Explain the electrolysis of aqueous copper sulphate.

Following reactions occur at the cathode during the electrolysis of aqueous silver chloride.

$$\begin{gathered} {\mathrm{Ag}}^{+}\left(\mathrm{aq}\right)+{\mathrm{e}}^{-}\to \mathrm{Ag}\left(\mathrm{s}\right); {\mathrm{E}}^{°}=+0.80 \mathrm{V} \\ {\mathrm{H}}^{+}\left(\mathrm{aq}\right)+{\mathrm{e}}^{-}\to \raisebox{1ex}{$1$}\!\left/ \!\raisebox{-1ex}{$2$}\right. {\mathrm{H}}_2\left(\mathrm{g}\right); {\mathrm{E}}^{°}=+0.00 \mathrm{V} \end{gathered}$$

On the basis of their standard reduction electrode potential$\left({\mathrm{E}}^{°}\right)$ values, which reaction is feasible at the cathode and why?

Identify the substance underlined in the following:

The electrode that increases in mass during the electro-refining of silver.

For the electro-refining of copper, write the reaction that takes place at the anode.

State one observation for the following:

Copper sulphate solution is electrolysed using copper electrodes.

Ions are the current carriers in electrolytes.

What are the products obtained at anode and cathode during the electrolysis of molten sodium chloride?

Draw the diagram of the apparatus used in electroplating and label the following part: 

The substance to be electroplated. 

The $\mathrm{pH}$ of the solution _________ during the electrolysis of dilute aqueous solution of ${\mathrm{CuSO}}_4.$