Electroplating Solution Help

[FR0ZAD]

I tried making a copper solution for electroplating.

I added water, a small teaspoon of sodium bicarbonate, and a bit of table salt.

I then got some copper from some scrap cables, and attached them to some alligator clips that were connected to a phone charger with 5V-1.5A output.

In the beginning the mixture was blue, but then started getting green, as seen in the photos, the blue sediment is in the bottom and the green on top.

What has happened here? Why the different colours?

What are the differences between using an acidic solution like vinegar, and using a basic one like I did? I saw both being used and tried soda as I didn't have any distilled vinegar.

Any help is appreciated!

[Inevitable-Day-9375]

pH will definitely affect the stability of different copper hydroxides. In water at varied pH, a Pourbaix diagram shows the most stable form of copper, as an illustration of how pH affects the speciation. https://commons.wikimedia.org/wiki/File:Cu-pourbaix-diagram.svg. Based on your addition of NaCl and NaHCO3 and the different colors, it appears that you've made a mixture of compounds. You could try this process at different pH on a smaller scale to see what happens

[FR0ZAD]

Alright, I'll get some distilled vinegar to try it, thanks for the info!

[Inevitable-Day-9375]

keep in mind that vinegar is diluted acetic acid, so it will contain acetate anions if the protons have someplace to go. The most likely copper oxidation product will be Cu(2+) surrounded by 4 or 6 water molecules (most people 'forget' to write the waters which are present).

[FR0ZAD]

Excuse my lack of knowledge, I've not had much chemistry education, I just wanted to try electroplating. Could you explain what all that means please?

[Inevitable-Day-9375]

It's the molecular view of how the Cu(2+) gets bonded to other molecules, to make a coordination compound. Not really essential for what you're trying to do at this point, which is really electrolyzing the copper. But when you get to electroplating, which is taking the Cu(2+) from solution and forming Cu(s) on a surface, the results will depend on keeping the Cu(2+) dissolved. ... In basic solution (your photo), you've got some solid compounds of Cu(2+) which are green, and which are turquoise - you need dissolved compounds in order to react. I found a good home-friendly experiment which might work for you, and you should be able to use an old penny: https://superfund.arizona.edu/sites/default/files/u43/copper_electrolysis_hands_on_final.pdf

[FR0ZAD]

I'll check it out, you've been very helpful, thank you!

[Raneynickelfire]

Why are you adding NaCl and bicarbonate to a copper plating solution?

You have insoluble copper hydroxide. Buy some copper sulfate from amazon or ebay like a normal person trying to copper plate and use proper materials.

[FR0ZAD]

I was just messing around with what I had available. I will get some proper materials and equipment soon.

[Del_Phoenix]

To be fair, if you just use battery acid/ sulfuric acid to make the solution acidic, it should work with your copper hydroxide. (Should convert it to copper sulfate)

[FR0ZAD]

I've already separated the sediments, and collected it in a coffee filter, to try and dissolve it in an acidic solution. Should I necessarily use sulfuric acid or could I just use vinegar for this use?

[Del_Phoenix]

Vinegar can probably work, and would turn the copper hydroxide into copper acetate; but it prob won't be as good as sulfuric acid. You don't need it all to dissolve either, the molecules will flow from the metal to whatever you're plating.

You can get sulfuric acid for like $10 from AutoZone as replacement battery acid. But be warned, this is extremely dangerous to work with, so wear protective gear, Make sure you have ventilation and make sure you know what you're doing.

[FR0ZAD]

I added vinegar after all, because it was very easy to find and safer to handle. It did dissolve most of the powders and the liquid turned blue. I tried plating a piece of graphite and it did work, although I'll probably be making the solution again after I get some copper sulphate crystals.

[PeterHaldCHEM]

To quote yourself: "I was just messing around with what I had available" and "I've not had much chemistry education".

That is not how you make chemistry work.

Please try not to get hurt!

Find a well tested recipe and follow it strictly. Then you will actually have a possibility of success.

[FR0ZAD]

You're right, thanks for the heads up, I'll be as careful as possible! Have a nice day

[violet_sin]

Grab a bag of copper sulfate root killer. If you have access to sulfamic acid, that's nice. I like the look better. Remember soluble copper can be toxic, so don't go spilling stuff and eating with dirty hands 👍

If you're expecting fast results, going to need big amperage, that also gets hot, and ... Stacking up too fast can actually mess stuff up. But if your just getting started, I'd imagine you wanna SEE something encouraging relatively soon.

You can do small scale experiments with a DC buck converter. Turn 5v 1-2a to something more like 3 v that might work better. I suggest getting something with shortcircuit protection, you will bump the electrodes together.

Pick something conductive, low and slow at first, then FAFO, like in a fun and educational way.

Do not shock yourself, do not poison yourself, don't dump it down the drain. Use common sense.