(
ii) If the pH of a hydrochloric acid solution is the same as the pH of a propanoic acid solution, then the
molar concentration of the hydrochloric acid solution must be less than the molar concentration of
the propanoic acid solution.
T
rue. HCl is a strong acid that ionizes completely. Fewer
moles of
H
Cl are needed to produce the same [H
3
O
+
] as
the propanoic acid solution, which only partially ionizes.
1 poi
nt is earned for noting that the
statement is true and providing a
supporting explanation.
A
student is given the task of determining the concentration of a propanoic acid solution of unknown
conc
en
t
r
ation. A 0.173 M NaOH solution is available to use as the titrant. The student uses a 25.00 mL
volumetric pipet to deliver the propanoic acid solution to a clean, dry flask. After adding an appropriate
indicator to the flask, the student titrates the solution with the 0.173 M NaOH, reaching the end point after
20.52 mL of the base solution has been added.
(d) Calculate the molarity of the propanoic acid solution.
Let x = moles of propanoic acid
3
0.173 mol NaOH 1 mol acid
then = (0.02052 L NaOH)
1 L NaOH 1 mol NaOH
= 3.55 10 mol propanoic acid
x
-
´´
´
3
3.55 10 mol acid
= 0.142
0.02500 L acid
M
-
´
OR
Since
32
CH C
H COOH is monoprotic and, at the equivalence point,
moles H = moles OH
+
, then
=
A A
B B
M V M V
(0.173 NaOH)(20.52 mL NaOH)
= = = 0.142
25.00 mL acid
BB
A
A
MV
M
M
V
M
-
1 point is earned for correctly
calculating the number of
moles of acid that reacted at
the equivalence point.
1 point is earned for the
correct molarity of acid.
(e) The student is asked to redesign the experiment to determine the concentration of a butanoic acid
solution instead of a propanoic acid solution. For butanoic acid the value of pK
a
is 4.83. The student
claims that a different indicator will be required to determine the equivalence point of the titration
accurately. Based on your response to part (b), do you agree with the student's claim? Justify your answer.