Ionic EquilibriumMedium
Question
The solubility product of AgCl is 1.0 × 10–10. The equilibrium constant of the reaction
AgCl(s) + Br–$\rightleftharpoons$AgBr(s) + Cl– is 200 and that of the reaction 2AgBr(s) + S2–$\rightleftharpoons$Ag2S(s) + 2Br– is 1.6 × 1024.
What is the Ksp of Ag2S?
Options
A.3.2 × 1016
B.1.56 × 10–49
C.3.95 × 10–25
D.3.13 × 10–17
Solution
(a) AgCl(s) $\rightleftharpoons$ Ag+ + Cl–; K1 = 10–10
(b) AgCl(s) + Br– $\rightleftharpoons$ AgBr (s) + Cl–; K2 = 200
(c) 2 AgBr(s) + S2– $\rightleftharpoons$ Ag2S(s) + 2Br–; K3 = 1.6 × 1024
From 2(a) – 2(b) – 2(c); Ag2S(s) $\rightleftharpoons$ 2Ag+ + S2–;
$K = \frac{\left( 10^{- 10} \right)^{2}}{(200)^{2} \times 1.6 \times 10^{24}} = 1.5625 \times 10^{- 49}$
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