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Assertion : $\mathrm{Na}_2 \mathrm{SO}_4$ is soluble in water while $\mathrm{BaSO}_4$ is not.
Reason : Lattice energy of $\mathrm{BaSO}_4$ exceeds its hydration energy.
Options:
Reason : Lattice energy of $\mathrm{BaSO}_4$ exceeds its hydration energy.
Solution:
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The correct answer is:
If both Assertion and Reason are true and Reason is the correct explanation of Assertion.
The large sized sulphate anion $\left(\mathrm{SO}_4{ }^{2-}\right)$ is stabilised better by a large sized cation. So the stability of sulphates down the group increases so the lattice energy is more in $\mathrm{BaSO}_4$ than in $\mathrm{Na}_2 \mathrm{SO}_4$.
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