Peroxymonosulfuric acid

Peroxymonosulfuric acid
Skeletal formula of peroxymonosulfuric acid
Skeletal formula of peroxymonosulfuric acid
Ball and stick model of peroxymonosulfuric acid
Ball and stick model of peroxymonosulfuric acid
Names
IUPAC names
Peroxysulfuric acid
Sulfuroperoxoic acid[1]
Systematic IUPAC name
(Dioxidanido)hydroxidodioxidosulfur[1][2]
Other names
Peroxosulfuric acid[1]
Peroxomonosulfuric acid
Persulfuric acid
Caro's acid
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
ECHA InfoCard 100.028.879
EC Number
  • 231-766-6
101039
UNII
UN number 1483
  • InChI=1S/H2O5S/c1-5-6(2,3)4/h1H,(H,2,3,4) checkY
    Key: FHHJDRFHHWUPDG-UHFFFAOYSA-N checkY
  • OOS(O)(=O)=O
  • [O].[O].OOSO
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
 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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Infobox references

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).

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]

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 occurs in the piranha solution.[8]

Uses in industry

H
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).[9]

Alkali metal salts of H
2SO
5, 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. ^ 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.
  2. ^ "Peroxysulfuric acid (CHEBI:29286)". Chemical Entities of Biological Interest. UK: European Bioinformatics Institute. 20 November 2007. Retrieved 17 November 2011.
  3. ^ 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.
  4. ^ a b 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. Retrieved 4 November 2025.
  5. ^ 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.
  6. ^ Brauer, G. (1965). Handbook of Preparative Inorganic Chemistry. Vol. 1. New York, NY: Academic Press. pp. 388–389.
  7. ^ A method and apparatus for producing a peroxyacid solution, retrieved 2018-10-12
  8. ^ O'Brein, Sean C. (1996). "The chemistry of the semiconductor industry". Chemical Society Reviews. 25 (6): 393. doi:10.1039/cs9962500393. ISSN 0306-0012.
  9. ^ 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.
  10. ^ Lim, Hyun Jeong; Kim, David J.; Rigby, Kali; et al. "Peroxymonosulfate-Based Electrochemical Advanced Oxidation: Complication by Oxygen Reduction Reaction". Environmental Science & Technology. doi:10.1021/acs.est.3c06156. Retrieved 21 December 2025.
  11. ^ Edwards, J.O. (1955). "Safety". Chem. Eng. News. 33 (32): 3336. doi:10.1021/cen-v033n032.p3336.
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