Picture details: (Pic 1 - Background) Picture showing how the electrolysis is done. (Pic 2 - Top Right) The result at cathode and anode. (Pic 3 - Bottom Left) The copper electrode at cathode before and after. (Pic 4 - Bottom Right) The copper electrode at anode before and after.

Electrolysis of copper(II) sulphate solution using copper electrodes gives a different result compared to carbon electrodes. Here, I attached a well-combined picture of the experiment and some details on what happened at the anode and cathode.

CATHODE (Electrode that is connected to the negative terminal of battery):
Equation:   Cu2+ --> Cu + 2e
Product: Copper
Observation: Copper electrodes become thicker / Brownish metal deposited.
Reason: Copper(II) ions, Cu2+ are being discharged because of its position is lower than hydrogen ions, H+ in the electrochemical series. It receives two electrons and converted to copper atom.

ANODE (Electrode that is connected to the positive terminal of battery)
Equation:   Cu + 2e -->  Cu2+
Product: Copper(II) ions
Observation: Copper electrode becomes thinner / Copper electrode dissolves in the solution.
Reason: Copper acts as an active electrode and get involved with the chemical changes. It dissolves in the solution and form copper(II) ions.

I thought my student to use the DEPAN formula for the formation of ions and PODNA for the discharge of ions. (I think this DEPAN and PODNA are a good action research title...)

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