An easy copper electroplating demo for your redox unit

Simple Electroplating Demonstration

My IB seniors are just wrapping up our unit on electrochemistry and redox. This has always been a challenging topic within the IB curriculum. Admittedly, electrochemistry has not ever been my strong suit either, so this year I aimed to strengthen the unit with two additional demonstrations.

Over the summer I ordered a Hofmann apparatus to demonstrate the electrolysis of aqueous solutions. When I tried this demo last fall, I discovered that my glassware was broken. But I'll write about that in a future blog post. Instead, I'll focus on one of the easiest demos I have ever set up. Here is the complete list of equipment and materials:

400 mL beaker

200 mL 1 M CuSO4

copper electrode

9V battery

A set of alligator clip wires

1 paperclip



The 9V battery provides the needed energy to drive the non-spontaneous process in this electrolytic cell. For my demonstration, I connected the battery and let the cell run for about 30 seconds. There isn't much happening visually. But there is a lot going on! The copper ions in solution are reduced, plating the paperclip in a nice coating of relatively pure copper. And the copper electrode is being oxidized, thus replacing the copper ions that plate the paperclip. This keeps the concentration of copper ions in solution at a constant level.

The oxidation half-reaction at the copper anode:

Cu(s) --> Cu 2+ (aq) + 2 e-

The reduction half-reaction at the paperclip cathode:

Cu 2+ (aq) + 2 e- --> Cu (s)

Below is a picture of the paperclip with a copper coating and the clean shine of the portion of the copper electrode that was submerged in the solution. I only ran the electrolysis for about 30 seconds, but I'd like to try it for a longer time and see how much copper will plate the paperclip. I've got some milligram balances in my room to put to the test to see if the rate of plating can be calculated also. In a scenario where I had a bit more time (and less need to plow through the HL Chemistry curriculum so quickly), I'd like to extend this a bit to have students explore factors that affect the rate of electroplating such as concentration, voltage and temperature of the solution.


Do you have any extensions for this demonstration? Or suggestions for additional ways to show students electrolysis? I would love to hear about your use of this or other demos related to electrochemistry.


Join the conversation.

Comments 5

Tom Kuntzleman's picture
Tom Kuntzleman | Mon, 11/21/2016 - 12:39

Love this. And it's so simple! 

Melissa Stewart | Tue, 01/10/2017 - 19:03

Has anyone tried this with less than 1M CuSO4?  Will it still work but just maybe take long for the reaction to occurr?  Thanks!

Lowell Thomson's picture
Lowell Thomson | Thu, 01/12/2017 - 04:03

Hi Melissa,

Thanks for the question. I have not yet tried usinng different concentrations - and in the IB model the students have a full self-designed lab to complete, so I don't often answer these types of questions explicitly with them. Instead, I prefer to say, "There's a great lab idea there!"

I think I might have a student working on this over the next couple months, so I'll report back if there are reasonable results.


Michele Richards's picture
Michele Richards | Mon, 06/18/2018 - 05:00

We teach our kids "OIL RIG", but redox reactions can remain an abstract concept. What a cheap and easy way for students to see the results of redox! Thanks for sharing. 

Lowell Thomson's picture
Lowell Thomson | Mon, 06/18/2018 - 08:40

Hi Michele,

Thanks for the positive feedback. Much appreciated. This is an interesting lab in another way also, as the blue color of the solution shouldn't really change much. Copper is being oxidized at the anode, and reduced at the cathode, so the concentration of copper ions in solution remains approximately the same throughout the electroplating.

As for OIL RIG, that's one of the ones I use - along with LEO the lion goes GER. (Loss of Electrons is Oxidation, Gain of Electrons is Reduction.)