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(B) The solubility of compounds depends on the balance between lattice energy and hydration energy.$(a)$ For $BeSO_4$ and $BaSO_4$,the hydration energ

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$BeSO_4, NaCl, AgCl$

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(B) The solubility of compounds depends on the balance between lattice energy and hydration energy.$(a)$ For $BeSO_4$ and $BaSO_4$,the hydration energy of the small $Be^{2+}$ ion is much higher than that of the $Ba^{2+}$ ion,making $BeSO_4$ more soluble.$(b)$ For $NaCl$ and $MgCl_2$,$NaCl$ is more soluble in water due to its lower lattice energy compared to $MgCl_2$.$(c)$ For $AgCl$ and $AgI$,$AgCl$ is more soluble because the $Cl^-$ ion is smaller and more easily hydrated than the larger,more polarizable $I^-$ ion,which leads to higher lattice energy for $AgI$.Therefore,the correct order is $BeSO_4, NaCl, AgCl$.

$I. Na_3N$	$II. Na_2O$
$III. NaO_2$	$IV. Na_2O_2$

Choose the compound of each of the following pairs that has the more solubility in water:
$(a) \, BeSO_4, BaSO_4$
$(b) \, NaCl, MgCl_2$
$(c) \, AgCl, AgI$

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Choose the compound of each of the following pairs that has the more solubility in water:$(a) \, BeSO_4, BaSO_4$ $(b) \, NaCl, MgCl_2$ $(c) \, AgCl, AgI$