Equilibrium Question 206
Question: The solubility product of silver sulphide is $ 3.2\times {10^{-11}}. $ Its solubility at the experimental temperature is
Options:
A) $ 2\times {10^{-4}} $ moles per litre
B) $ 6\times {10^{-6}} $ moles per litre
C) $ 1.2\times {10^{-5}} $ moles per litre
D) $ 8\times {10^{-4}} $ moles per litre
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Answer:
Correct Answer: A
Solution:
$ Ag_2S $ ⇌ $ 2A{g^{+}}+{S^{–}} $
$ K _{sp}=4S^{3} $
$ S=\sqrt[3]{\frac{K _{sp}}{4}} $
$ =\sqrt[3]{\frac{3.2\times {10^{-11}}}{4}}=2\times {10^{-6}} $
