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Question
Predict the product of electrolysis in the following:
An aqueous solution of \[\ce{AgNO3}\] with platinum electrodes.
Solution
At cathode: Silver ions will be reduced and silver metal will be deposited.
At anode: The anode is not attacked, hence \[\ce{OH−}\] ions have a lower discharge potential than \[\ce{NO3}\] ions. As a result, \[\ce{OH−}\] ions discharge first, followed by \[\ce{NO3}\] ions, which decompose to release \[\ce{O2}\].
\[\ce{OH^-_{( aq)}-> OH + e-}\]
\[\ce{4OH -> 2H2O_{(l)} + O2_{(g)}}\]
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