Which is more likely to dissolve in an acidic solution, silver sulfide or silver chloride? Why?

First, let's write down the solubility equilibrium reactions for each compound. For silver sulfide (Ag2S): \[Ag2S(s) \rightleftharpoons 2Ag^+(aq) + S^{2-}(aq)\] For silver chloride (AgCl): \[AgCl(s) \rightleftharpoons Ag^{+}(aq) + Cl^{-}(aq)\]

Now, let's study how each compound behaves in acidic environments by writing the reaction equation of the respective anions with H+ ions: For sulfide ion (S²⁻): \[S^{2-}(aq) + H^+(aq) \rightleftharpoons HS^-(aq)\] \[HS^-(aq) + H^+(aq) \rightleftharpoons H2S(g)\] For chloride ion (Cl⁻): \[Cl^-(aq) + H^+(aq) \rightarrow \text{No reaction}\] In acidic solutions, sulfide ions combine with H⁺ ions to form H2S gas which escapes from the solution, effectively removing sulfide ions from the solution. This reduces the concentration of S²⁻ ions, allowing more Ag2S to dissolve and establish equilibrium. On the other hand, chloride ions do not react with H⁺ ions in acidic environments, and thus their concentration is not affected.

Based on the behavior of these compounds in acidic solutions, we can conclude the following: Silver sulfide (Ag2S) is more likely to dissolve in acidic solutions when compared to silver chloride (AgCl). This is because, in acidic environments, sulfide ions combine with H⁺ ions to form H2S gas, which escapes the solution, decreasing the concentration of S²⁻ ions and allowing more Ag2S to dissolve to re-establish equilibrium. In contrast, silver chloride (AgCl) does not react with H⁺ ions, and its dissolution is not influenced by the acidity of the solution. So, the answer is: Silver sulfide (Ag2S) is more likely to dissolve in an acidic solution. The reason is that in acidic environments, sulfide ions combine with H⁺ ions to form H2S gas and decrease the concentration of S²⁻ ions, allowing more Ag2S to dissolve.