Observe the following statements:Statement-I: | vedclass

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(B) Statement-$I$ is correct because both $LiF$ and $CsI$ exhibit low solubility in water compared to other alkali metal halides.Statement-$II$ is inc

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Statement $I$ is correct, but statement $II$ is not correct

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(B) Statement-$I$ is correct because both $LiF$ and $CsI$ exhibit low solubility in water compared to other alkali metal halides.Statement-$II$ is incorrect because the reasons provided are swapped. The low solubility of $LiF$ is primarily due to its very high lattice enthalpy (because both $Li^+$ and $F^-$ are very small), while the low solubility of $CsI$ is due to its smaller hydration enthalpy (because both $Cs^+$ and $I^-$ are very large, leading to weak ion-dipole interactions with water).Therefore, Statement-$I$ is correct, but Statement-$II$ is not correct.

Observe the following statements:
Statement-$I$: Both $LiF$ and $CsI$ have low solubility in water.
Statement-$II$: Low solubility of $LiF$ in water is due to its high lattice enthalpy, and that of $CsI$ is due to its smaller hydration enthalpy of ions.

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Observe the following statements:Statement-$I$: Both $LiF$ and $CsI$ have low solubility in water.Statement-$II$: Low solubility of $LiF$ in water is due to its high lattice enthalpy, and that of $CsI$ is due to its smaller hydration enthalpy of ions.