How would you explain the following observations ?
(i) BeO is almost insoluble but `BeSO_(4)` is soluble in water
(ii) BaO is soluble but `BaSO_(4)` is insoluble in water
(iii) LiI is more soluble than KI in ethanol

Explanation

(i) BeO is almost insoluble in water and `BeSO_(4)` is soluble in water `Be^(2+)` is a small cation with a high polarising power and `O^(2-)` is a small anion The size compatibility of `Be^(2+)` and `O^(2-)` is high. Therefore, the lattice energy released during their formation is also very high. When BeO is dissolved in water, the hydration enegy of its ions is not sufficient to overcome the high lattice energy. Therefore BeO is insoluble in water. On the other hand `SO_(4)^(2-)` ion is a large anion. Hence, `Be^(2+)` can easily polarise `SO_(4)^(2-)` ions, making `BeSO_(4)` unstable thus, the lattice energy at `BeSO_(4)` is not very high and so it is soluble in water
(ii) BaO is soluble in water, but `BaSO_(4)` is not `Ba^(2+)` is a large cation and `O^(2-)` is a small anion. The size compatibility of `Ba^(2+)` and `O^(2-)` is not high. As a result, BaO is unstable. The lattice energy released during its formation is also not very large. It can easily be overcome by the hydration energy of the ions. Therefore, BaO is soluble in water. In `BaSO_(4), Ba^(2+)` and `SO_(4)^(2-)` are both large sized the lattice energy released is high Hence, it is not soluble in water
(iii) LiI is more soluble than KI in ethanol. As a result of its small size, the lithium ion has a higher polarising power than the potassium ion. It polarises the electron cloud of the iodide ion to a much greater extent than the potassium ion. This causes a greater covalent character in LiI than in KI. Hence, LiI is more soluble in ethanol.