Consider the titration of 100.0 mL of 0.200 M acetic acid (Ka = 1.8 10-5) by...

Consider the titration of 100.0 mL of 0.200 M acetic acid (Ka = 1.8 10-5) by 0.100 M KOH. Calculate the pH of the resulting solution after 0.0mL of KOH has been added.

Expert Solution

This titration leads to the formation of a buffer solution.

pH of the buffer solution can be calculated by using Handerson's equation.

pH = pKa + log [salt]/[acid]

but we need t calculate the pH of only the weak acid that is acetic acid.(since volume of KOH os 0.0ml)

CH3COOH <=> CH3COO^- +H⁺

I 0.2M 0 0

C -x +x +x

E 0.2-x x x

Ka = x² / (0.2-x)

1.8x10-5 = x² / 0.2 (since 0.2-x = 0.2 because 0.2>>x)

therefore x² = 3.6 x 10^-6

x = 1.897 x 10^-3

[H+] = 1.897 x 10^-3

pH = -log ( 1.897 x 10^-3)

= 2.72

queen_honey_blossom answered 2 years ago

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