Hexafluorophosphoric acid

From Wikipedia, the free encyclopedia
Hexafluorophosphoric acid[1]
Names
IUPAC name
Hydrogen hexafluorophosphate
Other names
Hexafluorophosphoric acid
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.037.263 Edit this at Wikidata
EC Number
  • 241-006-5
  • InChI=1S/F6P/c1-7(2,3,4,5)6/q-1/p+1 ☒N
    Key: LJQLCJWAZJINEB-UHFFFAOYSA-O ☒N
  • InChI=1/F6P/c1-7(2,3,4,5)6/q-1/p+1
    Key: LJQLCJWAZJINEB-IKLDFBCSAL
  • [H+].F[P-](F)(F)(F)(F)F
Properties
Chemical formula
 HPF6
Molar mass 145.972 g/mol
Appearance colorless oily liquid
Melting point decomposes at 25 °C
exists only in solution
Hazards
Main hazards Corrosive
GHS labelling:
GHS05: CorrosiveGHS06: Toxic
Signal word
 Danger
H301, H311, H314, H330
P260, P264, P271, P280, P284, P301+P330+P331, P303+P361+P353, P304+P340, P305+P351+P338, P310, P320, P321, P363, P403+P233, P405, P501
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N  (what is checkY☒N ?)
Infobox references

Hexafluorophosphoric acid is the inorganic compound with the chemical formula HPF
6 (also written H[PF
6]). 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. It exothermically reacts with water to produce oxonium hexafluorophosphate (H
3OPF
6) and hydrofluoric acid. 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[]

  1. ^ Lide, David R. (1998). Handbook of Chemistry and Physics (87 ed.). Boca Raton, FL: CRC Press. pp. 4–74. ISBN 0-8493-0594-2.
  2. ^ Arpad Molnar; G. K. Surya Prakash; Jean Sommer (2009). Superacid Chemistry (2nd ed.). Wiley-Interscience. p. 44. ISBN 978-0-471-59668-4.
  3. ^ a b D. W. Davidson; S. K. Garg (May 1972). "The Hydrate of Hexafluorophosphoric Acid". Canadian Journal of Chemistry. 50 (21): 3515–3520. doi:10.1139/v72-565.
Retrieved from ""