weak base and water is called a(an) _____ reaction.
46.
1.
proteomic
2.
neutralization
3.
autoionization
4.
decomposition
5.
hydrolysis
(Points: 1)
An aqueous solution of potassium benzoate is predicted to be
47.
1.
strongly acidic.
2.
weakly basic.
3.
strongly basic.
4.
weakly acidic.
5.
neutral.
(Points: 1)
Calculate the pH of a 0.051 M solution of sodium lactate. The Ka for lactic acid is 1.4  104.
1.
8.28
2.
1.29
3.
12.71
4.
2.57
5.
11.43
48.
(Points: 1)
Which of the following statements is not correct?
1.
Neutral molecules cannot act as Lewis acids
Ag(NH3)2+ is a complex ion, formed from a Ag+ ion (Lewis acid) and two NH3 molecules
(Lewis bases)
2.
49.
3.
Al(OH)3 is an amphoteric substance that can form either a positive or negative ion
4.
a Lewis acid is a substance that can accept a pair of electrons to form a new bond
5.
a Lewis base is a substance that can donate a pair of electrons to form a new bond
(Points: 1)
Which of the following is a Lewis acid but not a Bronsted-Lowry acid?
50.
1.
CO2
2.
NH4+(aq)
3.
acetic acid
4.
CO32
5.
HCO3 (aq)
(Points: 1)
Metal hydroxides that can act either as Lewis acids or Lewis bases are described as
51.
1.
amphihydrous.
2.
amphiphobic.
3.
amphihydric.
4.
amphoteric.
5.
amphiphilic.
(Points: 1)
Which compound would not be used as an antacid for the treatment of heartburn?
1.
KOH
2.
NaHCO3
3.
Mg(OH)2
4.
Al(OH)3
5.
CaCO3
52.
(Points: 4)
a.
Write the reaction for the ionization of the weak acid HA in water.
b.
Write the reaction for the ionization of the conjugate base of the weak acid HA in water.
c.
Using equilibrium constant expressions for the reaction of HA and of its conjugate base A with
water, prove that the product of Ka for a weak acid and Kb for its conjugate base always has the
value 1.0  1014 at 25C.
53.
(Points: 3)
A solution of acetic acid (Ka = 1.8  105) has a pH exactly 2 higher than a solution of HCl(aq) of the
same concentration. What is that concentration?