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RogueRose
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[*] posted on 13-1-2016 at 04:34
Purifying ammonium sulfate fert


I have some pretty nasty looking ammonium sulfate. It is in normal fertilizer bead/prill size but it is brownish to dark yellow. When added to water it turns to black water with a disgusting foam on top that can be skimmed off and it eventually goes away.

I first tried heating the solution to dissolve as much sulfate and then gravity filter - then evaporate, but I think it was decomposing at 212 around the edges of the evap pan as it would be way to slow to do it with a fan and low heat (I used 300-350F)

So I decided to heat to 205F with an excess of fert and pour the liquid through very fine mesh filter (catch undissolveables - fert & black dirt specks - like creosote flakes..) and then chilled to 0c (or lower at points, IDK how that effects sulfates...) where about 1/3 of the sulfate would form crystals. I then filter through a fine cloth again, keeping the new crystals. I squeeze and use centrifugal spinning to help get the liquid out of the crystals.

Next I repeat entire heating & dissolving, filtering, cooling/crystalizing, filtering, etc.

The thing is that I have crystals that are not exactly pure. They have a grey brown tint and still some moisture. When I dry them out, they do whiten up a good bit, but I suspect tha there is still "dirt" in there.

I tried washing the crystals with acetone and that didn't work at all. I finally got them to mix around and I thought any remaining black/brown that was in them (I think it is tar from production from coal). but teh acetone didn't seem to absorb anything. I have no methanol but I have vodka and isopropyl 91% if that may help.

The last resort is to use water to wash and I end up getting beer color water and loose a good bit of my crystals.

I'm working on some filtration setups as it seems that the contaminates are attracted to cotton and stick pretty well (and actually rinse off afterwards). The problem is how do I evaporate 3-5 gals water without boiling and decomposing the sulfate to bisulfate at 212F?

What I have been doing is just constantly filtering the waters (still saturated for room temp) with gravity fed (man i need to figure out a powered system!!) and I can get very light (like 6:1 water:apple juice) after filtering with good clean slow filters.


What is the best way to go about doing this? There has to be something I'm missing (that isn't vacuum distillation).



[Edited on 13-1-2016 by RogueRose]
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[*] posted on 13-1-2016 at 09:57


Your contaminant is likely Fe- Probably as a sulfate initially, possibly as a hydroxide after heating.

As far as water removal, it may not be required until you achieve your final destination product, which might simplify the process. Could you specify what the ammonium sulfate is to be used for, how pure it needs to be?

If you happen to have a big bag of fertilizer grade Calcium nitrate and a big bag of fertilizer grade ammonium sulfate? I can conjecture... Obviously, you are a commercial blueberry grower ;)

There are a couple of existing threads here regarding exactly this OTC material and purification methods. And some about very noisy blueberries. I could merge?




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Praxichys
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[*] posted on 13-1-2016 at 10:41


When you wash your crystals, are you using ice water? It should be so cold that it is starting to freeze. Otherwise the washing will cause heavy losses.

You could also try adding a flocculation agent to accumulate particles of dirt or tar during the boiling process. Add a few scoops of diatomaceous earth/bentonite clay/activated carbon/celite, etc. during the boil, and see if it clarifies and settles the dirty solution upon cooling/prolonged standing.

Failing that, I'd try adding a bunch of ammonia to get metals to precipitate as their hydroxides, then retry the flocculation procedure.




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[*] posted on 13-1-2016 at 10:49


Quote: Originally posted by Praxichys  
When you wash your crystals, are you using ice water? It should be so cold that it is starting to freeze. Otherwise the washing will cause heavy losses.


That will barely help. Ammonium sulfate's solubility in ice water is 70g/100ml. At room temp it's only 74g/100ml.

I'd say to chuck it in a flask with NaOH for an ammonia generator. The contaminants are very likely non-volatile. If you need clean ammonium sulfate, neutralize some aq. NH3 with clean sulfuric acid, but I suspect you don't.
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[*] posted on 13-1-2016 at 11:36


Quote: Originally posted by UC235  
That will barely help. Ammonium sulfate's solubility in ice water is 70g/100ml. At room temp it's only 74g/100ml.

Yes, but think about the kinetics of dissolution - dissolving 70g into 100ml of cold water will take far longer than 74g into 100ml of room temp water. Certainly a few seconds of washing is not enough to saturate the filtrate. The gains in practice are much larger than simple solubility would suggest.

Crystal size is also a big factor, which makes this hard to quantify. With a multi-liter solution I assume the cooling rate is low, and thus the crystals are fairly large. Obviously, finer crystals provide less benefit from washing cold.




