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AngelEyes
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Going to resurrect an earlier thread rather than start a new one.
I have some Copper Nitrate and Barium Chloride. I am trying to precipitate Barium Nitrate from an aqueous solution of the two.
The equation I have is
Cu(NO<sub>3</sub> <sub>2</sub> + BaCl2 --> CuCl2 +
Ba(NO<sub>3</sub><sub>2</sub>
Barium Nitrate (8.2g/100ml water @ 20c) has a much lower solubility in water than Copper II chloride (42.6g/100ml water @ 20c) so I am expecting it to
precipitate out. Is this feasible or am I way off track here?
I have used a stoichiometirc ratio of materials.
I want the Barium Nitrate for use in green lances and portfires, the BaCl2 just doesn't cut it. Also, the Copper Nitrate is green, I am assuming it's
a tri-hydrate - .3H<sub>2</sub>O?
Thanks
AngelEyes.
\'Silk and satin, leather and lace...black panties with an Angel\'s face\'
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woelen
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If your copper nitrate is green, then it is not pure. I also have copper nitrate, and it is a beautiful crystalline glittering solid, bright blue,
even nicer blue than copper sulfate. Its solutions also are nice blue.
Don't you have any other nitrates around? If you have ammonium nitrate from fertilizer (possibly mixed with chalk), then you can use that. Just
dissolve in as little as possible of water and let stand for a day. All crap settles and then you can mix that very concentrated solution of ammonium
nitrate with your barium chloride solution.
KNO3 also may do the job, but it is somewhat less soluble. NaNO3 is very soluble, but I do not recommend that, because your product will always
contain a little amount of the sodium ions. These produce very strong orange/yellow light and certainly will spoil your compositions. Traces of
potassium ions or ammonium ions, however, do not really harm.
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AngelEyes
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Actually...
...my Copper Nitrate <i>is</i> blue. Not sure why I put it as green. It's large, clumpy blue crystals. Looks like blue quartz.
I do have Sodium Nitrate but don't want the pollution from Na. I have no other Nitrates, but I figured this reaction would proceed OK with the
materials I have.
I have some precipitate drying, it has a slightly greenish tinge though this could be contamination with Copper Chloride I s'pose. I'll see how it
dries then try some flame tests to try and determine what I have.
Cheers
AngelEyes.
\'Silk and satin, leather and lace...black panties with an Angel\'s face\'
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AngelEyes
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Right...so I have a quantity of a light-turquoise powder after filtration. It's taken ages to dry but seems non-hygroscopic now that it is dry.
If I try a standard flame test on it, it just melts and turns black. There's a tinge of greeny-blue...but that's hardly conclusive. I guess I must
have a mix of compounds in there or something.
If I mix with sulphur and try to ignite it, it turns black and I can see the dance of the light blue sulphur flame on top...then it eventually ignites
with a bright white, plus a hint of green, flame. It burns slow and leaves a black residue. Maybe sulphur isn't the best fuel to use here.
One odd thing is that when the powder was not quite dry and I mixed in a little hexamine it turned a sandy beige colour before my very eyes. Still
didn't burn well though...
\'Silk and satin, leather and lace...black panties with an Angel\'s face\'
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neutrino
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Hexamine is an amine with lone pairs. The Cu<sup>2+</sup> ions probably got bound to these.
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Misanthropy
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| Quote: | Originally posted by IodineForLunch
Where could one purchase lithium carbonate? None of my pyro chemical suppliers carry it.
David Hansen |
http://unitednuclear.com/chem.htm
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AngelEyes
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Found some Ammonium Nitrate...
...in a Calcium multi action fertiliser. Seems it's a mix of Ammonium Nitrate (about 80%) and chalk or other calcium compound. It's assay says it
contains both nitric and ammoniacal nitrogen, as well as a soluble calcium compound.
I added about 500ml of water to the 750g contents which I figure will dissolve all the nitrate nicely. It does, and I am left with some undissolved
crap. I filter this off to leave a nice, clear solution of what must be mostly Ammonium Nitrate. I add some Ammonium Sulphate to precipatate any
Calcium Nitrate out but there's no reaction so I figure I have quite pure Ammonium Nitrate solution with no dissolved calcium ions. I then add some
concentrated Barrium Chloride solution and get a precipitate fairly soon. I leave this for a while, then come back and filter off what I presume must
be fairly pure Barium Nitrate.
However, after drying and trying to ignite with various fuels I get hardly any reaction at all.
Do you reckon I have a mix of Barium Nitrate and Ammonium Chloride rather than mostly just the barium nitrate?
Have I got my equations / solubilities wrong?
Is Barium Nitrate just a real PITA to make by this method?
Should I redissolve (or re-wash) the solid I have?
I can do a good red fire, as well as yellow, white, purple-ish and orange. Blue is hit and miss anyway, but green <i>should</i> be quite
straightforward dammit! I use Strontium Carbonate for the reds and it's really good - is Barium Carbonate equally good for greens or can you really
use only the nitrate or (per)chlorate?
Beofre anyone mentions Skylighter <i>et al</i>, be aware that I am in the UK and we have a nanny state. Plus, I am quite skint and so
would prefer to use what I currently have.
Cheers for any pointers
AngelEyes.
\'Silk and satin, leather and lace...black panties with an Angel\'s face\'
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12AX7
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I have good results making barium nitrate in a similar way (from a less concentrated fertilizer also containing potassium sulfate and calcium
phosphate). The sulfate is precipitated with Ba and washed, then excess Ba is added to form Ba(NO3)2 on evaporation. It forms regular, coarse
crystals with a hopper tendency.
Er.. um... hummm... did you happen to think that your ammonium sulfate would be causing the barium to precipitate!?
My product burns in starts with magnalium, being a basic strobe comp. Bright greenish light.
Tim
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AngelEyes
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| Quote: |
Er.. um... hummm... did you happen to think that your ammonium sulfate would be causing the barium to precipitate!?
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Well, no - I added the Ammonium Sulphate in the first step to precipitate out any Calcium ions that may have been there -, but now that you mention it
any soluble suplahte <i>would</i> ppt out any Barium in solution wouldn't it? But I added the sulphate before any Barium Chloride goes
near the solution, got no ppt so assumed that all the Calcium was the insoluble crap I filtered off.
I hav another batch drying that used excess Ammonium Nitrate solution. I will dry the hell out of it then try again with other fuels...like sugar
maybe.
Cheers
AngelEyes
[Edited on 12-6-2006 by AngelEyes]
\'Silk and satin, leather and lace...black panties with an Angel\'s face\'
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tetrahedron
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strontium, manganese, lithium nitrates
i had some success isolating strontium nitrate from strontium carbonate and ammonium nitrate, but the procedure is slow. see my post here.
with manganese it seems to proceed analogously, but i wasn't able to isolate the manganese nitrate due to it's good solubility.
i'm currently making lithium nitrate. the carbonate has some solubility, and this reaction appears to work much faster, and the ammonia evolution to
be much stronger. i improvised a distillation setup and am now recovering quite concentrated ammonia solution. more details to follow.
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