A student investigates the solubility of two metal sulfide salts, \(\text{ZnS}\) and \(\text{CuS}\), by adding \(10.0\text{ mL}\) of \(1.0\text{ M }\text{HCl(aq)}\) to separate test tubes each containing \(0.10\text{ g}\) of the solid salt. The relevant equilibrium equations and constants at \(298\text{ K}\) are shown below.

\[\text{ZnS}(s) \rightleftharpoons \text{Zn}^{2+}(aq) + \text{S}^{2-}(aq) \quad K_{sp} = 2.0 \times 10^{-24}\]
\[\text{CuS}(s) \rightleftharpoons \text{Cu}^{2+}(aq) + \text{S}^{2-}(aq) \quad K_{sp} = 6.0 \times 10^{-36}\]
\[\text{H}_2\text{S}(aq) \rightleftharpoons 2\text{H}^+(aq) + \text{S}^{2-}(aq) \quad K = 1.0 \times 10^{-20}\]

Which of the following best predicts and explains the outcome of adding \(1.0\text{ M }\text{HCl(aq)}\) to each test tube?