Spectrophotometry is a technique that uses the measurement of light absorption to determine the concentration of chemical substances. It operates based on Beer's Law, which states that absorbance is directly proportional to concentration. The methodology involves using a spectrophotometer to measure the intensity of light passing through reference and sample solutions. Applications include concentration measurement, detection of impurities, structure elucidation, and more. Spectrophotometry is a widely used analytical technique in clinical chemistry.
Spectrophotometer instrumentation & working Sabahat Ali
Spectrophotometric analysis is a technique to measure the concentration of solute solution by measuring the amount of light absorbed by solution.
Absorption can be calculated in terms of transmittance by using Beer's Lambert law.
This article illustrates the principle and working of Colorimeter and Photometer and how absorbance, transmittance and light intensity can be measured.
A spectrophotometer is an instrument that measures the amount of light absorbed by a sample. Spectrophotometer techniques are used to measure the concentration of solutes in solution by measuring the amount of the light that is absorbed by the solution in a cuvette placed in the spectrophotometer .
A spectrophotometer is an instrument containing a monochromator, a device which produces a light beam containing wavelengths in a narrow band around a selected wavelength, and a means of measuring the ratio of that beam's intensity as it enters and leaves a cuvette 99 This describes a single-beam photometer.
This is a powerpoint of automation in clinical chemistry. This comprises the definition of automation, steps of the analytical process, and detail about the continuous flow analyzer.Thus, this will be helpful for the students of medical laboratory, biochemistry students and teachers.
Spectrophotometer instrumentation & working Sabahat Ali
Spectrophotometric analysis is a technique to measure the concentration of solute solution by measuring the amount of light absorbed by solution.
Absorption can be calculated in terms of transmittance by using Beer's Lambert law.
This article illustrates the principle and working of Colorimeter and Photometer and how absorbance, transmittance and light intensity can be measured.
A spectrophotometer is an instrument that measures the amount of light absorbed by a sample. Spectrophotometer techniques are used to measure the concentration of solutes in solution by measuring the amount of the light that is absorbed by the solution in a cuvette placed in the spectrophotometer .
A spectrophotometer is an instrument containing a monochromator, a device which produces a light beam containing wavelengths in a narrow band around a selected wavelength, and a means of measuring the ratio of that beam's intensity as it enters and leaves a cuvette 99 This describes a single-beam photometer.
This is a powerpoint of automation in clinical chemistry. This comprises the definition of automation, steps of the analytical process, and detail about the continuous flow analyzer.Thus, this will be helpful for the students of medical laboratory, biochemistry students and teachers.
Spectroscopy is a method which measures the interaction of matter with electromagnetic radiation. it reveals different properties of substances such as absorbance, composition and interaction with other matter
principle, application and instrumentation of UV- visible Spectrophotometer Ayetenew Abita Desa
This Presentation powerpoint includes the principle, application, and instrumentation of UV- Visible Spectrophotometer. It covers beer-lambert low and its quantitative applications. It also includes the qualitative applications in different fields of study. Presented at Addis Ababa University, School of medicine, department of medical biochemistry.
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The spectrophotometer technique is to measures light intensity as a function of wavelength.
• Measures the light that passes through a liquid sample
• Spectrophotometer gives readings in Percent Transmittance (%T) and in Absorbance (A)
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3. INTRODUCTION
• Photometry is defined as the measurement of light;
• Spectrophotometry is defined as the measurement of the
intensity of light at selected wavelengths.
• Spectrophotometric analysis is a widely used method of
quantitative and qualitative analysis in Clinical Chemistry.
• Spectrophotometer measures the intensity of the light entering
a sample and the light exiting a sample and compares the two
intensities.
4. …introduction contd
It does this by:
- diffracting the light beam into a spectrum of wavelengths
- Directing it unto an object
- receiving the light reflected or returned from the object
- detecting the intensities with a charge-coupled device
- displaying the results on the detector and then the display device
5. • Spectrophotometer was invented in 1940 by Arnold Beckman and
Howard H Cary at National Technologies Laboratories
• This discovery streamlined and simplified chemical analysis, by
allowing researchers to perform a 99% accurate biological assessment
of a substance within minutes as opposed to the weeks required
previously for results with only 25% accuracy.
…introduction contd
7. Spectrophotometry operates on the principles of Beer-Lambert’s Law. Beer’s Law
states that the Concentration of a substance is directly proportional to the amount of
light absorbed, or inversely proportional to the logarithm of the transmitted light.
The Beer-Lambert law (or Beer's law) is the linear relationship between absorbance
and concentration of an analyte. The general Beer-Lambert law is usually written as:
A = a b c
where A is the measured absorbance, a is the wavelength(λ)-dependent absorptivity
coefficient, b is the light’s path length in cm, and c is the analyte concentration in
moles per litre.
