In an electrolysis setup involving aqueous copper(II) sulfate (\( \text{CuSO}_4 \)) solution, the products at the anode depend on the ions present in the solution and their discharge potentials.
At the anode, where oxidation occurs, the possible reactions can involve the oxidation of copper ions (\( \text{Cu}^{2+} \)) or the oxidation of water. The discharge potentials indicate that the oxidation of copper ions is more favorable under standard conditions.
As a result, in a typical electrolysis of aqueous copper(II) sulfate:
- The anode reaction is usually the oxidation of copper ions: \[ \text{Cu}^{2+} + 2e^- \rightarrow \text{Cu} \quad (\text{deposition of copper on the anode}) \]
However, if the anode is inert (like platinum or graphite), you may not see visible copper deposit. Instead, the oxygen evolution might occur due to water oxidation, especially when the current is high enough.
In summary, the predominant anode product in an aqueous copper(II) sulfate solution during electrolysis is typically copper metal, but in some cases, oxygen gas may be evolved if the conditions favor it.
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