Hexafluorophosphoric acid
| Names | |
|---|---|
| IUPAC name
Hydrogen hexafluorophosphate | |
| Other names
Hexafluorophosphoric acid | |
| Identifiers | |
16940-81-1  | |
| ChemSpider | 17339451  |
| EC Number | 241-006-5 |
| Jmol interactive 3D | Image |
| PubChem | 16211447 |
| |
| |
| Properties | |
| HPF6 | |
| Molar mass | 145.972 g/mol |
| Appearance | colorless oily liquid |
| Melting point | decomposes at 25 °C |
| reacts | |
| Hazards | |
| Main hazards |  C |
| 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 | |
Hexafluorophosphoric acid is the inorganic compound with the chemical formula H3OPF6. Although the formula is often written as HPF6, this compound is only available as the hydrate. This strong Brønsted acid features a non-coordinating anion, hexafluorophosphate (PF−
6). It is formed from the reaction of hydrogen fluoride with phosphorus pentafluoride.[2]
Like many strong acids, hexafluorophosphoric acid is not isolable but is handled only in solution. Its aqueous solutions consist of hydronium ion, H
3O+
, and PF−
6. Additionally, such solutions often contain products derived from hydrolysis of the P-F bonds, including HPO
2F
2, H
2PO
2F, and H
3PO
4, and their conjugate bases.[3] Hexafluorophosphoric acid attacks glass. Upon heating, it decomposes to generate HF. Crystalline HPF
6 has been obtained as the hexahydrate, wherein PF−
6 is enclosed in truncated octahedral cages defined by the water and protons. NMR spectroscopy indicates that solutions derived from this hexahydrate contain significant amounts of HF.[3]
See also
References
- ↑ Lide, David R. (1998). Handbook of Chemistry and Physics (87 ed.). Boca Raton, FL: CRC Press. pp. 4–74. ISBN 0-8493-0594-2.
- ↑ Arpad Molnar; G. K. Surya Prakash; Jean Sommer (2009). Superacid Chemistry (2nd ed.). Wiley-Interscience. p. 44. ISBN 0-471-59668-X.
- 1 2 D. W. Davidson; S. K. Garg (May 1972). "The Hydrate of Hexafluorophosphoric Acid". Canadian Journal of Chemistry 50: 3515–3520. doi:10.1139/v72-565.