Beer’s Law
OPERATING PRINCIPLE
of Spectrophotometry
8. The linearity of the Beer-Lambert law is limited by chemical and instrumental
factors. Causes of nonlinearity include
• High Concentration: deviations in absorptivity coefficients at high
concentrations (>0.01M) due to electrostatic interactions between
molecules in close proximity
• Scattering of light due to particulates in the sample
• Fluoresecence or phosphorescence of the sample
• Changes in refractive index at high analyte concentration
• Shifts in chemical equilibria as a function of concentration
• Non-monochromatic radiation, deviations can be minimized by using a
relatively flat part of the absorption spectrum such as the maximum of an
absorption band
• Stray light
Limitations of the Beer-Lambert’s Law
9. …operating principle
• The intensity of transmitted light passing through a solution
containing an absorbing substance (chromogen) is decreased by the
absorbed fraction. This fraction is detected, measured and used to
relate the light transmitted or absorbed to the concentration of the
analyte in question.
• If an incident light beam with intensity Io, passes through a square cell
containing a solution of a compound that absorbs light of a certain
wavelength, λ, given that the intensity of the transmitted light beam
is Is, then transmittance (T) of light is defined as: T = Is/Io. Percentage
Transmittance %T = Is/Io. X 100
• …and the amount of light absorbed is expressed as Absorbance, and
related to Transmittance by the equation A = -log T
10. • A portion of the incident light, however,
may be reflected by the surface of the cell
or may be absorbed by the cell wall or
solvent.
• To focus attention on the compound of
interest, elimination of these factors is
necessary. This is achieved using a reference
cell identical to the sample cell, except that
the compound of interest is omitted from
the solvent in the reference cell.
• The transmittance (T) through this
reference cell is IR divided by IO; and the
transmittance for the compound in solution
then is defined as Is divided by IR.
…operating principle
11. …operating principle
• In practice, the light beam is blocked and the detector signal set to
zero transmittance, then a reference cell is inserted and the detector
signal adjusted to an arbitrary scale reading of 100 (corresponding to
100% transmittance), followed by the cell containing the sample to be
measured, and the percentage transmittance reading is made on the
sample.
• Modern absorption instruments can usually display the data as either
transmittance, %-transmittance, or absorbance. An unknown
concentration of an analyte can be determined by measuring the
amount of light that a sample absorbs and applying Beer's law. If the
absorptivity coefficient is not known, the unknown concentration can
be determined using a working curve of absorbance versus
concentration derived from standards.
12. METHODOLOGY
• Turn the switch at ‘ON’ and “Warm up” the instrument for about 15 min.
• Zero adjust to read infinite absorbance (Zero % transmittance). With no
cuvette in the chamber, a shutter cuts off all light from passing thru the
cuvette chamber.
• Adjust wavelength control to read the wavelength at which the test is
desired.
• Blank, Control & Standard adjustments: fill the blank cuvette with the
solvent used to dissolve specimen. Polish to clean, insert into the cuvette
chamber, aligning mark to front of light source. Close chamber cover.
• Sample 1 & 2: Then, fill the cuvette with the desired specimen, insert into
the cuvette chamber, aligning mark to front of light source. Close chamber
cover.
15. …instruments
• Light source: provide a sufficient source of light which is
suitable for marking a measurement.
• The light source typically yields a high output of polychromatic
light over a wide range of the spectrum.
Types of light source
INCANDESCENT LAMPS: Tungsten light, Hydrogen light, Deuterium light
LASER light – extremely intense, focused & nearly non-divergent beam
of monochromatic light
17. …instruments
• Monochromator: Accepts polychromatic input light from a
lamp and puts out monochromatic light.
• Monochromator consists of these parts:
I.Entrance slit
II.Collimating lens or mirror
III.Dispersion element
IV.Focusing lens or mirror
V. Exit slit
9
18. …instruments
10
• Dispersion devices: A special plate with
hundreds of parallel grooved lines.
• The grooved lines act to separate the white light
into the visible light spectrum.
The more lines
the smaller
the wavelength
resolution.
20. …instruments
• Cuvettes: (also cuvet) designed to hold samples for
spectroscopic experiments. made of Plastic, glass or silica
• should be as clear as possible, without impurities that might
affect a spectroscopic reading.
21. …instruments
• Detectors: Convert radiant energy (photons) into an electrical
signal.
The photocell and phototube are the simplest photodetectors, producing
current proportional to the intensity of the light striking them.
22. …instruments
• Display devices: The data from a detector are displayed by a
readout device, such as an analog meter, a light beam reflected on a
scale, or a digital display, or LCD .
• The output can also be transmitted to a computer or printer.
14
24. • SINGLE BEAM;
Advantage include: low cost, high throughput and hence high sensitivity
because of optical system is simple.
