December 01, 2021, 01:53:29 AM
Forum Rules: Read This Before Posting

Topic: Electroplating Preferential Reactions  (Read 1476 times)

0 Members and 1 Guest are viewing this topic.

Offline offlinedoctor

  • Regular Member
  • ***
  • Posts: 26
  • Mole Snacks: +2/-0
Electroplating Preferential Reactions
« on: September 05, 2012, 04:23:41 AM »

I'm just wondering for Eletroplating, why do we assume that for something such as Copper, if we use that to coat an item, it would be oxidised at the anode, and also reduced at the Cathode (to form the coating), why isn't water reacted at all in these instances?

Offline 123456789

  • Regular Member
  • ***
  • Posts: 21
  • Mole Snacks: +2/-1
Re: Electroplating Preferential Reactions
« Reply #1 on: September 05, 2012, 05:07:27 AM »
For copper, at the anode, oxidation takes place. Since the electrode is not inert, the electrode will react. So copper is oxidised. Then at the cathode, it is reduction, so copper is reduced. There is nothing to do with H+: Hydrogen is more reactive than copper so copper will be preferentially discharged anyway.

However, if the metal is more reactive than Hydrogen, (for example iron (II), then yes hydrogen will be liberated, if I'm not wrong.

Sponsored Links