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Question
Predict the product of electrolysis in the following:
An aqueous solution of \[\ce{CuCl2}\] with platinum electrodes.
Solution
\[\ce{CuCl2_{(s)} + aq -> Cu^2+_{( aq)} + 2Cl^-_{ (aq)}}\]
\[\ce{H2O <=> H+ + OH-}\]
At cathode: \[\ce{Cu^{2+}}\] ions are preferentially converted to \[\ce{H+}\] ions.
\[\ce{Cu^2+ + 2e- -> Cu}\]
At anode: \[\ce{Cl−}\] ions are preferentially oxidised over \[\ce{OH−}\] ions.
\[\ce{Cl- -> Cl + e-}\],
\[\ce{Cl + Cl -> Cl2_{(g)}}\]
The cathode deposits \[\ce{Cu}\], whereas the anode releases \[\ce{Cl2}\].
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