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]blogfast25 - 24-4-2008 at 08:06
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...woelen - 24-4-2008 at 13:30
I also have made cuprates in solution under highly alkaline conditions. This is not difficult, but isolating them from such solutions is!elementcollector1 - 5-4-2013 at 18:33
Just made a solution of cuprate. How do I turn it back to copper hydroxide or oxide? Boil it?Hexavalent - 6-4-2013 at 08:10
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]Mixell - 6-4-2013 at 08:16
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. DraconicAcid - 6-4-2013 at 08:27
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.
