Peroxymonosulfuric acid, also known as persulfuric acid, peroxysulfuric acid is the inorganic compound with the formula H2SO5. 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).
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| Names | |
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| IUPAC names
Peroxysulfuric acid
Sulfuroperoxoic acid[1] | |
| Systematic IUPAC name | |
| Other names
Peroxosulfuric acid[1]
Peroxomonosulfuric acid[citation needed] Persulfuric acid[citation needed] Caro's acid | |
| Identifiers | |
3D model (JSmol)
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| ChEBI | |
| ChemSpider | |
| ECHA InfoCard | 100.028.879 |
| EC Number |
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| 101039 | |
PubChem CID
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| UNII | |
| UN number | 1483 |
CompTox Dashboard (EPA)
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| Properties | |
| H 2SO 5 | |
| Molar mass | 114.078 g mol−1 |
| Appearance | White crystals |
| Density | 2.239 g cm−3 |
| Melting point | 45 °C |
| Acidity (pKa) | 1, 9.3[3] |
| Conjugate base | Peroxomonosulfate |
| Structure | |
| Tetrahedral at S | |
| Hazards | |
| Occupational safety and health (OHS/OSH): | |
Main hazards
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strong oxidizer |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Structure
editIn 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
editThe German chemist Heinrich Caro first reported investigations of mixtures of hydrogen peroxide and sulfuric acid.[5]
Synthesis and production
editOne laboratory scale preparation of Caro's acid involves the combination of chlorosulfuric acid and hydrogen peroxide:[6]
- H2O2 + ClSO2OH ⇌ H2SO5 + 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]
- H2O2 + H2SO4 ⇌ H2SO5 + H2O
This reaction is related to "piranha solution".
Uses in industry
editH
2SO
5 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").
Alkali metal salts of H
2SO
5, especially oxone, are widely investigated.
Hazards
editThese peroxy acids can be explosive. Explosions have been reported at Brown University[8] and Sun Oil. As with all strong oxidizing agents, peroxysulfuric acid is incompatible with organic compounds.
See also
editReferences
edit- ^ a b c 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. Retrieved 17 November 2011.
- ^ Perrin, D. D., ed. (1982) [1969]. 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. LCCN 82-16524.
- ^ a b Jakob, Harald; Leininger, Stefan; Lehmann, Thomas; Jacobi, Sylvia; Gutewort, Sven (2007). "Peroxo Compounds, Inorganic". Ullmann's Encyclopedia of Industrial Chemistry. doi:10.1002/14356007.a19_177.pub2. ISBN 978-3-527-30673-2.
- ^ 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.
- ^ "Synthesis of Caro's acid". PrepChem.com. 2017-02-13. Retrieved 2018-10-12.
- ^ A method and apparatus for producing a peroxyacid solution, retrieved 2018-10-12
- ^ Edwards, J.O. (1955). "Safety". Chem. Eng. News. 33 (32): 3336. doi:10.1021/cen-v033n032.p3336.