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If electrolysis of aqueous CuSO $_{4}$ solution is carried out using Cu-electrodes, the reaction taking place at the anode is
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Verified Answer
The correct answer is:
$\mathrm{Cu}(\mathrm{s})-2 e^{-} \rightarrow \mathrm{Cu}^{2+}(\mathrm{aq})$
Electrolysis of copper sulphate solution using Cu-electrodes,
Ions present : $\mathrm{Cu}^{2+}, \mathrm{H}^{+}, \mathrm{SO}_{4}^{2-}, \mathrm{OH}^{-}$
At cathode $\mathrm{Cu}^{2+}(a q)+2 e^{-} \rightarrow \mathrm{Cu}(s)$
At anode $\mathrm{Cu}(s)-2 e^{-} \rightarrow \mathrm{Cu}^{2+}(a q)$
So, the option (d) is correct answer.
Ions present : $\mathrm{Cu}^{2+}, \mathrm{H}^{+}, \mathrm{SO}_{4}^{2-}, \mathrm{OH}^{-}$
At cathode $\mathrm{Cu}^{2+}(a q)+2 e^{-} \rightarrow \mathrm{Cu}(s)$
At anode $\mathrm{Cu}(s)-2 e^{-} \rightarrow \mathrm{Cu}^{2+}(a q)$
So, the option (d) is correct answer.
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