osula9a

2022-01-09

Consider the titration of 100.0 ml of 0.200 M acetic acid $({K}_{a}=1.8\times {10}^{-5})$ 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

0

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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