osula9a
2022-01-09
Consider the titration of 100.0 ml of 0.200 M acetic acid with 0.100 M KOH. After adding the subsequent volumes of KOH, determine the pH of the resulting solution. 50.0 mL
Fasaniu
Beginner2022-01-10Added 46 answers
We have a titration of 100.0 mL (0.100 L) of 0.200 M acetic acid
(b)
Let us calculate the pH of a solution, after 50.0 mL (0.050 L) of KOH has been added.
1) The total volume of a solution is now
First, let us calculate the number of moles of acetic acid
And the number of moles of KOH
2) KOH is strong base, and it will dissociate completely into
Therefore, when 0.005 mol of
Step 2
3) Now, let us calculate the concentration of
4) Let us calculate the pH using Henderson-Hasselbalch equation
Jonathan Burroughs
Beginner2022-01-11Added 37 answers
Step 1
Given:
100.0 mL of 0.200 M acetic acid
The reaction is
The expression for
Based on the balanced chemical equation
However, since 50 mL of KOH is added, the initial concentration of acetic acid and acetate will be reduced
Let
At equilibrium, the concentrations are:
Equating it with the equilibrium constant
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