[simon66]

Hi guys,

I'm not sure if I'm posting this in the right section but I need help here.


I understand the concept of Electrolysis, but I'm having some issues. I currently want to separate copper from zinc and tin. I understand that I need to have a pure copper in order to do this, but my question is, what type of chemical do I need? I read about Copper(II), but do I just put pure copper(II)? Also what is the Voltage I need? I read between 1.5V to 3V.

Thank you!

[doc_ross]

I assume that you mean that you have copper II ions, zinc II ions, and tin II ions in aqueous solution and wish to selectively reduce the copper ions in solution by plating them onto a cathode.  Is this so?
If so, the most easily reduced species in solution will be reduced and the most easily oxidized will be oxidized.  You need to refer to a table of 1/2 reaction reduction tables to predict the outcome and to calculate the minimum voltage needed to reduce your species.

[simon66]

I assume that you mean that you have copper II ions, zinc II ions, and tin II ions in aqueous solution and wish to selectively reduce the copper ions in solution by plating them onto a cathode.  Is this so?
If so, the most easily reduced species in solution will be reduced and the most easily oxidized will be oxidized.  You need to refer to a table of 1/2 reaction reduction tables to predict the outcome and to calculate the minimum voltage needed to reduce your species.

Well kinda. I got a copper "block" that contains tin and zinc. That block is my Anode. I also got a copper pipe ( I'm assuming is atleast 99.99% pure copper ) on my Cathode. Both items are dipped on a Copper (II) sulfate solution. I'm assuming that once there is power, Copper from the Anode will stick to the Cathode. But here is the thing, will the copper stick to the Cathode or will copper crystals form on the Cathode? I would love if there was a way to get the copper and keep it on it's crystallized form ( if that's even possible ).

Thanks once again.

PS. I'm kinda new to thi