Hexafluoro-2-propanol

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1,1,1,3,3,3-Hexafluoro-2-propanol
1,1,1,3,3,3-Hexafluoro-2-propanol
Hexafluoroisopropanol 3D.png
Names
IUPAC name
1,1,1,3,3,3-Hexafluoro-propan-2-ol
Other names
Hexafluoroisopropanol,
Hexafluoroisopropyl alcohol,
HFIP
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
ECHA InfoCard 100.011.873 Edit this at Wikidata
RTECS number
  • UB6450000
UNII
Properties
C3H2F6O
Molar mass 168.038 g·mol−1
Appearance Colorless liquid
Density 1.596 g/mL
Melting point −3.3 °C (26.1 °F; 269.8 K)
Boiling point 58.2 °C (136.8 °F; 331.3 K)
Miscible
Vapor pressure 16 kPa at 20 °C
Viscosity 1.65 cP at 20 °C
Hazards
Safety data sheet External MSDS
GHS pictograms GHS05: Corrosive GHS08: Health hazard
GHS Signal word Danger
H314, H361fd, H373
P201, P280, P303+361+353, P305+351+338+310, P308+313
NFPA 704 (fire diamond)
Flammability code 0: Will not burn. E.g. waterHealth code 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasReactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no codeNFPA 704 four-colored diamond
0
3
0
Flash point > 100 °C (212 °F; 373 K)
Related compounds
Hexafluoroacetone;
Isopropyl alcohol, 2,2,2-Trifluoroethanol
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

Hexafluoroisopropanol, commonly abbreviated HFIP, is the organic compound with the formula (CF3)2CHOH. This fluoroalcohol finds use as solvent and synthetic intermediate. It appears as a colorless, volatile liquid that is characterized by a strong, pungent odor. As a solvent hexafluoro-2-propanol is polar and exhibits strong hydrogen bonding properties enabling it to dissolve substances that serve as hydrogen-bond acceptors, such as amides and ethers. (CF3)2CHOH is classified as a hard Lewis acid and its acceptor properties are discussed in the ECW model. Its relative acceptor strength toward a series of bases, versus other Lewis acids, can be illustrated by C-B plots.[1][2] Hexafluoro-2-propanol is transparent to UV light with high density, low viscosity and low refractive index.

Production and uses[edit]

Hexafluoro-propan-2-ol is prepared from hexafluoropropylene through hexafluoroacetone, which is then hydrogenated.[3]

(CF3)2CO + H2 → (CF3)2CHOH

Hexafluoro-propan-2-ol is a speciality solvent for some polar polymers and organic synthesis.[4][5] It is especially effective for solubilizing a wide range of polymers, including those that are not soluble in the most common organic solvents, such as: polyamides, polyacrylonitriles, polyacetals, polyesters (e.g. polyglycolide), and polyketones. It has also found use in biochemistry to solubilize peptides and to monomerize β-sheet protein aggregates. Because of its acidity (pKa = 9.3), it can be used as acid in volatile buffers for ion pair HPLC - mass spectrometry of nucleic acids.[6]

Medicine[edit]

It is both the precursor and the chief metabolite of the inhalation anesthetic sevoflurane.

Safety[edit]

Hexafluoro-2-propanol is a volatile, corrosive liquid that can cause severe burns and respiratory problems. With prolonged or repeated exposure, HFIP is likely to impair fertility as well as harm the unborn child.[7]

Environment[edit]

The release of hexafluoroisopropanol into the environment must be avoided. HFIP belongs to the per- and polyfluoroalkyl substances.[8] These so-called PFAS, also known as forever chemicals, are considered non-degradable substances in nature due to their fluorination. They are therefore classified as persistent organic pollutants. Due to its good solubility in water, hexafluoroisopropanol is also highly mobile. Thus, hexafluoroisopropanol counts as a vPvM/PMT substance (very persistent, mobile substances that may have toxic potential).[9] As a volatile and fluorinated substance, hexafluoroisopropanol increases global warming. It has a global warming potential (GWP) of 195, making it 195 times more harmful to the atmosphere than CO2.[10]

References[edit]

  1. ^ Laurence, C. and Gal, J-F. Lewis Basicity and Affinity Scales, Data and Measurement, (Wiley 2010) pp 50-51 IBSN 978-0-470-74957-9
  2. ^ Cramer, R. E., and Bopp, T. T. (1977) Great E and C plot. Graphical display of the enthalpies of adduct formation for Lewis acids and bases. Journal of Chemical Education 54 612-613, Improved E&C parameters are listed in ECW model. The plots shown in this paper used older parameters.
  3. ^ Günter Siegemund, Werner Schwertfeger, Andrew Feiring, Bruce Smart, Fred Behr, Herward Vogel, Blaine McKusick “Fluorine Compounds, Organic” in Ullmann's Encyclopedia of Industrial Chemistry, John Wiley & Sons, 2007. doi:10.1002/14356007.a11_349
  4. ^ Bégué, J.-P.; Bonnet-Delpon, D.; Crousse, B. (2004). "Fluorinated Alcohols: A New Medium for Selective and Clean Reaction". Synlett (1): 18–29. doi:10.1055/s-2003-44973.
  5. ^ Shuklov, Ivan A.; Dubrovina, Natalia V.; Börner, Armin (2007). "Fluorinated Alcohols as Solvents, Cosolvents and Additives in Homogeneous Catalysis". Synthesis. 2007 (19): 2925–2943. doi:10.1055/s-2007-983902.
  6. ^ Apffel, A.; Chakel, J.A.; Fischer, S.; Lichtenwalter, K.; Hancock, W.S. (1997). "Analysis of oligonucleotides by HPLC-electrospray ionization mass spectrometry". Anal. Chem. 69: 1320–1325. doi:10.1021/ac960916h. PMID 21639339.
  7. ^ "HFIP MSDS". Sigma Aldrich. Retrieved 7 January 2021.
  8. ^ "PFAS structures in DSSTox". CompTox. Retrieved 7 January 2021.
  9. ^ Arp, Hans Peter (November 2019). REACH: Improvement of guidance and methods for the identification and assessment of PMT/vPvM substances (PDF). Umweltbundesamt. Retrieved 7 January 2021.
  10. ^ "MANDATORY GREENHOUSE GAS REPORTING" (PDF). epa.gov. Federal Register. Retrieved 7 January 2021.

Sources[edit]

External links[edit]