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[*] posted on 13-1-2016 at 13:58


Sometimes the impurities are water soluble or at least form colloidal suspensions. When I worked with ammonium sulfate, filtering left me with a pale yellow solution. I also noted that alcohols and acetone also dissolved whatever what was yellow. It was then I figured out I had organics with considerably sized molecules. I made a solution of my yellow sulfate along with a couple ounces of pet shop activated carbon and agitated. I was left with a water white solution.

[Edited on 1/13/2016 by chloric1]




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RogueRose
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[*] posted on 14-1-2016 at 04:14


Quote: Originally posted by Bert  
Your contaminant is likely Fe- Probably as a sulfate initially, possibly as a hydroxide after heating.

As far as water removal, it may not be required until you achieve your final destination product, which might simplify the process. Could you specify what the ammonium sulfate is to be used for, how pure it needs to be?

If you happen to have a big bag of fertilizer grade Calcium nitrate and a big bag of fertilizer grade ammonium sulfate? I can conjecture... Obviously, you are a commercial blueberry grower ;)

There are a couple of existing threads here regarding exactly this OTC material and purification methods. And some about very noisy blueberries. I could merge?



The purchase of the various fertilizers is one of many that have been purchased but as of yet the only two that make the water absolutely filthy when added in a 1:20 fert:water concentration. This is totally unacceptable if either if these were to be used in a hydroponics setup and will cause MAJOR fouling of some equipment and will eventually ruin equipment.

Hydroponics ready fert can be 20x more expensive (or more) so I am doing some research on purification.

I alsohave about 10+ bags of other chems that I'm running purification tests on. I plan on publishing start to finish pics, how to's etc when I'm done.
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[*] posted on 14-1-2016 at 04:45


Quote:
I can conjecture... Obviously, you are a commercial blueberry grower ;)

I grew it years ago ─ too Indica-dominant and too smelly!

My current PurpleHaze/OTH et al gives me what I like in a smoke . . .

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[*] posted on 14-1-2016 at 07:47


If you intend to use ammonium sulfate for hydroponics, why try to reduce it to a dry powder after cleaning it up? You will just need to dissolve it again for your end use.

Several others posting here on cleaning up ammonium sulfate are using with cheap Calcium nitrate fertilizer to obtain ammonium nitrate.

I do use ammonium sulfate for fertilizing blueberries as we don't have granite bedrock, my orchard soil is not quite acidic enough. I just spread it on the soil in early spring and let it dissolve into the soil.

Looking forward to your opus on purifying bulk OTC fertilizer chemicals-




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3. Mention anything you have learned from your target.
4. Only then are you permitted to say so much as a word of rebuttal or criticism.

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RogueRose
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[*] posted on 15-1-2016 at 00:11


Quote: Originally posted by Bert  
If you intend to use ammonium sulfate for hydroponics, why try to reduce it to a dry powder after cleaning it up? You will just need to dissolve it again for your end use.

Several others posting here on cleaning up ammonium sulfate are using with cheap Calcium nitrate fertilizer to obtain ammonium nitrate.

I do use ammonium sulfate for fertilizing blueberries as we don't have granite bedrock, my orchard soil is not quite acidic enough. I just spread it on the soil in early spring and let it dissolve into the soil.

Looking forward to your opus on purifying bulk OTC fertilizer chemicals-


Well Amm Sulf seems like a good starting point for a lot of compounds and it is a pretty decent fertilizer. The purification is an exercise in learning various aspects of compounds and how things react with each other. To me it is like a puzzle of sorts.

If the fert is going to be used outside, it will be used as-is but if I were to use it in a hydroponics setup I think I would purify it first.
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[*] posted on 15-1-2016 at 05:29


You do realize that one can prepare pure aqueous (NH4)2SO4 easily and quickly from high purity bath salt (Epsom salt is MgSO4 with low heavy metal impurities as people bathe in it and could absorb those toxins through their skin) and passing NH3 vapors through it by heating household ammonia, for example. Just cool and separate off the Mg(OH)2.

Albeit, a little more expensive up front, but impurities largely eliminated which otherwise may surface as a bigger problem latter!

In doing the math, remember that your time and labor is really not free either.

[Edit] If you are interested in manufacturing your own aqueous (NH4)2SO4, may I suggest a relatively simple recently invented route (see, "Hydrogen production via photocatalytic oxidation of aqueous ammonium sulfite solutions", by Cunping Huanga, et al.). To quote from the extract:

"The main process, unique to the S-NH3 cycle, is the visible light-induced photocatalytic oxidation of ammonium sulfite (NH4)2SO3) with production of hydrogen and ammonium sulfate ((NH4)2SO4). The (NH4)2SO4 product is processed to generate oxygen and recover NH3 and SO2, which are then recycled and combined with water to regenerate (NH4)2SO3 forming a closed cycle. In this paper, we report our experimental findings with regard to the photocatalytic oxidation of aqueous (NH4)2SO3 solutions containing suspended platinum-doped cadmium sulfide (Pt/CdS) particles irradiated by a xenon arc lamp. We achieved energy conversion efficiencies (absorbed light to chemical energy of hydrogen) of about 12%. The photocatalyst remained active for more than 70 hrs. "

Link: https://www.google.com/url?sa=t&source=web&rct=j&...

In your embodiment, I would pass clean air through burning pure sulfur as a source of SO2 and pass air through heated aqueous ammonia, and then combine the streams to form the ammonium sulfite (NH4)2SO3) in distilled water. Then add a suspension of 1% Pt doped CdS. While treating the resulting solution to sunlight in shallow pans, maintain the temperature at least at 50 C for best conversion. Heating the final solution to over 65 C and pass air into it should remove any remaining ammonium sulfite (decomposition temperature) or ammonia. Filter to recover the Pt/CdS catalyst.

Only major concern, perform a small scale test run and check soluble Cadmium content of final (NH4)2SO4 solution and/or final Cd levels in grown plants. Major issue is the employment of chlorinated water which may form trace amounts of soluble CdCl2 from CdS.

[Edited on 15-1-2016 by AJKOER]
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[*] posted on 15-1-2016 at 09:39


Purified some of my 25kg sack of ammonium sulphate last week.

Simply dissolve the fertiliser in a minimum of hot water then filter the solution.

Boil down to about 75% volume then allow to cool slowly.

Much purer crystals will form and sink to the bottom.
(if they don't, boil it down some more and let cool again).

Pour off the watery top layer (important: this is where the crud is) spread out your crystals and allow to dry.

If you want really pure crystals, repeat this recrystallisation process once or twice.

Not a fast or fancy process, but it works for many substances which dissolve much better in hot solvent than cold.




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[*] posted on 16-1-2016 at 04:38


Quote: Originally posted by aga  
Purified some of my 25kg sack of ammonium sulphate last week.

Simply dissolve the fertiliser in a minimum of hot water then filter the solution.

Boil down to about 75% volume then allow to cool slowly.

Much purer crystals will form and sink to the bottom.
(if they don't, boil it down some more and let cool again).

Pour off the watery top layer (important: this is where the crud is) spread out your crystals and allow to dry.

If you want really pure crystals, repeat this recrystallisation process once or twice.

Not a fast or fancy process, but it works for many substances which dissolve much better in hot solvent than cold.


That is kind of what I was thinking of doing - process wise - but I was adding a filtration process in there when in solution.

After my filter process I kept the crystals that formed while the solution was sitting above the filter (gravity filter), washed with cold ammonia solution, added them back to filtered solution and heated to dissolve again.

This time I allowed to cool slowly and when at room temp I added a fan. This is what I got from room temp evap.

nh4so4.jpg - 104kB

Notice the crystals are pretty white/clear and then there are "pillars" that look totally diffeent and are darker. They seem to consist of very fine powder/crystals vs the much larger and clearer crystals that can be seen.

Could these "pillars" be the bisulfate? Wiki says at 100C Amm Sulf decomposes to bisulfate so if the water boils, is that going to decompose the sulfate - leaving what you see as the final product?

I noticed in another thread that the bisulfate can be converted back to the original sulfate by mixing in an ammonia solution. I have yet to try this but I guess I could test some of these pillars with that process and see if it changes the way they form.

Can anyone identify these or whether if it is a normal crystalization process of some kind?
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[*] posted on 16-1-2016 at 14:03


Quote: Originally posted by RogueRose  

That is kind of what I was thinking of doing - process wise - but I was adding a filtration process in there when in solution.

Quote: Originally posted by aga  
Simply dissolve the fertiliser in a minimum of hot water then filter the solution.

Can you not read Logan ?




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[*] posted on 17-1-2016 at 11:00


The brown stuff definitely is not the bisulfate. The bisulfate of ammonium is colorless/white. The brown stuff simply is crap. I would carefully remove the brown material and keep the white crystalline material. The white crystalline material looks reasonably pure to me and most likely is good enough for most chemistry experiments. The brown stuff can be kept around. Good for making ammonia gas by adding NaOH and a small amount of water.



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[*] posted on 22-1-2016 at 08:51


In case the brown stuff is iron related, you could add some ammonia solution and then filter. Iron hydroxides/hydrated oxides are usually coarse, so can be filtered out easily.
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