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J-3
d.
0.1455 M
e.
0.1569 M
8.
(Exp G) A student was performing a titration of 25.96 mL of 0.4940 M CH3COOH,
acetic acid, with a NaOH, sodium hydroxide, solution of unknown concentration. The student carefully
washed the buret and rinsed it with distilled water, but neglected to coat the sides of the buret with the
NaOH solution before filling it for the titration. The titration took 25.24 mL of the NaOH solution. The
actual concentration of the NaOH would be:
a.
exactly 0.2540 M
b.
more than 0.2540 M
c.
less than 0.5080 M
d.
exactly 0.5080 M
e.
more than 0.5080 M
9.
(Exp H) The pH of the equivalence point of a titration is 5.10. Which of the following
pH indicators should be used for color indicator titrations?
a.
thymol blue
b.
bromothymol blue
c.
methyl red
d.
methyl orange
e.
phenol red
10.
(Exp H) Calculate the mass of benzoic acid (MM = 122.12 g mol
–1
) sample titrated if
29.11 mL of a standardized 0.5130 M NaOH solution was required to reach the equivalence point of
the titration.
a.
0.01493 g
b.
0.2384 g
c.
0.9118 g
d.
1.824 g
e.
3.647 g
11.
(Exp I) The point on a pH titration curve with the highest buffering capacity is:
a.
at the initial pH
b.
at the pH of the equivalence point
c.
at the pH where the [A
-
] = ½ [HA]
d.
at ½ the volume to the equivalence point
e.
at the final pH
12.
(Exp I) What is the pH of a solution of a weak acid and its conjugate base when the ratio of the
concentrations of the conjugate base/weak acid is 1/3? (the weak acid K
a
= 6.7x10
-5
)
