Bisulfide (or bisulphide in British English) is an inorganicanion with the chemical formula HS− (also written as SH−). It contributes no color to bisulfide salts, and its salts may have a distinctive putrid smell. It is a strong base. Bisulfide solutions are corrosive and attack the skin.
It is an important chemical reagent and an industrial chemical, mainly used in paper pulp industry (Kraft process), textiles, synthetic flavors, coloring brasses, and iron control.
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.
The UV–visible spectrum of septic sewage from three different sites. The absorption of bisulfide is observed around 230 nm in each case.
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]
Bisulfide should not be confused with the disulfide dianion, S2−2, or −S–S−.
Because of its affinity to accept a proton (H+), bisulfide has a basic character. In aqueous solution, it has a corresponding pKa value of 6.9. Its conjugate acid is hydrogen sulfide (H2S). However, bisulfide's basicity stems from its behavior as an Arrhenius base. A solution containing spectator-only counter ions, has a basic pH according to the following acid-base reaction:
Upon treatment with an acid, bisulfide converts to hydrogen sulfide. With strong acids, it can be doubly protonated to give H 3S+ . Oxidation of bisulfide gives sulfate. When strongly heated, bisulfide salts decompose to produce sulfide salts and hydrogen sulfide.
2 HS− → H2S + S2−
3
Biochemistry
At physiological pH, hydrogen sulfide is usually fully ionized to bisulfide (HS−). 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.[5]
^Goldhaber, M.B.; Kaplan, I.R. (1975), "Apparent dissociation constants of hydrogen sulfide in chloride solutions", Marine Chemistry, 3 (1): 83–104, doi:10.1016/0304-4203(75)90016-X
^Johnson, K.S.; Coletti, L.S. (2001), "In situ ultraviolet spectrophotometry for high resolution and long-term monitoring of nitrate, bromide and bisulfide in the ocean.", Deep-Sea Research, 49 (7): 1291–1305, Bibcode:2002DSRI...49.1291J, doi:10.1016/s0967-0637(02)00020-1
^Guenther, E.A.; Johnson, K.S.; Coale, K.H. (2001), "Direct ultraviolet spectrophotometric determination of total sulfide and iodide in natural waters", Analytical Chemistry, 73 (14): 3481–3487, doi:10.1021/ac0013812, PMID11476251
^Sutherland-Stacey, L.; Corrie, S.; Neethling, A.; Johnson, I.; Gutierrez, O.; Dexter, R.; Yuan, Z.; Keller, J.; Hamilton, G. (2007), "Continuous measurement of dissolved sulfide in sewer systems", Water Science and Technology
^J. W. Pavlik, B. C. Noll, A. G. Oliver, C. E. Schulz, W. R. Scheidt, “Hydrosulfide (HS−) Coordination in Iron Porphyrinates”, Inorganic Chemistry, 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, 49: 169–543, doi:10.1002/9780470166512.ch3, ISBN978-0-470-16651-2
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