An aqueous solution of a metal bromide MBr2 (0.05 M) is saturated with H2S. What is the minimum pH at which MS will precipitate? Ksp for M S = 6.0 × 10−21 : concentration of saturated H2S = 0.1 M : K1 = 10−7 and K2 = 1.3 × 10−13 for H2S.

An aqueous solution of a metal bromide MBr2 (0.05 M) is saturated with

1.	An aqueous solution of a metal bromide MBr2 (0.05 M) is saturated with H2S. What is the minimum pH at which MS will precipitate? Ksp for M S = 6.0 × 10−21 : concentration of saturated H2S = 0.1 M : K1 = 10−7 and K2 = 1.3 × 10−13 for H2S.
Answer» An aqueous solution of a metal bromide $M B r_{2} (0.05 M)$ is saturated with $H_{2} S$ . What is the minimum pH at which MS will precipitate? Ksp for M S = $6 .0 \times 10^{- 21}$ : concentration of saturated $H_{2} S$ = $0.1 M$ : $K_{1}$ = $10^{- 7}$ and $K_{2}$ = $1.3 \times 10^{- 13}$ for $H_{2} S$ .

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An aqueous solution of a metal bromide MBr2 (0.05 M) is saturated with H2S. What is the minimum pH at which MS will precipitate? Ksp for M S = 6.0 × 10−21 : concentration of saturated H2S = 0.1 M : K1 = 10−7 and K2 = 1.3 × 10−13 for H2S.

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