Which of the following compounds has a positi | vedclass

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(A) The enthalpy of solution $(\Delta H_{sol})$ is the sum of lattice energy $(\Delta H_{lattice})$ and hydration energy $(\Delta H_{hyd})$. For $LiF$

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$LiF$

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(A) The enthalpy of solution $(\Delta H_{sol})$ is the sum of lattice energy $(\Delta H_{lattice})$ and hydration energy $(\Delta H_{hyd})$. For $LiF$,the lattice energy is very high due to the small size of both $Li^+$ and $F^-$ ions. Since the lattice energy is significantly higher than the hydration energy,the overall enthalpy of solution for $LiF$ is positive,making it sparingly soluble in water at room temperature.

Which of the following compounds has a positive enthalpy of solution?

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