Electrochemistry Calculation User Guide Book: Metrohm

Electrochemistry
A workbook for 910 PSTAT mini
Monograph

All rights reserved, including translation rights.
Printed in Switzerland by Metrohm Ltd., CH-9101 Herisau, Switzerland.
8.108.5020EN – 2013-01
Barbara Zumbrägel
Electrochemistry
A workbook for 910 PSTAT mini

Electrochemistry – A workbook for 910 PSTAT mini 3
Content
Content ........................................................................................................................................3
1 Introduction ..........................................................................................................................5
2 Standard reduction potential
Reduction potential of different metals........................................................................................9
3 A reversible redox system
Cyclic voltammetry with p-aminophenol at slow scan rates .......................................................13
4 A quasi-reversible redox system
Cyclic voltammetry with p-aminophenol at fast scan rates.........................................................17
5 An irreversible redox system
Cyclic voltammetry with vitamin C.............................................................................................23
6 SAM – Self-assembled monolayers
Formation and characterization of self-assembled monolayer....................................................27
7 Quantification of vitamin C
Voltammetric determination of vitamin C on a carbon electrode ...............................................35
8 Quantification of mercury
Voltammetric determination of mercury at a gold electrode......................................................43
9 Quantification of cadmium and lead
Voltammetric determination of cadmium and lead at a mercury film electrode .........................53
10 The principle of a glucose sensor
Amperometric detection of glucose at an enzyme modified platinum electrode ........................63
11 Examples
Experiment 2: Standard reduction potential...............................................................................75
Experiment 3: A reversible redox system....................................................................................79
Experiment 4: A quasi-reversible redox system...........................................................................81
Experiment 5: An irreversible redox system ................................................................................83
Experiment 6: SAM – Self-assembled monolayers......................................................................85
Experiment 7: Quantification of vitamin C..................................................................................87
Experiment 8: Quantification of mercury....................................................................................95
Experiment 9: Quantification of cadmium and lead ................................................................ 105
Experiment 10: The principle of a glucose sensor.................................................................... 117
12 Abbreviations..................................................................................................................... 127
13 Bibliography ...................................................................................................................... 129

Introduction
1 Introduction
Electrochemistry has seen a tremendous revival in recent years. As a research tool for physical
chemists and having been a sensitive and powerful analytical technique for a long period of time
numerous new applications have now brought it back into the technological spotlight.
The most important techniques to mention here are related to the production and storage of
electrical energy. A few keywords in this context are: solar cells, batteries, fuel cells and
electromobility. All of these techniques deal with the production and storage of electrical energy and
are based on, or use, electrochemical cells. The development of electrochemical sensors has been an
important field for research and development for a number of years. Starting from classical macro
electrodes modern developments have brought new types of sensors for the detection of biological
molecules or for the detection of low level environmental contaminants.
Also, new methods for sensor production have been established: Screen-printing techniques are used
to produce sensors for routine measurements as well as for research purposes, lithographic
technologies are used to manufacture silicon-based sensors. As well as sensors for single
determinations, sensor arrays also exist that permit the determination of a number of substances in
parallel. These are known as electronic tongue or electronic nose. Miniaturization of the sensor, as
well as the electronics makes it possible to produce systems that allow the measurement of
biomolecules or pharmaceutical compounds in vivo. Even structures in nanoscale dimensions can be
depicted using technologies like scanning electrochemical microscopy.
Another important field of electrochemical application are the techniques used to characterize
surface properties: Corrosion measurements characterise the resistance of a metal against the
corrosion. Electrochemical plating technologies are used for decorative purposes and more
importantly for technical coatings in corrosion protection or in manufacturing printed circuit boards
or silicon microprocessors.
Last but not least, we should remember the classical quantitative electroanalytical techniques for the
determination of trace levels of metals or other electrochemically active substances in environmental
samples, in food, in pharmaceuticals, in quality control in the chemical industry, in mining or in the
plating industry.
A thorough understanding of the basic science is a prerequisite for successful development,
manufacture and application of all these technologies. With this monograph Metrohm presents a
small collection of basic experiments illustrating some of the essential principles of electrochemistry.
The experiments are designed to be carried out with the 910 PSTAT mini potentiostat in combination
with the disposable screen-printed electrodes. The experiment description includes detailed
information about the material required and a step-by-step guide. Examples are included in the
appendix to show what the student can expect.
The experiments include the determination of the standard reduction potential of some metal ions
using linear sweep voltammetry. Cyclic voltammetry is used for the experiments dealing with the
reversibility of electrochemical reactions, the determination of the reaction rate constant and the
diffusion coefficient. The fundamentals of quantitative analysis, like linear working range, limit of
quantification or the calibration techniques calibration curve and standard addition, are established
by means of the determination of vitamin C, mercury, cadmium and lead using differential pulse
voltammetry. The change of the surface properties of an electrode after the formation of a self-
assembled monolayer of molecules is illustrated and finally the principle of an amperometric glucose
sensor is explained.

Introduction
6 Metrohm Monograph 8.108.5020EN
1.1 General information
1.1.1 The instrument
910 PSTAT mini
1.1.2 The accessories
Screen printed electrode
USB connector – Connection to the PC
(includes power supply)
Connector for the electrode cable
6.2163.000
Status LED
Green – Instrument connected and ready
Orange – Measurement running
Red – Current overload
Electrode cable 6.2163.000
Measuring vessel cover 6.1412.010
Measuring vessel 6.1412.000
Measuring vessel holder
6.2703.020
Connector for PSTAT mini
AE (auxiliary electrode – carbon)
RE (reference electrode – silver)
Working electrode
Carbon 6.1208.110
Gold 6.1208.210
Platinum 6.1208.510
Electrical connections (AE•WE•RE)

Introduction
1.1.3 The electrode connection
Electrode connection
 The connector on the electrode cable is marked with SPE (screen printed electrode). This label and
the electrical connections on the electrode have to point in the same direction when connecting
the electrode.
 The electrical contacts of the electrode as well as the connector of the electrode cable have to be
completely dry and free from contaminants before the electrode is connected. The ingress of
moisture into the electrical contact should be avoided in any case.
Active electrode surface
 Touching the active electrode surface with bare fingers should be avoided in any case.
 The contact of the active electrode surface with the silicon of the measuring vessel cover should
be avoided. To fit the electrode into the measuring vessel cover, push the electrical contacts
through the silicon rubber.
Electrode connector
Active electrode surface (WE•AE•RE)

Standard reduction potential
2 Standard reduction potential
Reduction potential of different metals
The reduction potential is a measure for the affinity of a chemical substance to accept electrons.
Under given conditions it is specific for the element or substance. In this experiment the reduction
behavior of different metal ions will be tested and compared. The determination is carried out by
linear sweep voltammetry (LSV). For further reading on LSV see e.g. Metrohm Monograph,
Introduction to Polarography and Voltammetry(1)
or Monk, Electroanalytical Chemistry(2)
. For
further reading on the reduction potential see e.g. P.W. Atkins, Physical Chemistry(3)
or Hamann and
Vielstich, Electrochemistry(4)
.
2.1 Accessories and reagents
2.1.1 Accessories
 910 PSTAT mini
 Electrode cable 6.2163.000
 Carbon electrode 6.1208.110 (WE – C, AE – C, RE – Ag)
 Measuring vessel, measuring vessel cover and measuring vessel holder
Additional accessories (not included in the scope of delivery of the 910 PSTAT mini)
 Magnetic stirrer with stirrer bar (e.g. Metrohm 728 Stirrer)
 Pipettes
 Volumetric flasks
2.1.2 Reagents
 Potassium chloride solution, c(KCl) = 3 mol/L, e.g. Metrohm 6.2308.020
 Nitric acid, w(HNO3) = 65 %, for trace analysis*
, CAS 7697-37-2
 Gold standard solution, β(Au) = 1 g/L, H[AuCl4] in 1 mol/L HCl
 Mercury(II) nitrate monohydrate, Hg(NO3)2 · H2O, puriss. p.a., CAS 7783-34-8
 Copper nitrate trihydrate, Cu(NO3)2 · 3 H2O, puriss. p.a., CAS 10031-43-3
 Bismuth nitrate pentahydrate, Bi(NO3)3 · 5 H2O, puriss. p.a., CAS 10035-06-0
 Lead nitrate, Pb(NO3)2, p.a., CAS 10099-74-8
 Ultrapure water type 1 (electrical resistivity > 18.2 MΩ·cm, TOC < 10 ppb)
Ready-to-use solutions
Supporting electrolyte c(KCl) = 0.1 mol/L
c(HNO3) = 0.2 mol/L
Pipette 6.67 mL KCl solution (c(KCl) = 3 mol/L) into a 200 mL
volumetric flask. Add 2.856 mL nitric acid (w(HNO3) = 65%)
and make up to the mark with ultrapure water.
*
e.g. Merck suprapur®
, Sigma-Aldrich TraceSelect®
or equivalent

Au stock solution β(Au3+
) = 1 g/L
Can be used as purchased, equals 5.08 mmol/L Au3+
.
Bi stock solution c(Bi3+
) = 0.01 mol/L
Weigh in 0.485 g Bi(NO3)3 · 5 H2O and transfer into a 100 mL
volumetric flask. Add 2 mL nitric acid (w(HNO3) = 65 %) and
shake until everything is dissolved. Carefully add ultrapure
water. Make up to the mark with ultrapure water.
Cu stock solution c(Cu2+
) = 0.01 mol/L
Weigh in 0.242 g Cu(NO3)2 · 3 H2O and transfer into a 100 mL
volumetric flask. Dissolve in approx. 60 mL ultrapure water.
Add 2 mL nitric acid (w(HNO3) = 65 %) and make up to the
mark with ultrapure water.
Hg stock solution c(Hg2+
) = 0.01 mol/L
Weigh in 0.342 g Hg(NO3)2 · H2O and transfer into a 100 mL
Add 2 mL nitric acid (w(HNO3) = 65 %) and make up to the
Pb stock solution c(Pb2+
) = 0.01 mol/L
Weigh in 0.331 g Pb(NO3)2 and transfer into a 100 mL
Add 2 mL nitric acid (w(HNO3) = 65%) and make up to the
2.2 Reduction of different metals on a carbon electrode
Measuring solution
11 mL supporting electrolyte
Voltammetric parameters
Figure 1: Parameters for testing the reduction
potential of different metals (experiment 2.2).

2.2.1 Procedure
Measurement
Enter the voltammetric parameters given in Figure 1.
Reduction potential of lead
a) Prepare the measuring solution by pipetting 11 mL supporting electrolyte into the measuring
vessel. Put a stirrer bar into the measuring vessel.
b) Take a new carbon electrode (6.1208.110) and assemble it with the measuring vessel cover.
Take care not to touch the active electrode surface with bare fingers. Immerse the electrode
into the measuring solution and close the measuring vessel with the measuring vessel cover.
c) Switch on the stirrer.
d) Make sure that the electrical contacts of the electrode are dry and free from contaminants.
Then connect the electrode cable.
e) Switch off the stirrer
f) Start the measurement.
g) Repeat the measurement until the baseline is stable, which usually needs 3 to 5 replications.
The solution should be stirred before every measurement, but not during the potential scan.
h) Switch on the stirrer and add 0.2 mL of the Pb stock solution (c(Pb2+
) = 0.01 mol/L). Stir the
solution for at least 20 s.
i) Switch off the stirrer and record the curve to see the reduction of lead.
j) Save curves and parameters with «File / Save as …».
Reduction potential of copper
Repeat step a) to j) but add 0.2 mL of the Cu stock solution (c(Cu2+
) = 0.01 mol/L) instead in step h).
Reduction potential of bismuth
Repeat step a) to j) but add 0.2 mL of the Bi stock solution (c(Bi3+
Reduction potential of mercury
Repeat step a) to j) but add 0.2 mL of the Hg stock solution (c(Hg2+
Reduction potential of gold
Repeat step a) to j) but add 0.4 mL of the Au stock solution (β(Au3+
) = 1 g/L) instead in step h).
Evaluation
k) Evaluate the potential at the peak maximum of the reduction signal for the individual metal
ions as described in 2.2.2.
l) Compare the values for the peak maximum for the different metals and make a list sorted by
their reduction potential.
m) Compare the observed reduction potentials with data for the standard reduction potential
which can be found in literature. Think about reasons for the differences in the values.

