Peroxymonosulfuric Acid
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Peroxymonosulfuric Acid
Peroxymonosulfuric acid
Skeletal formula 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 Edit this at Wikidata
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
Molar mass 114.078 g mol-1
Appearance White crystals
Density 2.239 g cm-3
Melting point 45 °C
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).
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Infobox references

Peroxymonosulfuric acid, , also known as persulfuric acid, peroxysulfuric acid, or Caro's acid. 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.

is sometimes confused with , 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

was first described in 1898 by the German chemist Heinrich Caro, after whom it is named.[3]

Synthesis and production

The laboratory scale preparation of Caro's acid involves the combination of chlorosulfuric acid and hydrogen peroxide:

+ ? + HCl [4]

Published 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 patent for production of Caro's acid for this purpose gives the following reaction:

+ ? + [5]

This is the reaction that produces the acid transiently in "piranha solution".

Uses in industry

has been used for a variety of disinfectant and cleaning applications, e.g., swimming pool treatment and denture cleaning. Alkali metal salts of show promise for the delignification of wood.[6] It is also used in laboratories as a last resort in removing organic materials since can fully oxidize any organic materials.[]

Ammonium, sodium, and potassium salts of are used in the plastics industry as radical initiators for polymerization. They are also used as etchants, oxidative desizing agents for textile fabrics, and for decolorizing and deodorizing oils.

Potassium peroxymonosulfate, , is the potassium acid salt of peroxymonosulfuric acid. It is widely used as an oxidizing agent.

Hazards

Pure Caro's acid is highly explosive. Explosions have been reported at Brown University[7] 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 these compounds, creating highly unstable molecules such as acetone peroxide.

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 2011.
  3. ^ 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.
  4. ^ "Synthesis of Caro's acid". PrepChem.com. 2017-02-13. Retrieved .
  5. ^ A method and apparatus for producing a peroxyacid solution, retrieved
  6. ^ 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. Archived from the original on 2011-09-29. Retrieved .
  7. ^ Edwards, J.O. (1955). "Safety". Chem. Eng. News. 33 (32): 3336. doi:10.1021/cen-v033n032.p3336.

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