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An aqueous solution of a metal bromide M...

An aqueous solution of a metal bromide `MBr_(2)(0.05M)` is saturated with `H_(2)S`. What is the minimum pH at which MS will precipitate ? `K_(SP)` for `M S= 6.0xx10^(-21)` . Concentration of saturqated `H_(2)S=0.1M, K_(1)=10^(-7)and K_(2)=1.3xx10^(-13)` for `H_(2)S` .

Text Solution

Verified by Experts

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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