exp9 cyclic voltam
TRANSCRIPT
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EXPERIMENT NUMBER 9:
CYCLIC VOLTAMMETRY
APAGA
CLIMACOMONTES
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VOLTAMMETRY POTENTIOMETRY COULOMETRY
based on the
measurement of thecurrent that
develops in an
electrochemical cell
under conditions
where
concentration
polarization exists
Measurements
are made atcurrents that
approach zero and
where polarization
is absent
measures are taken
to minimize orcompensate for the
effects of
concentration
polarization
minimal
consumption of
analyte
all of the analyte is
converted to another
state
INTRODUCTION
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INTRODUCTION
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INTRODUCTION:
CYCLIC VOLTAMMETRY
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INTRODUCTION:
CYCLIC VOLTAMMETRY SET UP
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INTRODUCTION:
CYCLIC VOLTAMMETRY
TERMS:
Electrode - the interface at which dissolved substrates may
pick up or lose electron(s)Electrolyte - needed in order to provide electrical
conductivity between the two electrodes
*The presence of supporting electrolyte, such as KNO3, is
required to prevent charged electroactive species frommigrating in the electric field gradient.
Indicating electrode- known as the test or working
electrode; the electrode at which the electrochemical
phenomena (reduction or oxidation) being investigated are
taking place.
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INTRODUCTION:
CYCLIC VOLTAMMETRY
Reference electrode- the electrode whose potential is
constant enough that it can be taken as the reference
standard against which the potentials of the other electrodespresent in the cell can be measured. Ex. Calomel, silver-silver
chloride
Counter or auxiliary electrode -serves as a source or sink forelectrons so that current can be passed from the external
circuit through the cell. In general, neither its true potential
nor current is ever measured or known.
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INTRODUCTION:
CYCLIC VOLTAMMETRY
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INTRODUCTION:
CYCLIC VOLTAMMETRY
the current response of a small stationaryelectrode in an unstirred solution is excited by a
triangular voltage waveform
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INTRODUCTION:
CYCLIC VOLTAMMETRY
Switching potential determine
diffusion controlled process?
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CYCLIC VOLTAMMETRY:
Example
the current response when a
solution that is 6 mM in K3Fe(CN)6 and 1M
in KNO3 is subjected to the cyclic
excitation signal
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CYCLIC VOLTAMMETRY:
Example
the potential is
changed linearly with
time starting from apotential where no
electrode reaction
occurs and moving to
potentials where
reduction or oxidation
of a solute occurs
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CYCLIC VOLTAMMETRY
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OBJECTIVES
To determine the E values of the
[FeIII(CN)6]-3/[FeII(CN)6]-4 couple
To evaluate the effects of scan rate,
concentration of electroactivespecies, and supporting electrolyte
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THEORY
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Motion of the Particles in the Solution
Convection Migration
Diffusion
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Motion of the Particles in the Solution
Convection
Stirring, temperature
and/or density
gradient
Provides laminar flow
near the electrode
surface
d1
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Motion of the Particles in the Solution
Migration
Attraction of
electrode and ion
with opposite
charge
Repulsion between
two ions of same
charge
d1v3
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Motion of the Particles in the Solution
Diffusion
Spontaneous
movement of
electroactive
species to area of
lower concentration
d1v3
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Motion of the Particles in the Solution
During discharging
process the
electroactive
component nearelectrode is
depleted
d1v3
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Supporting electrolyte
Limits migration
salt, acid, base, buffer solution or a chelatingreagent
same charge with the electroactive species onsurface electrode
Decreases interaction between electrode and
electroactive species Increase in charge leads to higher effect in
decreasing interaction
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Supporting electrolyte
chemically not reactive
does not interfere with diffusion and with the
electrons exchange on the electrode surface
have a different discharge potential (at least
100 200 mV)
have an high ionic conductivity and guarantee
a low electrical resistance
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Double Layer
Consequence of too
high concentration of
supporting electrolyte
Cause capacitivecurrent
non specific
backgroundinterference of the
faradic current
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Diffusion Layer
Thin layer near theelectrode formedduring discharge
Motion only due todiffusion
Electrolyte reaching
electrode [electrolyte] insolution
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IR drop: E=IR
Overvoltage: =E-Eeq
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METHODS AND RATIONALE
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referenceelectrode
auxiliaryelectrode
workingelectrode
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Methods Rationale
A. Generating a CyclicVoltammogram
Fill cell with 1 M KNO3 Supporting electrolyte- added in excess-limit migration-ensure sufficient conductivity- sharpens the peak
Volume of electrolyte soln shouldbe enough for tip of electrode toimmerse
Ensure sufficient amt ofelectrolyte
Purge solution with N2 for 5 min. deoxygenate the sample
Can be reduced and interferew. cathodic wave
Set initial E= 600 mV and scanlimits at 600 mV and -600 mV
excitation signal
-600 mV: switching potential
Initiate scan in the negative
direction. Rate= 100 mV/s
Fe(CN)63 + e Fe(CN)6
4
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Methods Rationale
Switch on working electrode.Initiate potential scan.
