Match the column
Column I Column II
(P) ${Na}^{+} (a q) + e^{-} ⟶ Na (s)$ (1) Reaction taking place at anode
during electrolysis of very dilute
solution of NaCl using Pt
electrodes.
(Q) The concentration of
CuSO₄ solution does not
change on electrolysis (2) Reaction taking place at anode
during electrolysis of CuSO₄ using
Cu electrode.
(R) $Cu (s) ⟶ {Cu}^{2 +} (aq) + 2 e^{-}$ (3) Electrolysis of aqs CuSO₄ using Cu
electrodes
(S) $4 {OH}^{-} ⟶ 2 H_{2} O + O_{2} + 4 e^{-}$ (4) Reaction taking place at cathode
when electrolysis of aq NaCl is
done using Hg electrode

Difficult

Solution

When we take aqs NaCl in the cell we have $N a^{+}, C l^{-}, H^{+}, O H^{-}$ ions, among them, sodium ions do not get reduced, since they get reduced in molten state only.
Since Copper electrodes maintain equlibrium by $C u^{+ 2} + 2 e^{-} \Leftrightarrow C u (s)$ .
Oxidation of copper ions occur at anode.
Pt electrodes are inert and do not participate in the reaction.

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Column I		Column II
(P)	${Na}^{+} (a q) + e^{-} ⟶ Na (s)$	(1)	Reaction taking place at anode during electrolysis of very dilute solution of NaCl using Pt electrodes.
(Q)	The concentration of CuSO₄ solution does not change on electrolysis	(2)	Reaction taking place at anode during electrolysis of CuSO₄ using Cu electrode.
(R)	$Cu (s) ⟶ {Cu}^{2 +} (aq) + 2 e^{-}$	(3)	Electrolysis of aqs CuSO₄ using Cu electrodes
(S)	$4 {OH}^{-} ⟶ 2 H_{2} O + O_{2} + 4 e^{-}$	(4)	Reaction taking place at cathode when electrolysis of aq NaCl is done using Hg electrode