|Systematic IUPAC name
|Jmol 3D model||Interactive image|
|Main hazards||Extremely corrosive, Violent hydrolysis|
|H300, H310, H314, H330, H411|
|P260, P264, P273, P280, P284, P301+310|
|R-phrases||R26, R29, R35|
|S-phrases||(S1/2), S36/37/39, S45, S53, S60, S61|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|what is ?)(|
Fluoroantimonic acid (systematically named fluoranium hexafluorostibanuide and fluoranium hexafluoridoantimonate(1−)) is an inorganic compound with the chemical formula H
6 (also written H
6], 2HF·SbF5, or simply HF-SbF5). It is an ionic liquid created by reacting hydrogen fluoride (HF) with antimony pentafluoride (SbF5) in a stoichiometric ratio of 2:1. It is the strongest known superacid, which has been demonstrated to protonate even hydrocarbons to afford carbocations and H2. Similar acids can be created by using excess antimony pentafluoride.
The reaction to produce fluoroantimonic acid is:
- 2 HF ⇌ H2F+ + F−
- SbF5 + F− → SbF−
The overall reaction is:
- SbF5 + 2 HF → SbF−
6 + H2F+
The second reaction is not in equilibrium, therefore the overall reaction is not in equilibrium. The reaction is exothermic.
The F−, produced by autoionization of hydrogen fluoride, reacts with SbF5 to yield the adduct SbF−
6. In the fluoronium ion, hydrogen fluoride is coordinated to the hydrogen ion. The anion is classified as noncoordinating and is both a very weak nucleophile and a very weak base.
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). 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. 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.
Two related products have been crystallised from HF-SbF5 mixtures, and both have been analyzed by single crystal X-ray crystallography. These salts have the formulas [H
11] and [H
11]. In both salts, the anion is Sb
11. As mentioned above, SbF−
6 is weakly basic; the larger anion Sb
11 is expected to be still weaker.
- Fluoroantimonic acid (1990) (H0 value = −31.3)
- Magic acid (1974) (H0 value = −19.2)
- Carborane acid (1969) (H0 value = −18.0)
- Fluorosulfuric acid (1944) (H0 value = −15.1)
- Triflic acid (1940) (H0 value = −14.9)
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:
- (CH3)3CH + H+ → (CH3)3C+ + H2
- (CH3)4C + H+ → (CH3)3C+ + CH4
HF-SbF5 is extremely corrosive, toxic, and moisture sensitive. 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 hydrofluoric solution.
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