What must be concentration of `Ag^(+)` in an aqueous solution containing `Cu^(2+) =1.0 M` so that bot the metals can be deposited on the cathode simultaneously. Given that `E_(Cu//Cu^(2+))^(0)=-0.34V` and `E_(Ag^(+)//Ag)^(0)=0.812V,T=298K`

Options

A. nearly `10^(-19)M`
B. `10^(-12)M`
C. `10^(-8)M`
D. nearly `10^(-16)M`

Answer

3

Explanation

`S.R.P.+(0.0591)/(2)log[Cu^(+2)]=S.R.P.+(0.0591)/(1)log[Ag^(+)]`
`0.34+(0.059)/(2)log[1.0]=SRP+(0.0591)/(1)log[Ag^(+)]`
`0.34=0.812+(0.0591)/(1)log[Ag^(+)]`
`[Ag]^(+)=10^(-8)Ans.`