A) \[MgS{{O}_{4}}>CaS{{O}_{4}}>BaS{{O}_{4}}>BeS{{O}_{4}}>SrS{{O}_{4}}\]
B) \[BeS{{O}_{4}}>MgS{{O}_{4}}>CaS{{O}_{4}}>SrS{{O}_{4}}>BaS{{O}_{4}}\]
C) \[MgS{{O}_{4}}>BeS{{O}_{4}}>BaS{{O}_{4}}>CaS{{O}_{4}}>SrS{{O}_{4}}\]
D) \[BeS{{O}_{4}}>CaS{{O}_{4}}>MgS{{O}_{4}}>BaS{{O}_{4}}>SrS{{O}_{4}}\]
Correct Answer: B
Solution :
\[BeS{{O}_{4}}>MgS{{O}_{4}}>CaS{{O}_{4}}>SrS{{O}_{4}}>BaS{{O}_{4}}\] is the correct order because on moving down the group, lattice energy remains almost constant as sulphate ion is big and on increase in size of the cations does not make any difference. But hydration energy causes-which decreases from \[B{{e}^{2+}}\] to \[B{{a}^{2+}}\] appreciably as the size of cation increase down the group. Hence, solubility of alkaline earth metal decreases down the group.
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