The electrochemical reaction between Ag(s) and Cl2(g) is as follows: AgCl⇌Ag++Cl− Given, Ksp=1.8×10−10,[Cl−]=0.1M ∴Ksp=[Ag+][Cl−] 1.8×10−10=[Ag+]×0.1
∴[Ag+]=
1.8×10−10
0.1
=1.8×10−9M
∴1 L of solution contains 1.8×10−9 moles of Ag+ Quantity of electricity required =1.8×10−9×96500 =1.73×10−4C ∴ Time required (t)=