Predict the products of electrolysis in eaCHM of the following `:`
`a.` An aqueous solution of `AgNO_(3)` with silver electrodes.
`b.` An aqeous solution of `AgNO_(3)` with platinum electrodes,
`c.` A dilute solution of `H_(2)SSO_(4)` with platinum electrodes.
`d.` An aqueous solution of `CuCl_(2)` with platinum electrodes.

Explanation

(i) Electrolysis of aqueous solution of `AgNO_(3)` with silver electrodes.
`AgNO_(3)(s)+aqtoAg^(+)(aq)+NO_(3)^(-)(aq)`
`H_(2)OhArrH^(+)+OH^(-)`
At cathode: `Ag^(+)` ions have lower discharge potential than `H^(+)` ions. Hence, `Ag^(+)` ions will be deposited as Ag in preference to `H^(+)` ions.
Alternatively, we have stanard reduction potential potentials as
`Ag^(+)(aq)+e^(-)toAg(s),E^(@)=+0.80V`
`H^(+)(aq)+e^(-)to(1)/(2)H_(2)(g),E^(@)=0.00V`
As `Ag^(+)` ions hae higher standard reduction potential than that of `H^(+)` ions, hence `Ag^(+)` ions will be reduced more easily and deposited as Ag.
At anode: As Ag anode is attached by `NO_(3)^(-)` ions, Ag of the anode will dissolve to form `Ag^(+)` ions in the solution.
`AgtoAg^(+)+e^(-)`
Alternatively, out of the three possible oxidation reactions occurring at the anode, i.e.,
`AgtoAg^(+)+e^(-),2OH^(-)toH_(2)O+(1)/(2)O_(2)+e^(-) and NO_(3)^(-)toNO_(3)+e^(-)`,
Ag has highest oxidation potential. hence, Ag of anode is oxidized to `Ag^(+)` ions which pass into the solution.
(ii) Electrolysis of aqueous solution of `AgNO_(3)` using platinum electrodes.
At cathode: Same as above. ltBrgt At anode: As anode is not attackable, out of `OH^(-) and NO_(3)^(-)` ions, have lower discharge potential. hence, `OH^(-)` ions will be discharged in preference to `NO_(3)^(-)` ions, which then decompose to give out `O_(2)`.
`OH^(-)(aq)toOH+e^(-),4OHto2H_(2)O(l)+O_(2)(g)`
(iii) Electrolysis of dilute `H_(2)SO_(4)` with platinum electrodes.
`H_(2)SO_(4)(aq)to2H^(+)(aq)+SO_(4)^(2-)(aq)`
`H_(2)OhArrH^(+)+OH^(-)`
At cathode: `H^(+)+e^(-)toH,H+HtoH_(2)(g)`
At anode: `OH^(-)toOH,e,4OHto2H_(2)O+O_(2)(g)`
Thus, `H_(2)` is liberated at the cathode and `O_(2)` at the anode.
(iv) Electrolysis of aqueous solution of `CuCl_(2)` with platinum electrodes.
`CuCl_(2)(s)+aqtoCu^(2+)(aq)+2Cl^(-)(aq)`
`H_(2)OhArrH^(+)+OH^(-)`
At cathode: `Cu^(2+)` ios will be reduced in preference to `H^(+)` ions
`Cu^(2+)+2e^(-)toCu`
At anode: `Cl^(-)` ions will be oxidized in preference to `OH^(-)` ions
`Cl^(-)toCl+e^(-),Cl+CltoCl_(2)(g)`
Thus, Cu will be deposited on the cathode and `Cl_(2)` will be liberated at the anode.