What is the approximate quantity of electricity in coulombs required to deposit all the silver from 500 ml 1M $AgN{O}_3$ aqueous solution ? (At. wt. of Ag = 108)

$$\begin{gathered} \text{ Moles of silver }=\frac{250}{1000}\times 1=\frac{1}{4}\text{ mole } \\ {\mathrm{Ag}}^{+}+{\mathrm{e}}^{-}\to \mathrm{Ag} \\ 1\text{ mole Ag requires }1\text{ mole }{e}^{-}\text{. } \\ \frac{1}{4}\text{ mole Ag requires }\frac{1}{4}\text{ mole electron } \\ \text{ Total charge }=\frac{1}{4}\times 96500 = 24125C \end{gathered}$$

Therefore, the correct option is B