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Calculate the concentration of \( \mathrm{I}_{3}^{-} \)ions in a standard solution of iodine in \( 0.5 \mathrm{M} \mathrm{KI} \), making use of the following standard electrode potentials:
\[
\mathrm{I}_{2}+2 \mathrm{e} \rightleftharpoons 2 \mathrm{I}^{-} ; E^{\circ}=+0.5355 \mathrm{~V} \text { and } \mathrm{I}_{3}^{-}+2 \mathrm{e} \rightleftharpoons 3 \mathrm{I}^{-} ; E^{\circ}=+0.5365 \mathrm{~V} .
\]
The molarity of \( \mathrm{I}^{-} \)in the \( 0.5-\mathrm{M} \mathrm{KI} \) solution can be assumed to be \( 0.5 \mathrm{~mol} \mathrm{~L}{ }^{-1} \)
(A) \( 0.12 \mathrm{~mol} \mathrm{~L}^{-1} \)
(B) \( 0.88 \mathrm{~mol} \mathrm{~L}^{-1} \)
(C) \( 0.48 \mathrm{~mol} \mathrm{~L}^{-1} \)
(D) \( 0.24 \mathrm{~mol} \mathrm{~L}^{-1} \)
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