Joeychemist
Hazard to Others
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Goodbye to S2− in aqueous solution
Abstract
New Raman spectra of Na2S dissolved in hyper-concentrated NaOH(aq) and CsOH(aq) cast serious doubt on the widely-assumed existence of S2−(aq). To
avoid conceptual and practical problems with sulfide equilibria in numerous applications, S2−(aq) should be expunged from the chemical literature.
Thermodynamic databases involving sulfide minerals also need careful revision.
Certainly the S2- ion exists in various forms and conditions but could it be that we are only now just learning that so many reaction mechanisms -as
we understood them up 'till now- are erroneous? Would be nice to read the article in it's entirety... Hint 
Chemical Communication issue 16
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aga
Forum Drunkard
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Meh.
S2- in aqueous could easily be an effect of S0, S-1, S-1.5, S-2, S-2.5, S-3 etc.
I.e. S transitioning between 0 and wherever.
Nothing is in a steady state, Ever, so all same-same.
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DraconicAcid
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Every first-year text I've seen lately (apart from the really old ones) states clearly that S(2-) is a strong base and doesn't exist in aqueous
solutions, so this is hardly news.
Please remember: "Filtrate" is not a verb.
Write up your lab reports the way your instructor wants them, not the way your ex-instructor wants them.
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mayko
International Hazard
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Attachment: Goodbye to S2 in aqueous solution.pdf (1.6MB)
This file has been downloaded 469 times
al-khemie is not a terrorist organization
"Chemicals, chemicals... I need chemicals!" - George Hayduke
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byko3y
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I needed like 5 minutes reading to understand what they wanted to declare a truth. The true ions can be described with a single formula from the
paper:
HS- + OH- + Na+ <-> NaS- + H2O
So, basically, sulfide never loses its last cation in the presense of water.
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