Acidic buffer

Let an acidic solution be prepared by acetic acid to sodium acetate solution.

Acetic acid is a weak acid and sodium acetate is highly ionised.

The ionisamon of acetic acid is further suppressed due to the concentration of $CH_3COO^-$ ions obtained from $CH_3COONA$.

$CH_3COONa \leftrightharpoons CH_3COO^- + Na^+$

$CH_3 COOH \leftrightharpoons \underset{common ion}{CH_3} CO O^- + H^+$

Now, when a few drops of decinormal HCI are added to it, its $H^+$ ions combine with $CH_3COO^-$ ions present in solution and form feebly ionised $CH_3COOH$, with the result, all the$H^+$ ions are consumed and no appreciable change in $H^+$ ion concentration occurs. Hence pH value remains constant.

Acidic buffer

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