Consider the dissolution of MnS in water. [K_sp(MnS) =3.0 × 10^-14] MnS(s) + H₂O(l) Mn²⁺(aq) + HS^-(aq) + OH^-(aq)
How is the solubility of manganese(II) sulfide affected by the addition of aqueous potassium hydroxide to the system?

Question

Consider the dissolution of MnS in water. [K_sp(MnS) =3.0 × 10^-14] MnS(s) + H₂O(l)

Consider the dissolution of MnS in water. [K<sub>sp</sub>(MnS) =3.0 × 10<sup>-14</sup>] MnS(s) + H<sub>2</sub>O(l) Mn<sup>2+</sup>(aq) + HS<sup>-</sup>(aq) + OH<sup>-</sup>(aq) How is the solubility of manganese(II) sulfide affected by the addition of aqueous potassium hydroxide to the system? A) The solubility will be unchanged. B) The solubility will decrease. C) The solubility will increase. D) The amount of KOH added must be known before its effect can be predicted. E) The pK<sub>a</sub> of H<sub>2</sub>S is needed before a reliable prediction can be made.

Mn²⁺(aq) + HS^-(aq) + OH^-(aq)
How is the solubility of manganese(II) sulfide affected by the addition of aqueous potassium hydroxide to the system?

Quizplus · Accepted Answer

The addition of aqueous potassium hydroxide will increase the concentration of hydroxide ions in solution. These hydroxide ions will react with the dissolved hydrogen sulfide ions, causing a shift in the equilibrium towards the reactant side (Le Chatelier's principle). This will decrease the concentration of hydrogen sulfide ions in solution, decreasing the solubility of manganese(II) sulfide.

Consider the Dissolution of MnS in Water