camurgo
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Reaction between Lime Sulfur and HCL
The internet tells me that 'Lime Sulfur' is composed of polysulfides of general formula CaSx, where x varies from 2 to 7.
I know one of the products of mixing 'Lime Sulfur' and HCL is hydrogen sulfide, but what is (are) the other product(s) ? Does anyone know?
Possibly each polysulfide (CaS2, CaS3, CaS5...) will react in a different way?
I'm interested in understanding how this reactions actually happens, and knowing all the products would go a long way in helping with that.
Does anybody know? Thanks.
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teodor
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I think you will get H2S mixed with different sulfanes (hydrogen polysulfides), which mysterious presence you can always see because they deposit
sulfur on precisious glass surfaces (I think this fact makes their fractional separation almost impossible). Byt the way, It is very hard to remove
sulfur from glass with my usual set of cleaning solutions.
So, ask google for "sulfanes" or "hydrogen polysulfide". Like this: https://www.nrcresearchpress.com/doi/pdf/10.1139/v68-384
Also, I think the high ability of sulfur to polymerize in chains of different length makes the chemistry of sulfur a bit complex and insular.
[Edited on 9-9-2019 by teodor]
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mackolol
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Quote: Originally posted by teodor  |
Byt the way, It is very hard to remove sulfur from glass with my usual set of cleaning solutions.
[Edited on 9-9-2019 by teodor] |
Have you tried hot toluene or xylenes?
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camurgo
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Thank you very much @teodor.
With further research based on the additional info you gave me I think I'll be able to eventually completely answer my own question.
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teodor
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I didn't try it yet but I know the property of toluene to dissolve sulfur. Just didn't use it as a cleaning solution yet because already have a lot of
other bottles "for washing" and always tried to limit their number. But all they failed, so the next try will be toluene.
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woelen
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I use hot concentrated NaOH-solutions to clean sulfur from glassware. It dissolves fairly easily in that. Concentrated NaOH also attacks glass, but it
only does so very slowly and smooth clear glass (from beakers, erlenmeyers, test tubes, flasks) hardly is attacked.
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Polysulfides give H2S and H2Sn (with N > 1). In practice, the hydrogen polysulfide is so unstable, that it decomposes quickly to H2S and elemental
sulfur. The products, however, are not easily distinguishable. It is a dirty and very smelly mess of sulfur and hydrogen sulfides.
[Edited on 10-9-19 by woelen]
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teodor
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| Quote: Originally posted by woelen | I use hot concentrated NaOH-solutions to clean sulfur from glassware. It dissolves fairly easily in that. Concentrated NaOH also attacks glass, but it
only does so very slowly and smooth clear glass (from beakers, erlenmeyers, test tubes, flasks) hardly is attacked.
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Thank you for the suggestion. I still have sulfur inside my Dimroth cooler and don't want to put hot NaOH inside because it always eats a bit of
surface of glass joints. Also I try to use as little stages in cleaning as possible that means a less bathes etc. For most purposes HCl and/or chromic
acid works like an universal solution. Also I found Na3PO4 bath works pretty well so I often use it instead of NaOH. And actually I have a second
Dimroth (bought 2 by an error) so now I keep this specially for "durty" experiments (like with sulfur). But I will try to clean it with NaOH or Na3PO4
some day, thank you for the idea (indeed, NaOH dissolves sulfur).
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vmelkon
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| Quote: Originally posted by teodor | | Quote: Originally posted by woelen | I use hot concentrated NaOH-solutions to clean sulfur from glassware. It dissolves fairly easily in that. Concentrated NaOH also attacks glass, but it
only does so very slowly and smooth clear glass (from beakers, erlenmeyers, test tubes, flasks) hardly is attacked.
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Thank you for the suggestion. I still have sulfur inside my Dimroth cooler and don't want to put hot NaOH inside because it always eats a bit of
surface of glass joints. Also I try to use as little stages in cleaning as possible that means a less bathes etc. For most purposes HCl and/or chromic
acid works like an universal solution. Also I found Na3PO4 bath works pretty well so I often use it instead of NaOH. And actually I have a second
Dimroth (bought 2 by an error) so now I keep this specially for "durty" experiments (like with sulfur). But I will try to clean it with NaOH or Na3PO4
some day, thank you for the idea (indeed, NaOH dissolves sulfur). |
Couldn't you just burn away the sulfur?
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