Fluorosulfuric acid
| |||
| Names | |||
|---|---|---|---|
| IUPAC name
Sulfurofluoridic acid | |||
| Systematic IUPAC name
Fluorosulfuric acid | |||
| Other names
Fluorosulfonic acid, Fluorosulphonic acid, Fluorinesulfonic acid, Fluorinesulphonic acid, Fluoridosulfonic acid, Fluoridosulphonic acid, Sulfuric fluorohydrin, Epoxysulfonyl fluoride | |||
| Identifiers | |||
7789-21-1  | |||
| ChemSpider | 23005 | ||
| EC Number | 232-149-4 | ||
| Jmol 3D model | Interactive image Interactive image | ||
| MeSH | Fluorosulfonic+acid | ||
| PubChem | 24603 | ||
| RTECS number | LP0715000 | ||
| UN number | 1777 | ||
| |||
| |||
| Properties | |||
| FHO3S | |||
| Molar mass | 100.06 g·mol−1 | ||
| Appearance | Colorless liquid | ||
| Density | 1.84 g cm−3 | ||
| Melting point | −87.5 °C; −125.4 °F; 185.7 K | ||
| Boiling point | 165.4 °C; 329.6 °F; 438.5 K | ||
| Acidity (pKa) | -10 | ||
| Basicity (pKb) | 24 | ||
| Structure | |||
| Tetragonal at S | |||
| Tetrahedral at S | |||
| Hazards | |||
| Safety data sheet | ICSC 0996 | ||
| EU classification (DSD) |
 Xn  C | ||
| R-phrases | R20, R35 | ||
| S-phrases | (S1/2), S26, S45 | ||
| Related compounds | |||
| Related compounds |
Antimony pentafluoride Trifluoromethanesulfonic acid Hydrofluoric acid | ||
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |||
verify (what is  ?) | |||
| Infobox references | |||
Fluorosulfuric acid (IUPAC name: sulfurofluoridic acid) is the inorganic compound with the chemical formula HSO3F. It is one of the strongest acids commercially available. The formula HSO3F emphasizes its relationship to sulfuric acid, H2SO4; HSO3F is a tetrahedral molecule. It is a colourless liquid although commercial samples are often yellow.[1]
Chemical properties
Fluorosulfuric acid is a free-flowing colorless liquid. It is soluble in polar organic solvents (e.g. nitrobenzene, acetic acid, and ethyl acetate), but poorly soluble in nonpolar solvents such as alkanes. Reflecting its strong acidity, it dissolves almost all organic compounds that are even weak proton acceptors.[2] HSO3F hydrolyzes slowly to HF and sulfuric acid. The related triflic acid (CF3SO3H) retains the high acidity of HSO3F but is more hydrolytically stable. The self-ionization of fluorosulfonic acid also occurs:
- 2 HSO3F ⇌ [H2SO3F]+ + [SO3F]− K = 4.0 × 10−8 (at 298 K)
Production
Fluorosulfuric acid is prepared by the reaction of HF and sulfur trioxide:[1]
- SO3 + HF → HSO3F
Alternatively, KHF2 or CaF2 can be treated with oleum at 250 °C. Once freed from HF by sweeping with an inert gas, HSO3F can be distilled in a glass apparatus.[3]
Super-acids
HSO3F is one of the strongest known simple Brønsted acids, although carborane-based acids are still stronger.[4] It has an H0 value of −15.1 compared to −12 for sulfuric acid. The combination of HSO3F and the Lewis acid antimony pentafluoride produces "Magic acid", which is a far stronger protonating agent. These acids all fall into the category of "superacids", acids stronger than 100% sulfuric acid.
Applications
HSO3F is useful for regenerating mixtures of HF and H2SO4 for etching lead glass.
HSO3F isomerizes alkanes and the alkylation of hydrocarbons with alkenes,[5] although it is unclear if such applications are of commercial importance. It can also be used as a laboratory fluorinating agent.[3]
Safety
Fluorosulfuric acid is considered to be highly toxic and corrosive. It hydrolyzes to release HF. Addition of water to HSO3F can be violent, similar to the addition of water to sulfuric acid but much more violent.
See also
- Chlorosulfuric acid
- Fluoroboric acid
- Fluoroantimonic acid
- Sulfuryl fluoride
- Methyl fluorosulfonate, an organic ester of FSO3H
- Fluorosulfonylamine FSO2NH2, the formal acid amide
References
- 1 2 Erhardt Tabel, Eberhard Zirngiebl, Joachim Maas "Fluorosulfuric Acid" in "Ullmann's Encyclopedia of Industrial Chemistry" 2005, Wiley-VCH, Weinheim. doi:10.1002/14356007.a11_431
- ↑ Olah, G. A.; Prakash, G. K.; Wang, Q.; Li, X.-Y. (2001). "Fluorosulfuric Acid". Encyclopedia of Reagents for Synthesis. John Wiley & Sons. doi:10.1002/047084289X.rf014.
- 1 2 Cotton, F. A.; Wilkinson, G. (1980). Advanced Inorganic Chemistry (4th ed.). New York: Wiley. p. 246. ISBN 0-471-02775-8.
- ↑ Christopher A. Reed "Myths about the Proton. The Nature of H+ in Condensed Media" Acc. Chem. Res., 2013, 46 (11), pp 2567–2575. doi:10.1021/ar400064q
- ↑ Olah, G.; Farooq, O.; Husain, A.; Ding, N.; Trivedi, N.; Olah, J. (1991). "Superacid HSO3F/HF-Catalyzed Butane Isomerisation". Catalysis Letters 10 (3–4): 239–247. doi:10.1007/BF00772077.