azarnoosh - 25-8-2010 at 22:40
bbartlog - 26-8-2010 at 06:19
Metathesis. Give us a better question and maybe you'll get a better answer. Really this is detritus.
ScienceSquirrel - 26-8-2010 at 06:54
Reacting 2 equivalents of citric acid with one of nickel carbonate.
I would expect it to be a bit like iron (II) citrate.
http://en.wikipedia.org/wiki/Iron%28II%29_citrate
citrate nickel?how to produce?:(
azarnoosh - 29-8-2010 at 18:38
mr.crow - 29-8-2010 at 18:48
Please learn how to communicate properly
psychokinetic - 30-8-2010 at 00:05
US$0.05 + a lemon.
Stir.
Perhaps if you told us what you were using it for, what ways you were interested in making it etc. Ask the right question and you can get more than a
great answer, here.
ScienceSquirrel - 30-8-2010 at 11:38
I have already attempted to answer your question elsewhere.
Iron II forms a stable complex citrate.
Nickel II salts are far more stable to oxidation than iron II salts and I would expect nickel II carbonate to form a similar stable complex on
reacting one mole of the carbonate with two moles of citric acid.
Here is the dinickel tricitrate complex which is well known and defined.
http://www.chemicalbook.com/ChemicalProductProperty_EN_CB978...
You have a dibasic metal ion and a tribasic acid that forms complexes very readily, it is pretty obvious that a range of compounds can be formed in
which the ratio of nickel atoms to citrate anions varies and may even be non stochiometric!