Jmap science
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Making barium nitrate from barium carbonate without nitric acid
I do not have any nitric acid but I do have potassium and strontium nitrates. How do I make barium nitrate from barium carbonate. I was wondering
if there was a reaction to make barium nitrate without nitric acid or nitrogen oxides.
I will use the barium nitrate to make nitric acid by addition of H2SO4. The flask would be chilled and filtered to make conc. nitric acid.
I have been working on a way to make conc. nitric acid from a conc. acid and potassium nitrate without distillation. I got the idea from
chemistry hideout. I want to improve on it.
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TheChemiKid
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This should be posted in beginnings, just search on google, and with a tiny bit of you can figure this out.
Add hydrochloric acid to make barium chloride, then add to a hot solution of sodium nitrate and let cool. This was stated on wikipedia.
This other method may not work, but you could try adding copper nitrate to the barium carbonate.
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Brain&Force
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Won't work. Barium carbonate is insoluble.
A similar synthesis and distillation has been done before with calcium nitrate and sulfuric acid. Don't waste your valuable barium.
At the end of the day, simulating atoms doesn't beat working with the real things...
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bfesser
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Thread Moved
22-1-2014 at 15:28 |
phlogiston
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Dissolve in molten ammonium nitrate. Research well before attempting this, because melting ammonium nitrate can be dangerous.
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"If a rocket goes up, who cares where it comes down, that's not my concern said Wernher von Braun" - Tom Lehrer |
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bismuthate
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How about NO2 and barium oxide from the decomposition of barium carbonate.
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Jmap science
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Would barium carbonate and potassium nitrate work?
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TheChemiKid
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No. Barium Carbonate is insoluble in water and basically anything else.
Go for the calcium nitrate instead of the barium nitrate, but if you really want to use the barium, then try either the NO2 or the
HCl/NaNO3 method.
When the police come
\( * O * )/ ̿̿ ̿̿ ̿'̿'̵͇̿̿з=༼ ▀̿̿Ĺ̯̿̿▀̿ ̿ ༽
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HeYBrO
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if you have strontium and potassium nitrate, why don't you buy some? seems like the most logical solution, especially because barium is not the
friendliest ion to work with when soluble.
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Jmap science
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well I see your point
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woelen
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If you have hydrochloric acid, then you could try making a solution of BaCl2 from BaCO3. Making very pure BaCl2 from the pottery grade BaCO3 is not
trivial, but if you intend to use your product for pyro-purposes, then you need to be less stringent on purity. You also do not need to isolate the
BaCl2, you can keep it in solution.
Here is my webpage on making BaCl2.2H2O:
http://woelen.homescience.net/science/chem/exps/BaCl2_2H2O/i...
To the solution of BaCl2 you add a solution of KNO3. Ba(NO3)2 is much less soluble than KNO3, KCl and BaCl2, so that should drop out. From a single
step you get mostly Ba(NO3)2 with a small amount of K-ions and Cl-ions in it, but that is not a problem for pyro-purposes. Otherwise, you need to
recrystallize your Ba(NO3)2 from quite a large amount of water.
This also works with NaNO3 instead of KNO3, but the resulting Ba(NO3)2 will contain some Na-ions in that case and if you want to use it for
pyro-purposes, that is not good at all.
[Edited on 23-1-14 by woelen]
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Jmap science
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Thanks
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markx
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Well, the method that I used, was to add a slight stoichiometric excess of BaCO3 to ammonium nitrate solution and then boil, boil, boil until no more
ammonia fumes evolved. Ammonium carbonate will decompose in boiling water and will therefore be expelled from the solution. What you are left with is
Ba(NO3)2 solution. The boiling will take a LONG time though....as I remember I kept the kettle simmering for 2-3 days. But in the end you are left
with a nice crop of crystals. Filter, purify and dry them as needed. Beware though, that water soluble barium salts are very poisonous. Take the
neccesary precautions when handling them.
[Edited on 23-1-2014 by markx]
Exact science is a figment of imagination.......
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TheChemiKid
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Why did you take away the picture?
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Brain&Force
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Woelen's procedure sounds good to me, but if you take the KCl contaminated crystals and dissolve them in sulfuric acid, wouldn't you be making aqua
regia with the nitrate? Would distillation cause the nitrosyl chloride to escape and decompose?
At the end of the day, simulating atoms doesn't beat working with the real things...
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AJKOER
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Brain&Force:
Good thinking. Always expect interactions!
However, I suspect the only way to form some NOCl here would be by the action of conc H2SO4 on the dry chloride and nitrate salts.
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Zyklon-A
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This is rather off topic, but I want to make nitric acid from Barium nitrate, (Jmap science gave me the idea). I have 98% sulfuric acid, and pyro
grade Ba(NO3), I mixed them in stoichiometric proportions, and waited.
The problem was that even though Ba(NO3) is insoluble, there was just way to much solid in proportion to the liquid. It just looked like
there wasn't any liquid at all. The HNO3 was fuming out from the heat generated, what should I do. I'm not asking to be spoon fed here,
tried a few different ideas, and have worked on this since the day this topic was started, but nothing has worked.
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Metacelsus
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Dissolve the barium nitrate in water first. Or, you could distill the nitric acid (however, you might as well do this with any other nitrate.)
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Zyklon-A
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The whole reason that I want to use barium is because I don't have a distillation setup. I know I'll have to get one at some point, but I can't afford
to drop the required $100- $300, at least not now. Nitric acid >95% is not required, but I'd like it to be as con. as possible.
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servo
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Quote: Originally posted by woelen  |
To the solution of BaCl2 you add a solution of KNO3. Ba(NO3)2 is much less soluble than KNO3, KCl and BaCl2, so that should drop out. From a single
step you get mostly Ba(NO3)2 with a small amount of K-ions and Cl-ions in it, but that is not a problem for pyro-purposes. Otherwise, you need to
recrystallize your Ba(NO3)2 from quite a large amount of water.
[Edited on 23-1-14 by woelen] |
Can you use Ammonium Nitrate instead?
what I did is added an excess of ammonium nitrate solution (hot) to a hot saturated solution of Barium Chloride
what i noticed is an immediate crystalline sort of precipitation and I kept boiling the solution for about 2 hours during which more and more ppt
were formed finally I took it off the heat let it cool down filter the crystals
Now my question is are the crystals really Barium Nitrate? or its Barium Chloride that did not react with ammonium nitrate , I took excess of amonium
nitrate so that if they both react All of Barium chloride reacts
I know topic is old but chemistry never gets old
[Edited on 27-11-2021 by servo]
[Edited on 27-11-2021 by servo]
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Fulmen
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@Zyklon: Just wash it out with water and recover the dilute acid. I think it's the best you can hope for, tried the same with calcium nitrate and it
was literally a smoking mess. The stiff paste was unworkable and too corrosive to handle.
We're not banging rocks together here. We know how to put a man back together.
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chloric1
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Long shot, not sure it would even work but what about solvent extraction. Fuming nitric acid is supposed to be soluble in dichloromethane while
concentrated sulfuric acid is not according to the patent US3981975A. You add portions of methylene chloride to your fuming corrosive mess and only the nitric acid will dissolve. Then simply distill or
evaporate the methylene chloride.
Fellow molecular manipulator
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