Which of the reactions occurs at anode when electrolysis of CuSO4 solution is done using platinum electrodes?

A
$Cu \to {Cu}^{2 +} + 2 e^{-}$
B
$2 {SO}_{4}^{2 -} + 2 H_{2} O \to H_{2} {SO}_{4} + O_{2} + 4 e^{-}$
C
$2 Cu \to {Cu}_{2}^{2 +} + 2 e^{-}$
D
$2 H_{2} O \to O_{2} + 4 H^{+} + 4 e^{-}$

Solution:

Water is oxidized in preference to ${SO}_{4}^{2 -}, Cu$ metal is not available as anode is made of platinum.

Electrolysis is the technique of causing a chemical change in a material by passing an electric current through it. The material either loses or gets an electron during the chemical transition (oxidation or reduction).

Which of the reactions occurs at anode when electrolysis of ${CuSO}_{4}$ solution is done using platinum electrodes?

Solution:

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