108 g solution of $AgN{O}_3$ is electrolysed using $Pt$ electrodes by passing a charge of 0.1 F. The mass of the resultant solution left is:

The correct option is D 96.4 g
$A{g}^{+}+e^{-}\to Ag$
$2O{H}^{-}\to H_{2}O+0.5O_2+2e^{-}$

Equivalents of $A{g}^{+}$ lost= $0.1$ = Equivalents of $O_2$ formed and escaped

The total mass loss= $0.1\times 108+\frac{0.1\times 32}{4}=11.6$ g

Therefore, the mass of the solution= $108-11.6=96.4$ g