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Question

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.

BeF2 is soluble in water while fluorides of other alkaline earth metals are insoluble because of:

A
Covalent nature of BeF2
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B
Ionic nature of BeF2
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C
Greater hydration enthalpy of Be2+ ion
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D
Greater lattice enthalpy of Be2+ ion
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Solution

The correct option is C Greater hydration enthalpy of Be2+ ion
In case of BeF2, Be2+ has high hydration enthalpy which can overcome the lattice enthalpy which makes it soluble. However in case of other alkaline earth metals, hydration enthalpy is not that high.

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