Question

Show all work for full credit. You would like to determine the equilibrium constant for the binding of a ligand to a metal ion: Mt" + L-<-> ML2+, where K-[([M1.*.1)/(M1")(し11. The ML-complex has aunique absorbance in the visible region, so its concentration at equilibrium can be determined by measuring the absorbance of the solution at an appropriate wavelength. An ICE table can used to determine the concentrations of M+ and concentration change in going to equilibrium. The following experiment is determine the extinction coefficient of the complex at the wavelength chosen. 1) L from their initial conce ations and the carried out first to Calculate the complex concentration in each solution and then its extinction coefficient. 0.200 M || 0.1 M Il Ligan Extinction 0.0011 MComplex Coefficient d Concentration Absorbance (Mem) MaHNOIon (mL) 5.0 HNO Ligand SolutionIon 0.113 0.227 0.337 0.431 2.0 3.0 2.0 0.562 5.0 0.0 5.0 Plot the absorbance versus the solution concentration and determine the slope and intercept of the resulting line.

please help me with filling the table and show me how you did it. thanks

Answer 1

[M3+]>> [L], So [ Complex ]= [ L]

Solution	[L] M	[Complex] M	Abs	Extinction coefficient M-1 cm-1
1	0.00011	0.00011	0.113	1027.272727
2	0.00022	0.00022	0.227	1031.818182
3	0.00033	0.00033	0.337	1021.212121
4	0.00044	0.00044	0.431	979.5454545
5	0.00055	0.00055	0.562	1021.818182
			Mean	1016.3333

0.6 0.5 y1010.2x R2 = 0.9978 0.4 0.3 0.2 1.1 0 0.0001 0.0002 0.0003 0.0004 0.0005 0.0006

Extinction coefficient from calculation = 1016.333 M-1 cm-1

While from graph 1010.2 M-1 cm-1