Question
How would you explain the following observations?
BaO is soluble but $\mathrm{BaSO}_4$ is insoluble in water.
BaO is soluble but $\mathrm{BaSO}_4$ is insoluble in water.
✓
Answer
BaO is soluble in water, but $\mathrm{BaSO}_4$ is not. $\mathrm{Ba}^{2+}$ is a large cation and $\mathrm{O}^{2-}$ is a small anion. The size compatibility of $\mathrm{Ba}^{2+}$ and $\mathrm{O}^{2-}$ 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 $\mathrm{BaSO}_4$ $\mathrm{Ba}^{2+}$ and $\mathrm{SO}_4^{2-}$ are both large-sized. The lattice energy released is high. Hence, it is not soluble in water.
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