An aqueous solution of a metal bromide MBr2 (0.04 M) is saturated with H2S. What is the minimum pH a

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An aqueous solution of a metal bromide MBr2 (0.04 M) is saturated with H2S. What is the minimum pH at which MS will precipitate? The value of Ksp for MS = 6.0 × 10–21; concentration of saturated H2S = 0.1M, K1 = 10–7 and K2 = 1.5 × 10–13 for H2S.

Accepted Answer

M2+ + H2S $ightleftharpoons$ MS(s) + 2H+For ppt. of MS(s), Q < keq$	ext{or, }\frac{\left\lbrack H^{+} ightbrack}{\left\lbrack M^{2 +} ightbrack\left\lbrack H_{2}S ightbrack} < \frac{K_{a1},K_{a2}}{K_{sp}} $$${	ext{Or, }\frac{\left\lbrack H^{+} ightbrack^{2}}{0.04 	imes 0.1} < \frac{10^{- 7} 	imes 1.5 	imes 10^{- 13}}{6 	imes 10^{- 21}} }{	herefore{\left\lbrack H^{+} ightbrack	ext{ M}P_{\min}^{H}}_{\max}}$$

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