[Something]

After reading online how one person produced Cu(CH₃CO₂)₂ using vinegar and bits of copper boiled over a heat source (in this case, a stove), I felt like trying it out myself. After heating the solution for about 15 minutes, it started to turn a light blue color, which indicated to me that is was indeed working. The vinegar was soon boiled off and I was left with a light bluish powder. Success! However, I left it over my stove a bit too long and soon, smoke started to come off and the light bluish powder turned brown.

Now I'm assuming what I had before the smoking was copper II acetate, or atleast a hydrate of it. What I can not figure out, is what the brown-greenish powder is. I'm thinking the smoke was the acetate breaking down and releasing CO₂, but that does not account for the CH₃ unless that too formed water and CO₂ with the surrounding air. I'm thinking I was left with CuO. Any thoughts?

Please bear with me, I'm currently still in high school taking AP Chem.

[Arkcon]

Very likely correct.  Possibly a mixture of several products, some that you may not have heard of.  As a thought problem for you, can you write balanced equations, for possible reactions, that contain products that you've heard of, like CO2, H2O, CuO, and others?

[Something]

Thanks. Yea I did that to see what could possibly form. What are the other forms you said that be present? I'm kinda curious.

[408]

Household vinegar may not be pure acetic acid, many potential impurities may be present including flavoring agents etc.  Unless you used white distilled vinegar which I believe is relatively pure, although I did note some impurities upon making NaOAc from it followed by distilling with concentrated sulfuric acid to make glacial acetic acid.

Any impurities are likely to be organic, however salts may be present as well, so next time as opposed to boiling add some sodium bicarbonate to the solution to precipitate out malachite, a mixed copper hydroxide/carbonate.  This could then be dry heated to give you CuO.

By boiling Cu with vinegar you are relying on atmospheric oxygen combined with an acidic environment to be the oxidizing agent, the reaction will go faster if you add an oxidizing agent to the solution, even dilute household peroxide will do here.

Have fun, for this is how chemistry is really learned, by experimentation.

[Something]

I actually did use white distilled vinegar (5%).

Thanks for the tips, I'll be sure to try that out! Do you know the particular reaction with the baking soda added? Right now I have this: Cu + NaHCO₃ + Acetate ------ CuCO₃*Cu(OH)₂ + Unknown

[BluRay]

I actually did use white distilled vinegar (5%).

Thanks for the tips, I'll be sure to try that out! Do you know the particular reaction with the baking soda added? Right now I have this: Cu + NaHCO₃ + Acetate ------ CuCO₃*Cu(OH)₂ + Unknown

Cu + 2CH₃COOH + 1/2O₂ --> Cu(CH₃COO)₂ + H₂O

2Cu(CH₃COO)₂ + 2NaHCO₃ + H₂O --> Cu₂CO₃(OH)₂ + 2Na(CH₃COO) + 2CH₃COOH + CO₂

The Cu(CH₃COO)₂ crystals are of emerald-blue-green colour (I personally like it very much, for this reason I syntesized it).