Identify the correct order of solubility in aqueous medium:

B e S O_{4} > M g S O_{4} > C a S O_{4} > B a S O_{4}

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B e S O_{4} > C a S O_{4} > M g S O_{4} > B a S O_{4}

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B e S O_{4} < C a S O_{4} < M g S O_{4} < B a S O_{4}

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C a S O_{4} < B e S O_{4} < M g S O_{4} < B a S O_{4}

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Solution

The correct option is A $B e S O_{4} > M g S O_{4} > C a S O_{4} > B a S O_{4}$
As we move down the group, size increases $(B e < M g < C a < B a)$ . Solubility depends on the hydration energy and the latiice energy. Generally, as the difference in size of the cation and the anion increases, hydration energy dominates and solubility increases. Whereas, as the difference decreases, lattice energy dominates and solubility decreases.
So, here we have $S O_{4}^{2 -}$ anion whose size is large and as we move down the group, size difference decreases and hence solubility decreases.

Hence the order is : $B e S O_{4} > M g S O_{4} > C a S O_{4} > B a S O_{4}$

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