Electrolysis of copper sulphate solution?

What exam board is this for? I only need to know what ion goes where

AQA last topic of C2? (we're so behind arghhhh)

I'm with AQA and I've never seen a question on equations of electrolysis

@Mayhem™
For higher tier: "Candidates should be able to complete andbalance half equations for the reactions occurring at the electrodes during electrolysis."

I don't even look at specs; I just do past papers

Hi, I'm kinda confused on part of the electrolysis of copper sulphate solution (CuSO4)(aq):

Anode: 4OH(-) -----> 2H2O + O2 + 4e(-)
Cathode: Cu(2+) + 2e(-) -----> Cu

I understand the half equation at the cathode, but I'm confused on why so many products are formed at the anode?
Is it just something I have to memorise or is there a simple explanation as to why the products are produced? (This is probably a dumb question haha)

This is deffo on the AQA papers. Just remember that the Anodes positive, The Cathode is negative then remember the products. There's no explanation, just gotta learn it

Hi, I'm kinda confused on part of the electrolysis of copper sulphate solution (CuSO4)(aq):

Anode: 4OH(-) -----> 2H2O + O2 + 4e(-)
Cathode: Cu(2+) + 2e(-) -----> Cu

I understand the half equation at the cathode, but I'm confused on why so many products are formed at the anode?
Is it just something I have to memorise or is there a simple explanation as to why the products are produced? (This is probably a dumb question haha)

During electrolysis:the cathode gets coated with copper. bubbles of oxygen are given off at the anode As the copper ions are discharged as copper atoms at the cathode, the blue colour of the solution gradually fades and an oxidation reaction occurs which is the 4e- (electron loss).
The negative sulphate ions (SO42-) or the traces of hydroxide ions (OH–) are attracted to the positive electrode. But the sulfate ion is too stable and nothing happens. Instead either hydroxide ions or water molecules are discharged and oxidised to form oxygen.