2.2.2 Curve evaluation
Compare the baseline of the supporting electrolyte with the curve after the addition of the metal. In
scan direction, the first sharp increase in negative current indicates the beginning of the reduction of
the added metal. Evaluate the potential of the corresponding peak maximum.
Figure 2: Example for the curve
evaluation of experiment 2.2.
(–– electrolyte, –– with added
metal solution)
2.2.3 Additional information
Note! Mercury, lead and copper and their salts are very toxic to the environment. If the standard
solutions cannot be used anymore take care of an appropriate disposal.
 It is recommended to use a new electrode for every metal to be tested. In most cases it is not
possible to remove the metal quantitatively from the working electrode. Any remaining metals can
influence the reduction behavior of other metals in the following experiments.
Begin of
reduction
Scan direction
Peak maximum

A reversible redox system
3 A reversible redox system
Cyclic voltammetry with p-aminophenol at slow scan rates
Cyclic voltammetry is a valuable tool to study the mechanism and the reversibility of electrode
reactions. The organic compound p-aminophenol is used as an example for a substance showing
reversible behavior at slow scan rates. In this experiment the reversibility will be reviewed and the
diffusion coefficient of the oxidized and reduced species will be calculated from the experimental
data using the Randles-Sevcik equation. For further reading on cyclic voltammetry and reversibility of
redox systems see e.g. Bond, Broadening Electrochemical Horizons(5)
or Bard and Faulkner,
Electrochemical Methods(6)
.
3.1.1 Accessories
 910 PSTAT mini
 Electrode 6.1208.110 (WE – C, AE – C, RE – Ag)
 Pipettes
3.1.2 Reagents
 Ammonia solution, for analysis, w(NH3) = 25 %, CAS 1336-21-6
 Hydrochloric acid, for analysis, w(HCl) = 30 %, CAS 7647-01-0
 Sulfuric acid, for analysis, w(H2SO4) = 96 %, CAS 7664-93-9
 p-Aminophenol hydrochloride, H2NC6H4OH · HCl, MW 145.59 g/mol, CAS 51-78-5
Ammonia buffer pH 9.5 c(NH4Cl) = 1 mol/L
c(NH3) = 2 mol/L
Fill approx. 300 mL ultrapure water into a 500 mL volumetric
flask. Carefully add 53 mL HCl (30 %) and 112.5 mL NH3 (25
%). After cooling down to room temperature make up to the
Diluted sulfuric acid c(H2SO4) = 0.5 mol/L
Fill approx. 900 mL ultrapure water into a 1 L volumetric flask.
Carefully add 27.78 mL sulfuric acid (w(H2SO4) = 96%).
Attention, the solution becomes very hot! After cooling down
to room temperature make up to the mark with ultrapure
water.

p-AP stock solution c(p-AP) = 0.01 mol/L
Dissolve 0.145 g p-aminophenol hydrochloride in 10 mL
c(H2SO4) = 0.5 mol/L. Fill up to 100 mL with ultrapure water
3.2 Experiment
3.2.1 Procedure
Measuring solution
10 mL H2O
1 mL ammonia buffer pH 9.5
0.1 mL p-AP stock solution (c(p-AP) = 0.01 mol/L)
Figure 3: Parameters for experiment 3.2.
Measurement
a) Prepare the measuring solution by pipetting 10 mL ultrapure water, 1 mL ammonia buffer and
0.10 mL p-AP stock solution (0.01 mol/L) into the measuring vessel. Put a stirrer bar into the
measuring vessel and stir the solution well.
c) Make sure that the electrical contacts of the electrode are dry and free from contaminants.
d) Record the cyclic voltammogram with the voltammetric parameters from Figure 3. Make sure
the stirrer is switched off during the measurement. Save the voltammogram together with the
method parameters.

e) Stir the solution.
f) Change the scan rate in the voltammetric parameters to 0.02 V/s and record another cyclic
voltammogram using the same electrode. Make sure the stirrer is switched off during the
measurement.
g) Save the voltammogram together with the method parameters.
h) Repeat step e) to g) also with scan rates of 0.03, 0.04 and 0.05 V/s.
Evaluation
i) Evaluate peak height and peak potential for the different scan rates as described in 3.2.2.
j) Use the criteria mentioned in 3.2.3 to assess if the reaction is reversible. Propose a mechanism
for the reaction that is observed in the cyclic voltammogram.
k) Plot a graph with the peak height as a function of the square root of the scan rate √ for the
anodic signal as well as the cathodic signal. Calculate the linear regression for the two curves
and the diffusion coefficient for the reduced and the oxidized species using the slope of the
linear regression and the Randles-Sevcik equation.
Evaluate the peak potential and the peak height of the anodic peak as well as of the cathodic peak.
For the peak potential the cursor or «Peak measurement tool 1» can be used. For the evaluation of
the peak height it is recommended to use the «Step measurement tool» since this allows the
evaluation from the residual current to the peak maximum.
Figure 4: Example for the
evaluation of peak height in
experiment 3.2.

Criteria for a reversible process
 The peak potential is independent of the scan rate .
 The difference between anodic peak potential and cathodic peak potential is described
by (Eq. 1).
(Eq. 1) – Peak potential of the anodic signal
– Peak potential of the cathodic signal
– Molar gas constant (8.314 J·mol-1
·K-1
)
– Temperature in K
– Faraday constant (9.648·104
C·mol-1
)
– Number of electrons
For T = 298 K
(Eq. 2)
 Peak height √ .
 Anodic peak height and cathodic peak height are equal.
Randles-Sevcik equation
√ (Eq. 3) – Peak height
– Area of the working electrode
– Concentration
– Diffusion coefficient
– scan rate
Stability of p-aminophenol
p-Aminophenol is not very stable in alkaline solution. Therefore the measurements at different scan
rates should be done without interruption.
In alkaline solution p-aminophenol is oxidized by oxygen from ambient air to 4-imino-cyclohexa-2,5-
dienone, which can then easily polymerize:
Figure 5: Oxidation of
p-aminophenol
The reaction is indicated by a slight yellow color of the measuring solution. The polymer forms a
brown precipitate.
NH2
OH
O2
NH
O
O
H2
OH
1/2
+ +

A quasi-reversible redox system
4 A quasi-reversible redox system
Cyclic voltammetry with p-aminophenol at fast scan rates
reactions. Richard S. Nicholson(7)
developed and published a simple method to evaluate the standard
rate constant for the electron transfer from the peak potential separation and the scan rate of a
quasi-reversible system. As an example for a quasi-reversible system p-aminophenol will be used
again, but unlike in experiment 3 the measurement will be carried out at faster scan rates. In this
experiment the reversibility will be reviewed and Nicholson’s method will be used to calculate the
standard rate constant from the experimental data. For further reading on cyclic voltammetry and
reversibility of redox systems see e.g. Bond, Broadening Electrochemical Horizons(5)
or Bard and
Faulkner, Electrochemical Methods(6)
.
4.1.1 Accessories
 910 PSTAT mini
 Pipettes
4.1.2 Reagents
 Ammonia solution, for analysis, w(NH3) = 25 %, CAS 1336-21-6
 Hydrochloric acid, for analysis, w(HCl) = 30 %, CAS 7647-01-0
 Sulfuric acid, for analysis, w(H2SO4) = 96 %, CAS 7664-93-9
 p-Aminophenol hydrochloride, H2NC6H4OH · HCl, MW 145.59 g/mol, CAS 51-78-5
Ammonia buffer pH 9.5 c(NH4Cl) = 1 mol/L
c(NH3) = 2 mol/L
flask. Carefully add 53 mL HCl (30 %) and 112.5 mL NH3
(25 %). After cooling down to room temperature make up to
the mark with ultrapure water.
Diluted sulfuric acid c(H2SO4) = 0.5 mol/L
Fill approx. 900 mL ultrapure water into a 1 L volumetric flask.
Carefully add 27.78 mL sulfuric acid (w(H2SO4) = 96 %).
Attention, solution becomes very hot! After cooling down to
room temperature make up to the mark with ultrapure water.

p-AP stock solution c(p-AP) = 0.01 mol/L
Dissolve 0.145 g p-aminophenol hydrochloride in 10 mL
c(H2SO4) = 0.5 mol/L. Fill up to 100 mL with ultrapure water.
4.2 Experiment
4.2.1 Procedure
Measuring solution
10 mL H2O
1 mL ammonia buffer pH 9.5
0.1 mL p-AP stock solution (0.01 mol/L)
Measurement
a) Prepare the measuring solution by pipetting 10 mL ultrapure water, 1 mL ammonia buffer and
0.10 mL p-AP stock solution (0.01 mol/L) into the measuring vessel. Put a stirrer bar into the
d) Record the cyclic voltammogram with the voltammetric parameters shown in Figure 6. Make
sure the stirrer is switched off during the measurement.

e) Save the voltammogram together with the method parameters.
f) Stir the solution.
g) Change the scan rate in the voltammetric parameters to 0.2 V/s and record another cyclic
measurement.
h) Save the voltammogram together with the method parameters.
i) Repeat step f) to h) also with scan rates of 0.3, 0.4 and 0.5 V/s.
Evaluation
j) Evaluate peak height and peak potential for the different scan rates as described in 4.2.2.
k) Use the criteria mentioned in 4.2.3 to assess if the reaction is reversible.
l) Calculate the standard rate constant from the peak potential separation in your
experiment. The necessary formula (Eq. 4) and the tabled values for the charge transfer
parameter 𝜓 (Figure 8) can be found in 4.2.3.
Evaluate the peak potential and the peak height of the anodic signal as well as of the cathodic signal.
For the peak potential the cursor or «Peak measurement tool 1» can be used. For the evaluation of
the peak height it is recommended to use the «Step measurement tool» since this allows the
evaluation from the residual current to the peak maximum.
experiment 4.2.

Standard rate constant for electron transfer according to Nicholson(7)
𝜓
√
(Eq. 4)
√
𝜓 – Charge transfer parameter
– Charge transfer coefficient
– Standard rate constant for electron transfer
– Scan rate
– Diffusion coefficient of the reduced species
– Diffusion coefficient of the oxidized species
– Number of electrons
– Faraday constant (9.648·104
C·mol-1
)
– Molar gas constant (8.314 J·mol-1
·K-1
)
– Temperature in K
(a) * † / mV
20 61
7 63
6 64
5 65
4 66
3 68
2 72
1 84
0.75 92
0.5 105
0.35 121
0.25 141
0.1 212
(b)
Figure 8: Variation of peak potential separations with kinetic parameters for cyclic voltammetry. (a) table (b)
semi-logarithmic plot of the table values
(7)
For 𝜓 the values of are nearly independent from  if 0.3 <  < 0.7, therefore can
be used as a good approximation for the calculation.
If experiment 3 is not carried out to determine the diffusion coefficients, the following values can be
used for the calculation:
= 3.81·10-5
cm2
·s-1
= 3.17·10-5
cm2
·s-1
*
See (Eq. 4)
†
For  = 0.5
50
70
90
110
130
150
170
190
210
230
0.1 1 10
D
E
p
·n
/
mV

Criteria for a reversible process
 The peak potential is independent of the scan rate .
 The difference between anodic peak potential and cathodic peak potential is described
by (Eq. 2).
(for T = 298 K) (Eq. 2)
 Peak height √ .
 Anodic peak height and cathodic peak height are equal.
Stability of p-aminophenol
p-Aminophenol is not very stable in alkaline solution. Therefore the measurements at different scan
rates should be done without interruption.
In alkaline solution p-aminophenol is oxidized by oxygen from ambient air to 4-imino-cyclohexa-2,5-
dienone, which can then easily polymerize:
Figure 9: Oxidation of
p-aminophenol
The reaction is indicated by a slight yellow color of the measuring solution. The polymer forms a
brown precipitate.
Auto current ranging
For fast scan rates the auto current ranging has to be switched off. The current range of the
potentiostat has to be set to ±100 µA or ±10 µA depending on the maximum current that needs to
be measured.
NH2
OH
O2
NH
O
O
H2
OH
1/2
+ +

An irreversible redox system
5 An irreversible redox system
Cyclic voltammetry with vitamin C
reactions. Ascorbic acid, also known as vitamin C, is used as an example for a substance showing
irreversible behavior. In this experiment the reversibility will be reviewed. For further reading on cyclic
voltammetry and reversibility of redox systems see e.g. Bond, Broadening Electrochemical Horizons(5)
or Bard and Faulkner, Electrochemical Methods(6)
.
5.1.1 Accessories
 910 PSTAT mini
 Pipettes
5.1.2 Reagents
 Potassium chloride solution, c(KCl) = 3 mol/L, e.g. Metrohm 6.2308.020
 Ascorbic acid, puriss. p.a., C6H8O6, CAS 50-81-7
Supporting electrolyte c(KCl) = 0.1 mol/L
Pipette 6.67 mL KCl solution (c(KCl) = 3 mol/L) into a 200 mL
volumetric flask and make up to the mark with ultrapure
water.
Vitamin C standard solution c(Vitamin C) = 0.1 mol/L
Weigh in 0.88 g ascorbic acid and transfer it into a 50 mL
volumetric flask. Dissolve and make up to the mark with
ultrapure water.
Since vitamin C is sensitive against oxygen and light it is
recommended to use deaerated ultrapure water for the
preparation and keep the standard in the dark. Only use
standard solution that is prepared the same day.

