What wil be the products of electrolysis of an aqueous solution of `AgNO_(3)` with silver electrodes ?

Options

A. Ag from Ag anode dissolves while `Ag^(+)` from solution gets deposited on cathode.
B. Ag is liberated at cathode and `O_(2)` is liberated at anode.
C. Ag at cathode and nitric acid at anode is liberated.
D. No reaction takes place.

Answer

A

Explanation

`AgNO_(3)rarr Ag^(+)+NO_(3)^(-)` (aqueous solution)
At cathode : `Ag_((aq))^(+)+e^(-)rarr Ag, E^(@)=+0.80 V`
`2H_(2)O_((l))+2e rarr H_(2)+2OH^(-), E^(@)=-0.83 V`
Since reduction potential of `Ag^(+)` is higher than `H_(2)O`, `Ag^(+)` are reduced to Ag.
At anode :
`Ag rarr Ag_((aq))^(+) + e^(-), E^(@)=-0.80 V`
`2H_(2)O rarr O_(2)+4H^(-)+4e^(-), E^(@)= - 1.23 V`
Since oxidation potential of Ag is higher than `H_(2)O`, Ag of silver anode is oxidised. The oxidation potential of `NO_(3)^(-)` is lower than `H_(2)O`.