A) \[BeS{{O}_{4}}>MgS{{O}_{4}}>CaS{{O}_{4}}>SrS{{O}_{4}}>BaS{{O}_{4}}\]
B) \[BeS{{O}_{4}}>SrS{{O}_{4}}>CaS{{O}_{4}}>MgS{{O}_{4}}>BeS{{O}_{4}}\]
C) \[BeS{{O}_{4}}>CaS{{O}_{4}}>SrS{{O}_{4}}>BeS{{O}_{4}}>MgS{{O}_{4}}\]
D) \[BaS{{O}_{4}}>SrS{{O}_{4}}>MgS{{O}_{4}}>CaS{{O}_{4}}>BeS{{O}_{4}}\]
Correct Answer: A
Solution :
The solubility of the sulphates in water decreases down the group \[\underbrace{BeS{{O}_{4}}>MgS{{O}_{4}}}_{Soluble}>\underbrace{CaS{{O}_{4}}}_{\begin{smallmatrix} Sparingly \\ Soluble \end{smallmatrix}}>\underbrace{SrS{{O}_{4}}>BaS{{O}_{4}}}_{Insoluble}\] The high solubilities of \[BeS{{O}_{4}}\] and \[MgS{{O}_{4}}\] are due to the high enthalpy of hydration of the: smaller \[B{{e}^{2+}}\] and \[M{{g}^{2+}}\] ions, which overcomes the lattice energy factor.
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