bfesser
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Sodium Cuprate
I've tried to prepare sodium cuprate by the vague description from <a
href='http://webpages.charter.net/dawill/tmoranwms/Chem_Cu.html#Cuprate'>this site</a> twice now with no success. Has anyone else been able
to verify Tim's results? My copper(II) oxide is lab grade, not OTC or home made, and my sodium hydroxide as well.
[edit]
I just realized that I forgot to link to the site. Sorry for my absentmindedness.
[Edited on 4/23/08 by bfesser]
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blogfast25
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Although I haven't used Tim's exact method, I've made the cobalt blue solution of sodium cuprate inadvertently by precipitating CuO from Cu
(+II) salts at far too high a pH. CuO is indeed somewhat amphoteric and will dissolve in strong NaOH or KOH. You may want to use freshly prepared
CuO for that experiment...
Let us know how you get on...
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woelen
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I also have made cuprates in solution under highly alkaline conditions. This is not difficult, but isolating them from such solutions is!
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elementcollector1
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Just made a solution of cuprate. How do I turn it back to copper hydroxide or oxide? Boil it?
Elements Collected:52/87
Latest Acquired: Cl
Next in Line: Nd
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Hexavalent
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Do these complexed anions behave similarly to the cationic form of the element? Perhaps adding sodium carbonate solution to the sodium cuprate would
precipitate copper (II) carbonate, for example?
I don't think so, but it don't hurt to ask or try 
[Edited on 6-4-2013 by Hexavalent]
"Success is going from failure to failure without loss of enthusiasm." Winston Churchill
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Mixell
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It won't work, the cuprate is soluble in strong basic environment. Like it doesn't precipitate as Cu(OH)2, it won't precipitate as CuCO3. The best way
is to acidify the solution gradually, copper hydroxide would precipitate. Just be careful that the temperature won't exceed 60-70C and don't use
anything containing chlorides, as some oxy-/hydroxy chlorides may form.
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DraconicAcid
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Quote: Originally posted by Hexavalent  | | Do these complexed anions behave similarly to the cationic form of the element? Perhaps adding sodium carbonate solution to the sodium cuprate would
precipitate copper (II) carbonate, for example? |
It won't act as the cation, but you could acidify it with sodium bicarbonate to precipitate it as the basic carbonate.
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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