Trifluoroacetic anhydride

Trifluoroacetic anhydride
Names
	Preferred IUPAC name Trifluoroacetic anhydride
	Other names 2,2,2-Trifluoroacetic anhydride; TFAA;
Identifiers
CAS Number	407-25-0 ;
3D model (JSmol)	Interactive image;
ChemSpider	21106178;
ECHA InfoCard	100.006.349
EC Number	206-982-9;
PubChem CID	9845;
UNII	5ENA87IZHT ;
CompTox Dashboard (EPA)	DTXSID90861920 ;
	InChI InChI=1S/C4F6O3/c5-3(6,7)1(11)13-2(12)4(8,9)10 Key: QAEDZJGFFMLHHQ-UHFFFAOYSA-N ;
	SMILES C(=O)(C(F)(F)F)OC(=O)C(F)(F)F;
Properties
Chemical formula	C4F6O3
Molar mass	210.031 g·mol−1
Appearance	colorless liquid
Density	1.511 g/mL at 68 F
Melting point	−65 °C (−85 °F; 208 K)
Boiling point	40 °C (104 °F; 313 K)
Solubility in water	reacts
Solubility	soluble in benzene, dichloromethane, ether, DMF, THF, acetonitrile
Hazards
Safety data sheet	Oxford MSDS
GHS pictograms	[1]
GHS Signal word	Danger
GHS hazard statements	H314, H332[1]
GHS precautionary statements	P280, P305+351+338, P310 [1]
	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

Trifluoroacetic anhydride (TFAA) is the acid anhydride of trifluoroacetic acid. It is the perfluorinated derivative of acetic anhydride.

Preparation

Trifluoroacetic anhydride was originally prepared by the dehydration of trifluoroacetic acid with phosphorus pentoxide.[2] The dehydration might also be carried out with excess α-halogenated acid chlorides. For example, with dichloroacetyl chloride:[3]

2 CF₃COOH + Cl₂CHCOCl → (CF₃CO)₂O + Cl₂CHCOOH + HCl

Uses

Trifluoroacetic anhydride has various uses in organic synthesis.

It may be used to introduce the corresponding trifluoroacetyl group, for which it is more convenient than the corresponding acyl chloride, trifluoroacetyl chloride, which is a gas.

It can be used to promote reactions of carboxylic acids, including nucleophilic acyl substitution, Friedel-Crafts acylation, and acylation of other unsaturated compounds. Other electrophilic aromatic substitution reactions can also be promoted with trifluoroacetic anhydride, including nitration, sulfonation and nitrosylation.[2]

Similar to acetic anhydride, trifluoroacetic anhydride can be used as a dehydrating agent and as an activator for the Pummerer rearrangement.[4]

It can be used in place of oxalyl chloride in the Swern oxidation, allowing temperatures up to −30 °C.[5]

With sodium iodide, it reduces sulfoxides to sulfides.[4]

Trifluoroacetic anhydride is the recommended desiccant for trifluoroacetic acid.[6]

References

Sigma-Aldrich Co., Trifluoroacetic Anhydride. Retrieved on 2020-06-08.
Tedder, J. M. (1955). "The Use of Trifluoroacetic Anhydride and Related Compounds in Organic Synthesis". Chem. Rev. 55 (5): 787–827. doi:10.1021/cr50005a001.
US 4595541
Sweeney, Joseph; Perkins, Gemma; DiMauro, Erin F.; Hodous, Brian L. (2005). "Trifluoroacetic Anhydride". Encyclopedia of Reagents for Organic Synthesis. John Wiley & Sons. doi:10.1002/047084289X.rt237.pub2. ISBN 9780470842898.
Omura, Kanji; Sharma, Ashok K.; Swern, Daniel. "Dimethyl Sulfoxide-Trifluoroacetic Anhydride. New Reagent for Oxidation of Alcohols to Carbonyls". J. Org. Chem. 41 (6): 957–962. doi:10.1021/jo00868a012.
Chai, Christina Li Lin; Armarego, W. L. F. (2003). Purification of laboratory chemicals (Google Books excerpt). Oxford: Butterworth-Heinemann. p. 376. ISBN 0-7506-7571-3.

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[sigma-1] Sigma-Aldrich Co., Trifluoroacetic Anhydride. Retrieved on 2020-06-08.

[:0-2] Tedder, J. M. (1955). "The Use of Trifluoroacetic Anhydride and Related Compounds in Organic Synthesis". Chem. Rev. 55 (5): 787–827. doi:10.1021/cr50005a001.

[3] US 4595541

[encyclopedia-4] Sweeney, Joseph; Perkins, Gemma; DiMauro, Erin F.; Hodous, Brian L. (2005). "Trifluoroacetic Anhydride". Encyclopedia of Reagents for Organic Synthesis. John Wiley & Sons. doi:10.1002/047084289X.rt237.pub2. ISBN 9780470842898.

[5] Omura, Kanji; Sharma, Ashok K.; Swern, Daniel. "Dimethyl Sulfoxide-Trifluoroacetic Anhydride. New Reagent for Oxidation of Alcohols to Carbonyls". J. Org. Chem. 41 (6): 957–962. doi:10.1021/jo00868a012.

[6] Chai, Christina Li Lin; Armarego, W. L. F. (2003). Purification of laboratory chemicals (Google Books excerpt). Oxford: Butterworth-Heinemann. p. 376. ISBN 0-7506-7571-3.