In the process of electroplating of copper on a metallic spoon, the iron spoon is made the cathode. A thin sheet of pure copper is made the anode. When electricity is passed through the solution, Cu2+ ions move towards the cathode and get reduced to copper metal. This copper metal gets electroplated on the object, i.e., the metalic spoon.
The sulphate ions move towards anode. Here the sulphate ions do not get oxidied. Instead, the copper metal of the anode gets oxidised to Cu2+ ions. These copper ions go into the solution..............
But, why does ths happens? Why does the sulphate ions do not grt oxidised? Instead, why does the copper metal of the anode gets oxidised? Please explain me as fast as possible. I've to give an exam. Hope to get the answer from a MERITNATION EXPERT.
We are extremely sorry for the delay and deeply regret for this inconvenience caused. Hope, your exam went well.
The answer to your question is as follows:
Oxidation potential of Cu is more than sulphate ion. So, copper gets oxidized at anode. But at your level as you have not studied the concept of oxidation potential it can be explained only in terms of activity series, i.e Cu will have more tendency to get oxidized than the sulphate ion. So, copper will be oxidized at anode and Cu2+ ion will go in the solution and move toward cathode where they get deposited as copper by gaining 2 electrons.