2. Measure the wavelengths of visible light that
various colores dolutions absorb.
Understand reason/s as to why each solution
appears as a particular color after gathering
results.
Learn and appreciate the concepts of
spectrophotometry.
3. A spectrometer (spectrophotometer,
spectrograph or spectroscope) is an
instrument used to measure properties
of light over a specific portion of
theelectromagnetic spectrum, typically used
in spectroscopic analysis to identify
materials.
4.
5. Spectrophotometer
Distilled water
Colored solution (Red, Blue, Green & Yellow)
Cuvettes
6. 1. Turn on the power switch, set the desired
wavelength and allow to warm up at least 15
minutes.
2. Set the transmittance to zero.
3. Place the blank into the sample compartment
with the vertical line on the cuvette aligned with
the mark on the front edge of the sample
compartment, and close the lid.
4. Remove the blank from the sample
compartment. Change to "Absorbance" using the
"mode" button.
7. 6. Place a cuvette containing color sample
into the sample compartment, close the lid,
and read the absorbance from the meter.
7. Record readings and remove sample.
8. Repeat steps 1 – 7.
8. Special light filters may be required on some
spectrophotometers if working at certain
wavelengths.
The machine must be zeroed out after each
sample or if changing the wavelength.
Failure to allow the spectrophotometer
enough time to warm can result in erroneous
results.
Make sure cuvettes are free of any particles,
smudges or fingerprints, as these can throw
the machine's calculations off.
9. 4
2 distilled water
red
0 green
distilled water
425
450
yellow
475
500
525
550
575
-2 600
625
650
675
blue
-4
10. Distilled water – The highest spectrum is at
425nm
Red – The highest spectrum is at 525nm
Green – the highest spectrum is at 625 nm
Yellow – the highest spectrum is at 425nm
Blue – The highest spectrum is at 425nm
12. According to the result green has the higest
absorbance.
This is due to the combination of color which
is blue and yellow.
13. The concentration of colored solute in a
solution is directly proportional to the
intensity of its color,
which in turn is proportional to the amount of
absorbance of light at the wavelength that the
color absorbs.
The color, or absorbance, of a solution is also
proportional to the path length that the light
passes through. This is often expressed as
the Beer-Lambert Law, or Beer’s Law:
14. A=εCl
Where A is absorbance at a given wavelength
of light,
ε is the extinction coefficient (amount of
color of the solute per mole)
C is the concentration of solute in the
solution (doubling the concentration
doubles the amount of light absorbed)
and l is the pathlength (if you double the
length of the path of light, you double the
opportunities for it to be absorbed)
15. The sequence of events in a modern
spectrophotometer is as follows:
The light source is imaged upon the sample
A fraction of the light is transmitted or
reflected from the sample
The light from the sample is imaged upon the
entrance slit of the monochromator
The monochromator separates the
wavelengths of light and focuses each of
them onto the photodetector sequentially
16. Spectrophotometric techniques are used to
measure the concentration of solutes in
solution by measuring the amount of light
that is absorbed by the solution in a cuvette
placed in the spectrophotometer.
Spectrophotometry takes advantage of the
dual nature of light. Namely, light has:
1. a particle nature which gives rise to the
photoelectric effect
2. a wave nature which gives rise to the
visible spectrum of light
17. Absorbance is measured to see the
relationship between concentration of a
compound and its absorbance.
Editor's Notes
Plug in and power on the spectrophotometer. Run the machine for five up to 10 minutes to allow it to warm up.Prepare colored solution (red, blue, green & yellow.Fill cuvette with colored solution.Place the cuvette in the spectrophotometer.Adjust the wavelength from 425nm. Repeat steps by using the other coloured solution.