40 mL of an iodine solution 0.2 M was mixed with 20 mL of ether. After extraction, the iodine reminder in the aqueous phase is 0.6 mmole.Calculate the Extraction efficiency of iodine % E.
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Step 1
First, we need to find the initial amount of iodine in the solution. We can do this by multiplying the volume of the solution by its concentration: Initial amount of iodine = Volume × Concentration Initial amount of iodine = 40 mL × 0.2 M Show more…
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Iodine is sparingly soluble in water but much more so in carbon tetrachloride (CCl_). The equilibrium constant, also called the partition coefficient, for the distribution of $\mathrm{I}_{2}$ between these two phases $$\mathrm{I}_{2}(a q) \rightleftharpoons \mathrm{I}_{2}\left(\mathrm{CCl}_{4}\right)$$ is 83 at $20^{\circ} \mathrm{C}$. (a) $\mathrm{A}$ student adds $0.030 \mathrm{L}$ of $\mathrm{CCl}_{4}$ to $0.200 \mathrm{L}$ of an aqueous solution containing $0.032 \mathrm{g} \mathrm{I}_{2}$ The mixture is shaken and the two phases are then allowed to separate. Calculate the fraction of $\mathrm{I}_{2}$ remaining in the aqueous phase. (b) The student now repeats the extraction of $\mathrm{I}_{2}$ with another $0.030 \mathrm{L}$ of $\mathrm{CCl}_{4} .$ Calculate the fraction of the $\mathrm{I}_{2}$ from the original solution that remains in the aqueous phase. (c) Compare the result in (b) with a single extraction using $0.060 \mathrm{L}$ of $\mathrm{CCl}_{4} .$ Comment on the difference.
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