In a lab similar to this one. a student started with a stock solution of I; in m

Question

In a lab similar to this one. a student started with a stock solution of I; in methylene chloride. and extracted the methylene chloride with a 0.20 M I' solution. Would you expect the student to get similar or different values for the distribution coefficient than were obtained in this lab? Based upon the value you obtained for the distribution coefficient, is molecular iodine more soluble in methylene chloride or in aqueous 0.20 M I solution? Explain. solution that was 0.002 M in I: showed an absorbance of 0.84 units on an arbitrary scale. The aqueous solution by itself was used a the control blank and set to an absorbance of 0.00 on the same scale. draw up a graph of I: concentration (the independent variable) against absorbance (the dependent variable) assuming the relationship is linear using the Molecular iodine (I;) is a nonpolar molecule. It is nearly insoluble in water. molecular iodine reacts with iodide ion to form the lj' ion. which is polar and is therefore much more soluble in water than is molecular iodine (I;) If this lab had been carried out with pure water instead of the iodide ion solution, would you expect the ICj for the equilibrium shown below to have a greater or lesser value that what you found? b(aq) 4 rightarrow I:(CH;CI;) Explain.*

Explanation / Answer

4. In the physical science, distribution-coefficient(D) is the ratio of concentrations of a compound in a mixture of two immiscible phases at equilibrium. This ratio is therefore a measure of the difference in solubility of the compound in these two phases.

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