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Chapter 14: Aqueous Equilibria: Acids and Bases
Problem Solving Center
Self Quiz 2
Self Quiz 2
This activity contains 20 questions.
A sample of milk has a OH
-
ion concentration of 4.46 x 10
-8
M. The [H
3
O
+
] and pH of milk is
[H
3
O
+
] = 2.2 x 10
-7
M and pH = 6.65.
[H
3
O
+
] = 2.24 x 10
-7
M and pH = 6.649.
[H
3
O
+
] = 4.5 x 10
-8
and pH = 7.35.
[H
3
O
+
]= 4.5 x 10
-22
M and pH = 21.35.
[H
3
O
+
] = 4.46 x 10
6
M and pH = 6.649.
A(n) ______ solution having a [OH
-
] = 2.9 x 10
-8
M has a pH = ______ .
neutral, 6.46
basic, 7.54
acidic, 7.54
acidic, 6.46
basic, 6.46
An example of a conjugate acid-base pair is
HNO
3
, NO
2
-
.
KNO
3
(
aq
), HNO
3
.
H
3
PO
4
, HPO
4
2-
.
NH
4
+
, NH
4
OH.
HSO
4
-
, SO
4
2-
.
The number of grams of KOH that are required to make 1500.0 mL of a solution having a pH = 11.80 is
0.53 g.
5.310 x 10
-1
g.
1.1 x 10
-7
g.
1.3 x 10
-10
g.
5.3 x 10
2
g.
The percent dissociation of a 0.0500 M thiophenol solution is (K
a
= 3.2 x 10
-7
)
0.25 %
3.2 x 10
-5
%
1.3 x 10
-4
%
2.6 x 10
-5
%
1.1 %
The pH of a 0.0500 M aqueous solution of hydrazine is (K
b
= 8.9 x 10
-7
)
7.65
10.32
3.68
12.70
6.35
The pH of a 0.120 M phenol solution is (K
a
of phenol = 1.3 x 10
-10
)
5.40
1.000
10.81
4.48
11.11
The pH of a solution made by dissolving 0.100 g of phenol (C
6
H
6
O) in enough water to form 100.0 mL of solution is (K
a
of phenol = 1.3 x 10
-10
)
7.43
12.16
5.93
4.94
11.86
The pH of a solution made by dissolving 1.00 g HOCl in enough water to form 1.25 x 10
3
mL of solution is (K
a
of HOCl = 3.5 x 10
-8
)
3.78
9.58
9.27
6.14
4.64
The pH of an aqueous 0.100 M ephedrine solution is (K
b
= 9.1 x 10
-5
)
2.52
5.34
13.000
11.48
8.66
The reaction that does
not
show the reaction of H
2
PO
4
-
as a Brønsted-Lowry acid is
H
2
PO
4
-
+ OH
-
(
aq
)
HPO
4
2-
(
aq
) + H
2
O(
l
).
H
2
PO
4
-
+ NH
3
(
aq
)
HPO
4
2-
(
aq
) + NH
4
+
(
aq
).
H
2
PO
4
-
+ H
3
O
+
(
aq
)
H
3
PO
4
(
aq
) + H
2
O(
l
).
H
2
PO
4
-
+ HCO
3
-
(
aq
)
HPO
4
2-
(
aq
) + H
2
CO
3
(
aq
).
H
2
PO
4
-
(
aq
) + H
2
O(
l
)
HPO
4
2-
(
aq
) + H
3
O
+
(
aq
).
The solution that will give a pH = 12.00 is
0.20 g NaOH in 0.50 L of solution.
0.20 g NaOH in 2.0 L of solution.
0.40 g NaOH in 0.10 L of solution.
4.0 g NaOH in 1.0 L of solution.
12 g NaOH in 1.0 L of solution.
Using L.A. for Lewis acid and L.B. for Lewis base, in which reaction are the Lewis acid and base correctly identified?
CO
2
(
aq
)(L.B.) + H
2
O(
l
)(L.A.) ---> H
2
CO
3
(
aq
)
SO
2
(
aq
)(L.A.) + H
2
O(
l
)(L.B.) ---> H
2
SO
3
(
aq
)
Fe
3+
(
aq
)(L.B.) + 6CN
-
(
aq
)(L.A.) ---> Fe(CN)
6
3-
(
aq
)
HNO
3
(L.B.) + H
2
O(
l
)(L.A.) ---> NO
3
-
(
aq
) + H
3
O
+
(
aq
)
BH
3
(
g
)(L.B.) + NH
3
(
g
)(L.A.) ---> H
3
B-NH
3
(
g
)
What is the K
a
of the weak acid HClO
2
if a 0.100 M solution of the acid has a pH = 2.22 ?
-1.2
3.9 x 10
-4
0.13
3.6 x 10
-4
1.2
What is the probable pH of a solution that gives a blue solution when bromthymol blue is added, a colorless solution when thymolphthalein is added, and a yellow solution when m-nitrophenol is added? (The pH ranges for these indicators are as follows: bromthymol blue: yellow, 6.0 - blue, 7.6; m-nitrophenol: colorless, 6.8 - yellow, 8.7; and thymolphthalein: colorless, 9.5 - blue, 10.6.)
7.0
13.0
11.0
9.0
5.0
Which correctly relates the acid strength of the oxoacid pair?
HOClO
3
< HOClO
2
.
HOBrO < HOIO.
HNO
2
> HNO
3
.
HOI > HOCl.
HOBrO > HOBr.
Which H
3
O
+
concentration and classification (acidic
vs.
basic) are correctly matched for a solution in which the OH
-
concentration is 5.6 x 10
-6
M?
1.8 x 10
-9
M : basic
5.6 x 10
-6
M : acidic
1.8 x 10
-9
M : acidic
5.6 x 10
-6
M : basic
5.6 x 10
8
M : acidic
Which list gives acids in order of increasing strength?
NH
3
< PH
3
< HI < HCl
H
2
S < PH
3
< HCl < HBr
NH
3
< H
2
O < H
2
S < HBr
NH
3
< CH
4
< H
2
O < H
2
S
CH
4
< NH
3
< H
2
S < H
2
O
Which relationship between acid strengths is correct?
HNO
3
< HNO
2
H
2
O < OH
-
NH
2
-
> NH
3
HClO
4
> HF
H
2
SO
3
> H
2
SO
4
Which statement is
not
true?
The reaction of 2 moles of HC
2
H
3
O
2
with 1 mole of Ca(OH)
2
will produce a basic solution.
The reaction of 1 mole of HCl with 1 mole of KOH will produce a neutral solution.
The reaction of 2 moles of HF with 1 mole of Sr(OH)
2
will produce a basic solution.
The reaction of 1 mole of HCN with 1 mole of LiOH will produce a basic solution.
The reaction of 1 mole of NH
3
with 1 mole of HI will produce a neutral solution.
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