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(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.
Asked by Balakrishnasingh Last Modified
Answer 
Harshit Bhardwaj
(i) BeO is almost insoluble in water and BeSO4 is soluble in water. Be2+ is a small cation with a high polarising power and O2– is a small anion. The size compatibility of Be2+ and O2– is high. Therefore, the lattice energy released during their formation is also very high. When BeO is dissolved in water, the hydration energy of its ions is not sufficient to overcome the high lattice energy. Therefore, BeO is insoluble in water. On the other hand, 
ion is a large anion. Hence, Be2+ can easily polarise ions, making BeSO4 unstable. Thus, the lattice energy of BeSO4 is not very high and so it is soluble in water.
(ii) BaO is soluble in water, but BaSO4 is not. Ba2+ is a large cation and O2– is a small anion. The size compatibility of Ba2+ and O2– 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 BaSO4, Ba2+ and 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.
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BeO is almost insoluble in water and BeSO4is soluble in water. Be2+is a small cationwith a high polarising power and O2–is a small anion. The size compatibility of Be2+andO2–is high. Therefore, the lattice energy released during their formation is also veryhigh. When BeO is dissolved in water, the hydration energy of its ions is not sufficient toovercome the high lattice energy. Therefore, BeO is insoluble in water.
read less (i)The lattice energy of BeO is more significant than its hydration energy so, it is insoluble in water. While in the case of BeSO4, the hydration energy is greater than the lattice energy, so, it is readily soluble in water.
(ii) The lattice energy of BaO is much smaller than that of its hydration energy. So it is soluble in water. In BaSO4, lattice energy predominates over hydration energy so, it is insoluble in water.
(iii) According to Fazan's rule, covalent characters on LI is more than KI, and we know, the covalent compound is soluble in covalent compound very quickly. That's the reason LiI is more soluble than KI in ethanol(covalent compound).
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