Explain the factors affecting the solubility of salts in a solution.

(N/A) The solubility of ionic solids in water varies significantly.
Some ionic solids,such as $CaF_2$,are highly soluble,while others like $LiF$ (lithium fluoride) have very low solubility and are considered insoluble. The solubility of a salt depends on two primary factors:
$(i)$ Lattice enthalpy of the salt: This is the energy required to break one mole of a solid salt into its constituent ions. $A$ higher lattice enthalpy means more energy is needed to break the crystal lattice.
$(ii)$ Solvation enthalpy of ions: This is the energy released when one mole of a solid salt dissolves in a solvent. For a salt to dissolve,the energy released from ion-solvent interactions (solvation enthalpy) must be sufficient to overcome the strong electrostatic forces holding the ions together in the crystal lattice (lattice enthalpy).
Therefore,a salt is soluble in a solvent only when the solvation enthalpy is greater than the lattice enthalpy. If the solvation enthalpy is less than the lattice enthalpy,the salt remains insoluble.