By Beer’s Law, determine the molar absorptivity of the iron (II) phenanthroline complex using maximum absorbance, the molar concentration of the standard iron solution, and the cell path length.
I'm confused because on this lab we have calculated the max Wavelenth (497nm) and used a spectroscopy instrument to measue the max Absorbance at that wavelength for the other samples and unknown. Beers law seem simple, But how would I use it to find the molar absorptivity?
SAMPLE (in ppm) |
Max (nm) |
A Max (Lmol-1 cm-1) |
2.5 |
497 |
1.150 |
2.0 |
497 |
1.080 |
1.5 |
497 |
.9850 |
1.0 |
497 |
.8550 |
0.5 |
497 |
.7340 |
Unknown |
497 |
.8850 |
here's the data we collected. I'm stumped
for this experiment first u have to draw beers lamberts plot by
taking concentration on x-axis and absorbance on y -axis. u will
get a straight line after that for unknown, pointout the absorbance
on y axis draw straight line to the slope, u will get concentration
on x axis of unkown.when u got the unkown concentration by using
beers lamberts law u can calculate molar absorbivity(= A/cl
molar absobvity()=(
Absorbance)/ concentration *pathlength
u have A= 0.885 , cuvvetpathlength l=1cm, concentration c= got
by graph
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