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Question

The increasing order of acidity of pentafluorides (SbF5, NbF5, PF5, AsF5 and TaF5) in fluorosulphonic acid is :

The correct answer is

SbF5 > AsF5 > TaF5 > NbF5 > PF5

In fluorosulphonic acid, HSO3F, a pentafluoride acts as a Lewis acid by accepting a fluoride (or fluorosulfate) ion, which shifts the self-ionisation and raises the concentration of the protonated solvent H2SO3F+: \(2HSO_{3}F + MF_{5} \rightleftharpoons H_{2}SO_{3}F^{+} + [MF_{5}(SO_{3}F)]^{-}\).

The stronger the fluoride-ion acceptor (Lewis acid), the more stable its anion and the larger the increase in acidity. Conductivity and Hammett acidity measurements (Gillespie) give the acid-enhancing order SbF5 > AsF5 > TaF5 > NbF5 > PF5.

SbF5 is the strongest known fluoride acceptor (it forms "magic acid" with HSO3F); AsF5 is somewhat weaker; the heavier group 5 fluorides TaF5 and NbF5 are moderate acceptors, with TaF5 the stronger; and PF5, with a small central atom, is the weakest acceptor in the series.

Orders placing PF5 above TaF5 and NbF5, treating TaF5 and NbF5 as equal, or reversing the whole series do not agree with these measurements.

Therefore the acidity order is SbF5 > AsF5 > TaF5 > NbF5 > PF5.

Hence, SbF5 > AsF5 > TaF5 > NbF5 > PF5.

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