Abstract The experiment, Chemical Equilibrium in Solution, makes use of a titration of a heterogeneous solution. This is done in order to find the distribution of molecular Iodine, I2, as the solute between two immiscible liquid phases, water and a hexane solution. The average values obtained for (I2) = 6.11E-06 M, (I-) = 0.1097, (I3-) = 2.82E-04. The results that were found in this experiment show an inaccuracy. This may have been due to the third run in the titration of the Iodine in Hexanes. This inaccuracy is represented on the graph. There should be no variation with the concentration shown. Unfortunately, due to there being only three trials completed there can be no certainty as to which trail is the least inaccurate.
I. Introduction
The purpose of this experiment was to measure the chemical equilibrium in solution of a typical homogeneous equilibrium in aqueous solution. The equilibrium that is to be observed is that which occurs when Iodine, I2, is dissolved in aqueous potassium iodide (KI). The equilibrium constant, Kc, for each run was found using;
Kc = (I3-) (I2w) (I-) (1) The method involves the use of two immiscible liquid phases, aqueous and hexane solution. To determination of I2 present at equilibrium in the aqueous solution use is made of the heterogeneous solutions of hexanes and water. It is observed that the presence of I2 concentration in aqueous solution is very small. This is due to the fact that I2 is nonpolar and is attracted to the nonpolar hexanes. Although, some iodine will still be found in aqueous solution. The total iodine
