A) \[CaS{{O}_{4}}>BaS{{O}_{4}}>BeS{{O}_{4}}>MgS{{O}_{4}}>SrS{{O}_{4}}\]
B) \[BeS{{O}_{4}}>MgS{{O}_{4}}>CaS{{O}_{4}}>SrS{{O}_{4}}\]\[>BaS{{O}_{4}}\]
C) \[BaS{{O}_{4}}>SrS{{O}_{4}}>CaS{{O}_{4}}>MgS{{O}_{4}}\]\[>BaS{{O}_{4}}\]
D) \[BeS{{O}_{4}}>CaS{{O}_{4}}>MgS{{O}_{4}}>SrS{{O}_{4}}\]\[>BaS{{O}_{4}}\]
Correct Answer: B
Solution :
[b]: The solubilities of sulphates of alkaline earth metals decrease down the group because the hydration enthalpy decreases from \[B{{e}^{2+}}\]to \[B{{a}^{2+}}\]appreciably as the size of the cation increases. As the sulphate ion is too big, the magnitude of lattice enthalpy almost remains constant on moving down the group. So, the correct order of solubility in water is \[BeS{{O}_{4}}>MgS{{O}_{4}}>CaS{{O}_{4}}>SrS{{O}_{4}}>BaS{{O}_{4}}.\]
You need to login to perform this action.
You will be redirected in
3 sec