5.2 Experiment
5.2.1 Procedure
Measuring solution
0.1 mL Vitamin C standard solution (0.1 mol/L)
Measurement
a) Prepare the measuring solution by pipetting 11 mL supporting electrolyte and 0.10 mL
vitamin C standard solution (0.1 mol/L) into the measuring vessel. Put a stirrer bar into the
d) Record the cyclic voltammogram with the voltammetric parameters from Figure 10. Make
sure the stirrer is switched off during the measurement. Save the voltammogram together
with the method parameters.
e) Stir the solution.
f) Change the scan rate in the voltammetric parameters to 0.1 V/s and record another cyclic
measurement.
h) Repeat step e) to g) also with scan rates of 0.15, 0.2 and 0.25 V/s.

Evaluation
i) Evaluate peak height and peak potential for the different scan rates as described in 5.2.2.
j) Assess the influence of the scan rate on peak height and peak potential, find arguments why
it is an irreversible reaction and suggest a mechanism for the reaction that is seen in the
voltammogram.
Evaluate the peak potential and the peak height of the anodic peak. For the peak potential the cursor
or «Peak measurement tool 1» can be used. For the evaluation of the signal height it is recommended
to use the «Step measurement tool» since this allows the evaluation from the residual current to the
peak maximum.
experiment 5.2.

SAM – Self-assembled monolayers
6 SAM – Self-assembled monolayers
Formation and characterization of self-assembled monolayer
«Molecular self-assembly is the assembly of molecules without guidance or management from an
outside source.»(8)
An increasing number of publications can be found on this topic. The field of
applications ranges from biology and biosensors to electrochemistry and electronics to material
science and nanotechnology. A simple way of generating a self-assembled and organized monolayer
is to use the affinity of a thiol compound to a gold substrate. This experiment is a brief introduction
into coating and shows a simple electrochemical method to assess the quality of the self-assembled
monolayer. For further reading on self-assembly and the theory of self-assembled monolayers see
e.g. Sigma-Aldrich, Molecular Self-Assembly(8)
or Bond, Broadening Electrochemical Horizons(5)
.
Figure 12: Illustration of the assembly of
2-mercapto acetic acid (2-MAA), 3-mercapto
propionic acid (3-MPA), 6-mercapto hexanoic
acid (6-MHA) and 11-mercapto undecanoic
acid (11-MUA) to a gold electrode surface.
6.1.1 Accessories
 910 PSTAT mini
 Electrode 6.1208.210 (WE – Au, AE – C, RE – Ag)
 Pipettes

 Ultrasonic bath
 Small sample containers with cap (inner diameter approx. 1.5 cm) to hold the electrode during
self-assembly (e.g. Metrohm sample tubes 15 mL (6.2747.000))
 Tweezers
6.1.2 Reagents
 2-Mercapto acetic acid, HSCH2COOH, CAS 68-11-1
 3-Mercapto propionic acid, HSC2H4COOH, CAS 107-96-0
 6-Mercapto hexanoic acid, HSC5H10COOH, CAS 17689-17-7
 11-Mercapto undecanoic acid, HSC10H20COOH, CAS 71310-21-9
 Ethanol, puriss. p.a., CAS 64-17-5
 Potassium hexacyanoferrate(III), K3[Fe(CN)6], puriss. p.a., CAS 13746-66-2
 Acetic acid, w(CH3COOH) = 100 %, for trace analysis*
, CAS 64-19-7
 Ammonia solution, w(NH3) = 25 %, for trace analysis*
, CAS 1336-21-6
Ammonium acetate buffer
pH 4.6
c(CH3COOH) = 2 mol/L
c(NH3) = 1 mol/L
flask. Carefully add 55.5 mL acetic acid (100 %) and 37 mL
NH3 (25 %). Make up to the mark with ultrapure water.
2-MAA stock solution c(MAA) = 0.1 mol/L
Dissolve 92 mg 2-mercapto acetic acid (equals 69.4 µL) in
10 mL ethanol. The solution is stable for at least a month if
stored in the freezer.
3-MPA stock solution c(MPA) = 0.1 mol/L
Dissolve 106 mg 3-mercapto propionic acid (equals 87 µL) in
10 mL ethanol. The solution is stable for at least a month if
6-MHA stock solution c(MHA) = 0.1 mol/L
Dissolve 148 mg 6-mercapto hexanoic acid (equals 138.4 µL)
in 10 mL ethanol. The solution is stable for at least a month if
11-MUA stock solution c(MUA) = 0.1 mol/L
Dissolve 218 mg 11-mercapto undecanoic acid in 10 mL
ethanol. The solution is stable for at least a month if stored in
the freezer.
Hexacyanoferrate(III) stock
solution
c([Fe(CN)6]3-
) = 0.1 mol/L
Dissolve 0.33 g potassium hexacyanoferrate(III) in 10 mL
ultrapure water. The solution should be prepared freshly at the
day of use.
*
or equivalent

6.2 Experiment
6.2.1 Self-assembly
The self-assembly happens spontaneously, however the electrode needs to be prepared for the
coating. The electrode has to be cleaned initially by sonication in ethanol. Then it is electrochemically
conditioned before it is immersed into the coating solution for the self-assembly of the monolayer.
The coating usually takes about two days. First results can be seen after 24 h. But results are usually
much better if 48 h are allowed for self-assembly.
Cleaning of the electrode
Cleaning solution
Ethanol
Cleaning procedure
a) Place all gold electrodes (6.1208.210) that should be coated side by side in a bowl with
ethanol (cleaning solution) and sonicate them for approx. 15 minutes. The electrodes should
not be placed on top of each other to prevent damage of the active electrode surface.
Electrochemical conditioning of the electrode
Conditioning solution
10 mL H2O
1 mL ammonium acetate buffer pH 4.6
Figure 13: Parameters for the cyclic voltammetric
conditioning of the electrode in experiment 6.2.

Conditioning procedure
b) Prepare the conditioning solution by pipetting 10 mL ultrapure water and 1 mL ammonium
acetate buffer pH 4.6 into the measuring vessel. Put a stirrer bar into the measuring vessel and
stir the solution well.
c) Enter the parameters given in Figure 13.
d) Take one of the cleaned gold electrodes out of the ethanol. Rinse it thoroughly with ultrapure
water and assemble it with the measuring vessel cover. Take care not to touch the active
electrode surface with bare fingers. Immerse the electrode into the conditioning solution and
close the measuring vessel with the measuring vessel cover.
e) Use a soft tissue to thoroughly dry the electrical contacts of the electrode. Make sure that the
contacts are completely dry and free from contaminants before connecting the electrode
cable.
f) For electrochemical conditioning run one cyclic voltammogram in the conditioning solution.
Self-assembly
Coating solutions*
2-MAA 2.97 mL ethanol
0.03 mL 2-MAA stock solution
3-MPA 2.97 mL ethanol
0.03 mL 3-MPA stock solution
6-MHA 2.97 mL ethanol
0.03 mL 6-MHA stock solution
11-MUA 2.97 mL ethanol
0.03 mL 11-MUA stock solution
Coating procedure
g) Prepare the 2-MAA coating solution by pipetting 2.97 mL ethanol and 0.03 mL 2-MAA stock
solution into a sample tube 6.2747.000. If another vessel with different dimensions is used,
the volumes have to be adapted. It is important that the active electrode surface can be
completely immersed into the coating solution.
h) Take a gold electrode after electrochemical conditioning (step f) and thoroughly rinse it with
ultrapure water. Take care not to touch the active electrode surface with bare fingers.
i) Immerse the electrode into the sample tube with the 2-MAA coating solution. One sample
tube can hold two electrodes back-to-back for modification. Close the sample tube with the
cap to prevent the evaporation of ethanol.
j) Repeat step g) to i) with other cleaned electrodes and immerse them into sample tubes filled
with an appropriate volume of 3-MPA coating solution, 6-MHA coating solution or 11-MUA
coating solution. Make sure the sample tubes are properly closed to prevent the loss of
ethanol.
k) Leave the electrodes in the coating solutions for 2 days. First results can be seen after 24 h.
But results are usually much better if 48 h are allowed for self-assembly.
*
Volumes are for the use of Metrohm sample tubes 15 mL (6.2747.000)

6.2.2 Characterization of the monolayer by cyclic voltammetry
The thickness of a monolayer ranges from a few tenth of a nanometer to a few nanometers, a size
which cannot be seen visually. Therefore technical equipment is required to characterize the
monolayer. Usually sophisticated instruments, like scanning tunneling microscopes (STM) or atomic
force microscopes (AFM), are used. For studying the structure of monolayers these techniques are
essential, but sometimes a more simple approach will do. In a cyclic voltammetric measurement the
reaction [Fe(CN)6]3-
+ e-
⇌ [Fe(CN)6]4-
shows one distinct oxidation and one distinct reduction signal.
The presence of a coating at the electrode will have an influence on the measurement of these
signals. This effect can be used for an indirect characterization and comparison of electrodes with
different coatings.
Measuring solution
10 mL H2O
1 mL ammonium acetate buffer
0.1 mL hexacyanoferrate(III) stock solution
Figure 14: Parameters for testing the monolayer by
cyclic voltammetry (experiment 6.2).
Measurement
a) Prepare the measuring solution by pipetting 10 mL ultrapure water, 1 mL ammonium acetate
buffer pH 4.6 and 0.1 mL hexacyanoferrate(III) stock solution into the measuring vessel. Put a
stirrer bar into the measuring vessel and stir the solution well.
b) Use tweezers to take the electrode out of the 2-MAA coating solution.
c) Rinse the electrode thoroughly with ultrapure water and assemble it with the measuring
vessel cover. Take care not to touch the active electrode surface with bare fingers. Immerse
the electrode into the measuring solution and close the measuring vessel with the measuring
vessel cover.

d) Use a soft tissue to thoroughly dry the electrical contacts of the electrode. Make sure that the
contacts are completely dry and free from contaminants before connecting the electrode
cable.
e) Record the cyclic voltammogram with the voltammetric parameters given Figure 14. Make
sure the stirrer is switched off during the measurement.
f) Repeat step b) to e) with electrodes coated with 3-MPA, 6-MHA and 11-MUA instead of 2-
MAA.
Evaluation
g) Evaluate peak height of the cathodic signal as described in 6.2.3.
h) Plot a graph of the peak height as a function of the number of C atoms in the spacer group in
the molecule. What can be observed?
In principle the reduction and the oxidation signal can be used for the characterization. But in the
described measuring solution the effect of the monolayer on this cathodic signal is usually more
pronounced. This signal is related to the reduction [Fe(CN)6]3-
+ e-
⟶ [Fe(CN)6]4-
. For the evaluation of
the peak height it is recommended to use the «Step measurement tool».
experiment 6.2.

Note! 2-mercapto acetic acid and 3-mercapto propionic acid are toxic to the environment. If their
solutions cannot be used anymore take care of an appropriate disposal.
The process of self-assembly is rather sensitive to contamination of the reagents and electrodes.
Therefore it is recommended to:
 Work in a clean environment.
 Wear gloves when handling the electrodes, since the oil from finger prints can inhibit the
adsorption of the thiols.
 Make sure that all equipment (glassware, sample tubes, tweezers, …) is sufficiently clean. If you
are not sure, everything should be rinsed several times with ethanol.
 New accessories which were not used for this experiment before, especially the sample tubes,
should be soaked in ethanol for a few days.
 Label the volumetric flasks and sample tubes and always use the same containers for the
experiment.
Further useful information on the theory of self-assembly and on the preparation of SAM can be
found in literature e.g. from Sigma-Aldrich (8)
.

Quantification of vitamin C
7 Quantification of vitamin C
Voltammetric determination of vitamin C on a carbon electrode
As discussed in experiment 5, vitamin C can be easily oxidized to dehydroascorbic acid on a carbon
electrode:
Figure 16: Oxidation
of vitamin C
Besides kinetic studies this reaction can also be used to determine the concentration of vitamin C in
samples. Vitamin C has antioxidant properties and can be found in many foodstuffs. It is often
determined by titration, however voltammetry is more selective since other oxidizing or reducing
substances do not interfere. The determination is carried out by differential pulse voltammetry (DP).
DP shows increased sensitivity compared to linear sweep voltammetry (LSV) and cyclic voltammetry
(CV). Therefore DP is the method of choice for quantitative determinations. For further reading on
differential pulse votlammetry and on the quantification of vitamin C see e.g. Thomas and Henze,
Voltammetric Analysis(9)
.
In the first part of the experiment the limits of this method, like linear working range and limit of
quantification, will be determined. With this background the concentration of vitamin C in a
multivitamin product will be determined in the second part of the experiment. The quantification will
be carried out by calibration curve technique as well as by standard addition technique.
7.1.1 Accessories
 910 PSTAT mini
 Pipettes
7.1.2 Reagents
 Ascorbic acid, puriss. p.a., C6H8O6, CAS 50-81-7
, CAS 64-19-7
, CAS 1336-21-6
*
or equivalent
O
OH
O
H
O
O
H
O
H
H
+
e O O
O
H
O
H
O O
- 2 - 2

Ammonium acetate buffer
pH 4.6
c(CH3COOH) = 2 mol/L
c(NH3) = 1 mol/L
flask. Carefully add 55.5 mL acetic acid (100 %) and 37 mL
NH3 (25 %). Make up to the mark with ultrapure water.
Vitamin C standard stock
solution
β(Vitamin C) = 10 g/L
Weigh in 0.5 g ascorbic acid and transfer it into a 50 mL
ultrapure water.
Since vitamin C is sensitive to oxygen and light it is
recommended to use deaerated ultrapure water for the
preparation and keep the standard in the dark. Only use
standard solution that is prepared the same day.
Vitamin C standard solution β(Vitamin C) = 1 g/L
Use deaerated ultrapure water to dilute 1 mL vitamin C
standard stock solution to 10 mL.
7.2 Experiment
7.2.1 Linear working range
Measuring solution
10 mL H2O
0.02 mL vitamin C standard stock solution (β(Vitamin C) = 10 g/L)
Figure 17: Parameters for the determination of
vitamin C (experiment 7.2).

