In: Chemistry
Sketch the general shape/appearance of a “spectrophotometric
titration curve” for the following system.
You should label the axes of the graph, and show an approximate
numeric scale (including units) on both axes.
50.0 mL of 0.000100 M FeII(phen)32+ (aq) + 0.01000 M
Ce4+ (aq) ===>
FeIII(phen)33+ (aq) + Ce3+ (aq)
The substance being titrated, FeII(phen)32+, has ε = 12,100 M-1cm-1
at the wavelength of 510 nm that was used. During the course of the
spectrophotometric titration, the absorbance of the solution is
measured in 1.00 cm cells. The titrant Ce4+, as well as the
products FeIII(phen)33+ and Ce3+ are all colorless at 510 nm (you
may assume that ε = 0 M-1cm-1).
Note: since [Ce4+] >> [FeII(phen)32+] in the titration, you
may neglect the absorbance change that results from the “dilution
effect” of the volume increase from addition of the titrant.
Titration,
We would consider complex Fe(phen)3^2+ as Fe2+ ion working ion,
thus,
Fe2+ + Ce4+ ---> Fe3+ + Ce3+
initial Fe2+ = 0.0001 M x 50 ml = 0.005 mmol
Titrated with, 0.01 M Ce4+
Absorbance = molar absorptivity (M-1.cm-1) x concentration (M) x path length (cm)
with,
molar absorptivity = 12,100 M-1.cm-1
path length = 1 cm
concentration = Fe(phen)3^2+ left in solution
Volume of Ce4+ (ml) Absorbance
0 1.21
0.01 1.186
0.02 1.1616
0.04 1.1132
0.06 1.0648
0.08 1.0164
0.1 0.968
0.2 0.726
0.3 0.484
0.4 0.242
0.5 0
Plot volume Ce4+ on x-axis and absorbance on y-axis