Observe the following statements:Statement-I: | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(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

Vedclass · Accepted Answer

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

Vedclass · Answer

(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.

Similar Questions

Write a note on halides of alkali metal elements and their physical properties.

Which elements of group $1$ and $2$ differ from the other elements of the same group? Give a brief explanation of the diagonal relationship.

Which of the following is a property of alkali metals?

All compounds of alkali metals are easily soluble in water,but lithium compounds are more soluble in organic solvents. Explain.

Which of the following is the correct order of increasing solubility for the given compounds?

Vedclass Test Series

Exam Paper Generator

Online Exam Module

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.