Measurement
a) Prepare the measuring solution by pipetting 10 mL H2O, 1 mL ammonium acetate buffer and
0.02 mL vitamin C standard stock solution (β(Vitamin C) = 10 g/L) into the measuring vessel.
Put a stirrer bar into the measuring vessel and stir the solution well.
d) Record the voltammogram with the voltammetric parameters shown in Figure 17. Make sure
the stirrer is switched off during the measurement.
e) Save the voltammogram together with the method parameters.
f) Add another 0.02 mL of the vitamin C standard stock solution (β(Vitamin C) = 10 g/L). Stir the
solution.
g) Record another voltammogram using the same electrode. Make sure the stirrer is switched off
during the measurement.
i) Repeat step f) to h) until you have recorded curves with 10 different concentrations.
Evaluation
j) Evaluate the peak height for the individual concentrations as described in 7.2.4.
k) Plot a graph with the peak height as a function of the concentration.
l) From the graph determine the concentration range where there is a linear relation between
the concentration and the peak height.
7.2.2 Limit of quantification
In the literature many different approaches for the determination of the limit of determination (LOD)
and the limit of quantification (LOQ) are described. The choice is from the simple consideration of the
background noise as a measure for the sensitivity to rather complex statistical examinations of the
error of the measurement, which requires numerous measuring. For practical application the so
called «regression approach»(10)
was found to be very useful. On the one hand it is easy to carry out,
on the other hand it provides realistic values for the critical value or critical level (LC) and minimum
quantifiable (true) value or quantification limit (LQ), as the LOD and the LOQ should be named
according to IUPAC(11)
. In principle the regression approach is a simplified statistical approach. It uses
the residual standard deviation of a calibration curve recorded in the concentration range of the LOQ
for the calculation. The calibration curve has to fulfill the following requirements:
 Linear relation between concentration and signal, calibration curve y = A + B·x
 Blank measurement (c = 0) has to be included in the calibration curve
 5 to 10 calibration standards, calibration points equidistant
 5 to 10 replications per standard, same number of replications per standard
 Min. 40 measuring points for c ≠ 0
 Lowest concentration in the range of LOQ
 Highest concentration 10 ... 30 · LOD
 Standard addition can be used to record the calibration curve
 Standard deviation is homogenous (homoscedastic)
For the calculations the following rules should be considered:

Blank signals (c = 0) are included in the calculation of the residual standard deviation .
Blank signals (c = 0) are not included for the calculation of parameters A (intercept) and B (slope) of
the linear regression.
Formulas
y = A + B x (Eq. 5) y – Peak height
x – Concentration of the analyte
A – Intercept of the linear regression
B – Slope of the linear regression
∑
( ̂ ) (Eq. 6) – Standard error of estimate (residual
standard deviation) in regression
– Variance of
– Signal value of the ith
point in the
regression
̂ – Regression value of the signal at the ith
point of the linear regression
– Number of points on the regression
– Number of calibration standards
– Number of regression parameters (for
linear regression = 2)
oncentration (Eq. 7)
oncentration
10
(Eq. 8)
Recording the calibration curve for the determination of LOQ
Measuring solution
10 mL H2O
Standard addition
5 additions of 0.02 mL standard (β(Vitamin C) = 1 g/L) each.
See Figure 17.
Measurement
a) Prepare the measuring solution by pipetting 10 mL H2O and 1 mL ammonium acetate buffer
into the measuring vessel. Put a stirrer bar into the measuring vessel and stir the solution well.
d) Record the voltammogram with the voltammetric parameters shown in Figure 17. Make sure
the stirrer is switched off during the measurement.

e) Stir the solution and repeat the measurement of the blank (c = 0). Make sure the stirrer is
switched off during the measurement. In total 10 replications are required.
f) Save the voltammograms together with the method parameters.
g) Add 0.02 mL of the vitamin C standard solution (β(Vitamin C) = 1 g/L). Stir the solution.
h) Record another voltammogram using the same electrode. Make sure the stirrer is switched off
i) Stir the solution and repeat the measurement of this concentration. Make sure the stirrer is
switched off during the measurement. In total 10 replications are required.
j) Save the voltammograms together with the method parameters.
k) Repeat point g) to j) until you have recorded curves with 5 different concentrations.
Evaluation
l) Evaluate the peak height for the individual concentrations as described in 7.2.4.
m) Plot a graph with the peak height as a function of concentration.
n) Calculate the linear regression of the calibration curve.
o) Calculate the residual standard deviation of the calibration curve.
p) Using the residual standard deviation calculate the LOD and the LOQ of the vitamin C
determination.
7.2.3 Determination of vitamin C in multivitamin products
The voltammetric determination of vitamin C in a sample requires the calibration of the method. In
principle there are two ways, calibration curve or standard addition. Carry out both and discuss
advantages and disadvantages of the two calibration techniques. Decide, which one is recommended
for this application.
Calibration curve
Measuring solution «calibration curve»
10 mL H2O
0.05 mL vitamin C standard solution (β(Vitamin C) = 1 g/L)
Measuring solution «sample»
10 mL H2O
0.5 mL sample solution
See Figure 17.
Recording the calibration curve
a) Prepare the measuring solution «calibration curve» by pipetting 10 mL H2O, 1 mL ammonium
acetate buffer and 0.05 mL vitamin C standard solution (β(Vitamin C) = 1 g/L) into the
measuring vessel. Put a stirrer bar into the measuring vessel and stir the solution well.

d) Record the voltammogram with the voltammetric parameters from Figure 17. Make sure the
stirrer is switched off during the measurement. Save the voltammogram together with the
method parameters.
e) Add 0.05 mL of the vitamin C standard solution (β(Vitamin C) = 1 g/L). Stir the solution.
f) Record another voltammogram using the same electrode. Make sure the stirrer is switched off
h) Repeat step e) to g) until you have recorded curves with 8 to 10 different concentrations.
Establishing the calibration curve
i) Evaluate the peak height for the individual concentrations as described in 7.2.4.
j) Plot a graph with peak height as a function of the concentration and calculate the linear
regression of the calibration curve.
Determination in the sample
k) Prepare the measuring solution «sample» by pipetting 10 mL H2O, 1 mL ammonium acetate
buffer and 0.5 mL sample solution into the measuring vessel. Put a stirrer bar into the
l) Take a new carbon electrode (6.1208.110) and assemble it with the measuring vessel cover.
m) Make sure that the electrical contacts of the electrode are dry and free from contaminants.
n) Record the voltammogram with the voltammetric parameters from Figure 17. Make sure the
method parameters.
o) Evaluate the peak height for the vitamin C in the sample as described in 7.2.4.
p) Compare the peak height with the calibration curve and calculate the concentration of
vitamin C in the sample.
Standard addition
Measuring solution sample
10 mL H2O
Standard addition
Concentration is quantified by 2 additions of 0.1 mL standard (β(Vitamin C) = 1 g/L).
See Figure 17.

Measurement
a) Prepare the measuring solution by pipetting 10 mL H2O, 1 mL ammonium acetate buffer and
0.5 mL sample (e.g. multi-vitamin drink) into the measuring vessel. Put a stirrer bar into the
d) Record the voltammogram with the voltammetric parameters from Figure 17. Make sure the
method parameters.
e) Add 0.1 mL of the vitamin C standard solution (β(Vitamin C) = 1 g/L). Stir the solution.
f) Record another voltammogram using the same electrode. Make sure the stirrer is switched off
h) Add another 0.1 mL of the vitamin C standard solution (β(Vitamin C) = 1 g/L). Stir the solution.
i) Record another voltammogram using the same electrode. Make sure the stirrer is switched off
j) Save the voltammogram together with the method parameters.
Evaluation
k) Evaluate the peak height for the sample and the two standard additions as described in 7.2.4.
l) Plot a graph with peak height as a function of the concentration. The concentration in the
sample is set to zero.
m) Calculate the linear regression for the standard addition curve.
n) Extrapolate the linear regression onto the x-axis (concentration axis) to get the negative
concentration of vitamin C in the measuring solution. Calculate the concentration of vitamin C
in the sample from this value.

For the evaluation of the peak height «Peak measurement tool 1» can be used.
Peak potential of vitamin C is approx. +0.2 V.
evaluation of peak height
(c(vitamin C)  55 mg/L) in
experiment 7.2.
 The lifetime of the carbon electrode is limited. If measurements are done in clean standard
solutions, several measurements at thesame electrode are possible. A calibration curve for
example can be recorded using just one electrode. However, as soon as the matrix of a real
sample is involved, the lifetime decreases. For samples usually only one determination including
the standard additions is possible. A further determination at thesame electrode is not possible
anymore.

Quantification of mercury
8 Quantification of mercury
Voltammetric determination of mercury at a gold electrode
Mercury and its compounds are toxic and therefore their quantification, especially in environmental
samples, is of great interest. The determination of mercury by anodic stripping voltammetry (ASV) is
relatively easy. Stripping voltammetry in general is a two-step method which consists of a
preconcentration and a subsequent determination step. The preconcentration allows a significant
increase in sensitivity compared to a direct measurement. For the determination of mercury the
preconcentration step is a reduction. Mercury ions in the measuring solution are reduced at the gold
working electrode and deposited at the gold as an amalgam.
Preconcentration: Hg2+
+ 2 e-
 Hg0
(Au)
In the subsequent determination step the mercury is anodically stripped off the electrode, which
means the deposited mercury is re-oxidized.
Anodic stripping: Hg0
(Au)  Hg2+
+ 2 e-
The determination is carried out by differential pulse voltammetry (DP). DP shows increased sensitivity
compared to linear sweep voltammetry (LSV) and cyclic voltammetry (CV). Therefore DP is the
method of choice for quantitative determinations. For further reading on differential pulse
voltammetry and on the quantification of mercury see e.g. Thomas and Henze, Voltammetric
Analysis(9)
or Metrohm Application Bulletin 96/5, Determination of mercury(12)
.
In the first part of the experiment the limits of this method, like linear working range and limit of
quantification, will be determined. With this background information the concentration of mercury in
ambient air will be determined in the second part. This quantification will be carried out by
calibration curve technique as well as standard addition technique.
8.1.1 Accessories
 910 PSTAT mini
 Electrode 6.1208.210 (WE – Au, AE – C, RE – Ag)
 Measuring vessel and measuring vessel cover
 Pipettes
Equipment for sampling mercury in air
 Air pump with adjustable gas flow
 Sorbent tubes Anasorb C300 (500 mg) as specified in ISO 17733(13)
 Water bath

8.1.2 Reagents
 Perchloric acid, for trace analysis*
, w(HClO4) = 70%
 Sulfuric acid, for trace analysis*
, w(H2SO4) = 96%, CAS 7664-93-9
 Ethylenediaminetetraacetic acid disodium salt dihydrate, for analysis, Na2C10H14N2O8 · 2 H2O,
Na2EDTA, CAS 6381-92-6
 Sodium chloride, for trace analysis*
, NaCl, CAS 7647-14-5
 Nitric acid, for trace analysis*
, w(HNO3) = 65%
 Hg standard stock solution, β(Hg2+
) = 1 g/L (available commercially)
Supporting electrolyte c(H2SO4) = 2 mol/L
c(Na2EDTA) = 0.02 mol/L
c(NaCl) = 0.05 mol/L
Weigh in 0.372 g Na2EDTA and 0.146 g NaCl and transfer both
into a 50 mL volumetric flask. Dissolve it in approx. 40 mL
ultrapure water. Carefully add 5.56 mL concentrated H2SO4.
Attention solution becomes hot! After cooling down to room
temperature make up to the mark with ultrapure water.
10 mg/L Hg standard solution β(Hg) = 10 mg/L
flask. Add 50 µL concentrated HNO3 (65%) and 500 µL Hg
standard stock solution (1 g/L). Make up to the mark with
ultrapure water.
*
or equivalent

