Sulfoxylic acid
Chemical compound / From Wikipedia, the free encyclopedia
Dear Wikiwand AI, let's keep it short by simply answering these key questions:
Can you list the top facts and stats about Sulfoxylic acid?
Summarize this article for a 10 year old
Sulfoxylic acid (H2SO2) (also known as hyposulfurous acid or sulfur dihydroxide[1]) 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.[2] 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.[3]
Names | |
---|---|
IUPAC name
Sulfanediol | |
Other names
hyposulfurous acid sulfur dihydroxide dihydroxidosulfur sulfanediol 2-Thiatrioxidane | |
Identifiers | |
3D model (JSmol) |
|
ChEBI | |
ChemSpider |
|
1452 | |
PubChem CID |
|
| |
| |
Properties | |
S(OH)2 | |
Molar mass | 66.07 g·mol−1 |
Conjugate base | Bisulfoxylate (chemical formula SO2H−) |
Related compounds | |
Related isoelectronic |
trioxidane trisulfane |
Related compounds |
hydroxysulfonyl radical HOSO2 sulfinic acid sulfenic acid HSOH dihydroxydisulfane HOSSOH |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|
The complementary base is the sulfoxylate anion SO2−
2 which is much more stable. In between these states is the HSO−
2 ion, also somewhat stable.
Sulfoxylate ions can be made by decomposing thiourea dioxide in an alkaline solution.[4] To do this, thiourea dioxide first forms an amidine-sulfinic acid tautomer, H2NC(=NH)SO2H, which then breaks apart.[5] Sulfoxylate reacts with formaldehyde to yield a hydroxymethanesulfinate called rongalite:
- HSO−
2 + H2CO → HOCH
2SO−
2,
which is an important chemical for dyeing.[4]