First slide

Electrolysis

Question

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

Easy

A

pH progressively increases
B

Oxygen is liberated at anode
C

Copper is deposited at cathode
D

Colour of the solution slowly changes from blue to colourless

Solution

Upon electrolysis of aqueous ${CuSO}_{4}$ solution,
At anode: As the discharge potential of water is lower than Sulphate ion, Water undergoes oxidation to liberate oxygen.
$2 H_{2} O \to 4 H^{+} + O_{2} + 4 e;$
At cathode: Cupric ion gets reduced to copper.
$[{Cu}^{+ 2} + 2 e \to Cu] \times 2$
With the progress of electrolysis, ${Cu}^{+ 2}$ ions are replaced by $H^{+ 1}$ 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 ${Cu}^{+ 2}$ ions gradually it changes to colourless due the formation of sulphuric acid solution.

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