8.2 Experiment
8.2.1 Initial preparation of the electrode
Conditioning solution
11 mL H2O
0.1 mL HClO4
Conditioning parameters
Figure 19: Parameters for the conditioning of the
gold electrode for the determination of mercury
(experiment 8.2).
Conditioning
a) Prepare the conditioning solution by pipetting 11 mL H2O and 0.1 mL HClO4 into the
b) Take a new gold electrode (6.1208.210) and assemble it with the measuring vessel cover.
into the conditioning solution and close the measuring vessel with the measuring vessel cover.
d) Run the conditioning with the conditioning parameters given in Figure 19. The stirrer has to
be switched on during «tcond» and «tdep» but switched off during «tequil» and the potential
scan. Usually the electrode is well conditioned after 20 replications.
Measuring solution
10 mL H2O
0.04 mL Hg standard solution (β(Hg) = 10 mg/L)

mercury on a gold electrode (experiment 8.2).
Measurement
a) Condition a new electrode as described in 8.2.1 Initial preparation of the electrode.
b) Rinse the electrode well with ultrapure water. Take care not to touch the active electrode
surface with bare fingers.
c) Prepare the measuring solution by pipetting 10 mL H2O, 1 mL supporting electrolyte and
0.04 mL Hg standard solution (β(Hg) = 10 mg/L) into the measuring vessel. Put a stirrer bar
into the measuring vessel and stir the solution well.
d) With the measuring vessel cover assembled immerse the electrode into the measuring solution
and close the measuring vessel.
e) Make sure that the electrical contacts of the electrode are dry and free from contaminants.
f) Record the voltammogram with the parameters given in Figure 20. The stirrer has to be
switched on during «tcond» and «tdep» but switched off during «tequil» and the whole
potential scan.
h) Add another 0.04 mL Hg standard solution (β(Hg) = 10 mg/L). Stir the solution well.
i) Record another voltammogram using the same electrode and parameters. The stirrer has to
be switched on during «tcond» and «tdep» but switched off during «tequil» and the whole
potential scan.
k) Repeat step h) to j) until you recorded curves for 6 to 8 different concentrations.
Evaluation
l) Evaluate the peak height of the mercury signal for the individual concentrations as described
in 8.2.5.
m) Plot a graph with peak height as a function of the concentration.

n) From the graph determine the concentration range where there is a linear relation between
concentration and peak height.
 Linear relation between concentration and signal, calibration curve y = A + B x
 Highest concentration 10 ... 30 * LOD
Formulas
∑
– Variance of
point in the
regression

oncentration
10
(Eq. 8)
Measuring solution
10 mL H2O
Standard addition
5 additions of 0.020 mL Hg standard solution (β(Hg) = 10 mg/L) each.
See Figure 20.
Measurement
c) Prepare the measuring solution by pipetting 10 mL H2O and 1 mL supporting electrolyte into
the measuring vessel. Put a stirrer bar into the measuring vessel and stir the solution well.
potential scan.
g) Stir the solution and repeat the measurement of the blank (c = 0). In total 8 replications are
required.
h) Save the voltammograms together with the method parameters.
i) Add 0.02 mL of the Hg standard solution (β(Hg) = 10 mg/L). Stir the solution well.
j) Record again 8 voltammograms with this concentration. The stirrer has to be switched on
during «tcond» and «tdep» but switched off during «tequil» and the whole potential scan.
k) Save the voltammograms together with the method parameters.
l) Repeat step i) to k) until you have recorded curves with 5 different concentrations.
Evaluation
m) Evaluate the peak height for the individual concentrations as described in 8.2.5.
n) Plot a graph with the peak height as a function of the concentration.
o) Calculate the linear regression of the calibration curve.
p) Calculate the residual standard deviation of the calibration curve.
q) Using the residual standard deviation calculate the LOD and the LOQ for the determination
of mercury.

8.2.4 Determination of mercury in air
The working range of the mercury determination with the described parameters is approximately in
the middle and upper ppb range. An interesting application in this concentration range is the
determination of mercury in workplace air. In many countries the permissible exposure limit is
0.1 mg/m3
as specified by e.g. TRGS 900(14)
, Germany or OSHA(15)
, USA.
The determination of mercury in air consists of two parts, the sampling and the voltammetric
determination. The sampling is carried out by the so-called pumped sampling. Air is drawn through a
sorbent tube by means of an air pump. Mercury in the air adsorbs to the sorbent and from this
sorbent a test solution is prepared in which the mercury concentration can be determined. A detailed
description for the sampling of mercury in air can be found in ISO 17733(13)
.
Figure 21: Schematic setup for the
sampling of mercury in air.
The voltammetric determination of the mercury concentration in the test solution requires the
calibration of the method. In principle there are two ways, calibration curve or standard addition.
Carry out both and discuss advantages and disadvantages of the two calibration techniques. Decide
which one is recommended for this application.
Calibration curve
Measuring solution «calibration curve»
10 mL H2O
0.04 mL Hg Standard solution (β(Hg) = 10 mg/L)
Measuring solution «sample»
10 mL H2O
0.5 mL test solution
See Figure 20.
c) Prepare the measuring solution «calibration curve» by pipetting 10 mL H2O, 1 mL supporting
electrolyte and 0.04 mL Hg standard solution (β(Hg) = 10 mg/L) into the measuring vessel. Put
a stirrer bar into the measuring vessel and stir the solution well.
flow meter
sorbent tube
air pump
connecting tube
air flow
glass wool
sorbent

potential scan. Save the voltammogram together with the method parameters.
g) Add 0.02 mL of the Hg standard solution (β(Hg) = 10 mg/L). Stir the solution.
h) Record another voltammogram using the same electrode and parameters. The stirrer has to
potential scan.
i) Save the voltammogram together with the method parameters.
j) Repeat step g) to i) until you have recorded curves with 8 to 10 different concentrations.
k) Evaluate the peak height for the individual concentrations as described in 8.2.5.
l) Plot a graph with peak height as a function of the concentration and calculate the linear
regression of the calibration curve.
m) Condition a new electrode as described in 8.2.1 Initial preparation of the electrode.
n) Rinse the electrode well with ultrapure water. Take care not to touch the active electrode
o) Prepare the measuring solution «calibration curve» by pipetting 10 mL H2O, 1 mL supporting
electrolyte and 0.5 mL test solution into the measuring vessel. Put a stirrer bar into the
p) With the measuring vessel cover assembled immerse the electrode into the measuring solution
q) Make sure that the electrical contacts of the electrode are dry and free from contaminants.
r) Record the voltammogram with the same parameters used to record the calibration curve.
The stirrer has to be switched on during «tcond» and «tdep» but switched off during «tequil»
and the whole potential scan. Save the voltammogram together with the method parameters.
Concentration evaluation
s) Evaluate the peak height for mercury in the test solution as described in 8.2.5.
t) Compare the peak height with the calibration curve and calculate the concentration of
mercury in the test solution.
u) From the concentration in the test solution calculate the concentration of mercury with
respect to the air volume sampled.

Standard addition
Measuring solution
10 mL H2O
Standard addition
Concentration is quantified by 2 additions of 0.025 mL Hg standard solution (β(Hg) = 10 mg/L).
See Figure 20.
c) Prepare the measuring solution by pipetting 10 mL H2O, 1 mL supporting electrolyte and 0.5
mL test solution into the measuring vessel. Put a stirrer bar into the measuring vessel and stir
the solution well.
potential scan. Save the voltammogram together with the method parameters.
g) Add 0.025 mL Hg standard solution (β(Hg) = 10 mg/L). Stir the solution.
h) Record another voltammogram using the same electrode and parameters. The stirrer has to
potential scan.
i) Save the voltammogram together with the method parameters.
j) Add another 0.025 mL Hg standard solution (β(Hg) = 10 mg/L). Stir the solution.
k) Record another voltammogram using the same electrode and parameters. The stirrer has to
potential scan.
l) Save the voltammogram together with the method parameters.
m) Evaluate the peak height for mercury for the sample and the two standard additions as
described in 8.2.5.
n) Plot a graph with the peak height as a function of the concentration. The concentration in the
sample is set to zero.
o) Calculate the linear regression for the standard addition curve.
p) Extrapolate the linear regression onto the x-axis (concentration axis) to get the negative
concentration of mercury in the measuring solution. Calculate the concentration of mercury in
the test solution.
q) From the concentration in the test solution calculate the concentration of mercury with
respect to the air volume sampled.

For the evaluation of the peak height «peak measurement tool 1» can be used.
Peak potential of mercury is approx. +0.45 V
evaluation of peak height
(c(Hg)  90 µg/L) in
experiment 8.2.
Note! Mercury is very toxic to the environment. If the standard solution cannot be used anymore take
care of an appropriate disposal.
 The lifetime of the gold electrode is limited. If measurements are done in clean standard solutions
several measurements on the same electrode are possible. A calibration curve for example can be
recorded using just one electrode. But as soon as the matrix of a real sample is involved, the
electrode’s lifetime decreases. For samples approx. 5 determinations including the standard
additions are possible.

Quantification of cadmium and lead
9 Quantification of cadmium and lead
Voltammetric determination of cadmium and lead at a mercury film electrode
Cadmium and lead, as many other heavy metals, are toxic and therefore their quantification is of
great interest. At a mercury film electrode (MFE) both metals can easily be determined side by side. A
mercury film electrode is usually a carbon electrode with a thin film of metallic mercury plated to
form the actually working electrode material.
The determination of cadmium and lead is carried out by anodic stripping voltammetry (ASV).
Stripping voltammetry in general is a two-step method which consists of a preconcentration and a
subsequent determination step. The preconcentration allows a significant increase in sensitivity
compared to a direct measurement. For the determination of cadmium and lead the
preconcentration step is a reduction. Cadmium and lead ions in the measuring solution are reduced
at the mercury film electrode and dissolved in the mercury as an amalgam.
Preconcentration: Cd2+
+ 2 e-
 Cd0
(Hg)
Pb2+
+ 2 e-
 Pb0
(Hg)
In the subsequent determination step the cadmium and the lead are anodically stripped off the
electrode, which means the deposited metals are re-oxidized.
Anodic stripping: Cd0
(Hg)  Cd2+
+ 2 e-
Pb0
(Hg)  Pb2+
+ 2 e-
The determination is carried out by differential pulse voltammetry (DP). DP shows increased sensitivity
compared to linear sweep voltammetry (LSV) and cyclic voltammetry (CV). Therefore DP is the
method of choice for quantitative determinations. For further reading on differential pulse
voltammetry and on the quantification of cadmium and lead on the MFE see e.g. Thomas and Henze,
Voltammetric Analysis(9)
or Metrohm Application Bulletin 254/1, Determination of zinc, cadmium,
lead and copper(16)
.
In the first part of the experiment the deposition potential (potential applied for preconcentration) is
optimized. In the second part the limits of this method, like linear working range and limit of
quantification, are determined. With this background information the concentration of cadmium and
lead in articles of daily use are determined in the third part. The quantification is carried out by
standard addition technique.
9.1.1 Accessories
 910 PSTAT mini
 Measuring vessel and measuring vessel cover
 Pipettes

9.1.2 Reagents
, CAS 64-19-7
, CAS 1336-21-6
 Hydrochloric acid, w(HCl) = 30 %, for trace analysis*
, CAS 7647-01-0
 Hg standard stock solution, β(Hg2+
 Cd standard stock solution, β(Cd2+
 Pb standard stock solution, β(Pb2+
 Nitric acid, for trace analysis*
, w(HNO3) = 65%
Hg plating solution β(Hg) = 20 mg/L
c(HCl) = 0.1 mol/L
flask. Add 1 mL Hg standard stock solution (β(Hg2+
) = 1 g/L)
and 0.5 mL HCl (30 %). Make up to the mark with ultrapure
water.
Buffer pH 4.4 c(CH3COOH) = 2 mol/L
c(NH3) = 1 mol/L
c(HCl) = 0.1 mol/L
flask. Carefully add 5.55 mL acetic acid (100 %), 3.7 mL NH3
(25 %) and 0.5 mL HCl (30 %). Make up to the mark with
ultrapure water.
10 mg/L Cd standard solution β(Cd) = 10 mg/L
flask. Add 50 µL concentrated HNO3 (65%) and 500 µL Cd
ultrapure water.
10 mg/L Pb standard solution β(Pb) = 10 mg/L
flask. Add 50 µL concentrated HNO3 (65%) and 500 µL Pb
ultrapure water.
Mixed standard 1 β(Cd) = 0.2 mg/L
β(Pb) = 0.3 mg/L
flask. Add 50 µL concentrated HNO3 (65%) 1 mL 10 mg/L Cd
standard solution and 1.5 mL 10 mg/L Pb standard solution.
Make up to the mark with ultrapure water.
Mixed standard 2 β(Cd) = 0.5 mg/L
β(Pb) = 1.0 mg/L
flask. Add 50 µL concentrated HNO3 (65%) 2.5 mL 10 mg/L Cd
standard solution and 5 mL 10 mg/L Pb standard solution.
Make up to the mark with ultrapure water.
*
or equivalent

Extraction solution w(CH3COOH) = 4 % v/v
Dilute 40 mL acetic acid with 960 mL ultrapure water.
9.2 Experiment
9.2.1 Preparation of the mercury film
The mercury film can be plated in situ, but ex situ plating should be preferred since it significantly
reduces the consumption of mercury for this application.
Plating solution
11 mL Hg plating solution (β(Hg) = 20 mg/L)
Plating parameters
Figure 23: Parameters for the deposition of the
mercury film at the carbon electrode (experiment
9.2).
Plating
a) Pipette 12 mL Hg plating solution into the measuring vessel. Put a stirrer bar into the
into the plating solution and close the measuring vessel.
d) Deposit the mercury film with the plating parameters from Figure 23. The stirrer has to be
switched on during «tcond» and «tdep» but switched off during «tequil» and the potential
scan. Usually a deposition of 5 minutes is sufficient to get a proper mercury film.
Note! The Hg plating solution can be reused multiple times. If the solution cannot be used anymore
take care of an appropriate disposal.

