ANALYTIC METHODS II. PART Jana Švarcová. Chromatography Electrophoresis Potentiometry ...
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Transcript of ANALYTIC METHODS II. PART Jana Švarcová. Chromatography Electrophoresis Potentiometry ...
ANALYTIC METHODS
II. PART
Jana Švarcová
Chromatography Electrophoresis Potentiometry Titration Spectrophotometry
Chromatography methods Basic theory – separation of mixtures
distributed between two phases stationary phase (SF) mobile phase (MF) – carries the mixtures
The separation is based on differential partitioning between the mobile and stationary phases
Differential rates of migration as the mixture moves over adsorptive materials provide separation Various components of mixtures have different
affinities for the stationary phase
Chromatography methods
chromatography
paper
gas (GC)
distributive
liquid (LC)
adsorption
thin layer
ion-exchange gel affinity Gas-liquid Gas-solid
Chromatography techniques by: physical state of mobile phase layout of stationary phase (column/planar) separation mechanism
Basic term
w – width of peakw1/2 – half-widthtR – retention time
abso
rban
ce
(AU
)
time (min)
substance
w
w1/2
tM
tR
h
tR
Typical chromatographic separation of substance
Liquid chromatography
MF - a liquid of low viscosity which flows through the stationary phase bed
pump
Reservoir of mobile phase
sample
column
detector
waste
Computer data - results
http://www.pharmacelsus.de/hplc/
HPLC
High Performance Liquid Chromatography
higher flow rate of mobile phase (high pressure ∼ 107 Pa)
the better separation
Gas chromatography
The mobile phase in gas chromatography is generally an inert gas
TLC - thin layer chromatography
Plane layout of SF - layer of solid particles spread on a support Compounds in the sample mixture travel different
distances according to how strongly they interact with the stationary phase
start
start
a b
http://web.natur.cuni.cz/~pcoufal/tlcpc.html
Retention factor RF - RF = a/b
a - distance the spot traveled
b – maximum distance the eluent traveled
Electrophoresis
A class of separation techniques - analytes are separated by their ability to move in gel in response to an applied electric field
Separation – size of charge, shape and size of molecule
Migration – cations migrate towards the cathode (-), anions towards the anods (+)
Electrophoresis
Electroforeogram of serum proteins
proteins – fraction %
Potentiometry
Anlytical method – analytes are studied by measuring the potential (volts) in the electrochemical galvanic cell (the difference in electrode potentials)
Potentiometry – basic terms
Two electrodes (acording potential stability) Indicator electrode Reference electrode
The potential is related to the concentration of one or more analytes
Potentiometry
Nernst equation – calculation of the electrode potential E
R – the universal gas constant (8,314 J.K-1.mol-1)T – absolute temperature
F – the Faraday constant,the number of coulombs per mole of electrons (96 500 C.mol-1)
a – the chemical activity for the relevant species; ox/red formsEo – the standard reduction potential
Potentiometry – analytical application
Potentiometric titration curve
Volume of titrant (ml)
P
ote
nti
al
(V)
Electrodes
Referent electrodes: calomel Ag/AgCl
Indicator electrodes: Ion-selective
Potential in turn is described by the Nernst equation and is directly proportional to the pH difference between solutions on both sides of the glass.
Titration
laboratory method of quantitative chemical analysis - is used to determine the unknown concentration of an identified analyte
the titrant – reagent (is prepared as a standard solution) A known concentration and volume of titrant reacts with
a solution of analyte to determine concentration Titre – the volume of titrant reacted
Detection of the equivalence point appropriate pH indicator is added (reflecting the pH range
of the equivalence point)
Different methods to determine the endpoint include Spectroscopy Potentiometer Conductivity
Burette
Acid–base titration
Indicators – organic chemical compound which causes the colour of the solution to change depending on the pH (sensitivity to different concentration of H+ ions)
Calculate the mass of sulfuric acid in the sample solution when the consumption of standard titrant solution NaOH was 24.22 ml at a concentration of 0.1022 mol/l.
Acid-base titration
Spectrophotometry - VIS
Analytical applications - measure concentrations of absorbing (coloured) materials based on developed calibration curves To obtained the unknown concentration of
sample – calibration curve (graph of the transmittance or absorbance versus the wavelength)
Absorption of VIS light by a sample
390 – 750 nm
Spectrophotometry - measurement
the absorbance of a sample will be proportional to the number of absorbing molecules in the spectrometer light beam transmittance T absorbance A
beam of
monochrom.radiation Φo
beam of radiation leaving the sample Φ
l
Lambert-Beer low:
A = ε × c × l ε – Molar absorptivity c - sample concentration (mol/L)l – length of light path through the sample (cm)
Absorption spectroscopy
performed across the electromagnetic spectrum → choice of wavelength max absorption
sample
VIS – analytical applications
Blank Lambert-Beer low – unknown
concentrations Calibartion curve
Basic structure of spectrophotometers