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(D) The solubility of ionic compounds depends on the balance between lattice energy and hydration energy. $1$. For $MgF_2$ and $MgCl_2$: $MgF_2$ is sp

Vedclass · Accepted Answer

$Ag_2O > Ag_2S$

Vedclass · Answer

(D) The solubility of ionic compounds depends on the balance between lattice energy and hydration energy. $1$. For $MgF_2$ and $MgCl_2$: $MgF_2$ is sparingly soluble due to high lattice energy,while $MgCl_2$ is highly soluble. Thus,$MgF_2 $2$. For $BaF_2$ and $BaCl_2$: $BaF_2$ is less soluble than $BaCl_2$ due to the high lattice energy of the fluoride ion. Thus,$BaF_2 $3$. For $LiF$ and $LiCl$: $LiF$ has very high lattice energy due to the small size of both $Li^+$ and $F^-$,making it less soluble than $LiCl$. Thus,$LiF $4$. For $Ag_2O$ and $Ag_2S$: According to Fajan's rule,$Ag_2S$ is more covalent than $Ag_2O$ due to the higher polarizability of the $S^{2-}$ ion compared to $O^{2-}$. Increased covalency leads to decreased solubility. Therefore,$Ag_2O > Ag_2S$ is the correct order.

Which of the following represents the correct solubility order?

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