Strong acids can dissolve the salts of weak acid. When we consider the different salts of silver:
Salts of silver with the conjugate bases of a weak acid are soluble in strong acidic solutions. Some of these salts are:
[tex]2Ag^{+}(aq)+CO_{3}^{2-}(aq) --->Ag_{2}CO_{3}(s)[/tex]
[tex]Ag^{+}(aq)+C_{2}H_{3}O_{2}^{-}(aq)-->AgC_{2}H_{3}O_{2}(aq)[/tex]
[tex]2Ag^{+}(aq)+SO_{3}^{2-}(aq) --->Ag_{2}SO_{3}(s)[/tex]
Salts of silver with the conjugate bases of a strong acid are not affected by change in pH:
[tex]Ag^{+}(aq)+Cl^{-}(aq) --->AgCl(s)[/tex]
[tex]2Ag^{+}(aq)+SO_{4}^{2-}(aq) --->Ag_{2}SO_{4}(s)[/tex]
These two salts with Chloride and sulfate ions are not soluble in acidic solutions as the salts of silver with the conjugate bases of a strong acid are not soluble in acidic solutions, they remain unaffected by any change in pH.
So for salts of Ag and Ba with the conjugate bases of a weak acid, solubility is increased upon the addition of an acid. So, the interference from the ions of weak acids can be removed by decreasing the pH.
