Statement - I : BeSO₄ and MgSO₄ are readily soluble in water
Statement - I I : The greater hydration enthalpy of Be²⁺ and Mg²⁺ ions overcome the lattice enthalpy of BeSO₄ and MgSO₄

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Statement I and II are correct and II explains I

Statement I and II are correct and II does not explain I

Statement I is correct and Statement II is incorrect

Both statement I and II are incorrect

answer is A.

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Detailed Solution

If anion size is large [SO⁻²₄,CO⁻²₃]
then with small change in size of cation there is no considerable change in lattice energy, in such cases the solubility depends upon the hydration energy. As the size of metal ion increases hydration energy decreases, Therefore solubility decreases and hence BeSO₄ , MgSO₄& BeCO₃ ; MgCO₃are highly soluble, where as BaSO₄, BaCO₃ almost all insoluble
Hydration energy α Solubility.