deltaH
Dangerous source of unreferenced speculation
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Calcium nitrate perhydrate
THIS IS A HYPOTHETICAL, UNTRIED AND POTENTIALLY VERY DANGEROUS IDEA, SO DO NOT TRY IT AT HOME!
Calcium nitrate crystallises with four crystal waters, making it a poor oxidant for energetics.
Salts containing crystal waters like sodium carbonate can be crystallised with hydrogen peroxide replacing the crystal water to form perhydrates, for
example, the poorly named "sodium percarbonate" which is simply sodium carbonate perhydrate:
http://en.wikipedia.org/wiki/Sodium_percarbonate
I was wondering, therefore, whether this could be done with calcium nitrate to form something like Ca(NO3)2.2H2O2?
I couldn't find anything by a cursory search for such a compound.
It should make an interesting oxidant, plus you get to 'upgrade' calcium nitrate AND concentrate H2O2, but I don't know if hydrogen peroxide would
react with the nitrate in concentrated solutions when trying to prepare it? Perhaps one would need to use very cold solutions?
[Edited on 30-12-2014 by deltaH]
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Bert
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Not a clue if that's possible... But carbamide peroxide is. Get some anhydrous Calcium nitrate and dissolve it in high strength peroxide, crystallize
(maybe your theorized substance) out?
http://en.m.wikipedia.org/wiki/Hydrogen_peroxide_-_urea
(Edit)
Works for Potassium, Sodium and ammonium nitrates...
http://www.google.com/patents/US20080190525
[Edited on 1-1-2015 by Bert]
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deltaH
Dangerous source of unreferenced speculation
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Interesting... nice patent, thanks Bert
The reason I thought of calcium nitrate is because it is a simple OTC nitrate that has a helluva lot of crystal waters, so could potentially hold a
helluva lot of perhydrate... ok well two probably  maybe three or four is one's
really lucky.
It's available as the fertiliser CAN. CAN itself, not being a great oxidant... but this could be a way to remedy that. Nice to see from that patent
that the ammonium nitrate can also form a perhydrate. So CAN looks very attractive as a substrate.
The thing is that peroxide interacts more strongly as a 'hydrate' than water itself AFAIK, so you should be able to crystallise these things out of
reasonably conc. solutions fairly easily... don't think you need anhydrous conditions, but I might be mistaken of course, since this is all
hypothetical.
??Dissolve the salt to saturation in 35% peroxide and stick it into a freezer overnight, then filter crystals while cold??
BTW, since this is an oxidant only, would it be legal to prepare it?
[Edited on 1-1-2015 by deltaH]
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