Peracetic acid
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| Names | |||
|---|---|---|---|
| Preferred IUPAC name
Ethaneperoxoic acid[1] | |||
| Other names
Peroxyacetic acid
Acetic peroxide Acetyl hydroperoxide Proxitane | |||
| Identifiers | |||
3D model (JSmol)
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| Abbreviations | PAA | ||
| ChEBI | |||
| ChEMBL | |||
| ChemSpider | |||
| ECHA InfoCard | 100.001.079 | ||
| EC Number |
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| KEGG | |||
PubChem CID
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| RTECS number |
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| UNII | |||
| UN number | 3107 3105 | ||
CompTox Dashboard (EPA)
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| Properties | |||
| CH3CO3H | |||
| Molar mass | 76.05 g/mol | ||
| Appearance | Colorless liquid | ||
| Density | 1.0375 g/mL | ||
| Melting point | 0 °C (32 °F; 273 K)[2] | ||
| Boiling point | 105 °C (221 °F; 378 K) 25 C @ (1.6 kPa)[2] | ||
| Acidity (pKa) | 8.2 | ||
Refractive index (nD)
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1.3974 (589 nm, 20 °C)[2] | ||
| Viscosity | 3.280 cP | ||
| Pharmacology | |||
| QG51AD03 (WHO) | |||
| Hazards | |||
| GHS labelling: | |||
   
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| Danger | |||
| H226, H242, H302, H312, H314, H332, H400 | |||
| P210, P220, P233, P234, P240, P241, P242, P243, P260, P261, P264, P270, P271, P273, P280, P301+P312, P301+P330+P331, P302+P352, P303+P361+P353, P304+P312, P304+P340, P305+P351+P338, P310, P312, P321, P322, P330, P363, P370+P378, P391, P403+P235, P405, P411, P420, P501 | |||
| NFPA 704 (fire diamond) | |||
| Flash point | 40.5 °C (104.9 °F; 313.6 K) | ||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Peracetic acid (also known as peroxyacetic acid, or PAA) is an organic compound with the formula CH3CO3H. This peroxy acid is a colorless liquid with a characteristic acrid odor reminiscent of acetic acid. It can be highly corrosive.
Peracetic acid is a weaker acid than the parent acetic acid, with a pKa of 8.2.[2]
Production
[edit]Peracetic acid is produced industrially by the autoxidation of acetaldehyde:[2]
- O2 + CH3CHO → CH3CO3H
In the presence of a strong acid catalyst, such as sulfuric acid, acetic acid and hydrogen peroxide produce peracetic acid:[3]
- H2O2 + CH3CO2H ⇌ CH3CO3H + H2O
However, in concentrations (3-6%) of vinegar and hydrogen peroxide marketed for household use, mixing without a strong acid catalyst will not form peracetic acid.
As an alternative, acetyl chloride and acetic anhydride can be used to generate a solution of the acid with lower water content.
Peracetic acid is generated in situ by some laundry detergents. This is achieved by the action of bleach activators, such as tetraacetylethylenediamine and sodium nonanoyloxybenzenesulfonate, upon hydrogen peroxide formed from sodium percarbonate in water. The peracetic acid is a more effective bleaching agent than hydrogen peroxide itself.[4][5] PAA is also formed naturally in the environment through a series of photochemical reactions involving formaldehyde and photo-oxidant radicals.[6]
Peracetic acid is always sold in solution as a mixture with acetic acid and hydrogen peroxide to maintain its stability. The concentration of the acid as the active ingredient can vary.
