vano
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Copper (I) carbonate
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.
  
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DraconicAcid
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How did you make it?
Please remember: "Filtrate" is not a verb.
Write up your lab reports the way your instructor wants them, not the way your ex-instructor wants them.
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vano
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Easily. From copper monochloride and sodium carbonate.
[Edited on 1-1-2021 by vano.kavt]
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vano
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Now it has dark colour.
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ChemTalk
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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
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vano
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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]
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Maurice VD 37
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Seems to be impossible. Copper(I) chloride is not soluble into water !!! How can you mix its solution with carbonate ?
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Bedlasky
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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]
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vano
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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.
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vano
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[Edited on 3-2-2021 by vano]
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Bedlasky
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Vano: If you want to dissolve CuCl, you need complexing agent, adding acid/base isn't enough.
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vano
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In my opinion, bivalent chloride helps to dissolve, otherwise why would this carbonate precipitated.
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Bedlasky
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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.
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vano
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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
[Edited on 4-2-2021 by vano]
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Bedlasky
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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.
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DraconicAcid
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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.
Please remember: "Filtrate" is not a verb.
Write up your lab reports the way your instructor wants them, not the way your ex-instructor wants them.
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vano
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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]
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vano
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which compound do you mean?
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DraconicAcid
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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.
Please remember: "Filtrate" is not a verb.
Write up your lab reports the way your instructor wants them, not the way your ex-instructor wants them.
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vano
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| Quote: Originally posted by DraconicAcid |
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....
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woelen
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Dark in this situation is really dark. Nearly black, on very strong dilution brown/green. See
https://woelen.homescience.net/science/chem/riddles/copperI+...
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vano
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Thanks. But it need clorine gas.
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woelen
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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.
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vano
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Okay
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