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

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Solution

The hydration enthalpies of $B e S O_{4} a n d M g S O_{4}$ are quite high because of the small size of $B e^{2 +} a n d M g^{2 +}$ ions.

These hydration enthalpy values are higher than their corresponding lattice enthalpies and therefore $B e S O_{4} a n d M g S O_{4}$ are highly soluble in water.

However, hydration enthalpies of $C a S O_{4}, S r S O_{4} a n d B a S O_{4}$ are not very high as compared to their respective lattice enthalpies and hence these are insoluble in water.

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