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(B) The solubility of an ionic compound in water is determined by the balance between its lattice enthalpy and hydration enthalpy. For a salt to be so

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High lattice enthalpy

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(B) The solubility of an ionic compound in water is determined by the balance between its lattice enthalpy and hydration enthalpy. For a salt to be soluble,the hydration enthalpy must be sufficient to overcome the lattice enthalpy. In the case of $LiF$,the $Li^{+}$ ion is very small,leading to a very strong electrostatic attraction with the $F^{-}$ ion. This results in a very high lattice enthalpy for $LiF$,which is not compensated by the hydration enthalpy,making it the least soluble among alkali metal fluorides.

The solubility of metal halides depends on their nature,lattice enthalpy and hydration enthalpy of the individual ions. Amongst fluorides of alkali metals,the lowest solubility of $LiF$ in water is due to

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