Question: A buffer solution is 0.25 M CH 3 COOH-0.15 M NaCH 3 COO, saturated in H 2 S (0.10 M), and with [Mn 2+ ]

A buffer solution is 0.25 M CH₃COOH-0.15 M NaCH₃COO, saturated in H₂S (0.10 M), and with [Mn²⁺] = 0.15 M.

(a) Show that MnS will not precipitate from this solution (for MnS, K_spa = 3 x 10⁷).

(b) Which buffer component would you increase in concentration, and to what minimum value, to ensure that precipitation of MnS(s) begins? Assume that the concentration of the other buffer component is held constant.

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