| Pages:
1
2 |
obsessed_chemist
Hazard to Self
Posts: 65
Registered: 23-3-2007
Member Is Offline
Mood: electronegative
|
|
Controlled Bacterial Nitrification (salpeter production, using nitrosomonas etc)
Has anyone here ever prepped a fish tank with nitrosomas and nitrobacter bacteria and ammonia to establish the nitrogen cycle before adding fish?
Well, I was thinking, this could be an interesting experiement if done simply to produce nitrates. The pH and temperature have to be carefully
maintained, air bubbled in, kept in the dark (for optimal conversion/bacteria growth), etc., but I think it would be fun to give it a try. Clear
household ammonia could be used as the main food source for the bacteria, slowly adding until the bacteria count increase exponentially. Apparently
these nitrobacter need some phosphate, so I suggest adding a tiny amount of ammonium phosphate as the source. They also need carbonate and
bicarbonate. This could be provided with seltzer water if the air pumped in doesn't provide enough. From what I've read, the bacteria will
eventually be killed off when the nitrate levels get too high.
I was thinking of maintaining proper temp, pH, ammonia supply, and air until the nitrate level does just that; kills the bacteria. Then the solution
can be filtered through diatomaceous earth, leaving primarilly a dirty solution of ammonium nitrate and water. This could then be converted to other
nitrates or used as is following purification. In theory, if done correctly, one could have an endless supply of bacteria by making proper cultures.
Any thoughts on this?
[Edited on 3/23/2007 by obsessed_chemist]
Edit by Chemoleo: Title and thread merge.
[Edited on 29-10-2008 by chemoleo]
|
|
|
Levi
Hazard to Others
Posts: 196
Registered: 24-1-2007
Member Is Offline
Mood: No Mood
|
|
I expect it would be 10-20 months before you could harvest the nitrate but it would certainly work. Of course if you had 10-20 tanks you could be
harvesting continually =)
Chemcrime does not entail death. Chemcrime is death.
|
|
|
S.C. Wack
bibliomaster
Posts: 2419
Registered: 7-5-2004
Location: Cornworld, Central USA
Member Is Offline
Mood: Enhanced
|
|
The stated yield in 100+ year old research (aimed at assuring Chile-dependent France of nitrate should the Kaiserliche Marine cause problems) at 24
hours for 1 cubic meter of peat-supported nitrifying bacteria at 30C was 6.55 kg "nitrate" (probably calcium); probably using 7.5 g/L ammonium sulfate
with passes through beds in succession with fresh sulfate added to the flush water, and lime to bind the sulfate. I'm sure that there is research out
there in aerated solution where results (nitrite/nitrate) were measured in hours or days rather than months.
|
|
|
Levi
Hazard to Others
Posts: 196
Registered: 24-1-2007
Member Is Offline
Mood: No Mood
|
|
Hours!? I found a site a while back which discusses the construction of nitre beds (link supplied below) but all harvest times are greater than 1
year. If the aqueous method does indeed work in a matter of hours this would be an economical way to produce nitrates on a massive scale for
industry.
http://docsouth.unc.edu/imls/lecontesalt/leconte.html
Chemcrime does not entail death. Chemcrime is death.
|
|
|
12AX7
Post Harlot
Posts: 4803
Registered: 8-3-2005
Location: oscillating
Member Is Offline
Mood: informative
|
|
Active aeration does better than straw and poo...
Still sounds awfully fast, but I would believe the rate can be pretty good.
Seems to me an ion exchange resin that preferrentially picks up nitrates would be of use here.
Tim
|
|
|
chief
National Hazard
Posts: 630
Registered: 19-7-2007
Member Is Offline
Mood: No Mood
|
|
saltpeter/HNO3 from urea + bacteriae
With nitrates possibly getting banned from the hardware-store-fertilizer shelves, another sort of N-fertilizer is already available, as "substitute":
Urea ! Fine, since this is what the source of saltpeter was for centuries. In the past times it were stinking saltpeter-plantages, because the sources
of the urea were excrements from human/animal-sources.
Today this might be had much cleaner: Just only some reactor, some stirring, the right bacteriae . At least it doesn't consume electicity like the
birkeland-eyde-reactor ...
Although I have no exact Idea about how I would start this, probably It could work like this:
==> since it's a aerobic process: Air must reach the stuff
==> maybe some source of nutrition for the bacteriae, that contains the right minerals (since they may need something else besides the urea)
==>some temperatureabove 20 [Celsius]
Maybe the urea-solution might be rinsed over clay-granulate (for hydro-cultures) ? This would give a high liquid-air-surface ...
As I understand the ancient technique: They "harvested" the saltpeter off like "off the wall": Just scratched the white stuff fromwhere it appeared.
So this can be built into the reactor: Where a lot of evaporation occurs, there always fresh solution is transported to, giving off the H2O and
leaving the salts in place ...
The only question is: Where to get the bacteriae and how to meet their living-conditions best ....
[Edited on 27-10-2008 by chief]
|
|
|
Foss_Jeane
Harmless
Posts: 40
Registered: 14-5-2008
Member Is Offline
Mood: No Mood
|
|
I wouldn't do it that way. Back in the good ol' days, they really didn't have much choice. That manure/urine/bacteria method will stink to high
heaven, making you real popular with the neighbors, and it takes a dog's age. It is also hardly discreet. Purification of the resulting
nitrates is also going to be problematic (you don't want sh!t in your saltpeter, do you?).
Better to use the electrical method: strike an arc, pass in air (fortify with O2 if you can) collect the nitrogen oxides. If you can stand some
nitrite in the mix, you can also pass it straight into a basic solution until neutralized.
Anyway, that's how I would do it, although it's hardly necessary since I can find lots of products on the hardware shelf from which one can always
extract nitrates.
[Edited on 27-10-2008 by Foss_Jeane]
|
|
|
Formatik
National Hazard
Posts: 927
Registered: 25-3-2008
Member Is Offline
Mood: equilibrium
|
|
You can use urea to form potassium cyanate. This is done by heating urea with KOH around 240 deg. for 3-5 hours: KOH + 2 CO(NH2)2 -> (KCNO)x + 3
NH3 + CO2 (see USP 3935300). K2CO3 also works.
Air will oxidize KCNO in the presence of catalysts like Ag-powder, CuO, or NiO to form KNO3. NO also oxidizes KCNO without a catalyst above 210 deg.
Even KClO3 which is diluted with CaO or Na2CO3 due to explosion risk will oxidize KCNO to KNO3 (Ber. 59, [1926] 204).
|
|
|
jimmyboy
Hazard to Others
Posts: 235
Registered: 1-3-2004
Location: Texas
Member Is Offline
Mood: No Mood
|
|
Urea slowly converts to ammonia then to nitrates by bacteria - even with optimum conditions - temperature - PH - moisture this reaction takes a dogs
age and the yields will be horrible - you need pressure and heat and catalyst to drive the oxidation of ammonia - if you really are stuck without any
nitrates where you live then you should invest in metal catalysts to oxidize your own ammonia to nitrites and go from there - it will be slow but way
faster than waiting years for urea to be converted by bacteria
|
|
|
chief
National Hazard
Posts: 630
Registered: 19-7-2007
Member Is Offline
Mood: No Mood
|
|
| Quote: | Originally posted by Formatik
You can use urea to form potassium cyanate. This is done by heating urea with KOH around 240 deg. for 3-5 hours: KOH + 2 CO(NH2)2 -> (KCNO)x + 3
NH3 + CO2 (see USP 3935300). K2CO3 also works.
Air will oxidize KCNO in the presence of catalysts like Ag-powder, CuO, or NiO to form KNO3. NO also oxidizes KCNO without a catalyst above 210 deg.
Even KClO3 which is diluted with CaO or Na2CO3 due to explosion risk will oxidize KCNO to KNO3 (Ber. 59, [1926] 204). |
This seems the way to go then, since everybody has a chlorate-cell anyhow ! How high would have the temp to be ? What details are available ? Urea is
available by the kg-amounts as fertilizer in Germany here !
How poisonous is the cyanate ?
Would it work with the much more available sodium-compounds (Na2CO3, NaClO3) ?
[Edited on 27-10-2008 by chief]
|
|
|
kclo4
National Hazard
Posts: 916
Registered: 11-12-2004
Location:
Member Is Offline
Mood: No Mood
|
|
Check out this if you haven't already: http://docsouth.unc.edu/imls/lecontesalt/leconte.html
Every time I read it It makes me want to do it, but then I realize I have a plentiful amount of Nitrate... relatively. Looks fun though, Especially
if you could dope it with Urea to increase yield a lot.
|
|
|
S.C. Wack
bibliomaster
Posts: 2419
Registered: 7-5-2004
Location: Cornworld, Central USA
Member Is Offline
Mood: Enhanced
|
|
Dirt. I bet if you watered some dirt with a solution of urea in the summer, you'd soon have a lot of organisms busy converting urea to ammonia, and/or
turning ammonia into nitrate. I think it unlikely to take years. I'm aware of some French research a long time ago claiming rapid and exothermic
conversion of fairly large amounts of ammonia into nitrate by nitrifying bacteria under somewhat controlled conditions, (maybe there is lots of study
done to be found if you research the subject) and why not just make your own urease while you're at it.
If the process was slow, then urea would be pretty useless as a fertilizer. It is decomposed so quickly by soil urease that urease inhibitors have
been extensively researched, to retard ammonia loss by volatilzation.
|
|
|
kclo4
National Hazard
Posts: 916
Registered: 11-12-2004
Location:
Member Is Offline
Mood: No Mood
|
|
If I were to do it with what I know at this moment, I would probably buy some manure and mix it with urea, ash, and a large amount of vermiculite or
pertlite, and perhaps some other things to help keep the O2 in it. Then I'd always keep it moist in a a warm spot.
I'd probably want to fill a black garbage can half full so it would allow me to agitate the mixture often to mix in more air, and then also since its
black it can absorb the heat from the sun which would likely speed up the reaction.
Extracting the Nitrates from that might be a bit tricky.
One Idea would be to use a terracotta pot, with the same mixture (manure, urea, vermiculite) and also always keep it warm and moist.
But with this, the terracotta pot could have water slowly added to it, allowing the Nitrate to dissolve, and go to the outside of the pot. As the
water dries the nitrate would form a white crust on the pot. That is, if the ions would travel through the material.
It actually seems like a lot more work then I had realized at first to get significant amounts.
However, when I own my house I'll probably make one of these just for the heck of it. Seems like it would be pretty neat to have.
|
|
|
chemoleo
Biochemicus Energeticus
Posts: 3005
Registered: 23-7-2003
Location: England Germany
Member Is Offline
Mood: crystalline
|
|
Please check also this.
https://sciencemadness.org/talk/viewthread.php?tid=3986
I'll leave this as a separate thread as the approach taken is different.
It would be interesting if this could lead to efficient production of nitrates!
Never Stop to Begin, and Never Begin to Stop...
Tolerance is good. But not with the intolerant! (Wilhelm Busch)
|
|
|
The_Davster
A pnictogen
Posts: 2861
Registered: 18-11-2003
Member Is Offline
Mood: .
|
|
http://www.geocities.com/CapeCanaveral/Lab/1121/KNOstory.htm...
Why not use something like this, with added urea...should be able to get the nitrifing bacteria out of the ground and simply add urea.
|
|
|
not_important
International Hazard
Posts: 3873
Registered: 21-7-2006
Member Is Offline
Mood: No Mood
|
|
OK, Nitrosomonas oxidise ammonia to nitrite in several steps, Nitrobacter take nitrite to nitrate.
These bacteria use CO2 as their carbon source, and also as a source of oxygen for oxidising the nitrogen compounds although they still need molecular
oxygen.
Having reduced forms of carbon around, as from mixing manure into your culture, feeds the denitrifying bacteria which convert nitrate to N2 and reduce
your yields. I would say that mixing manure or soil into your system is not the best idea.
The buggers you want like a temperature range of 25-30°, the optimum pH range for Nitrosomonas is between 7,8-8,0 while for Nitrobacter it is between
7,3-7,5. They don't like light, take that into consideration. They will need a trace amount of phosphate, ordinary tap water contains enough of the
other needed trace elements.
You can buy mixed cultures of nitrifying bacteria. Ones like http://www.fritzpet.com/fritz-zyme-7/ include species than can directly utilise urea, instead of letting some other bacteria hydrolyse it.
These are slow growing bacteria, often taking the better part of a day to double in population. So you will have a very slow startup, and you want to
leave solid culture support behind when harvesting nitrate, so as to have a good culture to continue with.
|
|
|
Formatik
National Hazard
Posts: 927
Registered: 25-3-2008
Member Is Offline
Mood: equilibrium
|
|
| Quote: | Originally posted by chief This seems the way to go then, since everybody has a chlorate-cell anyhow ! How high would have the temp to be ?
What details are available ? Urea is available by the kg-amounts as fertilizer in Germany here !
How poisonous is the cyanate ?
Would it work with the much more available sodium-compounds (Na2CO3, NaClO3) ? |
That reference will likely have more details. I've only looked into the potassium salts. Cyanate is known to be about 1000 times less poisonous than
cyanide.
I would try the less hazardous oxidation routes first. But if you are starting from KClO3, then heating KClO3 to 220 deg. it will react exothermically
with NH3: 3 KClO3 + 2 NH3 = 2 KNO3 + KCl + Cl2 + 3 H2O. By a good spread of the KClO3 and with careful heat regulation, a yield of 60% can be
obtained. This process and reaction is described in Ber. 57 [1924] 818. The NH3 likely has to be dry.
|
|
|
chief
National Hazard
Posts: 630
Registered: 19-7-2007
Member Is Offline
Mood: No Mood
|
|
| Quote: | Originally posted by Formatik
The NH3 likely has to be dry. |
By NH3 you mean urea ?
[Edited on 28-10-2008 by chief]
|
|
|
12AX7
Post Harlot
Posts: 4803
Registered: 8-3-2005
Location: oscillating
Member Is Offline
Mood: informative
|
|
KClO3 burns tepidly with (NH2)2CO. I don't think I've ever ignited a properly stoichiometric mixture, but it sure isn't going to be flash powder, no
matter what ratio it's in. It may be a viable route to nitrates, since chucking stuff into a bucket doesn't work so hot.
Tim
|
|
|
chief
National Hazard
Posts: 630
Registered: 19-7-2007
Member Is Offline
Mood: No Mood
|
|
If this holds:
3 KClO3 + 2 NH3 = 2 KNO3 + KCl + Cl2 + 3 H2O
(@220 [Cels]), then how to get the NH3 from the urea ? (I never was into organics such "uninteresting" as urea)
Maybe I just could heat the NaClO3 in the furnace to 200 [Cels] and then stream NH3 throug it, watching the temp ?
If NH3 is oxidized by chlorate, could there be a direct electrolytic route (under avoidance of the explosive "Dulong Oil" NCl3), like eg.. giving NH3
to a chlorate cell ?
|
|
|
kclo4
National Hazard
Posts: 916
Registered: 11-12-2004
Location:
Member Is Offline
Mood: No Mood
|
|
It might work, but why not just oxidize the NH3 with air to produce HNO3?
That reaction isn't all that hard especially if you can improvise a nice catalyst.
I know a flask full of NH3 and Air plus a hot copper wire can produce White smoke, which if i remember correctly is Ammonium Nitrxtes.
Urea is actually pretty interesting, and you can produce Ammonia by adding a base, or by heating it. A base will produce water, Ammonia and a Cyanate.
The cyanate could later be oxidized to a nitrate later.
Would a hypochlorite do anything to a cyanate? Seems like it might possibly make a nitrate copper oxide and a cyanate can.
|
|
|
Formatik
National Hazard
Posts: 927
Registered: 25-3-2008
Member Is Offline
Mood: equilibrium
|
|
I don't know how much I trust urea here. Urea decomposes to varying organic compounds when heated all while releasing NH3 and H2O. I don't trust it
because NH4ClO3 formation has not been ruled out. NH4ClO3 can deflagrate or burn with a red flame when heated, but it can also detonate, it is known
for spontaneous explosions, even when wet with water it is an explosion risk. The only thing Gmelin mentions about this is that urea heated with
NaClO3 causes ignition at the melting point of NaClO3, which doesn't say much.
|
|
|
S.C. Wack
bibliomaster
Posts: 2419
Registered: 7-5-2004
Location: Cornworld, Central USA
Member Is Offline
Mood: Enhanced
|
|
Well there seems to be some interest, though not necessarily in this thread, and there seems to be some doubt. So if someone wants to try to duplicate
the work that I've mentioned, these are the 1905-1906 Compt. rend. (Gallica) articles that I was talking about above.
There is also a 136 page article by the same authors in Ann. chim. phys. (8) 11, 439 (1907)
[Edited on 28-10-2008 by S.C. Wack]
Attachment: nitrification.pdf (998kB)
This file has been downloaded 2112 times
|
|
|
kclo4
National Hazard
Posts: 916
Registered: 11-12-2004
Location:
Member Is Offline
Mood: No Mood
|
|
This is just like the other threads. Perhaps it wouldn't be a bad idea to merge this one with the other active one? I don't know be nice just to have
all of the references, ideas and what not all together I guess.
I wish I could read whatever the hell language that is! haha ok, well I can understand it a little bit, but not enough. 
We seem to be spitting out every idea about making nitrates from Bacteria and what not, lets not forget about using peas, or beans or whatever other
sort of thing that has nitrogen fixing bacteria on its roots. I think you could almost get Nitrates out of thin air this way! Bubbling water into a
"hydroponic" like set up with peas growing in it + nutrients for the bacteria as well as the plant. The plants bacteria react with atmospheric
nitrogen to produce ammonia. The ammonia could then be oxidized to nitrate with the other bacteria. Perhaps you could get the bacteria from the pea
roots to get established with out the need of the pea. This would be nice since I believe plants need a relatively low ppm of nutrients to live
hydroponically.
Perhaps putting a porous material on the side of the "tank" where the water meets would allow nitrate crust to form. All you'd need to do then is
scrape of the milligrams every week and purify it 
Edit: http://www.cahe.nmsu.edu/pubs/_a/a-129.pdf after reading that, my Pea idea doesn't seem all that great to me.
Does anyone know what percent of Nitrate kills them at? I think that is really an important factor when it comes to determining if it would be worth
doing a liquid culture.
I had read that it can get as high as 1000ppm in aquariums, But I bet it could go a ton higher.
Assuming they are only counting NO3- for the ppm and not the K+, you can get about 1.6 grams of KNO3 from every liter of water right?
[Edited on 28-10-2008 by kclo4]
|
|
|
not_important
International Hazard
Posts: 3873
Registered: 21-7-2006
Member Is Offline
Mood: No Mood
|
|
The levels of combined nitrogen from nitrogen fixing bacteria is low, on the order of 75 to 300 kilograms of N per hectare per year for symbiotic
bacteria growing in legume roots, about 1/100 of those values in the case of free-living bacteria. The low fixing rates is why development of
synthetic fixed nitrogen was so important.
For legumes almost all the fixed nitrogen is trapped by the plant for conversion into amino acids, not released into the soil. This is also true for
many of the non-symbiotic free living bacteria, the nitrogen they fix is stored as proteins and other organic compounds within the bacteria and become
available to plants after the bacteria die.
The fixing process is poisoned by oxygen, in legumes the bacteria live within the plants roots, many of the free living bacteria need anaerobic
conditions although some others do tolerate oxygen. The nitrification process requires oxygen.
The limiting concentrations of nitrite and nitrate for the bacteria are quit low, I believe around 10 to 20 mg/l There's a bit of a discussion in
this PDF https://dspace.lib.cranfield.ac.uk/bitstream/1826/1021/3/Din...
|
|
|
| Pages:
1
2 |
![[*]](images/xpblue/default_icon.gif){kind=icon}
