What happens to the pH during the electrolysi | vedclass

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(B) During the electrolysis of aqueous $CuSO_4$ using platinum electrodes,the following reactions occur:At the cathode: $Cu^{2+}(aq) + 2e^- \rightarro

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Decrease in $pH$

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(B) During the electrolysis of aqueous $CuSO_4$ using platinum electrodes,the following reactions occur:At the cathode: $Cu^{2+}(aq) + 2e^- \rightarrow Cu(s)$At the anode: $2H_2O(l) \rightarrow O_2(g) + 4H^+(aq) + 4e^-$As the reaction proceeds,$H^+$ ions are produced at the anode,which increases the concentration of $H^+$ in the solution.Since $pH = -\log[H^+]$,an increase in $[H^+]$ leads to a decrease in the $pH$ of the solution.

What happens to the $pH$ during the electrolysis of aqueous $CuSO_4$ using platinum electrodes?

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