Sciencemadness Discussion Board

Copper Acetate

kazaa81 - 8-5-2006 at 04:51


I have searched for copper acetate on some stores, grocery included (anything that isn't a chemical supplier), but I haven't found nothing or just CuSO4.
I've tried artistics too but they no longer sell it.

Does anyone suggest me a place to buy copper acetate? or instead another acetate, so that I will do a methasynthesis?


Copper (I) Acetate
CAS #: 598-54-9
Mol. 122.590 g/mol
Form: colored crystals
M.P. Decomposition
B.P. Sublimation
Sol. Reacts with H2O

Copper (II) Acetate
CAS #: 142-71-2
Mol. 181.635 g/mol
Form: blue-green hygroscopic powder

[Edited on 8-5-2006 by kazaa81]

The_Davster - 8-5-2006 at 04:55

CuSO4--(one of several methods)-->CuO

kazaa81 - 8-5-2006 at 05:02

unfortunately my acetic acid source is just food-grade 5% vinegar...too much impurities and water...
Can you post some of the methods of conversion of CuSO4 to CuO?

Thanks rogue

mantis - 8-5-2006 at 06:30


Can you post some of the methods of conversion of CuSO4 to CuO?

Add NaOH to a CuSO<sub>4</sub> solution and boil it.

gsd - 8-5-2006 at 06:49

It is better and easier to convert CuSO4 to Basic Copper Carbonate. Add stoichiometric quantity of Na2CO3 solution to CuSO4 solution and wash the green precipitate of CuCO3.Cu(OH)2 with water till neutral to pH. Then decant the water as much as possible and boil with slow addition of Acetic Acid till all carbonate reacts.

CuAc2.H2O has low solubility in water at room temp. (about 5% w/w) Hence you need to filter the boiling solution to get rid of insoluble impurities.

PainKilla - 8-5-2006 at 10:31

I used vinegar and CuO to get Cu(Ac)2 in excellent yields. You need to boil down the solution, but once you get it down to around 400ml or so (from 1L of vinegar and ~35g CuO), you can let it cool and lots of the copper acetate precipitates as fine greenish crystals. I would use that method, personally. Regular distilled vinegar is actually quite pure, so if your copper compound is pure, you will get extremely high grade crystals...

Note: Let the vinegar/CuO suspension sit for a while, it all reacts in the end. Using a slight excess of vinegar may help aid this.

[Edited on 8-5-2006 by PainKilla]

kazaa81 - 8-5-2006 at 14:33

Is CuSO4 able to shift metallic Pb?
I mean, if I have a solution of CuSO4 and I put a sheet of metallic Pb, will I get PbSO4 and Cu?

CuSO4 (aq) + Pb (s) ---> Cu (s) + PbSO4 (aq)


CuCO3 (aq) + Pb (s) ----> Cu (s) + PbCO3 (aq)

12AX7 - 8-5-2006 at 14:40

Well, no, those aren't soluble lead compounds. You'll get a layer of PbSO4 and that's that.

The second will never proceed under any circumstances, except possibly high pressure CO2. CuCO3 isn't soluble, so the best you could hope for would be fine powders and heat. But heat decomposes the carbonates, so it's not going to happen without a lot of help.


kazaa81 - 8-5-2006 at 14:58

So, because lead soluble salts in H2O are just the ones of organic acids...

Ca(NO3)2 (aq) + CuSO4 (aq) -----> Cu(NO3)2 (aq) + CaSO4 (s)

Cu(NO3)2 (aq) + Pb (s) -----> Pb(NO3)2 (aq) + Cu (s)

Pommie - 10-5-2006 at 05:42

That works. However, the Calcium sulphate is a bitch to filter and the copper nitrate is a bitch to dry.

Go for a Cu(NO<sub>3</sub>;)<sub>2</sub> solution and throw some lead in.

If you are trying to plate lead dioxide electrodes then you want a 50/10 mix of lead/copper nitrate.


[Edited on 11-5-2006 by Pommie]