9.2.2 Deposition potential
Measuring solution
10 mL H2O
1 mL buffer pH 4.4
0.1 mL Cd standard solution (β(Cd) = 10 mg/L)
0.1 mL Pb standard solution (β(Pb) = 10 mg/L)
Figure 24: Start parameters for the optimization of
deposition potential (experiment 9.2).
Measurement
a) Plate a mercury film on a new carbon electrode (6.1208.110) as described in 9.2.1
Preparation of the mercury film.
b) Rinse the electrode well with ultrapure water. Take care not to touch the mercury film with
bare fingers.
c) Prepare the measuring solution by pipetting 10 mL H2O, 1 mL buffer pH 4.4, 0.1 mL Cd
standard solution (β(Cd) = 10 mg/L ) and 0.1 mL Pb standard solution (β(Pb) = 10 mg/L) into
f) Record the voltammogram with the voltammetric parameters from Figure 24. The stirrer has
to be switched on during «tcond» and «tdep» but switched off during «tequil» and the whole
potential scan.
h) Change the deposition potential «Edep» to -0.6 V. Stir the solution.
i) Record another voltammogram using the same electrode. The stirrer has to be switched on
during «tcond» and «tdep» but switched off during «tequil» and the whole potential scan.

k) Repeat step h) to j) with deposition potentials of -0.7 V, -0.8 V, -0.9 V, -1.0 V, -1.2 V
and -1.4 V.
Evaluation
l) Evaluate the peak height of the cadmium and the lead signals at the different deposition
potentials as described in 9.2.6.
m) Plot graphs of the peak height as a function of the deposition potential for both elements.
n) What can be observed? Based on your observation choose a suitable deposition potential for
the following experiments.
Measuring solution
10 mL H2O
1 mL buffer pH 4.4
0.05 mL Cd standard solution (β(Cd) = 10 mg/L )
0.05 mL Pb standard solution (β(Pb) = 10 mg/L)
cadmium and lead at the mercury film electrode
(experiment 9.2).
Measurement
b) Rinse the electrode well with ultrapure water. Take care not to touch the mercury film.
c) Prepare the measuring solution by pipetting 10 mL H2O, 1 mL buffer pH 4.4, 0.05 mL Cd
standard solution (β(Cd) = 10 mg/L) and 0.05 mL Pb standard solution (β(Pb) = 10 mg/L) into

f) Use the parameters optimized in experiment 9.2.2 or enter the voltammetric parameters given
in Figure 25.
g) Record the voltammogram. The stirrer has to be switched on during «tcond» and «tdep» but
switched off during «tequil» and the whole potential scan.
i) Add another 0.05 mL of each Cd standard solution (β(Cd) = 10 mg/L) and Pb standard
solution (β(Pb) = 10 mg/L). Stir the solution well.
j) Record another voltammogram using the same electrode and parameters. The stirrer has to
potential scan.
k) Save the voltammogram together with the method parameters.
l) Repeat step i) to k) until you recorded curves for 8 to 10 different concentrations.
Evaluation
m) Evaluate the peak height of the cadmium and the lead signals for the individual
concentrations as described in 9.2.6.
n) Plot graphs with the peak height as a function of the concentration for both elements.
o) From the graph determine the concentration range where there is a linear relation between
concentration and peak height for both elements.
 Linear relation between concentration and signal, calibration curve y = A + B x
 Highest concentration 10 ... 30 * LOD

Formulas
∑
– Variance of
point in the
regression
oncentration
10
(Eq. 8)
Measuring solution
10 mL H2O
1 mL buffer pH 4.4
Standard addition
5 additions of 0.1 mL mixed standard solution 1 (β(Cd) = 0.2 mg/L, β(Pb) = 0.3 mg/L) each.
See Figure 25.
Measurement
c) Prepare the measuring solution by pipetting 10 mL H2O and 1 mL buffer pH 4.4 into the
in Figure 25.

h) Stir the solution and repeat the measurement of the blank (c = 0). In total 10 replications are
required.
i) Save the voltammograms together with the method parameters.
j) Add 0.1 mL of the mixed standard solution (with β(Cd) = 0.2 mg/L and β(Pb) = 0.3 mg/L). Stir
the solution well.
k) Repeat the measurement for this concentration. The stirrer has to be switched on during
«tcond» and «tdep» but switched off during «tequil» and the whole potential scan. In total 10
repetitive measurements of this standard are required.
l) Save the voltammograms together with the method parameters.
m) Repeat step j) to l) until you have recorded curves with 5 different concentrations.
Evaluation
n) Evaluate the peak height for the individual concentrations for both elements as described in
9.2.6.
o) Plot a graph with the peak height as a function of the concentration for both elements.
p) Calculate the linear regression of the calibration curve for both elements.
q) Calculate the residual standard deviation of the calibration curve for both elements.
r) Using the residual standard deviation calculate the LOD and the LOQ of the cadmium
determination as well as the lead determination.
9.2.5 Determination of cadmium and lead in articles of daily use
The working range of the determination of cadmium and lead with the described parameters is
approximately in the low and middle ppb range. An interesting application in this concentration
range is the analysis of cadmium and lead released from articles of daily use, such as ceramics,
glassware, PVC tubes or baby toys. Sampling and limits for the release of cadmium and lead from
glass ware in contact with food for example can be found in ISO 7086(17)(18)
. To quantify the release
of the metals the products are leached with w(acetic acid) = 4 % for 24 hours. Afterwards the
concentration of cadmium and lead in this extraction solution is determined. The quantification is
carried out by standard addition technique.
Measuring solution
10 mL H2O
1 mL buffer pH 4.4
1 mL extraction solution
Standard addition
Concentration is quantified by 2 additions of 0.1 mL mixed standard solution 2 (β(Cd) = 0.5 mg/L,
β(Pb) = 1.0 mg/L).
See Figure 25.

c) Prepare the measuring solution «sample» by pipetting 10 mL H2O, 1 mL buffer pH 4.4 and 1
mL extraction solution into the measuring vessel. Put a stirrer bar into the measuring vessel
and stir the solution well.
in Figure 25.
i) Add 0.1 mL of the mixed standard solution 2 (β(Cd) = 0.5 mg/L, β(Pb) = 1.0 mg/L). Stir the
solution.
j) Record another voltammogram using the same electrode and parameters. The stirrer has to
potential scan.
k) Save the voltammogram together with the method parameters.
l) Add another 0.1 mL of the mixed standard solution 2 (β(Cd) = 0.5 mg/L, β(Pb) = 1.0 mg/L).
Stir the solution.
m) Record another voltammogram using the same electrode and parameters. The stirrer has to
potential scan.
n) Save the voltammogram together with the method parameters.
o) Evaluate the peak heights for cadmium and lead for the sample and the two standard
additions as described in 9.2.6.
p) Plot a graph with peak height as a function of concentration for cadmium and lead. The
concentration in the sample is set to zero.
q) Calculate the linear regression for the standard addition curve.
r) Extrapolate the linear regression onto the x-axis (concentration axis) to get the negative
concentration of cadmium and lead in the measuring solution. Calculate the concentration of
cadmium and lead in the extraction solution from this value.

For the evaluation of the peak height «peak measurement tool 1» can be used.
Peak potential of cadmium is approx. -0.8 V
Peak potential of lead is approx. -0.6 V
evaluation of peak height of
cadmium and lead (both
approx 90 µg/L) in experiment
9.2.
Note! The Hg plating solution can be reused multiple times. If the solution cannot be used anymore
take care of an appropriate disposal. Cadmium and lead are toxic to the environment. Their standard
solutions should be disposed appropriately as well.
 The lifetime of the mercury film at the carbon electrode is limited. If measurements are done in
clean standard solutions several measurements at the same electrode are possible. A calibration
curve for example can be recorded using just one electrode. As soon as the matrix of a real
sample is involved the lifetime decreases. For samples approx. 3 to 5 determinations including the
standard additions are possible.
 The mercury film cannot be removed to plate a fresh film at the same electrode, therefore it is
recommended to plate a new mercury film only on a new electrode.
 The performance of the determination also depends on the quality of the mercury film. Problems
with the linearity of the calibration curve for example can be related to the quality of the mercury
film. In this case increase the plating time for the preparation of the mercury film from 5 minutes
to 10 minutes.

The principle of a glucose sensor
10 The principle of a glucose sensor
Amperometric detection of glucose at an enzyme modified platinum
electrode
The glucose sensor is one of the great success stories in the field of biosensors, from one of the first
publications of the principle by Updike and Hicks(19)
in 1967, millions of this kind of sensors are sold
today for monitoring blood glucose. The principle is both simple and brilliant. It is based on the
oxidation of glucose to glucono lactone and hydrogen peroxide catalyzed by the enzyme glucose
oxidase. The hydrogen peroxide produced in this reaction is then determined in an amperometric
measurement.
Figure 27: Principle of
a glucose sensor
In this experiment a simple glucose sensor will be manufactured. Its function will be tested in a flow
injection system by measuring the glucose content of different food products such as honey, fruit
juices and beverages. The determination is carried out by amperometric detection. For further
reading on the principle of the glucose sensor see e.g. Bond, Broadening Electrochemical
Horizons (5)
.
10.1.1 Accessories
 910 PSTAT mini
 Electrode 6.1208.510 (WE – Pt, AE – C, RE – Ag)
 Flow cell for screen printed electrodes (e.g. DropSens DRP-FLWCL)
 Peristaltic pump
 6-port injection valve with 0.5 mL sample loop
 Capillary tubings (PEEK or PTFE with inner diameter in the range of
0.5 … 0.9 mm)
 Pipettes
Figure 28: Flow cell (open) with electrode 6.1208.510
Pt electrode 2 e-
2 H+
+ O2
Gluconolactone
+
H2O2
Glucose + O2
GOx
immobilized
glucose
oxidase
(GOx)
Sample solution

10.1.2 Reagents
 Potassium dihydrogen phosphate, for analysis, KH2PO4, CAS 7778-77-0
 Sodium hydrogen phosphate, for analysis, Na2HPO4, CAS 7558-79-4
 Potassium chloride, for analysis, KCl, CAS 7447-40-7
 Glucose oxidase (GOx), 192000 units/gram, CAS 9001-37-0
 Nafion 117 solution, ~5% in a mixture of lower aliphatic alcohols and water, CAS 31175-20-9
 D-(+)-Glucose anhydrous, C6H12O6, CAS 50-99-7
Only for 10.2.4 Interferences:
 D-(-)-fructose, C6H12O6, CAS 57-48-7
 D-(+)-galactose, C6H12O6, CAS 59-23-4
 D-(+)-mannose, C6H12O6, CAS 3458-28-4
 Sucrose, C12H22O11, CAS 57-50-1
 Vitamin C (ascorbic acid), puriss. p.a., C6H8O6, CAS 50-81-7
Phosphate buffer pH 5.2 c(KH2PO4) = 0.06 mol/L
c(Na2HPO4) = 0.007 mol/L
c(KCl) = 0.1 mol/L
Weigh in 8.1654 g KH2PO4, 0.9937 g Na2HPO4 and 7.4551 g
KCl and transfer everything into a 1 L volumetric flask. Dissolve
and make up to the mark with ultrapure water. The solution
has approx. pH 5.2.
GOx stock solution c(GOx) ~ 3500 units/mL
Dissolve 2.8 mg glucose oxidase in 150 µL phosphate buffer
pH 5.2. When the solution is not used store it in the
refrigerator..
Glucose stock solution β(glucose) = 10 g/L
Weigh in 0.50 g D-(+)-glucose anhydrous and transfer it into a
50 mL volumetric flask. Dissolve and make up to the mark with
phosphate buffer pH 5.2.
Glucose standard solution β(glucose) = 50 mg/L
Pipette 0.05 mL glucose stock solution (β(glucose) = 10 g/L)
into a 10 mL volumetric flask. Make up to the mark with
β(glucose) = 100 mg/L
Prepare as described above, but use 0.1 mL glucose stock
solution (β(glucose) = 10 g/L) instead.
Use 0.2 mL glucose stock solution (β(glucose) = 10 g/L)

