For the cell (at 298 K ) `Ag_((g)) // 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^(+)]_a = [Ag^(+)]_(c)`
B. The amount of `AgCl_((s))` ppt in anodic compartment will decrease the working of the cell .
C. The `[Ag^+]`= constant in the anodic compartment during the working of the cell.
D. Anode is metal - sparingly soluble salt, half cell .

Answer

A, D

Explanation

`Ag_((9)) // Ag_((s))//Cl_(aq)^(-) // AgNO_(3(aq)) // Ag `
This is a concentration cell `:.` cell emf = 0 when `[Ag^(+)]_a = [Ag^(+)]_c`
Anode is metal sparingly soluble salt half cell