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Fluoroacetic acid

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Fluoroacetic acid

  Carbon, C
  Hydrogen, H
  Oxygen, O
  Fluorine, F
Names
Preferred IUPAC name
Fluoroacetic acid
Other names
  • 2-Fluoroacetic acid
  • Cymonic acid
  • Fluoroethanoic acid
  • Monofluoroacetic acid
Identifiers
3D model (JSmol)
3DMet
1739053
ChEBI
ChEMBL
ChemSpider
ECHA InfoCard 100.005.120 Edit this at Wikidata
EC Number
  • 205-631-7
25730
KEGG
RTECS number
  • AH5950000
UNII
UN number 2642
  • InChI=1S/C2H3FO2/c3-1-2(4)5/h1H2,(H,4,5)
    Key: QEWYKACRFQMRMB-UHFFFAOYSA-N
  • InChI=1/C2H3FO2/c3-1-2(4)5/h1H2,(H,4,5)
    Key: QEWYKACRFQMRMB-UHFFFAOYAF
  • FCC(O)=O
Properties
FCH2CO2H
Molar mass 78.042 g·mol−1
Appearance White solid
Density 1.369 g/cm3
Melting point 35.2 °C (95.4 °F; 308.3 K)
Boiling point 165 °C (329 °F; 438 K)
Soluble in water and ethanol
Acidity (pKa) 2.586[contradictory]
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
Highly toxic and corrosive
GHS labelling:
GHS05: CorrosiveGHS06: ToxicGHS09: Environmental hazard
Danger
H300, H314, H400
P260, P264, P270, P273, P280, P301+P310, P301+P330+P331, P303+P361+P353, P304+P340, P305+P351+P338, P310, P321, P330, P363, P391, P405, P501
Lethal dose or concentration (LD, LC):
7 mg/kg (rat, oral)
Related compounds
Related compounds
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Fluoroacetic acid is a organofluorine compound with the chemical formula FCH2CO2H. It is a colorless solid that is noted for its relatively high toxicity.[1] The conjugate base, fluoroacetate occurs naturally in at least 40 plants in Australia, Brazil, and Africa. It is one of only five known organofluorine-containing natural products.[2]

Toxicity

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Fluoroacetic acid is a harmful metabolite of some fluorine-containing drugs (median lethal dose, LD50 = 10 mg/kg in humans). The most common metabolic sources of fluoroacetic acid are fluoroamines and fluoroethers. Fluoroacetic acid can disrupt the Krebs cycle.[3]The metabolite of fluoroacetic acid is Fluorocitric acid and is very toxic because it is not processable using aconitase in the Krebs cycle (where fluorocitrate takes place of citrate as the substrate). The enzyme is inhibited and the cycle stops working.[4]

In contrast with fluoroacetic acid, difluoroacetic acid and trifluoroacetic acid are far less toxic. Its pKa is 2.66[contradictory], in contrast to 1.24 and 0.23 for the respective di- and trifluoroacetic acid.[5]

Uses

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Fluoroacetic acid is used to manufacture pesticides especially rodenticides (see sodium fluoroacetate). The overall market is projected to rise at a considerable rate during the forecast period, 2021 to 2027.[6]

See also

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References

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  1. ^ Timperley, Christopher M. (2000). "Highly-toxic fluorine compounds". Fluorine Chemistry at the Millennium. pp. 499–538. doi:10.1016/B978-008043405-6/50040-2. ISBN 9780080434056.
  2. ^ K.K. Jason Chan; David O'Hagan (2012). "The Rare Fluorinated Natural Products and Biotechnological Prospects for Fluorine Enzymology". Natural Product Biosynthesis by Microorganisms and Plants, Part B. Methods in Enzymology. Vol. 516. pp. 219–235. doi:10.1016/B978-0-12-394291-3.00003-4. ISBN 9780123942913. PMID 23034231.
  3. ^ Kyzer, Jillian L.; Martens, Marvin (15 March 2021). "Metabolism and Toxicity of Fluorine Compounds". Chemical Research in Toxicology. 34 (3): 678–680. doi:10.1021/acs.chemrestox.0c00439. PMC 8023797. PMID 33513303.
  4. ^ Horák, J.; Linhart, I.; Klusoň, P. (2004). Úvod do toxikologie a ekologie pro chemiky (in Czech) (1st ed.). Prague: VŠCHT v Praze. ISBN 80-7080-548-X.
  5. ^ G. Siegemund; W. Schwertfeger; A. Feiring; B. Smart; F. Behr; H. Vogel; B. McKusick. "Fluorine Compounds, Organic". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a11_349. ISBN 978-3527306732.
  6. ^ Industry Research (October 25, 2021). "Global Fluoroacetic Acid Market Share, Size 2021: Consumption Analysis By Applications, Future Demand, Top Leading Players, Competitive Situation and Emerging Trends, and Forecast to 2027". MarketWatch. Archived from the original on 2022-01-05. Retrieved 5 January 2022.