Which of the following compounds has a negati | vedclass

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(C) The enthalpy of solution $(\Delta H_{sol})$ is the sum of the lattice enthalpy and the hydration enthalpy. For alkali metal halides,as the size of

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$KF$

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(C) The enthalpy of solution $(\Delta H_{sol})$ is the sum of the lattice enthalpy and the hydration enthalpy. For alkali metal halides,as the size of the anion increases,the lattice enthalpy decreases significantly. However,the hydration enthalpy also decreases as the anion size increases. $F^-$ is a small anion,which results in a very high hydration enthalpy. This high hydration energy released during the dissolution of $KF$ outweighs the lattice energy,making the overall enthalpy of solution negative (exothermic). For other halides like $KCl$,$KBr$,and $KI$,the lattice energy is relatively lower,but the hydration energy is not high enough to make the process exothermic,resulting in a positive enthalpy of solution.

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

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