what is more likely to dissolve in acidic solution, silver chloride or sliver sulfide? Why?

Silver sulfide (Ag₂S) is more likely to dissolve in acidic solution.

Ag₂S(s) ⇌ 2Ag⁺(aq) + S²⁻(aq)
HS⁻ ion is a weak acid which incompletely dissociates in aqueous solution. In acidic solution, the hydronium ions (hydrogen ions) would combine with S²⁻ ions to form HS⁻ ions, and thus the concentration of S²⁻ ions decreases. According to Le Chatelier's principle, the equilibrium position will shift to the right of the reaction in order to encounter the loss of S²⁻ ions. This leading to the dissolving of Ag₂S. (Furthermore, HS⁻ would react with the excess acid to give H₂S gas.)

AgCl(aq) ⇌ Ag⁺(aq) + Cl⁻(aq)
HCl is a strong acid which completely dissociates in aqueous solution. In acidic solution, the hydronium ions (hydrogen ions) would NOT combine with Cl⁻. The acidity of the solution has no effect on the equilibrium position of the above reaction.