For the cell (at 298K)
`Ag(s) | AgCl(s) | Cl^(-)(aq)|| AgNO_(3)(aq) | Ag(s)`
Which of the following is correct?

Options

A. The cell emf will be zero when `[(Ag^(+))]` in anodic compartment =`[Ag^(+)]` in cathodic compartment
B. The amount of AgCl(s) precipitate in anodic compartment will decrease with the working of the cell
C. The concentration of `[Ag^(+)]`=constant, in anodic compartment during working of cell
D. `E_(cell)=E_(Ag^(+)|Ag)^(0)-E_(Cl^(-)|AgCl|Ag)^(0)-0.059/1"log"1/[Cl^(-)]_(a)`

Answer

A

Explanation

`E_(cell)=E_(Ag|Ag^+)^0+0.0591/1."log"([Cl^(-)])/([ksp])+E_(Ag^+|Ag)-0.0591/1."log"1/[Ag^+]_c`
`E_cell=0+0.0591/1 "log" ([Ag^+]_c[Cl^(-)])/([Ag^+]_a[Cl^(-)])=0.0591 "log" ([Ag^+]_c)/([Ag^+]_a)`
If `[Ag^+]_c=[Ag^+]_a` then `E_cell=0`