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(A) During the electrolysis of an aqueous solution of sodium sulphate $(Na_2SO_4)$,the ions present are $Na^+$,$SO_4^{2-}$,$H^+$,and $OH^-$.At the cat

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$H_2, O_2$

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(A) During the electrolysis of an aqueous solution of sodium sulphate $(Na_2SO_4)$,the ions present are $Na^+$,$SO_4^{2-}$,$H^+$,and $OH^-$.At the cathode,$H^+$ ions are reduced in preference to $Na^+$ ions because the reduction potential of $H^+$ is higher than that of $Na^+$.The reaction at the cathode is: $2H_2O(l) + 2e^- 	o H_2(g) + 2OH^-(aq)$.At the anode,$OH^-$ ions (or $H_2O$) are oxidized in preference to $SO_4^{2-}$ ions.The reaction at the anode is: $2H_2O(l) 	o O_2(g) + 4H^+(aq) + 4e^-$.Therefore,the products at the cathode and anode are $H_2$ and $O_2$ respectively.

$A$ solution of sodium sulphate in water is electrolysed using inert electrodes. The products at the cathode and anode are respectively:

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