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An aqueous solution of a metal bromode M...

An aqueous solution of a metal bromode `MBr_(2) (0.05M)` is saturated with `H_(2)S`. What is the minimum `pH` at which `MS` will precipitate? `K_(sp)` for `MS = 6.0 xx 10^(-21)`. Concentration of satured `H_(2)S = 0.1M, K_(1) = 10^(-7)` and `K_(2) = 1.3 xx 10^(-13)` for `H_(2)S`.

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For `H_(2)S , H_(2)S rarr 2H^(+) + S^(2-)`
`K = K_(1)xxK_(2) = 1.3 xx 10^(-20)`
Minimum `[S^(2-)]` required to begin precipitation of
`[s^(2-)] = 6 xx 10^(-21)/0.05 = 1.2 xx 10^(-19)/0.10`
`[H^(+)] = 0.10 M implies pH = 1`
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