Respuesta :
Answer:
Option (E) is correct
Explanation:
Solubility equilibrium of [tex]Pb(IO_{3})_{2}[/tex] is given as follows-
[tex]Pb(IO_{3})_{2}\rightleftharpoons Pb^{2+}+2IO_{3}^{-}[/tex]
Hence, if solubility of [tex]Pb(IO_{3})_{2}[/tex] is S (M) then-
[tex][Pb^{2+}]=S(M)[/tex] and [tex][IO_{3}^{-}]=2S(M)[/tex]
Where species under third bracket represent equilibrium concentrations
So, solubility product of [tex]Pb(IO_{3})_{2}[/tex] , [tex]K_{sp}=[Pb^{2+}][IO_{3}^{-}]^{2}[/tex]
Here, [tex][Pb^{2+}]=S(M)=5.0\times 10^{-5}M[/tex]
So, [tex][IO_{3}^{-}]=2S(M)=(2\times 5.0\times 10^{-5})M=1.0\times 10^{-4}M[/tex]
So, [tex]K_{sp}=(5.0\times 10^{-5})\times (1.0\times 10^{-4})^{2}=5.0\times 10^{-13}[/tex]
Hence option (E) is correct
