(Solved): Shown below is the reaction for the dissolution of cadmium sulfide. \( K_{e q} \) for this reaction ...

Shown below is the reaction for the dissolution of cadmium sulfide. \( K_{e q} \) for this reaction is \( 1.00 \) \( \times 10^{-27} \) at \( 25^{\circ} \mathrm{C} \). \( \mathrm{CdS}(\mathrm{s}) \longleftrightarrow \mathrm{Cd}^{2+}(\mathrm{aq})+\mathrm{S}^{2-}(\mathrm{aq}) \) \( 10.0 \mathrm{~g} \) of \( \mathrm{CdS} \) is added to two different solutions, which are described below. Which solution will have the highest \( \left[\mathrm{Cd}^{2+}\right] \) once equilibrium is reached? Solution 1: \( 100.0 \mathrm{~mL} \) pure water Solution 2: \( 100.0 \mathrm{~mL} \) of \( 50 \mathrm{mM} \mathrm{NaS} \) Solution 1: \( 100.0 \mathrm{~mL} \) pure water Solution 2: \( 100.0 \mathrm{~mL} \) of \( 50 \mathrm{mM} \mathrm{NaS} \)