Section 19.3
What is pH?
Practice Test
1.
Why is it possible to derive the ion product constant for water, but not for aqueous acids?
a.
At a given temperature, aqueous acids have constant concentrations.
b.
Aqueous acids never reach equilibrium.
c.
The concentration of pure water is constant.
d.
Water does not ionize completely.
Hint
2.
pH is defined as __________.
a.
log [H
+
]
b.
-log [H
+
]
c.
log [OH
-
]
d.
-log [OH
-
]
Hint
3.
A solution of pH = 2.1 would be described as __________.
a.
distinctly basic
b.
slightly basic
c.
slightly acidic
d.
distinctly acidic
Hint
4.
When a solution has a pH of 4, what is the pOH of that solution?
a.
10
b.
4
c.
18
d.
7
Hint
5.
At 298 K, pure water has a pH of __________.
a.
0
b.
14
c.
-14
d.
7
Hint
6.
What is the concentration of hydrogen ions in a solution that has a pH of 4.32?
a.
4.8 x 10
-5
M
b.
6.2 x 10
-4
M
c.
5.1 x 10
-4
M
d.
8.6 x 10
-5
M
Hint
7.
Calculate the pH of 0.075
M
KOH.
a.
10.4
b.
11.12
c.
11.46
d.
12.88
Hint
8.
Calculate the pH of a solution that has a [OH
-
] = 2.50 x 10
-4
M
.
a.
0.4
b.
3.6
c.
-3.6
d.
10.4
Hint
