Difficult
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.
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.
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View SolutionThe $K_{H}$ values for some gases at the same temperature '$T$' are given below:
Gas
$K_{H} / \text{kbar}$
$Ar$
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where $K_{H}$ is Henry's Law constant in water. The order of their solubility in water is:
| Gas | $K_{H} / \text{kbar}$ |
|---|---|
| $Ar$ | $40.3$ |
| $CO_{2}$ | $1.67$ |
| $HCHO$ | $1.83 \times 10^{-5}$ |
| $CH_{4}$ | $0.413$ |
where $K_{H}$ is Henry's Law constant in water. The order of their solubility in water is:
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