Hispanopedia WikiBisulfide (or bisulphide in British English) is an inorganicanion with the chemical formula HS− (also written as SH−). It contributes no color to bisulfide salts. It often coexists with hydrogen sulfide, which has a distinctive putrid smell. It is a strong base.
It is an important chemical reagent and an industrial chemical, mainly used in paper pulp industry (Kraft process).
Properties
A variety of salts are known, including sodium hydrosulfide and potassium hydrosulfide. Ammonium hydrosulfide, a component of "stink bombs" has not been isolated as a pure solid. Some compounds described as salts of the sulfide dianion contain primarily hydrosulfide. For example, the hydrated form of sodium sulfide, nominally with the formula Na2S · 9 H2O, is better described as NaSH · NaOH · 8 H2O.
Aqueous bisulfide absorbs light at around 230 nm in the UV–visible spectrum.[1] Using this approach, bisulfide has been detected in the ocean[2][3] and in sewage.[4]
Basicity
At physiological pH, hydrogen sulfide is almost fully ionized to bisulfide (HS−).[5] Therefore, in biochemical settings, "hydrogen sulfide" is often used to mean, bisulfide. Hydrosulfide has been identified as the third gasotransmitter along with nitric oxide and carbon monoxide.[6]
Reactions
Upon treatment with an acid, bisulfide converts to hydrogen sulfide. Oxidation of bisulfide gives polysulfides and eventually sulfate. When anstrongly heated, alkali bisulfide salts decompose to produce sulfide salts and hydrogen sulfide. 2NaHS → H2S + Na2S
When treated with metal salts, bisulfide gives the corresponding sulfide:
- 2NaHS + M2+→ MS + 2 Na+ (M = Ni(II), Pb(II), Cd(II), etc)
Esta conversión es la base de algunos esquemas en el análisis inorgánico cualitativo .
En condiciones específicas, el SH − forma algunos complejos que contienen ligandos SH. Algunos ejemplos son [Au(SH) 2 ] − y (C 5 H 5 ) 2 Ti(SH) 2 , derivados del cloruro de oro(I) y del dicloruro de titanoceno , respectivamente. [ 7 ]
Seguridad
Las sales de bisulfuro liberan sulfuro de hidrógeno tóxico al acidificarse.
Véase también
Referencias
- ↑ Goldhaber, MB; Kaplan, IR (1975), "Constantes de disociación aparentes del sulfuro de hidrógeno en soluciones de cloruro", Marine Chemistry , 3 (1): 83–104 , Bibcode : 1975MarCh...3...83G , doi : 10.1016/0304-4203(75)90016-X
- ↑ Johnson, KS; Coletti, LS (2001), "Espectrofotometría ultravioleta in situ para el monitoreo a largo plazo y de alta resolución de nitrato, bromuro y bisulfuro en el océano.", Deep-Sea Research , 49 (7): 1291– 1305, Bibcode : 2002DSRI...49.1291J , doi : 10.1016/s0967-0637(02)00020-1
- ↑ Guenther, EA; Johnson, KS; Coale, KH (2001), "Determinación espectrofotométrica ultravioleta directa de sulfuro y yoduro totales en aguas naturales", Analytical Chemistry , 73 (14): 3481– 3487, doi : 10.1021/ac0013812 , PMID 11476251
- ↑ Sutherland-Stacey, L.; Corrie, S.; Neethling, A.; Johnson, I.; Gutierrez, O.; Dexter, R.; Yuan, Z.; Keller, J.; Hamilton, G. (2007), "Medición continua de sulfuro disuelto en sistemas de alcantarillado", Water Science and Technology
- 1 2 Pluth, Michael D.; Tonzetich, Zachary J. (2020). "Complejos de hidrosulfuro de los elementos de transición: Diversos roles en la química bioinorgánica, de clústeres, de coordinación y organometálica". Chemical Society Reviews . 49 (12): 4070– 4134. doi : 10.1039/C9CS00570F . PMID 32420562 .
- ↑ JW Pavlik, BC Noll, AG Oliver, CE Schulz, WR Scheidt, “Coordinación de hidrosulfuro (HS − ) en porfirinatos de hierro”, Química inorgánica, 2010, vol. 49(3), 1017-1026.
- ↑Peruzzini, M.; de los Rios, I. & Romerosa, A. (2001), "Coordination Chemistry of Transition Metals with Hydrogen Chalcogenide and Hydrogen Chalcogenido Ligands", Progress in Inorganic Chemistry, vol. 49, pp. 169–543, doi:10.1002/9780470166512.ch3, ISBN 978-0-470-16651-2
- Anions
- Sulfur ions
- Acid–base chemistry