Only for 10.2.4 Interferences:
Fructose stock solution β(fructose) = 10 g/L
Weigh in 0.1 g D-(-)-fructose and transfer it into a 10 mL
Fructose standard solution β(fructose) = 400 mg/L
Pipette 0.4 mL fructose stock solution (β(fructose) = 10 g/L)
Galactose stock solution β(galactose) = 10 g/L
Weigh in 0.1 g D-(+)-galactose and transfer it into a 10 mL
Galactose standard solution β(galactose) = 400 mg/L
Pipette 0.4 mL galactose stock solution (β(galactose) = 10 g/L)
Mannose stock solution β(mannose) = 10 g/L
Weigh in 0.1 g D-(+)-mannose and transfer it into a 10 mL
Mannose standard solution β(mannose) = 400 mg/L
Pipette 0.4 mL mannose stock solution (β(mannose) = 10 g/L)
Sucrose stock solution β(sucrose) = 10 g/L
Weigh in 0.1 g sucrose and transfer it into a 10 mL volumetric
flask. Dissolve and make up to the mark with phosphate buffer
pH 5.2.
Sucrose standard solution β(sucrose) = 400 mg/L
Pipette 0.4 mL mannose stock solution (β(sucrose) = 10 g/L)
Vitamin C stock solution β(vitamin C) = 10 g/L
Weigh in 0.1 g vitamin C and transfer it into a 10 mL
Vitamin C standard solution β(vitamin C) = 10 mg/L
Pipette 0.01mL vitamin C stock solution (β(vitamin C) = 10 g/L)

10.2 Experiment
10.2.1 Setup of the flow injection system
Figure 29: Schematic setup of the flow injection system.
Working conditions
Tubing connections PEEK or PTFE capillary tubings with an inner diameter in the
range of 0. … 0.9 mm
Sample loop 0.5 mL
Flow rate 0.9 mL/min
Carrier solution Phosphate buffer pH 5.2
10.2.2 Preparation of GOx modified electrode
GOx coating solution
80 µL GOx stock solution (c(GOx) ~ 3500 units/mL)
20 µL Nafion 117 solution
Coating
a) Prepare the GOx coating solution by thoroughly mixing of 80 µL GOx stock solution (c(GOx) ~
3500 units/mL) and 20 µL Nafion 117 solution.
b) Pipette 2 µL of the GOx coating solution on the platinum electrode (6.1208.510). The droplet
should be positioned in the middle of the working electrode area. Take care not to coat the
reference and the auxiliary electrode.
c) Let the electrode air dry for 10 to 20 min.
d) Pipette 2 µL nafion 117 solution (w(nafion) ~ 5 %) on top of the GOx coating. Take care not
to coat the reference and the auxiliary electrode.
e) Let the electrode air dry for 10 to 20 min.
f) Before use immerse the electrode in the phosphate buffer for approx. 30 min.

g) Install the GOx modified electrode in the flow cell. Take care not to touch the active electrode
h) Flush the flow cell with the phosphate buffer pH 5.2 and make sure that the flow cell and all
tubing connections are free from air bubbles.
i) Make sure that the electrical contacts of the electrode are dry and free from contaminants.
Then connect the electrode cable. Now the system is ready to use.
Standard solutions
glucose on a GOx modified electrode (experiment
10.2).
Measurement
a) Prepare the 5 glucose standard solutions of β(glucose) = 200 mg/L, 400 mg/L, 600 mg/L, 800
mg/L and 1000 mg/L by the dilution of the appropriate amount of glucose standard stock
solution (β(glucose) = 10 g/L) with the phosphate buffer pH 5.2.
b) Start the peristaltic pump. Make sure that the phosphate buffer shows a steady flow without
pulsation.
c) Start the data recording with the parameters given in Figure 30.
d) Fill the sample loop with glucose standard solution β(glucose) = 200 mg/L.
e) When the current of the amperometric measurement is stable, inject the standard solution.
f) Wait until the standard solution has passed the flow cell. This is indicated by the current
which returns to the initial value before the injection. Then fill the sample loop again with the
standard solution.

g) Repeat the injection of glucose standard solution β(glucose) = 200 mg/L. In total 3 to 5
injections of the standard should be done. After the last injection stop the data recording.
h) Repeat step c) to g) also for the other standard solutions. Use β(glucose) = 400 mg/L, 600
mg/L, 800 mg/L and 1000 mg/L instead in step d) and f).
Evaluation
i) Evaluate the peak area of the glucose signals as described in 10.2.6. For each concentration
calculate the mean value from the repeated injections.
j) Plot a graph with the averaged peak area as a function of the concentration.
k) From the graph determine the concentration range where there is a linear relation between
concentration and peak area.
10.2.4 Interferences
Before determining the concentration of glucose in food products, check for possible interferences
from e.g. other monosaccharides such as fructose, galactose or mannose or from the common
disaccharide sucrose which consists of one molecule fructose and one molecule glucose. Also the
interference of vitamin C, which is present in many fruit juices either naturally or as antioxidant,
should be tested.
Standard solutions
β(galactose) = 400 mg/L
β(mannose) = 400 mg/L
β(sucrose) = 400 mg/L
β(vitamin C) = 10 mg/L
See Figure 30.
Measurement
a) Prepare the glucose standard solution of β(glucose) = 400 mg/L by diluting the glucose
standard stock solution (β(glucose) = 10 g/L) with the phosphate buffer pH 5.2.
b) Prepare the fructose standard solution of β(fructose) = 400 mg/L by diluting the fructose
standard stock solution (β(fructose) = 10 g/L) with the phosphate buffer pH 5.2.
c) Start the peristaltic pump. Make sure that the phosphate buffer shows a steady flow without
pulsation.
d) Start the data recording with the parameters given in Figure 30.
e) Fill the sample loop with glucose standard solution β(glucose) = 400 mg/L.
f) When the current of the amperometric measurement is stable, inject the glucose standard
solution.
g) Wait until the standard solution has passed the flow cell. This is indicated by the current
which returns to the initial value before the injection.
h) Fill the sample loop with fructose standard solution β(fructose) = 400 mg/L.
i) When the current of the amperometric measurement is stable, inject the fructose standard
solution.
j) Stop the data recording when you are sure that the fructose standard solution has passed the
flow cell.

k) Repeat step b) to j) also for the other standard solutions. Prepare β(galactose) = 400 mg/L,
β(mannose) = 400 mg/L, β(sucrose) = 400 mg/L or β(vitamin C) = 10 mg/L in step b) and use
the corresponding standard in step h).
Evaluation
l) Compare the signal for the glucose standard (β(glucose) = 400 mg/L) with the signals of the
other tested standard solutions. Decide which substances will interfere. Keep possible
interferences in mind when selecting samples for experiment 10.2.5.
10.2.5 Determination of glucose in different food products
Many food products contain sugar. However, how much of this sugar is glucose, which plays an
important role in the catabolism of humans and other living organism? Food products containing
glucose are fruit juices, such as grape juice or apple juice and beverages such as iced tea or cola soft
drink. Honey typically contains between 22 % and 41 % glucose.
The quantification of glucose requires a calibration. Record a calibration curve and carry out the
determinations in the different samples using this calibration curve. To verify the results check the
recovery in one sample.
Sample solutions
Juice or beverage sample
solution
Pipette 0.1 mL of the sample into a 10 mL volumetric flask. Make up
to the mark with phosphate buffer pH 5.2.
Honey stock solution Weigh out 1.0 g of the sample and transfer it into a 25 mL
volumetric flask. Add approx. 20 mL phosphate buffer and mix until
the honey is completely dissolved. Make up to the mark with
Honey sample solution Pipette 0.1 mL of the honey stock solution into a 10 mL volumetric
flask. Make up to the mark with phosphate buffer pH 5.2.
Recovery test solution Pipette 0.1 mL of the honey stock solution and 0.1 mL of the glucose
stock solution (β(glucose) = 10 g/L) into a 10 mL volumetric flask.
Make up to the mark with phosphate buffer pH 5.2.
Note! The volume of glucose stock solution might need to be
adapted depending on the concentration in the sample. See also the
additional information on the recovery in chapter 10.2.7.
Calibration standard solutions
See Figure 30.

a) Prepare the glucose standard solutions of β(glucose) = 50 mg/L, 100 mg/L, 200 mg/L, 300
mg/L, 400 mg/L, 500 mg/L and 600 mg/L by the dilution of the appropriate amount of
glucose standard stock solution (β(glucose) = 10 g/L) with the phosphate buffer pH 5.2.
b) Start the peristaltic pump. Make sure that the phosphate buffer shows a steady flow without
pulsation.
c) Start the data recording with the parameters given in Figure 30.
d) Fill the sample loop with glucose standard solution β(glucose) = 50 mg/L.
e) When the current of the amperometric measurement is stable, inject the standard solution.
f) Wait until the standard solution has passed the flow cell. This is indicated by the current
which returns to the initial value before the injection. Then fill the sample loop again with the
standard solution.
g) Repeat the injection of glucose standard solution β(glucose) = 50 mg/L. In total 3 to 5
injections of the standard should be done. After the last injection stop the data recording.
h) Repeat step c) to g) also for the other standard solutions. Use β(glucose) = 100 mg/L, 200
mg/L, 300 mg/L, 400 mg/L, 500 mg/L or 600 mg/L instead in step d) and f).
i) Evaluate the peak area of the glucose signals as described in 10.2.6. For each concentration
calculate the mean value from the repeated injections.
j) Plot a graph with the averaged peak area as a function of the concentration and calculate the
linear regression for the calibration curve.
k) Start the data recording with the parameters given in Figure 30.
l) Fill the sample loop with the sample solution (e. g. honey diluted in phosphate buffer pH 5.2).
m) When the current of the amperometric measurement is stable, inject the sample solution.
n) Wait until the sample solution has passed the flow cell. This is indicated by the current, which
returns to the initial value before the injection. Then fill the sample loop again with the sample
solution.
o) Repeat the injection of sample solution. In total 3 to 5 injections of the sample should be
done. After the last injection stop the data recording.
p) Repeat step k) to o) also with the recovery test solutions and the other sample solutions.
q) Evaluate the peak area of the glucose signals as described in 10.2.6. For each sample calculate
the mean value from the repeated injections.
r) Compare the averaged peak area with the calibration curve and calculate the concentration in
the diluted sample.
s) From this value calculate the concentration of glucose in the undiluted sample and the
recovery for the recovery test solutions.

For the evaluation of the peak area «peak measurement tool 1» can be used. The peak area
corresponds to the charge stated on the tab «Measurements».
evaluation of the peak area of
the glucose signal (3 injections
of β(glucose) = 400 mg/L
each) in experiment 10.2.
 A GOx coated electrode can be stored dry for a few days.
 When the electrode is not in use, e.g. over night, take it out of the flow cell, rinse it carefully with
ultrapure water, let it air dry and store it dry.
 The sensitivity of the determination depends on the amount of GOx immobilized at the electrode.
Therefore only measurements can be compared which have been done on electrodes coated with
the same procedure using the same GOx coating solution. Furthermore the sensitivity decreases
over time. For this reason the calibration curve should be checked from time to time by measuring
a standard solution with a known concentration.
 Instead of the peak area it is also possible to evaluate the peak height. The application will show
similar results.
 For the preparation of the recovery test solution the concentration in the sample should be
increased by 50 % to 100 %. The recovery is then calculated with respect to the spiked amount.
( ) With
– concentration in the recovery test
solution
– concentration in the sample
solution
– spiked concentration

Examples
11 Examples

Examples
Experiment 2: Standard reduction potential
Measuring data and evaluation
Pb Eobs = -0.68 V E0 = -0.13 V
Pb2+
(aq) + 2 e-
⇌ Pb(s)
Cu Eobs = -0.41 V E0 = +0.34 V
Cu2+
(aq) + 2 e-
⇌ Cu(s)
Bi Eobs = -0.28 V E0 = +0.308 V
Bi3+
(aq) + 3 e-
⇌ Bi(s)

Experiment 2: Standard reduction potential
Hg Eobs = -0.01 V E0 = +0.85 V
Hg2+
(aq) + 2 e-
⇌ Hg(l)
Au Eobs = +0.33 V E0 = +0.93 V
[AuCl4]-
(aq) + 3 e-
⇌ Au(s) + 4 Cl-
Figure 32: Linear sweep voltammograms of different metal ions (gray line – supporting electrolyte, black line –
c(metal) = 0.18 mmol/L in the supporting electrolyte). Eobs – observed reduction potential, E0 – standard
reduction potential
(20)
.
Result discussion
When the metals are sorted by their reduction potential it can be seen that precious metals like gold
have the more positive potential, means they can more easily be reduced to their metallic form. Base
metals like lead have a more negative potential and can therefore more easily be oxidized to their
ionic form.
Base metal Precious metal
Negative reduction potential Positive reduction potential
Figure 33: Lead, copper, bismuth, mercury and gold sorted by their reduction potentials.
Pb2+
-0.68 V
Cu2+
-0.41 V
Bi3+
-0.28 V
Hg2+
-0.01 V
Au3+
+0.33 V +
–

Examples
The differences between the observed reduction potential and the standard reduction potential can
be explained by the differences in the experimental setup. For the measurement of the standard
reduction potential a metal cathode is immersed into a 1 molar solution of the corresponding metal
ion. The resulting potential at equilibrium is measured against a reference electrode. In contrast to
the measurement of the standard reduction potential experiment 2 is carried out under
potentiodynamic conditions. The reaction at the electrode is driven by an externally applied voltage
which is continuously changed. Another important difference is the reference electrode. Potentials
cannot be measured as absolute potentials but as potential difference between two electrodes. In
electrochemical experiments the potential difference is measured between the reference electrode,
which provides a stable potential, and the working electrode, where the electrochemical reaction
takes place. As a consequence the displayed potential depends on the reference electrode used for
the experiment. The values for the standard reduction potential are specified with respect to the
standard hydrogen electrode (SHE), whereas in this experiment the reference electrode is metallic
silver.
Despite the offset between the tabled value for the standard reduction potentials and the observed
reduction potentials the experiment allows a good differentiation between precious and base metals.

