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Indicator Electrodes, Potentiometry, Electrochemistry, Electrode Kinetics, Electrogravimetry, Polarography, Square Wave Voltammetry, Wavelength Selection, Types of Spectroscopy, Detectors, Theory of Molecular Absorption, Absorption by Organic Molecules, Applying UV-vis Spectroscopy are major topics of this course. Main points from these slides are: Electroanalytical Methods, Galvanic Cell, Electrolytic Cell, Electrochemical Reaction, Voltammetric Systems, Potentiometry, Cell Potential, Reference
Typology: Slides
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Two general categories:
(produces electricity spontaneously)voltage (i.e., potential) of a galvanic cellPotentiometric Systems – measure
occur)cause an electrochemical reaction toelectrolytic cell (consumes power to& usually measure current in anVoltammetric Systems – control potential
of an electrochemical cell (galvanic cell)measuring the potential (i.e., voltage)
Indicator Electrode – potential
responds to activity of species of interest
Reference Electrode – chosen so
composition.that its potential is independent of solution
conductor electronic
conductorelectronic
electrode
electrode
∆ E V
cabd
Cathode or
Indicator
Anode or
Reference
V or electrometer (high input impedance > 100 Mwithout drawing significant current i.e potentiometer- (^) Represents device to measure potential (voltage)
Ω
(mega ohms)
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cell (^) = E
ind (^) – E
ref
(+ E
E J = junction potential, a non-ideal potential
two dissimilar solutionswhich develops across the interface betweenCell Potential (Voltage)
impractical, requiring a source of Ha reference electrode today, however, it isis important historically and could serve as
2 gas at
flammable.constant pressure, and is highly
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saturated KCl
AgCl + e
(^) Ag + Cl
silver chloride
silver wire
potassium
coating on wire
solutionchloride
Nernst Equation
RT
[Red]
E = E
o
nF
[Ox]
2 E o = 0.000 v
(^2) Cl
(^2)
(^) 2 Hg + 2Cl
E o = 0.268 v
(^) Ag + Cl
E o = 0.222 v
Ag
(^) Ag
o = 0.799 v
At 25
(^) o C this becomes
RT
[Red]
E = E
o
[Ox]
[Red]
E = E
o
n
[Ox]
