APO
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Preparation of Anhydrous Magnesium Nitrate
Could Liquid Nitrogen Dioxide dissolve Magnesium and form Anhydrous Magnesium Nitrate? I saw on another forum that that's how Anhydrous Copper Nitrate
is made industrially.
"Damn it George! I told you not to drop me!"
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Fantasma4500
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i dont think it would be a really comfortable reaction to perform in a testtube tbh, or well without great protection.. im quite sure N2O4 would react
violently with Mg metal..
i see the reason for using liquid NO2, but why not just use NO2 on some magnesium chippings, and also what would the reason be for the magnesium
nitrate anyways? if it would be to drag water out of nitric acid then i think it might be better to use something alike silica gel, which is
insoluble, dont know if it would react with HNO3 tho.. doubt it..
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AndersHoveland
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It would depend whether Mg(NO3)2 has any solubility in N2O4. I am not sure that it does. If there is no solubility, it cannot dissolve, and then a
protective layer would just form on the surface of the metal preventing further reaction. If there is a reaction, it is likely to be very energetic.
Magnesium is a much more electropositive metal than copper.
I'm not saying let's go kill all the stupid people...I'm just saying lets remove all the warning labels and let the problem sort itself out.
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AJKOER
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Perhaps a better approach, to quote from Wikipedia (http://en.wikipedia.org/wiki/Nitrogen_dioxide ):
"Conversion to nitrates
NO2 is used to generate anhydrous metal nitrates from the oxides:[6]
MO + 3 NO2 → 2 M(NO3)2 + NO "
So try warming MgO in dry NO2 (note, Mg(NO3)2 decomposes at 330 C).
Here is an alternate embodiment of this path that may yield some anhydrous nitrate. First note on heating at 256 C:
2 Cu(NO3)2 → 2 CuO + 4 NO2 + O2
so if a tube was first packed with Cu(NO3)2, which was directly heated, and then a layer of MgO, which is not directly subject to heat, perhaps some
anhydrous nitrate is produced.
Note the oxygen from the Cu(NO3)2 decomposition can also be consumed via:
2 NO + O2 --> 2 NO2
so the best net reaction could be:
2 MgO + 4 NO2 + O2 → 2 Mg(NO3)2
Note, this procedure does not require anhydrous copper nitrate as the hydrate can be carefully heated until red NO2 fumes are apparent and then the
layer of MgO added.
Bottom line, the suggested procedure may be able to convert a hydrated nitrate (in the form of Copper nitrate) into an anhydrous nitrate via an
established process for the creation of anhydrous nitrates.
[Edited on 10-3-2013 by AJKOER]
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blogfast25
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This patent should give some clues:
http://www.google.com/patents/US20090189117
One thing's for sure: you can't obtain anhydrous magnesium nitrate as you would anhydrous magnesium sulphate; by simple heating. On heating Mg(NO3)2
hydrate decomposes, like Be(NO3)2 hydrate.
[Edited on 10-3-2013 by blogfast25]
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AJKOER
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Quote: Originally posted by AJKOER  | Perhaps a better approach, to quote from Wikipedia (http://en.wikipedia.org/wiki/Nitrogen_dioxide ):
"Conversion to nitrates
NO2 is used to generate anhydrous metal nitrates from the oxides:[6]
MO + 3 NO2 → 2 M(NO3)2 + NO "
So try warming MgO in dry NO2 (note, Mg(NO3)2 decomposes at 330 C).
Here is an alternate embodiment of this path that may yield some anhydrous nitrate. First note on heating at 256 C:
2 Cu(NO3)2 → 2 CuO + 4 NO2 + O2
so if a tube was first packed with Cu(NO3)2, which was directly heated, and then a layer of MgO, which is not directly subject to heat, perhaps some
anhydrous nitrate is produced.
Note the oxygen from the Cu(NO3)2 decomposition can also be consumed via:
2 NO + O2 --> 2 NO2
so the best net reaction could be:
2 MgO + 4 NO2 + O2 → 2 Mg(NO3)2
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I believe this procedure will be successful as elsewhere on this forum, I recall reading a report of the accidental formation of anhydrous Aluminum
nitrate when NO2 escaped and attacked an Al foil covering.
I would further increase the reactivity of the Magnesium oxide with the creation of MgO nanocrystals prepared from a thermal decomposition of
magnesium oxalate powder (see http://www.sciencedirect.com/science/article/pii/S0022369710... ). Magnesium oxalate dihydrate can be prepared as follows:
MgSO4 + H2C2O4 + 2 H2O --> MgC2O4.2H2O (s) + H2SO4
Be careful, the created Sulfuric acid could be very strong depending on the level of hydration. Then, on heating Magnesium oxalate dihydrate (see http://books.google.com/books?id=i9nyvTYBQtAC&pg=PA459&a... ):
MgC2O4.2H2O (s) --Heat 623 to 723 K--> MgO (s) + CO (g) + CO2 (g) + 2 H2O (g)
If so desired, one could have a layer of Magnesium oxalate on top of (or adjacent to) the Copper nitrate, and subject the MgC2O4.2H2O to thermal
decomposition first. To implement this, perhaps using a long horizontally placed test tube and selectively heating sections would work.
[Edited on 15-3-2013 by AJKOER]
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Motherload
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I am going to try this unless someone already has and it doesn't work.
To dry methanol ... Anhydrous Ca(NO3)2 and anhydrous MgSO4 is added in molar quantities and agitated.
Mg(NO3)2 is alcohol soluble and CaSO4 isn't.
This is then filtered and alcohol distilled off or just evaporated.
"Chance favours the prepared mind"
"Fuck It !! We'll do it live !!"
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