Fluoroantimonic acid

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Fluoroantimonic acid
H2FSbF6.png
Fluoroantimonic acid-3D-balls.png
Names
IUPAC name
Fluoroantimonic acid
Systematic IUPAC name
Fluoranium hexafluorostibanuide
Fluoranium hexafluoridoantimonate(1−)
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.037.279
EC Number 241-023-8
Properties
H
2
SbF
7
Molar mass 256.765
Appearance Colorless liquid
Density 2.885 g/cm3
Solubility SO2ClF, SO2
Acidity (pKa) −31.3
Basicity (pKb) 39
Hazards
Main hazards Extremely corrosive, Violent hydrolysis
H300, H310, H314, H330, H411
P260, P264, P273, P280, P284, P301+310
NFPA 704
Flammability code 0: Will not burn. E.g., water Health code 4: Very short exposure could cause death or major residual injury. E.g., VX gas Reactivity code 3: Capable of detonation or explosive decomposition but requires a strong initiating source, must be heated under confinement before initiation, reacts explosively with water, or will detonate if severely shocked. E.g., fluorine Special hazard W: Reacts with water in an unusual or dangerous manner. E.g., cesium, sodiumNFPA 704 four-colored diamond
Related compounds
Related acids
Antimony pentafluoride

Hydrogen fluoride
Magic acid

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Fluoroantimonic acid is an inorganic compound with the chemical formula H
2
FSbF
6
(also written H
2
F[SbF
6
]
, 2HF·SbF5, or simply HF-SbF5). It is an ionic liquid produced by treating hydrogen fluoride (HF) with antimony pentafluoride (SbF5) in a stoichiometric ratio of 2:1. It is the strongest superacid.[1][2] It has been shown to protonate even hydrocarbons to afford pentacoordinate carbocations.[3] Similar acids can be created by using excess antimony pentafluoride.[4]

The reaction to produce fluoroantimonic acid is:

SbF5 + 2 HF → SbF
6
+ H2F+

The acid is often said to contain "naked protons", but the "free" protons are, in fact, always bonded to hydrogen fluoride molecules to make the fluoronium cations (similar to the hydronium cation in aqueous solution).[5] It is the fluoronium ion that accounts for fluoroantimonic acid's extreme acidity. Fluoroantimonic acid is 1016 (10 quadrillion) times stronger than 100% sulfuric acid.[6] The protons easily migrate through the solution, moving from H2F+ to HF, when present, by the Grotthuss mechanism:

H2F+ + HF ⇌ HF + H2F+

Fluoroantimonic acid thermally decomposes at higher temperatures, generating hydrogen fluoride gas.

Structure[edit]

Two related products have been crystallized from HF-SbF5 mixtures, and both have been analyzed by single crystal X-ray crystallography. These salts have the formulas [H
2
F+
][Sb
2
F
11
]
and [H
3
F+
2
][Sb
2
F
11
]
. In both salts, the anion is Sb
2
F
11
.[7] As mentioned above, SbF
6
is weakly basic; the larger anion Sb
2
F
11
is expected to be still weaker.

The following values show that fluoroantimonic acid is much stronger than other superacids.[8] are based upon the Hammett acidity function. Increased acidity is indicated by smaller (in this case, more negative) values of H0.

Applications[edit]

This extraordinarily strong acid protonates nearly all organic compounds. In 1967, Bickel and Hogeveen showed that 2HF·SbF5 will remove H2 from isobutane and methane from neopentane to form carbenium ions:[9][10]

(CH3)3CH + H+ → (CH3)3C+ + H2
(CH3)4C + H+ → (CH3)3C+ + CH4

Materials compatible with fluoroantimonic acid as a solvent include SO2ClF, and sulfur dioxide; some chlorofluorocarbons have also been used. Containers for HF-SbF5 are made of PTFE.

Safety[edit]

HF-SbF5 is extremely corrosive, toxic, and moisture sensitive.[4] Like most strong acids, fluoroantimonic acid can react violently with water, owing to the exothermic hydration. Consequently, it cannot be used in aqueous solution, only in hydrogen fluoride as solvent.

See also[edit]

References[edit]

  1. ^ "What Is the World's Strongest Superacid?". ThoughtCo.com. 
  2. ^ Gillespie, R. J.; Peel, T. E. (1973-08-01). "Hammett acidity function for some superacid systems. II. Systems sulfuric acid-[fsa], potassium fluorosulfate-[fsa], [fsa]-sulfur trioxide, [fsa]-arsenic pentafluoride, [sfa]-antimony pentafluoride and [fsa]-antimony pentafluoride-sulfur trioxide". Journal of the American Chemical Society. 95 (16): 5173–5178. doi:10.1021/ja00797a013. ISSN 0002-7863. 
  3. ^ Olah, G. A. (2001). A Life of Magic Chemistry: Autobiographical Reflections of a Nobel Prize Winner. John Wiley and Sons. pp. 100–101. ISBN 0-471-15743-0. 
  4. ^ a b Olah, G. A.; Prakash, G. K. Surya; Wang, Qi; Li, Xing-ya (15 April 2001). "Hydrogen Fluoride–Antimony(V) Fluoride". Encyclopedia of Reagents for Organic Synthesis. New York: John Wiley and Sons. doi:10.1002/047084289X.rh037m. ISBN 9780470842898. 
  5. ^ Klein, Michael L. (October 25, 2000). "Getting the Jump on Superacids" (pdf). Pittsburgh Supercomputing Center (PSC). Retrieved 2012-04-15. 
  6. ^ Olah, G. A. (2005). "Crossing Conventional Boundaries in Half a Century of Research". Journal of Organic Chemistry. 70 (7): 2413–2429. doi:10.1021/jo040285o. PMID 15787527. 
  7. ^ Mootz, Dietrich; Bartmann, Klemens (March 1988). "The Fluoronium Ions H2F+ and H
    3
    F+
    2
    : Characterization by Crystal Structure Analysis". Angewandte Chemie International Edition. 27 (3): 391–392. doi:10.1002/anie.198803911.
     
  8. ^ Gillespie, R. J.; Peel, T. E. (1973-08-01). "Hammett acidity function for some superacid systems. II. Systems sulfuric acid-[fsa], potassium fluorosulfate-[fsa], [fsa]-sulfur trioxide, [fsa]-arsenic pentafluoride, [sfa]-antimony pentafluoride and [fsa]-antimony pentafluoride-sulfur trioxide". Journal of the American Chemical Society. 95 (16): 5173–5178. doi:10.1021/ja00797a013. ISSN 0002-7863. 
  9. ^ Bickel, A. F.; Gaasbeek, C. J.; Hogeveen, H.; Oelderik, J. M.; Platteeuw, J. C. (1967). "Chemistry and spectroscopy in strongly acidic solutions: reversible reaction between aliphatic carbonium ions and hydrogen". Chemical Communications. 1967 (13): 634–635. doi:10.1039/C19670000634. 
  10. ^ Hogeveen, H.; Bickel, A. F. (1967). "Chemistry and spectroscopy in strongly acidic solutions: electrophilic substitution at alkane-carbon by protons". Chemical Communications. 1967 (13): 635–636. doi:10.1039/C19670000635.