BeSO₄ is water soluble while CaSO₄ is not. This is because of:

Q. 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:

Q. Solubility of an ionic compound in water is mainly dependent on:
a. Lattice enthalpy
b. Hydration enthalpy
Both these factors oppose each other, and the resultant of these factors determines the solubility of an ionic compound in water. If the lattice enthalpy has a larger value, the compound is less soluble. If the hydration enthalpy has larger value, the compound is highly soluble in water.

$Be{F}_2$ is soluble in water while fluorides of other alkaline earth metals are insoluble because of:

Q. Assertion :$BeS{O}_4$ and $MgS{O}_4$ are insoluble in water. Reason: $B{e}^{2+}$ and $M{g}^{2+}$ have low hydration enthalpies.

Q. Solubility of an ionic compound in water is mainly dependent on:
a. Lattice enthalpy
b. Hydration enthalpy
Both these factors oppose each other, and the resultant of these factors determines the solubility of an ionic compound in water. If the lattice enthalpy has a larger value, the compound is less soluble. If the hydration enthalpy has larger value, the compound is highly soluble in water.

A compound is soluble in water if the hydration enthalpy is:

Q. Solubility of an ionic compound in water is mainly dependent on:
a. Lattice enthalpy
b. Hydration enthalpy
Both these factors oppose each other, and the resultant of these factors determines the solubility of an ionic compound in water. If the lattice enthalpy has a larger value, the compound is less soluble. If the hydration enthalpy has larger value, the compound is highly soluble in water.

$Be{F}_2$ is soluble in water while fluorides of other alkaline earth metals are insoluble because of: