# the following question as a Word document for ```Royal Society of Chemistry ‘Study Guide’ - G Currell
-------------------------------------------------------------------------------------------------------------------------Spectrophotometric measurement of concentration: Beer-Lambert Law
The absorbance, A, (sometimes known as optical density, OD), of light passing through a
solution is given by the Beer-Lambert law as:
A = ε&times;b&times;C
where
ε (Greek letter, epsilon) is the molar absorptivity of the solute with units of M-1 cm-1
(or (mol L-1)-1 cm-1 or mol-1 dm3 cm-1)
b is the path length of the light through the solution in units of cm.
C is the concentration of the solution in mol L-1 (or mol dm-3 or M)
This straight line relationship works well for dilute solutions (low values of C), but it is
important to remember that, at higher concentrations, the equation can cease to be valid and
the relationship between A and C becomes non-linear.
In a simple spectrophotometric experiment to measure the concentration of a solution of
potassium permanganate:
1. the spectrophotometer is zeroed to give A = 0 when C = 0, by using a 'blank'
solution (this can occur automatically in a double-beam instrument),
2. the absorbances, A, are measured for a series of standard concentrations, C,
of potassium permanganate at a wavelength of 522 nm,
3. a 'best-fit' line of regression in a graph of the measured values of A against C,
gives a calibration line for the particular measurement,
4. the absorbance, Ao, of the solution being tested is measured and the
equivalent value of concentration, Co, is calculated from the calibration line.
The absorbance, Ao, of the solution being tested is measured three times, giving replicate
values, Ao = 0.763, 0.741, 0.749.
The calibration values of absorbances, A, of the six standard concentrations, C, are given in
the table below:
C (mg L-1)
0
20
40
60
80
100
120
A
0
0.267
0.583
0.824
1.120
1.313
1.499
Molar mass of potassium permanganate, KMnO4, Mm = 158 g mol-1.