Triflic acid

Triflic acid

Names
IUPAC name Trifluoromethanesulfonic acid
Other names Triflic acid
Identifiers
CAS Number	1493-13-6 Y
3D model (JSmol)	Interactive image
ChEBI	CHEBI:48511 Y
ChemSpider	56192 Y
ECHA InfoCard	100.014.625
PubChem CID	62406
UNII	JE2SY203E8 Y
CompTox Dashboard (EPA)	DTXSID70892979 DTXSID2044397, DTXSID70892979
InChI InChI=1S/CHF3O3S/c2-1(3,4)8(5,6)7/h(H,5,6,7) Y Key: ITMCEJHCFYSIIV-UHFFFAOYSA-N Y InChI=1/CHF3O3S/c2-1(3,4)8(5,6)7/h(H,5,6,7) Key: ITMCEJHCFYSIIV-UHFFFAOYAW
SMILES C(F)(F)(F)S(=O)(=O)O
Properties
Chemical formula	CF3SO3H
Molar mass	150.07121 g/mol
Appearance	Colorless liquid
Density	1.696 g/mL
Melting point	−40 °C (−40 °F; 233 K)
Boiling point	162 °C (324 °F; 435 K)
Solubility in water	1600 g/L
Vapor pressure	3.2
Acidity (pKa)	−14.7±2.0[1]
Conjugate base	Triflate anion
Viscosity	1.864–1.881 mm2/s at 20 °C
Hazards
Occupational safety and health (OHS/OSH):
Main hazards	Causes severe acid burns
GHS labelling:
Pictograms
Signal word	Danger
Hazard statements	H290, H302, H314, H335, H402
Precautionary statements	P234, P261, P264, P270, P271, P273, P280, P301+P312+P330, P301+P330+P331, P303+P361+P353, P304+P340+P310, P305+P351+P338+P310, P363, P390, P403+P233, P405, P501
NFPA 704 (fire diamond)	4 0 2 ACID
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). Y verify (what is YN ?) Infobox references

Triflic acid, the short name for trifluoromethanesulfonic acid, TFMS, TFSA, HOTf or TfOH, is a sulfonic acid with the chemical formula CF₃SO₃H. It is one of the strongest known acids. Triflic acid is mainly used in research as a catalyst for esterification.^[2][3] It is a hygroscopic, colorless, slightly viscous liquid and is soluble in polar solvents.

Trifluoromethanesulfonic acid is produced industrially by electrochemical fluorination (ECF) of methanesulfonic acid:

${\displaystyle {\ce {CH3SO3H + 4 HF ->CF3SO2F + H2O + 3 H2}}}$

The resulting CF₃SO₂F is hydrolyzed, and the resulting triflate salt is reprotonated. Alternatively, trifluoromethanesulfonic acid arises by oxidation of trifluoromethylsulfenyl chloride:^[4]

${\displaystyle {\ce {CF3SCl + 2 Cl2 + 3 H2O -> CF3SO3H + 5 HCl}}}$

Triflic acid is purified by distillation from triflic anhydride.^[3]

Trifluoromethanesulfonic acid was first synthesized in 1954 by Robert Haszeldine and Kidd by the following reaction:^[5]

In the laboratory, triflic acid is useful in protonations because the conjugate base of triflic acid is nonnucleophilic. It is also used as an acidic titrant in nonaqueous acid-base titration because it behaves as a strong acid in many solvents (acetonitrile, acetic acid, etc.) where common mineral acids (such as HCl or H₂SO₄) are only moderately strong.

With a K_a = 5×10¹⁴, pK_a = −14.7±2.0,^[1] triflic acid qualifies as a superacid. It owes many of its useful properties to its great thermal and chemical stability. Both the acid and its conjugate base CF₃SO⁻
₃, known as triflate, resist oxidation/reduction reactions, whereas many strong acids are oxidizing, such as perchloric or nitric acid. Further recommending its use, triflic acid does not sulfonate substrates, which can be a problem with sulfuric acid, fluorosulfuric acid, and chlorosulfonic acid. Below is a prototypical sulfonation, which triflic acid does not undergo:

${\displaystyle {\ce {C6H6 + H2SO4 ->[{\ce {SO3}}] C6H5(SO3H) + H2O}}}$

Triflic acid fumes in moist air and forms a stable solid monohydrate, CF₃SO₃H·H₂O, melting point 34 °C.

The triflate ligand is labile, reflecting its low basicity. Trifluoromethanesulfonic acid reacts exothermically with metal carbonates, hydroxides, and oxides. Illustrative is the synthesis of Cu(OTf)₂.^[6]

${\displaystyle {\ce {Cu2CO3(OH)2 + 4 CF3SO3H -> 2 Cu(O3SCF3)2 + 3 H2O + CO2}}}$

Chloride ligands can be converted to the corresponding triflates:

${\displaystyle {\ce {3 CF3SO3H + [Co(NH3)5Cl]Cl2 -> [Co(NH3)5O3SCF3](O3SCF3)2 + 3 HCl}}}$

This conversion is conducted in neat HOTf at 100 °C, followed by precipitation of the salt upon the addition of ether.

Triflic acid reacts with acyl halides to give mixed triflate anhydrides, which are strong acylating agents, e.g. in Friedel–Crafts reactions.

${\displaystyle {\ce {CH3C(O)Cl + CF3SO3H -> CH3C(O)OSO2CF3 + HCl}}}$

${\displaystyle {\ce {CH3C(O)OSO2CF3 + C6H6 -> CH3C(O)C6H5 + CF3SO3H}}}$

Triflic acid catalyzes the reaction of aromatic compounds with sulfonyl chlorides, probably also through the intermediacy of a mixed anhydride of the sulfonic acid.

Triflic acid promotes other Friedel–Crafts-like reactions including the cracking of alkanes and alkylation of alkenes, which are very important to the petroleum industry. These triflic acid derivative catalysts are very effective in isomerizing straight chain or slightly branched hydrocarbons that can increase the octane rating of a particular petroleum-based fuel.

Triflic acid reacts exothermically with alcohols to produce ethers and olefins.

Dehydration gives the acid anhydride, trifluoromethanesulfonic anhydride, (CF₃SO₂)₂O.

Triflic acid is one of the strongest acids. Contact with skin causes severe burns with delayed tissue destruction. On inhalation it causes fatal spasms, inflammation and edema.^[7]

Like sulfuric acid, triflic acid must be slowly added to polar solvents to prevent thermal runaway.