Re: Advice for resolving Cu(NO3)2-3H2O issues?


Nobody Important wrote:
I am currently trying to synthesize some yttrium barium cuprates
(YBCO-123) and have a paper that references the use of Cu(NO3)2-3H2O as
an initial reagent. The difficulty that I am having is in that the
copper nitrate is so deliquescent that it is actually partially
dissolving in it's own waters of hydration, before even cracking the
wax seal on the bottle, making stoichoimetric manipulations of the
material difficult, to say the least. I had the idea of dissolving the
entire unused bottle of the nitrate salt in something like 1M HNO3 and
portioning off the appropriate amount of the solution, then heating to
dryness before adding the other salts, but this introduces problems of
metallic contaminants from the acid, spattering from the heating /
drying process, etc. Does anyone have suggestions for working with
this unruly reagent? Am I simply overlooking something terribly
simple? Any help or suggestions would be most appreciated.

Do you need the solid copper nitrate? If you need standard copper
nitrate solution (which is rather difficult to make from copper
nitrate), I found that pure copper turnings dissolved in minium amount
of high purity HNO3 is a very good substitute for std. copper
solutions?

Seconldy, note that a large number of crystals sit in the bottom of the
bottle filled with the solution. Carefully decant the supernatant
solution, and transfer the crystals over a whatman ashless filter
paper. Dab them dry. Repeat if necessary. I had used copper nitrate for
some (unrelated) experiment. Hopefully, this experience may be of help.

A J.Chem.Ed. reference uses copper oxide instead, there are more
relevent experiments search their index., which seems to be less
problematic.

Cogdell, Connie D.; Wayment, Darcey G.; Cassadonte
A Convenient, One-Step Synthesis of YBa2Cu307-x Superconductors: An
Undergraduate Inorganic/Material, Volume 72 Issue 9 / September 1995
pp. 840-841

.

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