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# Iodine is sparingly soluble in water but much more so in carbon tetrachloride $\left(\mathrm{CCl}_4\right)$. 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 $20^{\circ} \mathrm{C}$. (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.

Solution

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The equilibrium constant for the reaction:

$\mathrm{I_{2(aq)} \rightleftarrows I_{2(CCl_4)}}$

is 83 at 20 degrees Celsius.

b)We need to calculate the fraction of the repeated extraction of $\mathrm{I_2}$ remaining in the aqueous phase if another 0.030 liters of $\mathrm{CCl_4}$ were added to 0.200 liters of aqueous solution containing 0.032 grams of $\mathrm{I_2}$

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