Ionic EquilibriumMedium
Question
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.
Options
A.1.0
B.1.3
C.13.0
D.0.7
Solution
M2+ + H2S $\rightleftharpoons$ MS(s) + 2H+
For ppt. of MS(s), Q < keq
$\text{or, }\frac{\left\lbrack H^{+} \right\rbrack}{\left\lbrack M^{2 +} \right\rbrack\left\lbrack H_{2}S \right\rbrack} < \frac{K_{a1},K_{a2}}{K_{sp}} $$${\text{Or, }\frac{\left\lbrack H^{+} \right\rbrack^{2}}{0.04 \times 0.1} < \frac{10^{- 7} \times 1.5 \times 10^{- 13}}{6 \times 10^{- 21}} }{\therefore{\left\lbrack H^{+} \right\rbrack\text{ M}P_{\min}^{H}}_{\max}}$$
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