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Lattice enthalpy for $\mathrm{NaCl}$ is $+788 \mathrm{~kJ} \mathrm{~mol}^{-1}$ and $\Delta H_{\text {hyd }}^{\circ}=-784 \mathrm{~kJ} \mathrm{~mol}^{-1}$. Enthalpy of solution of $\mathrm{NaCl}$ is
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$+4 \mathrm{~kJ} \mathrm{~mol}^{-1}$
$\Delta H_{\text {sol }}=\Delta H_{\text {lattice }}+\Delta H_{\text {hydration }}$
$=788+(-784)=4 \mathrm{~kJ} \mathrm{~mol}^{-1}$
$=788+(-784)=4 \mathrm{~kJ} \mathrm{~mol}^{-1}$
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