A number of ionic compounds e.g. AgCl, CaF_2, | vedclass

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(D) The solubility of an ionic compound in water depends on the balance between its lattice energy and hydration energy.For a compound to dissolve,the

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These molecules have exceptionally high lattice energy

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(D) The solubility of an ionic compound in water depends on the balance between its lattice energy and hydration energy.For a compound to dissolve,the hydration energy must be greater than the lattice energy.In the case of $AgCl, CaF_2,$ and $BaSO_4$,the lattice energy is exceptionally high,which overcomes the hydration energy released during the solvation process.Therefore,these compounds remain insoluble in water.

$I$. Ion-ion	$a$. $1/r$
$II$. Dipole-dipole	$b$. $1/r^{2}$
$III$. London dispersion	$c$. $1/r^{3}$
	$d$. $1/r^{6}$

$A$ number of ionic compounds e.g. $AgCl, CaF_2, BaSO_4$ are insoluble in water. This is because

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