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Question
State your observation for the following electrolytic reaction
Aqueous copper sulphate is electrolysed between platinum electrodes.
Solution
When the electrolysis of copper sulphate(aqueous) is electrolysed between platinum electrodes the following reaction follows :
\[\ce{CuSO4 ⇌ Cu^{+2} + SO^{2-}4 }\]
\[\ce{H2O ⇌ H+ + OH-}\]
Reaction at cathode : Copper ions and hydrogen ions migrate towards the cathode, `"Cu"^(+2)` ions being lower in the electrochemical series are preferentially discharged to hydrogen ions to form neutral copper atoms at platinum cathode.
\[\ce{Cu^{+2} + 2^{e-} -> Cu}\]
Reaction at anode : Sulphate ions and hydroxyl ions migrate towards the anode, Hydroxyl ions are preferentially discharged to sulphate ions at anode, to form neutral particles of `"OH"^-`, The electrically neutral hydroxyl reacts
among themselves to give water and oxygen.
\[\ce{OH- - e- -> OH}\]
\[\ce{4(OH) ->[-4e-] 2H2O + O2}\]
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