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) An aqueous solution of `AgNO_(3)` using platinum electrodes:
Both `AgNO_(3)` and water will ionise in aqueous solution
`AgNO_(3)(S)overset(aq)rarrAg^(+)(aq)+NO^(=)(aq)`
`H_(2)Ooverset(aq)(ltimplies)H^(+)(aq)+HO^(-)(aq)`
At cathode: `Ag^(+) "ions with less discharge potential are reduced in preference to" H^(+)` ions which will remain in solution. As a aresult,silver will be deposited at cathode.
`Ag^(+)(aq)+e^(-)rarrAg(deposited)`
At anode: An equivalent amount of silver will be oxidised to `Ag^(+)` ions by releasing electrons
`Ag(s) overset(aq)rarrAg^(+)(aq)+e^(-)`
As result of electrolysis, Ag from silver anode dissolves as `Ag^(+) "ions while an equivalent amount of" Ag^(+)(aq) "ions from the aqueous" AgNO_(3)` solution get deposited on the cathode.
(ii) An aqueous solution of `AgNO^(3)` using platinum electrodes:
In the case, the platinumbn electrodes are the non attackable electrodes.On passing curent the folowing changes will occur at the electrodes.
At cathode: `Ag^(+)` ions will be reduced to Ag which will get deposited at the cathode
At anode: Both `NO_(3)^(-) "and" OH^(-) "ions will migrate.But" OH^(-) "ions with less descharge potential will be oxidised in preference to" NO_(3)^(-)` "ions which will remain in solution"
`OH^(-)(aq)rarrOH+e^(-),4OHrarr2H^(2)O(l)+O_(2)(g)`
Thus as a result of elctorlysisi, silver is kdeposited on the cathode while `O_(2)` is evolved at the anogde.The solution will be acidic due to the presence of" `HNO_(3)`
(iii) "Adilute solution of" `H_(2)SO_(4)` using platinum electrodes:
On pasing current both acid and water will ionise as follows:
`H_(2)S_(4)overset(aq)rarr2H^(+)(aq)SO_(4)^(2-)(aq)`
`H_(2)Ooverset(aq)(ltimplies)H^(+)(aq)+OH^(-)(aq)`
at cathode: `H^(+) (aq)` "ions will migrate to the cathode and will be reduced to" `H_(2)`
`H^(+)(aq)+e^(-)rarrH,H+HrarrH_(2)(g)`
Thus,`H_(2)(g)` will evolve at cathode.
At anode: `OH^(-) "ions will be released in preference to" SO_(4)^(2-)` ions because their discharge potential is less. They will be ovidised as follows:
`OH^(-)(aq)rarrOH+e^(=),4Ohrarr2H_(2)O(l)+O_(2)(g)`
Thus, `O_(2)(g)` "will be evolved lat anode. The solution will be acidic and will contain" `H_(2)SO_(4)`
(iv) " An aqueous solution of" `CuCI_(2)` "using platinum electrodes:"
"The electrolysis proceeds in the same manner as discussed in the of" `AgNO_(3) "solution.Both" CuCI_(2) "and" H_(2)O` will ionise as follows:
Thus ,`O_(2)(g) "will be evolved at anode. The solutin will be acidic and will contain" H_(2)SO_(4)`
(iv)"An aqueous solutioon of" `CuCI_(2)` "using platinum electrodes:"
"The electrolyisi proceeds in the same manner as discussed in the case of" `AgNO_(3) "Solution.Both" CuCI_(2) "and" H_(2)O` will ionise as follows:
`CuCI_(2)overset(aq)rarrCu^(2+)(aq)+2CI_(-)(aq)`
`H_(2)Ooverset(aq)(ltimplies)H^(+)OH^(-)(aq)`
At cathode: `Cu^(2+) " ions will be reduced in preference to " H^(+)` "ions and copper will be deposited at cathode"
`Cu^(2+)`ions will be reduced in preference to `H^(+)` ions and copper will be deposited at cathode
`Cu^(2+)(aq)+2e^(-)rarr`(deposited)
At anode: `CI^(-0) "ions will be discharged in preference to" OH^(-)` "ions which will remain in solution"
`CI^(-)rarrCI_(-)+e^(-=),CI+CIrarrCI_(2) (g)` (evolved)
Thus, `CI_(2)` will envole at anode: