vano
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Very pure sulfur without recrystallization
Hi. I have developed a good method to get pure sulfur. There may be this method but I have not read it anywhere. This method is very simple, cheap and
not need expensive and rare chemicals.
Reagents: sulfur, NaOH and citric acid or oxalic acid or other acids.
I used technical sulfur. I dissolved it in sodium hydroxide solution and made polysulfide. Next i filtered it and add citric acid solution slowly.
Hydrogen sulfide and maybe other polysulfide produced(2 and 3?), but many sulfur stayed in solution. When polysulfide colour disappeared then i wash
sulfur 5 times and filter with liter of water again. It has white colour, it think it is very pure and particles are very small, because many of them
penetrated the filter paper.
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Bedlasky
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Toluene is quite cheap and common chemical.
Quote: Originally posted by vano  |
Hydrogen sulfide and maybe other polysulfide produced(2 and 3?), but many sulfur stayed in solution. |
Polysulfides aren't form - they are unstable at room temperature, if you want to produce polysulfane oil, you must work below 0°C. Btw. not just
hydrogen sulfide is formed, but also sulfur dioxide. Sulfur disproportionates in NaOH solution in to polysulfide and thiosulfate:
(x+2)S + 6NaOH --> 2Na2Sx + Na2S2O3 + H2O
Polysulfides decompose in acidic solution in to hydrogen sulfide and sulfur, but thiosulfate decompose in to variety of products like SO2, S, H2S,
Na2SO4, maybe also in to polythionates. You may purified sulfur by this way, but you some of it lost in the form of various sulfur compounds. I think,
that recrystallization from toluene is cheaper, less smelly and losses are minimal. You can recover your toluene and use it again for sulfur
purification. But NaOH is definitely lost after this reaction.
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unionised
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You seem to have missed the bit where the H2S produced by decomposition of polysulphide in acid reacts with the SO2 produced by the reaction of acid
with sulphites and thiosulphates .
H2S + SO2 --> S + H2O
(I will leave you to the joy of balancing that equation)
In principle, the sulphur is all reprecipitated when you acidify the stuff.
There will be some loss due to oxidation by air.
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Bedlasky
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2H2S + SO2 = 3S + 2H2O
But Vano's reaction produce (ideally) 1:1 H2S:SO2 mixture. In the mixture is slightly more H2S than SO2, because of other ways of thiosulfate
decomposition. But still you have excess of SO2 + other side products.
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Sulaiman
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have you tried melting
some (m.p. 115.2 oC [106 t0 119]) ?
(about the same m.p. as iodine, 113.5)
[Edited on 24-2-2021 by Sulaiman]
CAUTION : Hobby Chemist, not Professional or even Amateur
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vano
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| Quote: Originally posted by Bedlasky |
Toluene is quite cheap and common chemical.
Polysulfides aren't form - they are unstable at room temperature, if you want to produce polysulfane oil, you must work below 0°C.
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I know, but this is a other method, so I mentioned it in the title. Also everyone don't have toluene and xylene.
I do not think so. Ammonium polysulfides ( where n = 2… 9…) are used for steel bluing. Calcium and barium polysulfides are used in pest control
in agriculture. I do not think farmers keep it in the refrigerator.
[Edited on 24-2-2021 by vano]
[Edited on 24-2-2021 by vano]
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vano
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Yes. These balls shine like pearls.
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Bedlasky
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| Quote: Originally posted by vano | | Quote: Originally posted by Bedlasky |
Toluene is quite cheap and common chemical.
Polysulfides aren't form - they are unstable at room temperature, if you want to produce polysulfane oil, you must work below 0°C.
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I know, but this is a other method, so I mentioned it in the title. Also everyone don't have toluene and xylene.
I do not think so. Ammonium polysulfides ( where n = 2… 9…) are used for steel bluing. Calcium and barium polysulfides are used in pest control
in agriculture. I do not think farmers keep it in the refrigerator.
[Edited on 24-2-2021 by vano]
[Edited on 24-2-2021 by vano] |
Sorry, I meant polysulfanes, not polysulfides. Polysulfides are formed, when you dissolve sulfur in NaOH, of course. But after acidification just
sulfane is released, polysulfanes are unstable at room temperature.
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vano
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| Quote: Originally posted by Bedlasky |
Sorry, I meant polysulfanes, not polysulfides. Polysulfides are formed, when you dissolve sulfur in NaOH, of course. But after acidification just
sulfane is released, polysulfanes are unstable at room temperature. |
Ok, no problem. Yes i agree with you that polysulfanes are unstable at room temperature. But i think small amounts of low molecular weight can be
produced, very very small amount.
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RogueRose
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Toluene is getting MUCH more difficult to find as the 4-5 places I used to see it stocked, only 1 still sells it and the other products like lacquer
thinner or paint thinner/remover seems to have moved away from using this for some reason. I'd gladly use a safer method other then heating toluene!
I've tried dissolving sulfur in toluene and found it does a very poor job at regular room temp, I think I got maybe 20-25 grams per liter. It does do
a fairly good job when heated (still not very high - maybe 120-150g/liter), but I think it needs to get very close to it's BP to dissolve good amounts
and that gets a little dangerous. I had this ignite one time and I'll tell you I've never seen so much soot produced in ~10 seconds as it left a
THICK cloud floating strands of carbon and a huge soot mark above where it was being heated (5-6ft diameter). This was such a mess and I'm still not
100% sure how it started as I didn't have the power up very high on the heating element - but I guess it was hot enough to reach flash point..
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Bedlasky
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| Quote: Originally posted by RogueRose |
Toluene is getting MUCH more difficult to find as the 4-5 places I used to see it stocked, only 1 still sells it and the other products like lacquer
thinner or paint thinner/remover seems to have moved away from using this for some reason. I'd gladly use a safer method other then heating toluene!
I've tried dissolving sulfur in toluene and found it does a very poor job at regular room temp, I think I got maybe 20-25 grams per liter. It does do
a fairly good job when heated (still not very high - maybe 120-150g/liter), but I think it needs to get very close to it's BP to dissolve good amounts
and that gets a little dangerous. I had this ignite one time and I'll tell you I've never seen so much soot produced in ~10 seconds as it left a
THICK cloud floating strands of carbon and a huge soot mark above where it was being heated (5-6ft diameter). This was such a mess and I'm still not
100% sure how it started as I didn't have the power up very high on the heating element - but I guess it was hot enough to reach flash point..
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I am not saying that Vano's method is bad, it's interesting alternative which I never thought about. I am talking from my experience, because in my
country isn't problem to buy some technical grade toluene and it's cheap. But I can imagine, that in other countries situation may be different. I
agree that big advantage of Vano's method is, that you don't need to heat flammable solvent.
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vano
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In some places toluene is not sold at all, but these reagents are available in all countries, and I did not spend anything on these reagents, I
received 1 kg of sulfur and 500 grams of citric acid as a gift, because it is already very cheap. I have sodium hydroxide granules, and in this
reaction I used old hydroxide, which was looks like rocks. Plus the problem is the poisonous gases, and the smell of hydrogen sulfide is very strong,
but for me it is not a problem, although I know it is bog problem in many countries.
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Vomaturge
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| Quote: Originally posted by RogueRose |
Toluene is getting MUCH more difficult to find as the 4-5 places I used to see it stocked, only 1 still sells it and the other products like lacquer
thinner or paint thinner/remover seems to have moved away from using this for some reason. I'd gladly use a safer method other then heating toluene!
I've tried dissolving sulfur in toluene and found it does a very poor job at regular room temp, I think I got maybe 20-25 grams per liter. It does do
a fairly good job when heated (still not very high - maybe 120-150g/liter), but I think it needs to get very close to it's BP to dissolve good amounts
and that gets a little dangerous. I had this ignite one time and I'll tell you I've never seen so much soot produced in ~10 seconds as it left a
THICK cloud floating strands of carbon and a huge soot mark above where it was being heated (5-6ft diameter). This was such a mess and I'm still not
100% sure how it started as I didn't have the power up very high on the heating element - but I guess it was hot enough to reach flash point..
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I think the flash point is 6C. It probably got just hot enough to flood vapors over the side of the vessel, and then they were ignited by static or
electrical contacts in your heat source,
I now have a YouTube channel. So far just electronics and basic High Voltage experimentation, but I'll hopefully have some chemistry videos soon. |
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ChemTalk
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Vomaturge - we just subscribed to your youtube channel. Looking forward to the chemistry videos!
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unionised
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The flash point of toluene is about 4 oC.
Once you are above the flash point there's enough vapour to produce a flammable cloud.
A spark from the thermostat or the stirrer is a plausible guess as the ignition source.
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pneumatician
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wow, you now, after some centuries, know what is Lac Sulphuris! :-) in vulgo english, milk of sulphur. De res.
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macckone
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It would seem other acids like vinegar (obviously purified to remove other organics) would work.
Citric acid is commonly available as food grade for use in baking, so using different acids is not an issue.
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