BeO is almost insoluble but BeSO₄ is soluble in water?

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Solution

Beryllium sulphate is soluble in water because it has high hydration energy as the size of Be²⁺ ion is small. It lattice enthalpy is smaller than its hydration energy making it soluble in water.
In case of BeO, Be²⁺ is a small cation with high polarising power. Also, O^2- is a small anion. So the lattice energy released during their formation is also very high. Their hydration energy is not large enough to overcome them lattice energy to make them insoluble in water.

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How would you explain the following observations?

(i) BeO is almost insoluble but BeSO₄ in soluble in water,

(ii) BaO is soluble but BaSO₄ is insoluble in water,

(iii) LiI is more soluble than KI in ethanol.

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