Uses
[edit]The United States Environmental Protection Agency first registered peracetic acid as an antimicrobial in 1986 for indoor use on hard surfaces. Use sites include agricultural premises, food establishments, medical facilities, and home bathrooms. Peracetic acid is also registered for use in dairy and cheese processing plants, on food processing equipment, and in pasteurizers in breweries, wineries, and beverage plants.[7] It is also applied for the disinfection of medical supplies, to prevent biofilm formation in pulp industries, and as a water purifier and disinfectant. Peracetic acid can be used as a cooling tower water disinfectant, where it prevents biofilm formation and effectively controls Legionella bacteria. Nu-Cidex is the trade name for a brand of antimicrobial peracetic acid.[8]
In the European Union, peroxyacetic acid was reported by the EFSA after submission in 2013 by the US Department of Agriculture.[9]
Decontamination kits for cleaning fentanyl analogues from surfaces (as used by many police forces, amongst others) often contain solid peracetyl borate, which mixes with water to produce peracetic acid.[10]
Epoxidation
[edit]Although less active than more acidic peracids (e.g., m-CPBA), peracetic acid in various forms is used for the epoxidation of various alkenes (Prilezhaev reaction). Useful applications are for unsaturated fats, synthetic and natural rubbers, and some natural products such as pinene. A variety of factors affect the amount of free acid or sulfuric acid (used to prepare the peracid).[11]
Safety
[edit]Peracetic acid is a strong oxidizing agent and severe irritant to the skin, eyes, and respiratory system. The U.S. Environmental Protection Agency published the following Acute Exposure Guideline Levels (AEGL):[12]
| eight-hour TWA AEGL | Definition | mg/m3 | ppm |
|---|---|---|---|
| 1 | The concentration at which the general population will experience transient and reversible problems, such as notable discomfort, irritation, or certain asymptomatic non-sensory effects. | 0.52 | 0.17 |
| 2 | The concentration that results in irreversible or other serious, long-lasting adverse health effects or an impaired ability to escape. | 1.6 | 0.52 |
| 3 | The concentration that results in life-threatening health effects or death. | 4.1 | 1.3 |
See also
[edit]References
[edit]- ^ Nomenclature of Organic Chemistry: IUPAC Recommendations and Preferred Names 2013 (Blue Book). Cambridge: The Royal Society of Chemistry. 2014. p. 749. doi:10.1039/9781849733069-FP001 (inactive 2024-06-30). ISBN 978-0-85404-182-4.
{{cite book}}: CS1 maint: DOI inactive as of June 2024 (link) - ^ a b c d e Klenk, Herbert; Götz, Peter H.; Siegmeier, Rainer; Mayr, Wilfried. "Peroxy Compounds, Organic". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a19_199. ISBN 978-3527306732.
- ^ Rangarajan, B.; Havey, A.; Grulke, E.; Culnan, P. D. (1995). "Kinetic parameters of a two-phase model for in situ epoxidation of soybean oil". J. Am. Oil Chem. Soc. 72 (10): 1161–1169. doi:10.1007/bf02540983. S2CID 98196947.
- ^ Smulders, Eduard; Von Rybinski, Wolfgang; Sung, Eric; Rähse, Wilfried; Steber, Josef; Wiebel, Frederike; Nordskog, Anette (2007). "Laundry Detergents". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a08_315.pub2. ISBN 978-3527306732.
- ^ "Peracetic acid" (PDF). Agriculture Marketing Service. United States Department of Agriculture. Retrieved 2006-11-11.
- ^ "Hazardous Substances Data Bank". ToxNet. U.S. National Library of Medicine. Retrieved 2006-11-11.
- ^ "Hydrogen Peroxide and Peroxyacetic Acid". U.S. Environmental Protection Agency. Retrieved 2006-11-11.
- ^ Lynam, P. A.; Babb, J. R.; Fraise, A. P. (1995). "Comparison of the mycobactericidal activity of 2% alkaline glutaraldehyde and 'Nu-Cidex' (0.35% peracetic acid)". J. Hosp. Infect. 30 (3): 237–240. doi:10.1016/s0195-6701(95)90322-4. PMID 8522783.
- ^ "EFSA publishes a favourable opinion on the use of peroxyacetic acid on poultry".
- ^ "First Line Technologies' Dahlgren Decon'". CBRNE Tech. Retrieved 19 August 2020.
- ^ Sienel, Guenter; Rieth, Robert; Rowbottom, Kenneth T. (2000). "Epoxides". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a09_531. ISBN 978-3527306732.
- ^ "Peracetic Acid Results - AEGL Program". US EPA. 29 September 2014.
| Authority control databases: National |
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