❓ Question The <strong data-end="210" data-start="188"> hydration energies</strong> of K + \text{K}^+  and Cl − \text{Cl}^-  are − x -x  and − y  kJ/mol -y~\text{kJ/mol}  respectively. If the <strong data-end="334" data-start="316"> lattice energy</strong> of KCl is − z  kJ/mol -z~\text{kJ/mol} , then what is the <strong data-end="406" data-start="386"> heat of solution</strong> of KCl? đź–Ľ️ Question Image ✍️ Short Explanation This problem is based on: 👉 Enthalpy of solution 👉 Lattice energy 👉 Hydration energy. Main idea: Heat of solution: Δ H sol = Lattice dissociation energy + Hydration energies \boxed{ \Delta H_{\text{sol}} = \text{Lattice dissociation energy} + \text{Hydration energies} } đź”· Step 1 — Understand Sign Convention đź’Ż Given: Hydration energy of: K + = − x K^+=-x C l − = − y Cl^-=-y Lattice energy of KCl: − z -z This corresponds to lattice formation. For dissolving crystal, we need lattice dissociation energy: + z +z đź”· Step 2 — Write Enthalpy of Solution Δ H sol = ( + z ) + ( − x ) + ( − y ) \Delta H_{\text{sol}} = (+z)+(-x)+(-y) = z − x − y = z-x-y z − ( x + y ) \boxed{ z-(x+y) } đź”· Step 3 — Physical Meaning Solution process has two parts: Breaking crystal lattice ✔ Requires energy + z +z Hydration of ions ✔ Rel…
