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
We have a titration of 100.0 mL (0.100 L) of 0.200 M acetic acid
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
3) Now, let us calculate the concentration of
4) Let us calculate the pH using Henderson-Hasselbalch equation
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
At equilibrium, the concentrations are:
Equating it with the equilibrium constant
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