Take background cyclicvoltammogram of KNO3
For calibration purposes
Turn off working electrode.Clean the cell.
Eliminate layering of analytes-alter electrode surface
Refill cell with 4 mM K3[Fe(CN)6] in1 M KNO3. Repeat procedure.(E range: 600 to -800 mV)
To obtain voltammogram of[FeIII(CN)6]
-3/[FeII(CN)6]-4
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Figure 1. Background cyclic voltammogram of
the supporting electrolyte
Figure 2. Cyclic voltammogram of the
[FeIII(CN)6]-3/[FeII(CN)6]-4 couple
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Important parameters
Epc= -0.47 V
ipc
Epa= -0.10 V
ipa
Fe(CN)63 + e Fe(CN)6
4
Fe(CN)64 Fe(CN)6
3+ e-
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Peak separation for a reversible process:
Ep > 0.0592/n, irreversible
1 electron transferred:
Theoretical: Ep = 0.0592 V
Exptl: Ep = 0.37 V
[% error: 525 %] Formal reduction potential:
Ep = |Epa - Epc| = 2.303 RT/nF = 0.0592/n V
Eo = Epa + Epc
2
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Quantitative information obtained from the
peak heights according to the RandlesSevcik
equation:
wwhere:
ip- peak current amperesn- mols of e-
A- electrode area (cm2)
D- diffusion coefficient (cm2/s)
C- conc. (mol/cm3)
V- sweep/scan rate (V/s)
ip = (2.69 x 105) n3/2 A D1/2 C v1/2
B. Effect of Scan Rate Variation Use 4 mM K3[Fe(CN)6] in 1 M
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B. Effect of Scan Rate Variation Use 4 mM K3[Fe(CN)6] in 1 M
KNO3. Scan rates 50, 80, 100, and
200 mV
scan rate = 50 mV/s
scan rate = 80 mV/s
scan rate = 100 mV/s scan rate = 200 mV/s
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Scan rate (V/s) Epa (V) Epc (V) Ep (V) E0 (V)
0.05 -0.1140 -0.4200 0.306 -0.2670
0.08 -0.0980 -0.4380 0.34 -0.2680
0.100 -0.0900 -0.4520 0.37 -0.2710
0.200 -0.0640 -0.4780 0.414 -0.2710
Irreversibilityis when the rate of electron transfer is sufficiently slow so
that the potential no longer reflects the equilibrium activity of the redox
couple at the electrode surface.
-0.2715
-0.271
-0.2705
-0.27
-0.2695
-0.269
-0.2685
-0.268-0.2675
-0.267
-0.2665
0 0.05 0.1 0.15 0.2 0.25
E0(
V)
Scan rate (V/s)
C. Effect of Electroactive Species Use 2, 6, 8, 10 mM K3[Fe(CN)6] in
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C. Effect of Electroactive Species
Concentration Variation
Use 2, 6, 8, 10 mM K3[Fe(CN)6] in
1 M KNO3. Scan rate = 100 mV.
Record also unknown solution.
Conc. = 2 mM K3[Fe(CN)6] Conc. = 6 mM K3[Fe(CN)6]
Conc. = 8 mM K3[Fe(CN)6]Conc. = 10 mM
K3[Fe(CN)6]
C. Effect of Electroactive Species Use 2, 6, 8, 10 mM K3[Fe(CN)6] in
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C. Effect of Electroactive Species
Concentration Variation
Use 2, 6, 8, 10 mM K3[Fe(CN)6] in
1 M KNO3. Scan rate = 100 mV.
Record also unknown solution.
Unknown conc.
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Concentration of
[FeIII(CN)6]-3 (mM)
Ipc(A)
2 4
4 7
6 11
8 12.2
10 15
unknown 11.5
y = 1.36x + 1.68
R = 0.97718
0
2
4
6
8
10
12
14
16
0 1 2 3 4 5 6 7 8 9 10
Ipc
(
A)
Concentration of [FeIII(CN)6]-3 (mM)
Ipc = 1.36conc + 1.68
Conc. = (11.5 - 1.68) / 1.36
Conc.(unknown) = 7.22 mM
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Unknown conc.
Conc. = 6 mM K3[Fe(CN)6] Conc. = 8 mM K3[Fe(CN)6]
D. Effect of supporting electrolyte Compare 4 mM K3[Fe(CN)6] in 1 M
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pp g y
variation
p 3[ ( )6]
KNO3 and in 1 M Na2SO4
1 M Na2SO4
1 M KNO3
KNO3 K+ + NO3
-Na2SO4 Na
+ + SO42-
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Remember
Do not stir any of the solutions when running acyclic voltammogram. But, always stir thesolution for at least 10 seconds before scanning.
Do not fill the cell any higher than 1 cm below thecover.
Make sure that the working electrode and thereference electrode are approximately at the
same height. Be sure that the surface of the working electrode
is clean.
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Migration attraction of electrode and ion
Convection laminar flowDiffusion concentration based!
SOURCES OF ERROR
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Thank You!