Question

You have two salts$\mathrm{AgX}\mathrm{and}\mathrm{AgY}$ with very similar ${\mathbf{K}}_{\mathbf{sp}}$values. You know that the ${\mathbf{K}}_{\mathbf{a}}$value for $\mathbf{HX}$is much greater than the value for $\mathbf{HX}$ is much greater than the ${\mathbf{K}}_{\mathbf{a}}$value for role="math" localid="1657729586796" $\mathbf{HY}$. Which salt is more soluble in an acidic solution? Explain.

Short answer

$\text{AgY}$will dissolve better in the acidic solution that $\text{AgY}$.

Step-by-step solution

Definition of acidic solution

Any aqueous solution which has a $\text{pH}$less than$7$ is defined as an acidic solution.

Find which salt is more soluble in an acidic solution

If any of the dissolved ions react with acid the salt is more soluble in an acidic solution.

The value of HX has a very high acid dissociation constant, it will be the strong acid and the weak acid will be its conjugate base which is${\text{X}}^{\text{-}}$.

The acid dissociation constant value of HY is lower than HX, it is a weaker acid than HX ${\text{Y}}^{\text{-}}$will be the weakest base.

Being the weakest base, it will react with ${\text{H}}_{\text{3}}{\text{O}}^{\text{+}}$. So $\text{AgY}$will dissolve better in the acidic solution than $\text{AgY}$