How does nature of electrode affect selective discharge of ions.

Arrange the following according to the instructions given in bracket:

${\mathrm{Mg}}^{2+}, {\mathrm{Cu}}^{2+}, {\mathrm{Na}}^{1+}, {\mathrm{H}}^{1+}$ (In the order of preferential discharge at the cathode)

Select the ion in each case, that would get selectively discharged from the aqueous mixture of the ions listed below:

${\mathrm{Pb}}^{2+},{\mathrm{Ag}}^{+}$ and ${\mathrm{Cu}}^{2+}$.

When an aqueous solution of sodium chloride is electrolysed using platinum electrodes, what are the ions discharged at the electrodes?

Complete the following equation which show electrode reactions during certain electrolysis:

$2{\mathrm{O}}^{2-}\to {\mathrm{O}}_2+.......$

Complete the following equation which show electrode reactions during, certain electrolysis:

$........+{\mathrm{e}}^{-}\to \mathrm{Ag}$

Complete the following equation which show electrode reactions during certain electrolysis:

$.........\to {\mathrm{Cl}}_2+2{\mathrm{e}}^{-}$

Select the ion in each case, that would get selectively discharged from the aqeuous mixture of the ions listed below:

${\mathrm{SO}}_4^{2-},{\mathrm{NO}}_3^{-}$ and ${\mathrm{OH}}^{-}$.

Name the kind of particle present in : 

(i) Sodium hydroxide solution

(ii) Carbonic acid 

(iii) Sugar solution

Complete the following equation which show electrode reactions during certain electrolysis:

$2{\mathrm{H}}^{+}+2{\mathrm{e}}^{-}\to ...........$