Peroxymonosulfuric acid
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| Names | |
|---|---|
| IUPAC name
(Dioxidanido)hydroxidodioxidosulfur[1] | |
| Other names
Peroxomonosulfuric acid Peroxysulfuric acid | |
| Identifiers | |
10361-76-9  | |
| ChEBI | CHEBI:29286  |
| ChemSpider | 2035480 |
| EC Number | 231-766-6 |
| 101039 | |
| Jmol 3D model | Interactive image Interactive image |
| PubChem | 2754594 |
| UN number | 1483 |
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| |
| Properties | |
| H 2SO 5 | |
| Molar mass | 114.078 g mol−1 |
| Appearance | White crystals |
| Density | 2.239 g cm−3 |
| Structure | |
| Tetrahedral at S | |
| Hazards | |
| Main hazards | strong oxidizer |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| verify (what is ?) | |
| Infobox references | |
Peroxymonosulfuric acid, (H2SO5), also known as persulfuric acid, peroxysulfuric acid, or Caro's acid, is a liquid at room temperature. In this acid, the S(VI) center adopts its characteristic tetrahedral geometry; the connectivity is indicated by the formula HO–O–S(O)2–OH. It is one of the strongest oxidants known (E0 = +2.51 V) and is highly explosive.
H2SO5 is sometimes confused with H2S2O8, known as peroxydisulfuric acid. The disulfuric acid, which appears to be more widely used as its alkali metal salts, has the structure HO–S(O)2–O–O–S(O)2–OH.
History
H2SO5 was first described in 1898 by Heinrich Caro, after whom it is named.[2]
Synthesis and production
The laboratory scale preparation of Caro's acid involve the combination of chlorosulfuric acid and hydrogen peroxide.
- H2O2 + ClSO2OH ⇌ H2SO5 + HCl
Large scale production of Caro's acid is usually done on site, due to its instability. According to the patent by Martin, Caro's acid is produced by reacting >85% sulfuric acid and <50% hydrogen peroxide ("Piranha solution").[3]
- H2O2 + H2SO4 ⇌ H2SO5 + H2O
Uses in industry
H2SO5 has been used for a variety of disinfectant and cleaning applications, e.g., swimming pool treatment and denture cleaning. Alkali metal salts of H2SO5 show promise for the delignification of wood.[4]
Ammonium, sodium, and potassium salts of H2SO5 are used in the plastics industry as polymerization initiators, etchants, desizing agents, soil conditioner, and for decolorizing and deodorizing oils.
Potassium peroxymonosulfate, KHSO5, is the potassium acid salt of peroxymonosulfuric acid. It is widely used as an oxidizing agent.
Dangers
Pure Caro's acid is highly explosive. Explosions have been reported at Brown University[5] and Sun Oil. As with all strong oxidizing agents, peroxysulfuric acid should be kept away from organic compounds such as ethers and ketones because of its ability to peroxidize the compound, creating a highly unstable molecule such as acetone peroxide.
See also
References
- ↑ "peroxysulfuric acid (CHEBI:29286)". Chemical Entities of Biological Interest. UK: European Bioinformatics Institute. 20 November 2007. Retrieved 17 November 2011.
- ↑ Caro, H. (1898). "Zur Kenntniss der Oxydation aromatischer Amine" [[Contribution] to [our] knowledge of the oxidation of aromatic amines]. Zeitschrift für angewandte Chemie 11 (36): 845–846. doi:10.1002/ange.18980113602.
- ↑ Martin, P. L. (USA). U.S. Pat. Appl. Publ. (2005), 21 pp. CODEN: USXXCO US 2005031530 A1 20050210 Patent written in English. Application: US 2004-878176 20040628. Priority: US 2003-494009 20030807. CAN 142:179838 AN 2005:122569 CAPLUS
- ↑ Springer, E. L.; McSweeny, J. D. (1993). "Treatment of softwood kraft pulps with peroxymonosulfate before oxygen delignification". Tappi Journal 76 (8): 194–199. ISSN 0734-1415.
- ↑ J.O. Edwards (1955). "SAFETY". Chem. & Eng. News 33 (32): 3336. doi:10.1021/cen-v033n032.p3336.