A weak acid has an initial concentration of 0.0415 M. After undergoing dissociation the pH is 5.31.
HA + H2O ⇌ H3O+ + A-
What is the percent ionization of the acid?
use:
pH = -log [H3O+]
5.31 = -log [H3O+]
[H3O+] = 4.898*10^-6 M
Now use:
% ionisation = [H3O+]*100 / [HA]
= (4.898*10^-6)*100 / 0.0415
= 0.0118 %
Answer: 0.0118 %
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