Why are $B e S O_{4}$ and ${M g S O}_{4}$ readily soluble in water while ${C a S O}_{4}, {S r S O}_{4}$ and $B a S O_{4}$ are insoluble?

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Solution

The solubility of sulfates of group 2 elements depends on their hydration energy which decreases down the group. The lattice energy of group 2 sulfates is almost the same. Very high hydration enthalpy ${B e}^{+ 2}$ and ${M g}^{+ 2}$ ions overcome the lattice enthalpy and their sulphates are soluble. However, the hydration enthalpy of ${C a}^{2 +}, {S r}^{2 +}$ and ${B a}^{2 +}$ cannot overcome their lattice enthalpy and remain insoluble in water.

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