h0lx Posted January 26, 2007 Posted January 26, 2007 I was filtering a copper nitrate solution from impurities and noticed, the dried filter burned green and almost as fierce as KNO3 soaked paper. Never thought some heavy metal nitrate would be such a strong oxidizer. Would it be possible to use it in some kind of compositions? It would have to be dehydraed first ofcourse.
Pretty green flame Posted January 26, 2007 Posted January 26, 2007 A possible application might be an oxidizer in dragons eggs but i have no idea if it would work.
h0lx Posted January 27, 2007 Author Posted January 27, 2007 Hygroscopity is not a problem, you bind with water insoluble material, or use some non-polar liquid, if powder form is required, just like HE's with ammonium or sodium nitrate.
Douchermann Posted January 27, 2007 Posted January 27, 2007 The only problem would be getting it anhydrous. Sure you could probably use it in it's hydrate, but it would perform much better anhydrous.
ltf Posted January 27, 2007 Posted January 27, 2007 Cu(NO3)2/Mg lit spontaneously after less than a secound and exploded in open air almost like TATP.Cu(NO3)2/Fe was week and slow but relesed NOx (saw the NO2).
Mumbles Posted January 27, 2007 Posted January 27, 2007 I think one big problem this will cause is that it is very corrosive to metals. If there is any water in there it is going to corrode about anything. Just something else to be aware of. As for drying it, it should be easily done in an oven or grill or something. 150C should probably do it. It will probably change color as it dries. It will possibly be a brown. I'm trying to think back to Inorganic chem but don't remember where nitrate lies on the spectra.
hashashan Posted January 27, 2007 Posted January 27, 2007 my copper nitrate/mg burnt like a very furious flash. but no self ignition. its really powerful . but its damn hygroscopic, much more then AN. it takes about 10 minutes to become a puddle of water
Douchermann Posted January 28, 2007 Posted January 28, 2007 Yes, once you get it to it's pure hydrate form. However boiling a copper nitrate solution down (if you choose to make it), decomps some of the copper nitrate into copper hydroxide. Thats what I was talking about, I just didn't word it correctly.
Mardec Posted January 30, 2007 Posted January 30, 2007 Maybe just cook the copper nitrate dry.When it is dry mix under a parlon/acetone slurry. Mix good and try to get it slightly powdery. Then reducing the heat and a thick acetone/Mg/parlon slurry and stir it up real good. Then when nearly dry quickly press it in a tube? Not very easy & possibly very dangerous. But would make a nice blue flare though..
Mumbles Posted January 30, 2007 Posted January 30, 2007 I would suggest not boiling it off. Spread in a thin layer on a glass plate or pan and allow to naturally evaporate. I would then use low heat to dry it, maybe 50-60C. Higher heat (100C) after this to drive off the water would probably be the best shot after this. The salt decomposes to cupric oxide, NO2 and oxygen at 170C. Pure anhydrous Cupric nitrate is formed by reacting N2O4 with copper metal.
hashashan Posted January 30, 2007 Posted January 30, 2007 mumbles ... either I'm not understanding something or it will be very problematic. I had some experience with copper nitrate, and its highly hygroscopic, if left to sit in open air (at least where i live) for something like 10 minutes it turns into a blue puddle. so you cant just dry it without heating.
Mumbles Posted January 31, 2007 Posted January 31, 2007 hmmmmm, that would be problematic. Maybe start with the 50-60 thing then. A dessicator would also probably work with a strong dessicant.
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