Statement I: For all the salts completely soluble in water, the magnitude of sum of enthalpies of hydration of ions is greater than the magnitude of lattice enthalpy of the salt.

Statement II:

Question

Statement I: For all the salts completely soluble in water, the magnitude of sum of enthalpies of hydration of ions is greater than the magnitude of lattice enthalpy of the salt.

Statement II: If the magnitude of sum of enthalpies of hydration of ions is less than the magnitude of lattice enthalpy of the salt, the salt is completely insoluble in water.

Prashant Kotian · Accepted Answer

Correct answer: C. If hydration energy is greater than lattice energy, dissolution is exothermic, which is favorable. However, many endothermic salts (like ) are highly soluble because the positive entropy change of dissolution (ΔS_sol > 0) overcomes the endothermic enthalpy term at room temperature. Thus, Statement II is incorrect. Statement I is correct.

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