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Author: Subject: Sodium chloride and sodium nitrate seperation.
MadHatter
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[*] posted on 14-10-2021 at 11:42
Solubility


https://en.wikipedia.org/wiki/Solubility_table

This should be of some help. It's a cycling process.

1) Boil down the solution until NaCl crashes out then hot filter.
2) Add 10% more water by volume. This should keep the remaining
NaCl in solution at freezing.
3) Freeze the solution so that NaNO3 crashes out. Note: Solubility of
NaNO3 at freezing is 73 grams per 100 ml water. The amount in your
solution must exceed this value in order to work.

Depending how much NaNO3 you want, or need, repeat the cycle.

Before it became cheap and too time consuming for my lazy ass, I
used this method to obtain KNO3 from NaNO3 and KCl.

[Edited on 2021/10/15 by MadHatter]




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danieldavies
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[*] posted on 15-10-2021 at 00:10


Thanks everyone, looks like i can reuse all my waste nitrate.
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Antiswat
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[*] posted on 22-10-2021 at 03:59


ppt it out using lead
prior this you use fractional recrystallization, reference solubility table

i have this solubility data
NaNO3 SOLUBLE EtOH INSOLUBLE acetone EtOH 0.31 19.5*C ethanol: 0.036, MeOH 0.41
NaCl INSOLUBLE EtOH, 1.5/100mL MeOH, insoluble acetone
so theres conflicting ideas of NaNO3 solubility in EtOH

PbAc + NaCl = PbCl2 (ppt) + NaAc

depending on what the actual NaNO3 EtOH solubility is, this may help..

NaAc SOLUBLE 5.3g/100ml 15

but really whatever you cant fractionally crystallize out just leave it for now, but to remove all chloride you would still wanna ppt out as lead chloride

lead acetate may be made by CuAc + Pb metal
it takes time, or just HAc + H2O2 + Pb




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Truth is ever growing - but without context theres barely any such.

https://en.wikipedia.org/wiki/Solubility_table
http://www.trimen.pl/witek/calculators/stezenia.html
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theAngryLittleBunny
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[*] posted on 6-12-2021 at 15:46


Quote: Originally posted by MadHatter  
https://en.wikipedia.org/wiki/Solubility_table

This should be of some help. It's a cycling process.

1) Boil down the solution until NaCl crashes out then hot filter.
2) Add 10% more water by volume. This should keep the remaining
NaCl in solution at freezing.
3) Freeze the solution so that NaNO3 crashes out. Note: Solubility of
NaNO3 at freezing is 73 grams per 100 ml water. The amount in your
solution must exceed this value in order to work.

Depending how much NaNO3 you want, or need, repeat the cycle.

Before it became cheap and too time consuming for my lazy ass, I
used this method to obtain KNO3 from NaNO3 and KCl.

[Edited on 2021/10/15 by MadHatter]


Maybe adding some ethanol to the solution would maybe get 50% ethanol might crash out any NaCl while leaving the NaNO3 mostly in solution, because NaCl is very insoluble in ethanol even with a lot of water present. It might crash out some NaNO3 too, but you can just increase the volume. You will have to experiment yourself, since barely anyone here had any reason to separate these salts.

You have to look up the solubilities of the salts in different solvents, this website has been very useful to me for that http://chemister.ru/Database/search-en.php

But it might also be easier to buy a nitrate fertilizer and extract nitrates from that. Nowadays it's always mixed with some other salt to prevent people making explosives (at least in europe), but often they could be separated more easily then NaNO3/ NaCl. There is one fertilizer which is a 45/55 mix of ammonium nitrate and ammonium sulfate, the ammonium nitrate is soluble in methanol (and sparingly in ethanol) while ammonium sulfate isn't, so it could be separated that way. At around 30 euros/dollars for a 25Kg bag it makes this fertilizer a very cheap source for nitrates.
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MadHatter
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[*] posted on 6-12-2021 at 22:15
Ammonium Nitrate/Sulphate


The same technique, in theory, could be used to separate that 45/55 mix.

In step 2 add 46% more water to keep (NH4)2SO4 in solution at freezing.

Step 3 would require > 118 grams NH4NO3 per 100 ml water to crash it
out with freezing.

This process was beautiful for KNO3 from NaNO3 and KCl because
KNO3's solubility at 0C is 13.3 grams/100 ml water. The method was
cheap because the starting reactants were bought in a garden shop.

I wish everybody success !




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[*] posted on 7-12-2021 at 18:47


Add more silver nitrate until the chloride is removed entirely.

Then add hydrogen sulfide, or sodium hydroxide to precipitate any remaining silver ions, leaving behind only sodium nitrate?




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theAngryLittleBunny
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[*] posted on 8-12-2021 at 12:00


Quote: Originally posted by kclo4  
Add more silver nitrate until the chloride is removed entirely.

Then add hydrogen sulfide, or sodium hydroxide to precipitate any remaining silver ions, leaving behind only sodium nitrate?


Using silver nitrate for that would be insane, sodium nitrate is extremely cheap and can be made from nitrate fertilizers. Silver nitrate is like 1000 times more valuable then sodium nitrate. And H2S is just unnessecarily dangerous.
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