Trifluoroacetic acid
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Names | |||
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IUPAC name
2,2,2-Trifluoroethanoic acid
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Other names
Perfluoroacetic acid
Trifluoroethanoic acid TFA |
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Identifiers | |||
76-05-1 | |||
ChEBI | CHEBI:45892 | ||
ChEMBL | ChEMBL506259 | ||
ChemSpider | 10239201 | ||
Jmol 3D model | Interactive image | ||
PubChem | 6422 | ||
RTECS number | AJ9625000 | ||
UNII | E5R8Z4G708 | ||
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Properties | |||
C2HF3O2 | |||
Molar mass | 114.02 g/mol | ||
Appearance | colorless liquid | ||
Density | 1.489 g/cm3, 20 °C | ||
Melting point | −15.4 °C (4.3 °F; 257.8 K) | ||
Boiling point | 72.4 °C (162.3 °F; 345.5 K) | ||
miscible | |||
Acidity (pKa) | 0.23 [1] | ||
Vapor pressure | {{{value}}} | ||
Related compounds | |||
Related perfluorinated acids
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Perfluorooctanoic acid Perfluorononanoic acid |
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Related compounds
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Acetic acid Trichloroacetic acid |
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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verify (what is ?) | |||
Infobox references | |||
Trifluoroacetic acid (TFA) is an organofluorine compound with the chemical formula CF3CO2H. It is a colorless liquid with a sharp odor similar to vinegar, but stronger in acidity. TFA is an analogue of acetic acid with the three hydrogen atoms replaced by three fluorine atoms. The acidity of TFA is approximately 34,000 times stronger[2] than that of acetic acid due to the electronegativity of the trifluoromethyl group. TFA is widely used in organic chemistry for various purposes.
Contents
Synthesis
TFA is prepared industrially by the electrofluorination of acetyl chloride and acetic anhydride, followed by hydrolysis of the resulting trifluoroacetyl fluoride:[3]
- CH
3COCl + 4 HF → CF
3COF + 3 H
2 + HCl - CF
3COF + H
2O → CF
3COOH + HF
Where desired, this compound may be dried by addition of trifluoroacetic anhydride.[4]
An older route to TFA proceeds via the oxidation of 1,1,1-trifluoro-2,3,3-trichloropropene with potassium permanganate. The trifluorotrichloropropene can be prepared by Swarts fluorination of hexachloropropene.
TFA occurs naturally in sea water, but only in small concentrations (<200 ng/L).[5][6]
Uses
TFA is the precursor to many other fluorinated compounds such as trifluoroacetic anhydride and 2,2,2-trifluoroethanol.[3] It is a reagent used in organic synthesis because of a combination of convenient properties: volatility, solubility in organic solvents, and its strength as an acid.[7] TFA is also less oxidizing than sulfuric acid but more readily available in anhydrous form than many other acids. One complication to its use is that TFA forms an azeotrope with water (b. p. 105 °C).
TFA is popularly used as a strong acid in peptide synthesis and other organic synthesis to remove the t-butoxycarbonyl protecting group.[8][9]
At a low concentration, TFA is used as an ion pairing agent in liquid chromatography (HPLC) of organic compounds, particularly peptides and small proteins. TFA is a versatile solvent for NMR spectroscopy (for materials stable in acid). It is also used as a calibrant in mass spectrometry.[10]
TFA is used to produce trifluoroacetate salts.[11]
Safety
Trifluoroacetic acid is a corrosive acid but it does not pose the hazards associated with hydrofluoric acid because the carbon-fluorine bond is not labile. Toxic.
See also
- Fluoroacetic acid
- Trichloroacetic acid, the chlorinated analog.
References
- ↑ Ref 1 in Lua error in package.lua at line 80: module 'strict' not found.
- ↑ Note: Calculated from Ka ratio of TFA and acetic acid
- ↑ 3.0 3.1 Lua error in package.lua at line 80: module 'strict' not found.
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