Silverado79523CYBER - 15-1-2009 at 12:08
I know that one way to produce hydrogen sulfide is to pour concentrated/not concentrated hydrochloric acid over iron sulfide (produced by heating both
sulfur and iron together).
Just curious: Hydrogen sulfide in water (obviously a solution), hydrogen sulfide in ammonia, hydrogen sulfide in iodine, bromine water, or anything
else?
Might be fun to discuss if you are interested.
Silverado79523CYBER - 15-1-2009 at 12:09
Oh, I meant iodine solution.
Jor - 15-1-2009 at 12:34
First off all, if you are going to experiment with it, be warned that it an exceptionally dangerous gas. Extremely toxic, and you lose your sense of
smell at toxic levels. A single breath at 0,1% will get you in coma. Compare toxicity to hydrogen cyanide.
Hydrogen sulphide does not dissolve to well in water, with ammonia it reacts, forming an NH4HS-solution, wich smells badly like rotten eggs, and is
used as stink bombs.
Because this is your first post, and you don't sound too serious, I rather keep the answer to the H2S in iodine solution for myself.
woelen - 15-1-2009 at 12:37
H2S + water --> very faint acid, solution turns turbid quickly, due to oxidation of H2S by oxygen from air
H2S + ammonia --> Formation of ammonium sulfide and/or ammonium hydrogen sulfide, depending on relative amounts of H2S and NH3. Such solutions tend
to turn yellow, due to aerial oxidation, in which sulfide is oxidized to sulphur, which in turn dissolves again, giving polysulfide solutions
H2S in iodine/bromine solution --> Immediate oxidation of sulfide to sulphur, the halogen is reduced to iodide/bromide
Hydrogen sulfide gives precipitates with many metals, e.g. with copper(II) ions and mercury(II) ions a black precipitate is formed. With silver(I)
ions, dark brown Ag2S is formed. Even free H2S forms such precipitates, due to the extremely low solubility of the metal sulfides.
Silverado79523CYBER - 15-1-2009 at 12:41
Who said anythin about experimenting? I just wanted to get aquainted with this highly toxic gas in study, not in actual experimentation.
Silverado79523CYBER - 15-1-2009 at 12:46
any other ideas for hydrogen sulfide?
panziandi - 15-1-2009 at 12:58
Hydrogen Sulphide can be liquified as can Sulphur Dioxide and Ammonia and is used sometimes by crazy people as some funky solvent for electrochemical
and inorganic non-aqueous reactions...
bquirky - 15-1-2009 at 20:11
The other day I was making Iron Chloride by dissolving a sizable amount of electrolytic iron granules in HCL and i noticed a substantial odor of
Hydrogen Sulfide Now while this on its own should not be possible but I think this is what happened.
The iron granules had been prepaird by electrolysis in a bath of Sulfuric Acid and Iron Sulfate and then stored for quite some time 'damp' without
being thouroly washed (sloppy yes but i wasn't worried about purity at the time)
Id guess that somehow some of the stray FeSO4 Lost its oxygen (perhaps absorbed by the excess iron to form FeO) to form a small amount of FeS leading
to the smell of Hydrogen Sulfide when i desolved the mess in hydrocloric acid.
Now while this was entirely accidental I wonder if there might be a more controlled way to preform the same synthesis.
woelen - 15-1-2009 at 23:42
bquirky, your iron was not contaminated with FeS, it was the FeSO4 which caused the smell. In the process of dissolving the iron, the iron, or nascent
hydrogen formed at the surface of the iron, is capable of reducing sulfate ion. Part of it is reduced to SO2, another part is reduced to H2S.
This effect is noticeable best when very pure iron (or even ebtter: zinc) is added to very pure dilute H2SO4. Most of the gas is hydrogen, but there
is a clear smell of H2S. Given the purity of the starting reactants, the only explanation is reduction of sulfate to H2S.
bquirky - 16-1-2009 at 01:10
Ahhhh,
Now that is interesting
thanks 
Sauron - 16-1-2009 at 02:11
slverado, this thread is titles THE ART AND SCIENCE OF AMATUER EXPERIMENTALISM
You state you are not into experimenting.
In thta case read a book and stop wasting our time. You appear to have nothing at all to contribute.