In an attempted determination of the solubility product constant of TI – InterviewSolution

1.	In an attempted determination of the solubility product constant of TI2S the solubility of this compound in pure CO2− free water was determined as 6.3 × 10−6 mol/L. Assume that the dissolved sulfidehydrolyzes almost completely to HS− and that the further hydrolysis to H2S can be neglected. What is the computed Ksp ?
Answer» In an attempted determination of the solubility product constant of $T I_{2} S$ the solubility of this compound in pure $C O^{2 -}$ free water was determined as $6.3 \times 10^{- 6} m o l / L$ . Assume that the dissolved sulfidehydrolyzes almost completely to $H S^{-}$ and that the further hydrolysis to $H_{2} S$ can be neglected. What is the computed $K_{s p}$ ?

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