Chemistry:Peroxymonosulfuric acid
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| Names | |
|---|---|
| IUPAC names
Peroxysulfuric acid
Sulfuroperoxoic acid[1] | |
| Systematic IUPAC name | |
| Other names | |
| Identifiers | |
3D model (JSmol)
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| ChEBI | |
| ChemSpider | |
| EC Number |
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| 101039 | |
PubChem CID
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| UNII | |
| UN number | 1483 |
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| Properties | |
| H2SO5 | |
| Molar mass | 114.078 g mol−1 |
| Appearance | White crystals[citation needed] |
| Density | 2.239 g cm−3 |
| Melting point | 45 °C |
| Acidity (pKa) | 1, 9.3[3] |
| Conjugate base | Peroxomonosulfate |
| 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   ?)
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| Infobox references | |
Peroxymonosulfuric acid, also known as persulfuric acid, peroxysulfuric acid is the inorganic compound with the formula H
2SO
5. It is a white solid. It is a component of Caro's acid, which is a solution of peroxymonosulfuric acid in sulfuric acid containing small amounts of water.[4] Peroxymonosulfuric acid is a very strong oxidant (E0 = +2.51 V).
Structure
In peroxymonosulfuric acid, the S(VI) center adopts its characteristic tetrahedral geometry; the connectivity is indicated by the formula HO–O–S(O)2–OH. The S-O-H proton is more acidic.[4]
History
The German chemist Heinrich Caro first reported investigations of mixtures of hydrogen peroxide and sulfuric acid.[5]
Synthesis and production
One laboratory scale preparation of Caro's acid involves the combination of chlorosulfuric acid and hydrogen peroxide:[6]
- H
2O
2 + ClSO
2OH ⇌ H
2SO
5 + HCl
Patents include more than one reaction for preparation of Caro's acid, usually as an intermediate for the production of potassium monopersulfate (PMPS), a bleaching and oxidizing agent. One route employs the following reaction:[7]
- H
2O
2 + H
2SO
4 ⇌ H
2SO
5 + H
2O
This reaction occurs in the piranha solution.[8]
Uses in industry
H2SO5 and Caro's acid have been used for a variety of disinfectant and cleaning applications, e.g., swimming pool treatment and denture cleaning. It is used in gold mining to destroy the cyanide in the waste stream (tailings).[9]
Alkali metal salts of H2SO5, especially oxone, are widely investigated.[10]
Hazards
These peroxy acids can be explosive. Explosions have been reported at Brown University[11] and Sun Oil. As with all strong oxidizing agents, peroxysulfuric acid is incompatible with organic compounds.
See also
References
- ↑ 1.0 1.1 1.2 International Union of Pure and Applied Chemistry (2005). Nomenclature of Inorganic Chemistry (IUPAC Recommendations 2005). Cambridge (UK): RSC–IUPAC. ISBN 0-85404-438-8. p. 139. Electronic version.
- ↑ "Peroxysulfuric acid (CHEBI:29286)". Chemical Entities of Biological Interest. UK: European Bioinformatics Institute. 20 November 2007. http://www.ebi.ac.uk/chebi/searchId.do?chebiId=CHEBI:29286.
- ↑ Perrin, D. D., ed (1982). Ionisation Constants of Inorganic Acids and Bases in Aqueous Solution. IUPAC Chemical Data (2nd ed.). Oxford: Pergamon (published 1984). Entry 176. ISBN 0-08-029214-3.
- ↑ 4.0 4.1 Jakob, Harald; Leininger, Stefan; Lehmann, Thomas; Jacobi, Sylvia; Gutewort, Sven (2007). "Peroxo Compounds, Inorganic". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim, Germany: Wiley-VCH. doi:10.1002/14356007.a19_177.pub2. ISBN 9783527306732. https://onlinelibrary.wiley.com/doi/10.1002/14356007.a19_177.pub2. Retrieved 4 November 2025.
- ↑ Caro, H. (1898). "Zur Kenntniss der Oxydation aromatischer Amine". Zeitschrift für angewandte Chemie 11 (36): 845–846. doi:10.1002/ange.18980113602. http://babel.hathitrust.org/cgi/pt?id=mdp.39015073166319;view=1up;seq=855.
- ↑ Brauer, G. (1965) (in en-US). Handbook of Preparative Inorganic Chemistry. 1. New York, NY: Academic Press. pp. 388–389.
- ↑ A method and apparatus for producing a peroxyacid solution, https://patents.google.com/patent/WO2005016511A1/da, retrieved 2018-10-12[non-primary source needed]
- ↑ O'Brein, Sean C. (1996). "The chemistry of the semiconductor industry" (in en). Chemical Society Reviews 25 (6): 393. doi:10.1039/cs9962500393. ISSN 0306-0012. https://xlink.rsc.org/?DOI=cs9962500393.
- ↑ Schmidt, Hugo Gerald (2022-01-24). "Safe Piranhas: A Review of Methods and Protocols". ACS Chemical Health & Safety 29 (1): 54–61. doi:10.1021/acs.chas.1c00094. https://doi.org/10.1021/acs.chas.1c00094.
- ↑ Lim, Hyun Jeong et al.. "Peroxymonosulfate-Based Electrochemical Advanced Oxidation: Complication by Oxygen Reduction Reaction". Environmental Science & Technology. doi:10.1021/acs.est.3c06156. https://pubs.acs.org/doi/10.1021/acs.est.3c06156. Retrieved 21 December 2025.
- ↑ Edwards, J.O. (1955). "Safety". Chem. Eng. News 33 (32): 3336. doi:10.1021/cen-v033n032.p3336.
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