Sulfoxylic acid
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| Other names
dihydroxidosulfur sulfanediol
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| Identifiers | |
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3D model (JSmol)
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| ChEBI | |
| ChemSpider | |
| 1452 | |
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PubChem CID
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| Properties | |
| S(OH)2 | |
| Molar mass | 66.07 g·mol−1 |
| Related compounds | |
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Related isoelectronic
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hydrogen trioxide trisulfane |
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Related compounds
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hydroxysulfonyl radical HOSO2 sulfinic acid sulfenic acid HSOH dihydroxydisulfane HOSSOH |
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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| Infobox references | |
Sulfoxylic acid (H2SO2) (also known as hyposulfurous acid or sulfur dihydroxide)) is an unstable oxoacid of sulfur in an intermediate oxidation state between hydrogen sulfide and dithionous acid. It consists of two hydroxy groups attached to a sulfur atom. Sulfoxylic acid contains sulfur in an oxidation state of +2. Sulfur monoxide (SO) can be considered as a theoretical anhydride for sulfoxylic acid, but it is not actually known to react with water.
The complementary base is the sulfoxylate anion SO22− which is much more stable. In between these states is the SO2H− ion, also somewhat stable. Sulfoxylate ions can be made by decomposing thiourea dioxide in an alkaline solution. To do this, thiourea dioxide first forms a tautomer, aminoiminomethanesulfinic acid (H2NC(=NH)SO2H, abbreviated AIMS) which breaks apart. Sulfoxylate reacts with formaldehyde to yield a hydroxymethane sulfinate called rongalite: SO2H− + H2CO → HOCH2SO2− which is an importance chemical for dyeing.
Sulfoxylic acid has been detected in the gas phase. It is likely to be formed as an intermediate when hydrogen sulfide is oxidised by living organisms, or in the atmosphere, or anywhere else in the natural environment. It may also exist in circumstellar disks. When H2S is oxidised it starts from oxidation state -2, and should then pass through intermediate values of 0 and +2 before getting to well known sulfite at +4 and sulfate at +6. When sulfide in alkaline conditions is oxidised by air in the presence of nickel ions, sulfoxylate concentration first increases to around 5% and then decreases over several days. Polysulfide concentration also grows and then shrinks on a slower timescale reaching about 25% of the sulfide. The sulfur ends up forming thiosulfate.
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