The solubility of metal halides depends on their nature, lattice enthalpy and hydration enthalpy of the individual ions. Amongst flurides of alkali metals, the lowest solubility of LiF in water is due to
(a) Ionic nature fo lithium fluoride
(b) high lattice enthalpy
(c) high hydration enthalpy for lithium ion
(d) low ionisation enthalpy of lithium atom
The solubility of metal halides depends on their nature, lattice enthalpy and hydration enthalpy of the individual ions. Amongst flurides of alkali metals, the lowest solubility of LiF in water is due to
(a) Ionic nature fo lithium fluoride
(b) high lattice enthalpy
(c) high hydration enthalpy for lithium ion
(d) low ionisation enthalpy of lithium atom
Solubilities of alkali metal halides in water can be explained in terms of lattice enthalpy and hydration enthalpy. Lower lattice enthalpies and higher hydration enthalpies favour dissolution.
Among fluorides, the order of solubility is LiF < NaF < Kf < RbF < CsF. Low solubility is due to very high lattice energy On moving down in the group LIF to CsF solubility increases because lattice energy decreases, hence the answer is (b) high lattice enthalpy.
Note: Except LiF, other halides fo Lithium are highly soluble in water.
Solubilities of alkali metal halides in water can be explained in terms of lattice enthalpy and hydration enthalpy. Lower lattice enthalpies and higher hydration enthalpies favour dissolution.
Among fluorides, the order of solubility is LiF < NaF < Kf < RbF < CsF. Low solubility is due to very high lattice energy On moving down in the group LIF to CsF solubility increases because lattice energy decreases, hence the answer is (b) high lattice enthalpy.
Note: Except LiF, other halides fo Lithium are highly soluble in water.
