Question

You would like to determine the equilibrium constant for the binding of a ligand to a metal ion: M^ 3 + + L^ - equivalence ML^ 2 + where k = [(ML^ 2+])/(M^ 3+][L])]. The ML^ 2 + complex has a unique absorbance of the solution at an appropriate wavelength. The concentrations and the n going to equilibrium using an ICE table. The following experiment order to determine the extinction coefficient of the complex at the wavelength chosen.

Answer 1

The data given here is incomplete the calculations are not possibled based on the data provided. Since the absorbance data is provided I assume there has to be a standard for which absorbance has been measured using that and from Beer's law we have to calculate the equilibrium concentration of [M³⁺], [L^-] and [ML²⁺] and using that data we have to calculate K.

The reaction should be

M³⁺ + L^- $\rightleftharpoons$ ML²⁺

We need data where absorbance has been measured for some standrds containing the ML2+ complex to calculate the K in the data provided or the $\varepsilon$ *l from the slope

Refer to the comple procedures here

http://course1.winona.edu/cmiertschin/213/colorlab.htm

http://www.scienceteacherprogram.org/chemistry/Tehilla98.html