10.29. How would you explain the following observations?
(i) BeO is almost insoluble but BeSO4 is soluble in water,
(ii) BaO is soluble but BaSO4is insoluble in water,
(iii) LiI is more soluble than KI in ethanol.
10.29. How would you explain the following observations?
(i) BeO is almost insoluble but BeSO4 is soluble in water,
(ii) BaO is soluble but BaSO4is insoluble in water,
(iii) LiI is more soluble than KI in ethanol.
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1 Answer
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(i) Lattice energy of BeO is comparatively higher than the hydration energy. Therefore, it is almost insoluble in water. Whereas, BeSO4 is ionic in nature and its hydration energy dominates the lattice energy.
(ii) Both BaO and BaSO4 are ionic compounds but the hydration energy of BaO is higher than the lattice energy therefore it is soluble in water.
(iii) Since the size of Li+ ion is very small in comparison to K+ ion, it polarises the electron cloud of I– ion to a great extent. Thus, Lil dissolves in ethanol more easily than the KI.
Similar Questions for you
Li+ has the highest hydration enthalpy.
Hence it is most hydrated
Therefore, Correct order of hydrated radii is Cs+ < Rb+ < K+ < Na+ < Li+
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