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| HFIP | |
|---|---|
| Name | Hexafluoroisopropanol |
| Formula | C3H2F6O |
| Molar mass | 168.04 g·mol−1 |
| CAS number | 920-66-1 |
| Density | 1.596 g·cm−3 (20 °C) |
| Boiling point | 58–60 °C |
| Melting point | −9 to −12 °C |
| Appearance | colorless liquid |
HFIP
Hexafluoroisopropanol is a volatile, highly fluorinated secondary alcohol with marked acidity and exceptional hydrogen-bonding properties. It is employed across chemical research, pharmaceutical synthesis, materials science, and analytical chemistry in roles ranging from solvent to reagent and additive. Major industrial producers and research centers in the United States, Japan, Germany, and China handle HFIP under controlled conditions due to its reactivity and regulatory oversight.
HFIP is a secondary alcohol bearing two trifluoromethyl groups attached to the carbinol carbon, yielding the structural formula (CF3)2CHOH. Its notable physical parameters include a relatively low boiling point near 58–60 °C, high density, and significant vapor pressure at ambient temperatures; these attributes influence storage and transport practices used by firms such as BASF, DuPont, 3M Company, Dow Chemical Company, and Mitsui Chemicals. Chemically, HFIP displays an anomalously low pKa for an alcohol (~9.3 in water) compared with typical aliphatic alcohols, attributed to strong electron-withdrawing effects of the Trifluoromethyl group and resonance stabilization; this acidity is exploited in reactions referenced in literature from Harvard University, Massachusetts Institute of Technology, and ETH Zurich. HFIP is a strong hydrogen-bond donor yet a weak hydrogen-bond acceptor, enabling it to disrupt hydrogen-bonded networks in substrates such as peptides and nucleic acids studied at institutions like Max Planck Society and Scripps Research. Its high dielectric constant and low nucleophilicity make it a polar, noncoordinating medium favored in transformations reported from University of California, Berkeley, Imperial College London, and Stanford University.
Commercial HFIP is typically synthesized by fluorination or fluorinated alkylation routes starting from precursors like isopropanol derivatives or hexafluoroacetone. Industrial methods include hydrogenation of Hexafluoroacetone or controlled reduction of Hexafluoroacetone hydrate using catalysts and hydrogen sources, processes developed and scaled by companies such as Honeywell, Solvay, and Asahi Glass Co.. Alternative laboratory preparations involve Friedel–Crafts–type reactions and the use of trifluoromethylating reagents employed in academic reports from Columbia University, University of Tokyo, and Seoul National University. Production facilities are sited near petrochemical hubs and chemical parks associated with Port of Rotterdam, Gulf Coast (United States), Yokkaichi, and Shanghai Chemical Industry Park to facilitate feedstock supply and export logistics. Quality control standards and batch testing often adhere to specifications applied by standards bodies such as ASTM International and pharmacopeial monographs maintained by agencies like the U.S. Pharmacopeia.
HFIP is used as a specialty solvent and reagent across synthetic and analytical contexts. In asymmetric and organocatalytic reactions, researchers from University of Cambridge, University of Oxford, and California Institute of Technology report HFIP as a promoter for enantioselective transformations, influencing reaction rates and selectivities. In peptide chemistry and protein folding studies conducted at Cold Spring Harbor Laboratory and Pasteur Institute, HFIP is used to solubilize and induce secondary structure in peptides and amyloidogenic sequences. In materials science, laboratories at MIT, CNRS, and Riken employ HFIP to process fluorinated polymers, influence film formation, and assist in electrospinning protocols for fibers used in collaborations with NASA and European Space Agency. Analytical chemists at Agilent Technologies and Shimadzu use HFIP as a mobile phase additive in liquid chromatography–mass spectrometry to improve ionization and separation of basic compounds. HFIP also appears in photochemical and electrochemical research programs at Lawrence Berkeley National Laboratory and Brookhaven National Laboratory where it modulates solvent cages and radical lifetimes.
The distinctive behavior of HFIP arises from its strong hydrogen-bond donating capacity, low nucleophilicity, and high polarity. HFIP stabilizes cationic intermediates and electrophilic transition states, which explains its utility in facilitating carbocation-mediated rearrangements and solvolysis reactions studied by groups at University of Chicago and Princeton University. Its ability to form tight, directed hydrogen bonds disrupts intra- and intermolecular hydrogen bonding in biomolecules, altering conformational equilibria analyzed by researchers at Johns Hopkins University and University of Pennsylvania. HFIP can coordinate with Lewis acids like Boron trifluoride and metal catalysts such as Palladium and Rhodium complexes, modifying catalytic cycles and turnover frequencies reported in collaborations with National Institute of Standards and Technology and Argonne National Laboratory. In mass spectrometry workflows, HFIP suppresses adduct formation and enhances protonation of analytes, improving signal-to-noise ratios as documented by analytical groups at Thermo Fisher Scientific.
HFIP is flammable and presents inhalation and dermal exposure risks; industrial hygiene practices are guided by occupational exposure limits proposed by Occupational Safety and Health Administration and National Institute for Occupational Safety and Health. Acute exposure can cause respiratory irritation, central nervous system effects, and dermal burns in cases of concentrated contact; clinical case reports have been published in journals affiliated with Mayo Clinic and Cleveland Clinic. Personal protective equipment and engineering controls are recommended by standards organizations such as OSHA and NIOSH, and spill response is coordinated with emergency services trained under International Maritime Organization guidelines when transporting by sea. HFIP is incompatible with strong bases and reactive metals, requiring storage in corrosion-resistant containers maintained by chemical suppliers like Sigma-Aldrich and TCI Chemicals.
Due to its persistence and fluorinated nature, HFIP is monitored in environmental studies by agencies including the Environmental Protection Agency, European Chemicals Agency, and Ministry of the Environment (Japan). While not as persistent as perfluorooctanoic acid, HFIP and its transformation products are subject to scrutiny in wastewater and atmospheric chemistry investigations led by United States Geological Survey, NOAA, and CSIC. Regulatory measures focus on emission controls, wastewater treatment, and reporting requirements under frameworks such as REACH and national chemical inventories like the TSCA Inventory. Disposal often routes HFIP-containing waste to incineration facilities certified by EPA standards or to specialized fluorinated-waste handlers contracted by utilities and industrial partners including Veolia and SUEZ.
Category:Fluorinated alcohols