What is the approximate quantity of electricity in coulombs required to deposit all the silver from 500 ml 1M AgNO₃ aqueous solution ?
(At. wt. of Ag = 108)

$Moles of Silver = M \times \frac{V_{\left(ml\right)}}{1000}= 1X\frac{250}{1000}=0.25mol$

$A{g}^{+}+e^{-}\to Ag$

1 mol of Ag deposited by 1 mol of electron

0.25 mole of Ag deposited by 0.25 mol electron = 0.25 X 96500 c = 24125 coulombs.