Calculate the $p H$ of an aqueous solution of 1.0 M ammonium formate assuming complete dissociation.
( $p K_{a}$ of formic acid = 3.8 and $p K_{b}$ of ammonia = 4.8.)

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Detailed Solution

For ammonium formate which is a salt of weak acid with weak base, we know that
$p H = \frac{1}{2} [p K_{w} + p K_{a} - p K_{b}] = \frac{1}{2} [14 + 3.8 - 4.8] = 6.5$

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