Solubility of an ionic compound in water is mainly dependent on:
a.Lattice enthalpy , b. Hydration enthalphy
Both these factors oppose each other and the resultant of these determines the solubility of an ionic compound in water. If lattce enthalpy has greater value, the compound is less soluble.
In case hydration enthalpy has greater value, the compound is highly soluble in water.
`BeF_(2)` is soluble in water while fluorides of other alkaline earth metals are insoluble because of:

Options

A. ionic nature of `BeF_(2)`
B. greater hydration energy of `Be^(2+)` ion as compared to lattice energy
C. covalent nature of `BeF_(2)`
D. none of these

Answer

B

Explanation

Fluorides of alkaline earth metals except `BeF_(2)` are insoluble in water. The solubility of `BeF_(2)` in water is due to higher hydration energy on accound of small size of `Be^(2+)` ion and `F^(-)` ion and high charge density of `Be^(2+)` ion.