Statement - I : BeSO4 and MgSO4 are readily soluble in waterStatement - II : The greater hydration enthalpy of Be2+ and Mg2+ ions overcome the lattice enthalpy of BeSO4 and MgSO4

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Statement I and II are correct and II explains I

Statement I and II are correct and II does not explain I

Statement - I is correct and Statement - II is incorrect

Both statement - I and II are incorrect

answer is A.

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Detailed Solution

→ If anion size is large SO4-2,CO3-2 then with small change in size of cation there is no considerable change in lattice energy, in such cases the solubility depends upon the hydration energy. As the size of metal ion increases hydration energy decreases, Therefore solubility decreases and hence BeSO4 , MgSO4 & BeCO3 ; MgCO3 are highly soluble, where as BaSO4, BaCO3 almost all insolubleHydration energy α SolubilityTRICK - I :-In general in all IA group compounds except fluorides & hydroxides solubility down the group decreases.But the two exceptions are carbonates & bicarbonates of IA group where solubility increases down the groupTRICK - II :-More the difference between the sizes of cation and anion then more will be the solubility

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