Final answer:
In the electrolysis of a CuSO4 solution using platinum electrodes, copper metal is deposited at the cathode, and oxygen gas is released at the anode. Additionally, the solution becomes more acidic.
Step-by-step explanation:
Electrolysis of CuSO4 Solution
During the electrolysis of an aqueous solution of CuSO4 using platinum electrodes, there are two primary reactions that take place, one at each electrode. At the cathode, the copper ions (Cu2+) in solution are reduced to copper metal (Cu). At the anode, water molecules are typically oxidized instead of sulfate ions (SO42-), leading to the generation of oxygen gas (O2) and hydrogen ions (H+).
The half-reactions at each electrode can be written as follows:
- Cathode (reduction): Cu2+ (aq) + 2e- → Cu(s)
- Anode (oxidation): 2H2O(l) - 4e- → O2(g) + 4H+
As a result of these reactions, copper metal is deposited at the cathode, while oxygen gas is released at the anode. The overall chemical reaction also causes the solution to become more acidic due to the production of H+ ions.