Disadvantage include: An appreciable amount of time elapses between taking
the reference and making the sample measurement such that there can be
problems with drift.
• DOUBLE BEAM: this is designed to eliminate drift by measuring blank and
sample virtual simultaneously.
Advantage: High stability because reference and sample are measured
virtually at the same moment in time.
Disadvantages include: Higher cost, lower sensitivity as throughput of light is
poorer because of the optical complexity.
27. − Set spectrophotometer to the λ of maximum light
absorption
− Measure the absorption of the unknown, and
from the standard plot, read the related
concentration.
…applications
28. 17
2. Detection of Impurities
•UV absorption spectroscopy is one of the
best methods for determination of impurities in
organic molecules.
Additional peaks can be
observed due to impurities
in the sample and it can be
compared with that of
standard raw material.
…applications
29. 3. Structure elucidation of organic compounds.
•From the location of peaks and combination of
peaks UV spectroscopy elucidate structure of
organic molecules:
othe presence or absence of unsaturation
…applications
30. 4. Chemical kinetics
•Kinetics of reaction can also be studied using UV
spectroscopy. The UV radiation is passed through
the reaction cell and the absorbance changes can
be observed.
…applications
31. 5. Detection of Functional Groups
•Absence of a band at particular wavelength
is regarded as an evidence for absence of
particular group
…applications
32. 6. Molecular weight determination
•Molecular weights of compounds can be measured
spectrophotometrically by preparing the suitable
derivatives of these compounds.
•For example, if we want to determine
the molecular weight of amine then it is converted in to
amine picrate.
…applications
33. CONCLUSION
• Spectrophotometric analysis is a widely used method of quantitative
and qualitative analysis in Clinical Chemistry. It is a veritable
diagnostic technique for rapid turnover of analytes
35. REFERENCES
1. Tietz Textbook of Clinical Chemistry & Molecular Medicine 6th Edition
2014
2 Clinical Chemistry – Principles, Techniques, Correlations; Bishops; 7th
Edition 2015
3. Fundamentals of UV-visible spectroscopy, Tony Owen, 1996
4. UNIT: Spectrophotometry, Clinical Chemistry Lab Manual
Editor's Notes
It depends on the light absorbing properties of the substance or a derivative of the substance being analyzed
Photo-filter: Collimator lens and Monochromator prism
Application of Beer’s Law
In practice, a calibration relationship between absorbance and concentration is established experimentally for a given instrument under specifed conditions using a series of reference solutions that contain increasing concentrations of analyte.
Frequently, a linear relationship exists up to a certain concentration or absorbance. When this linear relationship exists, the solution is said to obey Beer’s law up to this point. Within this limitation, a calibration constant (K) may be derived and used to calculate the concentration of an unknown solution by comparison with a calibrating solution
Fluorescence occurs when the energy supplied by electromagnetic radiation kicks an electron of an atom from a lower energy state into an "excited" higher energy state; then the electron releases more light energy when it falls back to a lower energy state
Phosphorescence is light emitted after exposure to radiation, by something that doesn't produce flame or heat. An example of phosphorescence is the light from a glow stick.
Is=intensity of Sample light, Io=intensity of original incident light
A portion of the incident light, however, may be reflected by the surface of the cell or may be absorbed by the cell wall or solvent. To focus attention on the compound of interest, elimination of these factors is necessary. Tis is achieved using a reference cell identical to the sample cell, except that the compound of interest is omitted from the solvent in the reference cell. The transmittance (T) through this reference cell is IR divided by IO; the transmittance for the compound in solution then is defned as I divided by IR.
In such an instrument, a beam of light is passed through a monochromator that isolates the desired region of the spectrum to be used for measurements. The light next passes through an absorption cell (cuvet), where a portion of the radiant energy is absorbed, depending on the nature and concentration of the substance in the solution. Any light not absorbed is transmitted to a detector, which converts light energy to electrical energy that is registered on a meter or recorder or digitally displayed.
In operation, an opaque block is substituted for the cuvet, so that no light reaches the photocell, and the meter is adjusted to read 0% T. Next, a cuvet containing a reagent blank is inserted, and the meter is adjusted to read 100% T (zero absorbance). The composition of the reagent blank should be identical to that of calibrating or unknown solutions except for the substance to be measured. Calibrating solutions containing various known concentrations of the substance are inserted, and readings are recorded. Finally, a reading is made of the unknown solution, and its concentration is determined by comparison with readings obtained on the calibrators.
A blank gives you a baseline absorbance reading of your reagent solution. A control assures the experiment is working properly such as adding the final product to your solution without the precursors
Laser = light amplification by stimulated emission of radiation
Usually square of round cylindrical clear transparent tubes designed to hold liquid samples in spect. Highly alkaline samples can dissolve cuvets or cause etching
Picric acid is a reducing sugar, detectable by spectrophotometric technique