Why does hf not dissociate in water

Clicking on the donut icon will load a page at altmetric. Find more information on the Altmetric Attention Score and how the score is calculated. HF may not be dissociated at 0 K solely by water molecules because the HF H bond is stronger than the OH H bond, against the expectation that the dissociated HF H 2 O n would be more stable than the undissociated one in the presence of a number of water molecules.

The dissociation would be possible for only a fraction of a number of hydrated HF clusters by the Boltzmann distribution at finite temperatures. Corresponding author. Such files may be downloaded by article for research use if there is a public use license linked to the relevant article, that license may permit other uses.

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Journal of the American Chemical Society , 11 , The hydration enthalpy of Fluoride ion is very high. That proves that the hydration enthalpy is sufficient enough to supply required energy for H-F bond breaking, beside producing extra heat.

So I don't understand why HF don't ionise in water, where hydration enthalpy is large enough to promote ionization. HF is water soluble, but it doesn't ionizate because unlike all other hydrogen halogens it doesn't exist in monomolecular form. Instead it forms polymeric structures, chains that are kept together by hydrogen bonds between hydrogen and adjacent molecule's fluoride. I think ATMyller is right. HF is misible in water.

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