A) \[{{10}^{-2}}\]
B) \[2\times {{10}^{-2}}\]
C) \[5\times {{10}^{-3}}\]
D) \[5.4\times {{10}^{-9}}\]
Correct Answer: B
Solution :
\[A{{s}_{2}}{{O}_{3}}\rightleftharpoons 2A{{s}^{3+}}+3{{O}^{2-}}\] \[{{K}_{sp}}={{(2S)}^{2}}{{(3S)}^{3}}\] \[10.8\times {{10}^{-9}}=108{{S}^{3}}\] \[S={{10}^{-2}}\] If dissociation is 50% then solubility is \[2\times {{10}^{-2}}mol/L\].
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