Aqueous solution of copper sulphate is subjected to electrolysis using Pt electrodes. False statement about this process is

Upon electrolysis of aqueous ${\mathrm{CuSO}}_4$ solution, 

At anode: As the discharge potential of water is lower than Sulphate ion, Water undergoes oxidation to liberate oxygen.

$2{\mathrm{H}}_2\mathrm{O}\to 4{\mathrm{H}}^{+}+{\mathrm{O}}_2+4\mathrm{e};$

At cathode: Cupric ion gets reduced to copper.

$\left[{\mathrm{Cu}}^{+2}+2\mathrm{e}\to \mathrm{Cu}\right]\times 2$

With the progress of electrolysis, ${\mathrm{Cu}}^{+2}$ions are replaced by ${\mathrm{H}}^{+1}$ions. So, there will be gradual increase in $H^{+1}$ion concentration that decreases the pH.

Aqueous copper sulphate is blue in colour; with the loss of ${\mathrm{Cu}}^{+2}$ ions gradually it changes to colourless due the formation of sulphuric acid solution.