Which one of the following is true about NaCl | vedclass

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(D) The melting point of an ionic compound depends on the lattice energy.
Since the ionic radius of $Na^{+}$ $(0.95 \ \mathring{A})$ is smaller than

Vedclass · Accepted Answer

Melting point of $NaCl$ is higher than $M.P.$ of $KCl$ but solubility of $NaCl$ is lower as compared to $KCl$.

Vedclass · Answer

(D) The melting point of an ionic compound depends on the lattice energy.
Since the ionic radius of $Na^{+}$ $(0.95 \ \mathring{A})$ is smaller than $K^{+}$ $(1.33 \ \mathring{A})$,the lattice energy of $NaCl$ is higher than that of $KCl$,resulting in a higher melting point for $NaCl$.
Regarding solubility,$KCl$ is more soluble in water than $NaCl$ because the hydration energy of $K^{+}$ and $Cl^{-}$ ions is more favorable relative to the lattice energy compared to $NaCl$.
Therefore,$NaCl$ has a higher melting point but lower solubility than $KCl$.

Which one of the following is true about $NaCl$ and $KCl$?

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