Alchemist
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Urea Nitrate Procedure Mechanism
Hello all,
Please don't flame me if this has been answered before or if it's a stupid question, but I can't find any info on it.
On the making of Urea Nitrate via HCL, and a Nitrate (I've seen it done with Ammonium or Potassium Nitrate used), and of course Urea. What is the
balanced equation? What is the mechanism here? What happens to the Ammonium or Potassium Ion and what is the purpose of the Hydrochloric Acid? I
always thought for a nitration you needed concentrated Sulfuric Acid!
Just wondering, the Alchemist.....
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12AX7
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Urea nitrate sounds ionic to me (i.e., urium nitrate, or whatever that particular aminium is called). In that case, HCl is only needed to protonate
the urea; essentially an ionic metathesis proceeds, seperating urea nitrate and KCl / NH4Cl -- assuming the solubilities work out in favor of these
products forming.
Nitrourea (presumably, N-nitro) would be formed by a different mechanism.
Tim
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Sauron
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Correct.
H2NC(=O)NH2 + NH4NO3 + H+Cl- -> H2NC(=O)NH3+NO3- + NH4Cl
[Edited on 16-4-2008 by Sauron]
Sic gorgeamus a los subjectatus nunc.
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guy
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Sauron that is NITRITE
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Sauron
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Duh!
That's what I get for not paying attention.
Thanks for correction.
Does ammonium nitrite exist?
Sic gorgeamus a los subjectatus nunc.
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not_important
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| Quote: | Originally posted by Sauron
Does ammonium nitrite exist? |
http://www.vias.org/encyclopedia/chem_ammonia_salts_no2.html
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Preparation of ammonium nitrite by the sublimation in a vacuum of a mixture of ammonium chloride and alkali nitrites
Panchānan Neogi, Birendra Bhusan Adhicāry
Journal of the Chemical Society, Transactions 99, 116-118, Royal Society of Chemistry, 1911
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| Quote: | | Abstract : Ammonium nitrite is highly unstable, both in a dry state and in concentrated aqueous solutions. When such solutions are used industrially
they are normally stored at a pH of 8 - 9 and a temperature of 5C. or less. The effect of additions of chromium compounds on the decomposition of
ammonium nitrite solutions was studied, under isothermic and non-isothermic conditions. It was found that such compounds catalyze the decomposition of
ammonium nitrite more intensely than HCl. This led to the conclusion that contamination by even small amounts of such compounds should be carefully
avoided in industrial work with ammonium nitrite solutions in order to minimize the danger of explosive decomposition. |
http://stinet.dtic.mil/oai/oai?verb=getRecord&metadataPr...
[Edited on 17-4-2008 by not_important]
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