# Basic buffer

Let a basic buffer solution be prepared by mixing $NH_4OH$ to ammonium chloride solution. $NH_4OH$ is a weak base and does not produce appreciable $oh^-$ ions.

Further, in presence of highly ionised $NH_4Cl$, its ionization is largely suppressed.

$NH_4Cl \leftrightharpoons NH^+_4 + Cl^- \\[5mm] NH_4OH \leftrightharpoons \underset{(Common ion)}{NH^+_4} + OH^-$

Now, when few drops of decinormal NaOH are added to this mixture, all its $OH^-$ ions combine with $NH^+_4$ ions to form feebly ionised$NH _4 OH$ and thus are consumed.

S0, no appreciable change in $OH^-$ ion concentration occurs, hence pH value remains constant.

Acidic buffer

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