Sciencemadness Discussion Board

Copper (I) carbonate

vano - 1-1-2021 at 07:32

Hi, today i made Copper (I) carbonate. It is a yellow solid. I thought it might have been oxide, but when I add acetic acid carbon dioxide was released. It os a very nice and stable monovalent compound.

received_403263710780608.jpeg - 200kB received_755118628432619.jpeg - 65kB PicsArt_01-01-07.31.11.jpg - 99kB

DraconicAcid - 1-1-2021 at 07:51

How did you make it?

vano - 1-1-2021 at 07:54

Easily. From copper monochloride and sodium carbonate.

[Edited on 1-1-2021 by vano.kavt]

vano - 30-1-2021 at 04:28

Now it has dark colour.

IMG_20210130_162625.jpg - 2.9MB

ChemTalk - 31-1-2021 at 11:48

Thanks Vano, we love how you are always coming up with very interesting compounds.

Did you mix the solids, or was sodium carbonate in solution? And did you have to heat them?

ChemTalk
chemistrytalk.org

vano - 1-2-2021 at 08:51

Thanks. I just mixed the solutions, and soon the copper carbonate precipitated. I did not heat the solution, although I remember using warm water, but not hot.

[Edited on 1-2-2021 by vano]

Maurice VD 37 - 2-2-2021 at 13:43

Seems to be impossible. Copper(I) chloride is not soluble into water !!! How can you mix its solution with carbonate ?

Bedlasky - 2-2-2021 at 13:55

Copprous chloride is unstable in alkaline solution - it turn in to oxide/carbonate (depending on what makes your solution alkaline). Btw. CuCl is soluble in slightly acidic sodium chloride solution, so this is option how to dissolve it.

[Edited on 2-2-2021 by Bedlasky]

vano - 3-2-2021 at 00:09

In the second photo when I added acid the carbon dioxide was generated intensely. Also as far as I know chloride is soluble in both acid and alkaline solution. However, as Bedlasky said, it is not so stable. If you are interested i can re-synthesizing in more detail.

vano - 3-2-2021 at 00:23



[Edited on 3-2-2021 by vano]

Bedlasky - 3-2-2021 at 12:11

Vano: If you want to dissolve CuCl, you need complexing agent, adding acid/base isn't enough.

vano - 3-2-2021 at 20:59

In my opinion, bivalent chloride helps to dissolve, otherwise why would this carbonate precipitated.

Bedlasky - 4-2-2021 at 03:34

CuCl dissolves in acidic, neutral or slightly alkaline solutions in the presence of complexing agents (like chlorides, bromides, sulfites, thiosulfates, thiourea, cyanides, ammonia etc.). Copper carbonate precipitate because it have lower solubility than chloride.

vano - 4-2-2021 at 04:05

Yes i agree with you. My cloride has greenesh colour, because it is old. I'm sure bivalent cloride helps to dissolve. It actually has a darker color(chloride in jar).I have other chloride but it has almost the same color.
https://commons.wikimedia.org/wiki/File:Copper(I)_chloride.%E1%83%95%E1%83%99.jpg

IMG_20210204_160139.jpg - 2.7MB


[Edited on 4-2-2021 by vano]

Bedlasky - 4-2-2021 at 08:15

CuCl dissolves in aqueous solutions of any soluble chlorides, not just divalent chlorides. Cation doesn't affect it.

Old samples of CuCl are always green due to aerial oxidation of CuCl in to Cu(II) oxychlorides.

DraconicAcid - 4-2-2021 at 08:20

Quote: Originally posted by Bedlasky  
CuCl dissolves in aqueous solutions of any soluble chlorides, not just divalent chlorides. Cation doesn't affect it.

Old samples of CuCl are always green due to aerial oxidation of CuCl in to Cu(II) oxychlorides.

I suspect vano is referring to CuCl2 rather than any divalent chloride, and that will form the weird black mixed-valence complexes that so often show up.

vano - 4-2-2021 at 09:10

I know why it has a green color I do not see for the first time. It contains enough CuCl2 to dissolve CuCl.

[Edited on 4-2-2021 by vano]

vano - 4-2-2021 at 09:13

Quote: Originally posted by DraconicAcid  
weird black mixed-valence complexes .
which compound do you mean?

DraconicAcid - 4-2-2021 at 09:57

Quote: Originally posted by vano  
Quote: Originally posted by DraconicAcid  
weird black mixed-valence complexes .
which compound do you mean?


CuCl is insoluble in water. CuCl2 dissolves in water to give green or blue solutions, depending on concentration. A mixture of the two will give a dark solution with a mixed-valence complex of uncertain composition.

vano - 4-2-2021 at 10:06

Quote: Originally posted by DraconicAcid  
Quote: Originally posted by vano  
Quote: Originally posted by DraconicAcid  
weird black mixed-valence complexes .
which compound do you mean?


CuCl is insoluble in water. CuCl2 dissolves in water to give green or blue solutions, depending on concentration. A mixture of the two will give a dark solution with a mixed-valence complex of uncertain composition.


Dark? Do you mean black and such colours? Or dark green....

woelen - 4-2-2021 at 10:55

Dark in this situation is really dark. Nearly black, on very strong dilution brown/green. See

https://woelen.homescience.net/science/chem/riddles/copperI+...

vano - 4-2-2021 at 23:24

Quote: Originally posted by woelen  
Dark in this situation is really dark. Nearly black, on very strong dilution brown/green. See

https://woelen.homescience.net/science/chem/riddles/copperI+...


Thanks. But it need clorine gas.

woelen - 5-2-2021 at 03:02

No, it does not need chlorine gas. Copper(I) compounds are easily oxidized by oxygen from air, and such oxidized compounds usually have a dark greenish or brownish color.

vano - 5-2-2021 at 03:23

Okay