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Question
How would you explain the following observation?
BaO is soluble but BaSO4 is insoluble in water.
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Solution
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 `"SO"_4^(2-)` are both large-sized. The lattice energy released is high. Hence, it is not soluble in water.
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