(i) AgNO₃ ionizes in aqueous solutions to form Ag⁺ and NO₃^- ions.

On electrolysis, either Ag⁺ ions or H₂O molecules can be reduced at the cathode. But we know that the reduction potential of Ag⁺ ions is higher than that of H₂O.

Hence, Ag⁺ ions are reduced at the cathode. Similarly, Ag metal or H₂O molecules can be oxidized at the anode. But the oxidation potential of Ag is higher than that of H₂O molecules.

Therefore, Ag metal gets oxidized at the anode.

(ii) We know that Pt cannot be oxidized easily. Hence, at the anode, oxidation of water occurs to liberate O₂ . At the cathode, Ag⁺ ions are reduced and gets deposited.

(iii) H₂SO₄ ionizes in aqueous solutions to give H⁺ and SO₄^2- ions as follows –

On electrolysis, either of the H⁺ ions or H₂O molecules can get reduced at the cathode. But we know that the reduction potential of H⁺ ions is higher than that of H₂O molecules.

Hence, at the cathode, H⁺ ions are reduced to liberate H₂ gas.

On the other hand, at the anode, either of ions or H₂O molecules can get oxidized. But the oxidation of involves breaking of more bonds than that of H₂O molecules. Hence, ions have a lower oxidation potential than H₂O. Thus, H₂O is oxidized at the anode to liberate O₂ molecules.

(iv) In aqueous solutions, CuCl₂ ionizes to give Cu²⁺ and Cl^- ions as shown below:

On electrolysis, either of Cu²⁺ ions or H₂O molecules can get reduced at the cathode. But we know that the reduction potential of Cu²⁺ is more than that of H₂O molecules.

Hence, Cu²⁺ ions are reduced at the cathode and gets deposited there.

Similarly, at the anode, either of Cl^- or H₂O is oxidized. The oxidation potential of H₂O is higher than that of Cl^- .

But oxidation of H₂O molecules occurs at a lower electrode potential than that of Cl^- ions because of over-voltage (extra voltage required to liberate gas). As a result, Cl^- ions are oxidized at the anode to liberate Cl₂ gas.