Hexafluorophosphoric acid

Hexafluorophosphoric acid^[1]
Names
	IUPAC name Hydrogen hexafluorophosphate
	Other names Hexafluorophosphoric acid
Identifiers
CAS Number	16940-81-1 ;
3D model (JSmol)	Interactive image;
ChemSpider	17339451 ;
ECHA InfoCard	100.037.263
EC Number	241-006-5;
PubChem CID	16211447;
CompTox Dashboard (EPA)	DTXSID40884947 ;
	InChI InChI=1S/F6P/c1-7(2,3,4,5)6/q-1/p+1 Key: LJQLCJWAZJINEB-UHFFFAOYSA-O ; InChI=1/F6P/c1-7(2,3,4,5)6/q-1/p+1 Key: LJQLCJWAZJINEB-IKLDFBCSAL;
	SMILES [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
Solubility in water	reacts
Hazards
	Occupational safety and health (OHS/OSH):
Main hazards	Template:Hazchem 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]

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.
^ ^a ^b 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.

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[hand-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 0-471-59668-X.

[davidson-3] 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.

[1]

[2]

[3]

See also

References