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Statement-1: Lattice energy of BaSO(4) i...

Statement-1: Lattice energy of `BaSO_(4)` is less than its hydration energy.
Statement-2: `|Delta_(L)H^(Theta)|&|Delta_(hyd)H^(Theta)|` both are smaller.

A

Statement-1 is true, statement-2 is true, statement-2 is a correct explanation for statement-1

B

Statement-1 is true, statement-2 is true, statement-2 is not correct explanation for statement-1

C

Statement-1 is true, statement-2 is false

D

Statement-1 is false, statement-2 is true

Text Solution

AI Generated Solution

The correct Answer is:
To analyze the statements regarding the lattice energy and hydration energy of barium sulfate (BaSO₄), we can follow these steps: ### Step 1: Understand the Definitions - **Lattice Energy (ΔLatticeH)**: This is the energy released when gaseous ions combine to form an ionic solid. It is a measure of the strength of the forces between the ions in an ionic solid. - **Hydration Energy (ΔHydH)**: This is the energy released when ions are surrounded by water molecules and solvated. It reflects how well the ions interact with water. **Hint**: Remember that lattice energy is associated with the formation of the solid, while hydration energy is related to the interaction of the solid with water. ### Step 2: Analyze Statement 1 - Statement 1 claims that the lattice energy of BaSO₄ is less than its hydration energy. - If this statement were true, BaSO₄ would be expected to dissolve in water because the energy released during hydration would be greater than the energy required to break the ionic lattice. **Hint**: Consider the solubility of BaSO₄ in water to evaluate this statement. ### Step 3: Check the Solubility of BaSO₄ - BaSO₄ is known to be insoluble in water. This indicates that the lattice energy must be greater than the hydration energy, as the solid does not dissolve. **Hint**: Use the known solubility rules for sulfates to confirm the behavior of BaSO₄. ### Step 4: Analyze Statement 2 - Statement 2 claims that the magnitudes of lattice energy and hydration energy are similar. - While both energies can be significant, the fact that BaSO₄ is insoluble suggests that the lattice energy is greater than the hydration energy, making this statement incorrect as well. **Hint**: Compare the relative magnitudes of these energies based on the solubility behavior. ### Step 5: Conclusion - Both statements are incorrect: - Statement 1 is false because the lattice energy of BaSO₄ is greater than its hydration energy. - Statement 2 is also false because the energies are not similar; the lattice energy is significantly higher than the hydration energy. **Final Answer**: Both statements are false.
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