Examples
Experiment 3: A reversible redox system
Anodic Cathodic
 / V·s-1
/ V / µA / V / µA
0.01 0.068 1.882 0.000 -1.805
0.02 0.060 2.672 0.000 -2.540
0.03 0.056 3.258 -0.004 -3.087
0.04 0.056 3.765 -0.008 -3.546
0.05 0.052 4.204 -0.012 -3.915
 / V·s-1
/ mV | ⁄ |
0.01 68 1.04
0.02 60 1.05
0.03 60 1.06
0.04 64 1.06
0.05 64 1.07
Figure 34: Cyclic voltammograms of c(p-aminophenol) = 0.09 mmol/L with scan rate of 10, 20, 30, 40 and
50 mV/s
Result discussion
At scan rates between 10 and 50 mV·s-1
p-aminophenol fulfills the criteria of a reversible reaction.
The peak height increases with increasing sweep rate and the peak heights for the anodic and the
cathodic signal are almost equal. The peak potentials for the anodic and cathodic signal slightly shift
to negative potentials with increasing sweep rate, but the potential difference between the two
signals is constant at 64 mV ± 4 mV. Considering the experimental setup (e.g. no IR drop
compensation) this potential difference suggests a reaction with the transfer of one electron. A
possible reaction mechanism could be as follows:
p-AP p-AP
+ 1 e-
+ 1 H+
Reduced species Oxidized species
Figure 35: Potential mechanism for the redox reaction of p-aminophenol.
NH2
OH O
NH2
e H
+
+ +

Experiment 3: A reversible redox system
Calculation of the diffusion coefficient
Randles-Sevcik equation
√ (Eq. 3)
With
= 96480 C·mol-1
= 8.314 J·mol-1
·K-1
= 298 K √ (Eq. 9)
And
= 1
= 0.09 mmol·L-1
= 9·10-8
mol·cm-3
= (4 mm/2)2
· = 0.1256 cm2
√ (Eq. 10)
Figure 36: Peak height of anodic and cathodic peak of cyclic voltammograms of c(p-aminophenol) = 0.09
mmol/L plotted versus the square root of the scan rate.
 / V·s-1
√( s 1) / A / A
0.01 0.10 1.88·10-6
-1.81·10-6
0.02 0.14 2.67·10-6
-2.54·10-6
0.03 0.17 3.26·10-6
-3.09·10-6
0.04 0.20 3.77·10-6
-3.55·10-6
0.05 0.22 4.20·10-6
-3.92·10-6
slope 1.88·10-5
-1.71·10-5
Transforming (Eq. 10)
√
√ slope =
3.81·10-5
cm2
·s-1
=
3.17·10-5
cm2
·s-1
-5
-4
-3
-2
-1
0
0
1
2
3
4
5
0.10 0.15 0.20
Ip,c / µA
Ipa,, / µA
√( / V·s-1)
anodic
cathodic
Linear (anodic)
Linear (cathodic)

Examples
Experiment 4: A quasi-reversible redox system
Anodic Cathodic
 / V·s-1
/ V / µA / V / µA
0.1 0.054 5.795 -0.022 -5.172
0.2 0.054 8.182 -0.026 -6.972
0.3 0.058 9.507 -0.034 -7.910
0.4 0.058 11.207 -0.042 -9.007
0.5 0.062 12.395 -0.046 -9.746
 / V·s-1
/ mV | ⁄ |
0.1 76 1.12
0.2 80 1.17
0.3 92 1.20
0.4 100 1.24
0.5 108 1.27
Figure 37: Cyclic voltammograms of c(p-aminophenol) = 0.09 mmol/L with scan rate of 100, 200, 300, 400 and
500 mV/s.
Result discussion
At scan rates between 0.1 and 0.5 V/s the peak heights are still proportional to √ , but the peak
heights of the anodic signal and the cathodic signal are not completely equal anymore.
However, the most obvious indication that the process is not completely reversible anymore is the
separation of anodic and cathodic peak potential. The difference of the peak potentials is
significantly bigger than 59 mV and the separation of the two signals increases with faster scan rates.
Therefore the reaction of p-aminophenol at higher scan rates can be considered to be quasi-
reversible.
Calculation of the standard rate constant for electron transfer
The following reaction is assumed for the calculation
p-AP p-AP
+ 1 e-
+ 1 H+
Reduced species Oxidized species
Charge transfer parameter 𝜓
𝜓
√
(Eq. 4)
By transforming (Eq. 4) the standard rate constant can be calculated as
𝜓
√
√ (Eq. 11)

Experiment 4: A quasi-reversible redox system
With the diffusion coefficients from experiment 3:
= 3.81·10-5
cm2
·s-1
= 3.17·10-5
cm2
·s-1
and
 = 0.5 √ 1.10 (Eq. 12)
1.0 (Eq. 13)
With
= 1
= 96480 C·mol-1
= 8.314 J·mol-1
·K-1
= 298 K 8.9 1 (Eq. 14)
With the values from (Eq. 13) and (Eq. 14) the equation for standard rate constant (Eq. 11) can be
written as
𝜓 √ (Eq. 15)
(a) * † / mV
20 61
7 63
6 64
5 65
4 66
3 68
2 72
1 84
0.75 92
0.5 105
0.35 121
0.25 141
0.1 212
(b)
Figure 38: Variation of peak potential separations with kinetic parameters for cyclic voltammetry. (a) table (b)
semi-logarithmic plot of the tabl values
(7)
/ V·s-1
√ / mV / cm·s-1
0.1 0.32 76 1.50 0.031
0.2 0.45 80 1.21 0.035
0.3 0.55 92 0.75 0.027
0.4 0.63 100 0.57 0.024
0.5 0.71 108 0.47 0.022
*
See (Eq. 4)
†
For  = 0.5
50
70
90
110
130
150
170
190
210
230
0.1 1 10
D
E
p
·n
/
mV

Examples
Experiment 5: An irreversible redox system
Anodic Cathodic
 / V·s-1
/ V / µA / V / µA
0.05 0.325 24.283 -- --
0.10 0.340 33.217 -- --
0.15 0.350 40.104 -- --
0.20 0.360 46.167 -- --
0.25 0.365 51.441 -- --
Figure 39: Cyclic voltammograms of c(vitamin C) = 0.9 mmol/L with scan rate of 50, 100, 150, 200 and
250 mV/s.
Result discussion
Vitamin C shows the typical cyclic voltammogram for an irreversible process. The most obvious
indication is the absence of a cathodic reduction signal. Furthermore the oxidation signals
significantly shift to more positive potentials with faster scan rates.
The most likely mechanism of the observed reaction is the oxidation of ascorbic acid to
dehydroascorbic acid.
Figure 40: Oxidation of vitamin C.
O
OH
O
H
O
O
H
O
H
H
+
e O O
O
H
O
H
O O
- 2 - 2

Examples
Experiment 6: SAM – Self-assembled monolayers
Figure 41: Example for curves obtained for the electrochemical conditioning of the gold electrodes.
Coating Formula No.
of C
atoms
/ µA / µA
2-MAA HS(CH2)1COOH 1 -17.415 16.372
3-MPA HS(CH2)2COOH 2 -16.641 15.802
6-MHA HS(CH2)5COOH 5 -16.144 15.732
11-MUA HS(CH2)10COOH 10 -8.943 10.648
Figure 42: Cyclic voltammograms of gold electrodes coated with 2-MAA, 3-MPA, 6-MHA and 11-MUA
(measuring solution: c(hexacyanoferrate(III)) = 1.5 mmol/L in c(acetate buffer) = 0.1 mol/L).
Result discussion
The graph in Figure 42 shows that there is an effect of the monolayer on the redox behavior
Fe(III)/Fe(II) in the hexacyanoferrate complex. The signals become smaller the longer the molecule
used for the coating. That means that the electrode is not just insulated by the coating, but the
shielding depends on the thickness of the monolayer.
-20
-16
-12
-8
-4
0
0
4
8
12
16
20
0 2 4 6 8 10
Ip,c / µA
Ip,a / µA
No. of C atoms in the spacer group
anodic cathodic Linear (cathodic)

Examples
Experiment 7: Quantification of vitamin C
Concentration standard: β(vitamin C) = 10 g/L
/
mL
/ mL β(vitamin C)
/ mg·L-1
*
/ µA
0.02 11.02 18.1 0.690
0.04 11.04 36.2 1.323
0.06 11.06 54.2 1.936
0.08 11.08 72.2 2.510
0.10 11.10 90.1 2.997
0.12 11.12 107.9 3.478
0.14 11.14 125.7 3.991
0.16 11.16 143.4 4.451
0.18 11.18 161.0 4.927
0.20 11.20 178.6 5.366
*
Mean of 2 replications.
Concentrations outside the linear working range are
marked gray.
Figure 43: Linear working range for the determination of vitamin C. (Measuring solution: 10 mL H2O + 1 mL
ammonium acetate buffer + ).
Figure 44: Linear working range for the determination of vitamin C.
0
1
2
3
4
5
6
0 50 100 150 200
I
p
/
µA
c(vitamin C) / mg·L-1
Linear working range

Calibration curve for the determination of LOD and LOQ
Figure 45: Example for curves recorded for the determination of LOD and LOQ of vitamin C. (Measuring
solution: 10 mL H2O + 1 mL ammonium acetate buffer + ).
Solution /
mL
/ mL β(vitamin C) /
µg·L-1
*
/ µA ̂ / µA
Blank 0.000 11.000 0.0 0.004 0.003
Standard 1 0.025 11.025 2.3 0.081 0.090
Standard 2 0.050 11.050 4.5 0.180 0.176
Standard 3 0.075 11.075 6.8 0.272 0.262
Standard 4 0.100 11.100 9.0 0.350 0.347
Standard 5 0.125 11.125 11.2 0.424 0.432
*
Mean of 10 replications
Linear regression: y = A + B·x
Regression parameters: Intercept (A) 0.003 µA
Slope (B) 0.038 µA·L·mg-1
Calculation of the residual standard deviation
∑
( ̂ )
(Eq. 6)
0.00
0.10
0.20
0.30
0.40
0.0 2.0 4.0 6.0 8.0 10.0
Ip / µA
Concentration / mg·L-1

Examples
Solution β(vitamin C) /
mg·L-1
/ µA ̂ / µA ̂ ( ̂ )
Blank 0.0 0.003
0.004
0.003
0.006
0.002
0.001
0.006
0.001
0.001
0.003
0.003 0.000
0.001
0.000
0.003
-0.001
-0.002
0.003
-0.002
-0.002
0.000
6.67E-08
5.50E-07
6.67E-08
7.52E-06
1.58E-06
5.10E-06
7.52E-06
5.10E-06
5.10E-06
6.67E-08
Standard 1 2.3 0.078
0.080
0.082
0.083
0.081
0.083
0.082
0.081
0.082
0.083
0.090 -0.012
-0.010
-0.008
-0.007
-0.009
-0.007
-0.008
-0.009
-0.008
-0.007
1.39E-04
9.57E-05
6.06E-05
4.60E-05
7.72E-05
4.60E-05
6.06E-05
7.72E-05
6.06E-05
4.60E-05
0.177
0.182
0.184
0.179
0.183
0.183
0.182
0.181
0.183
0.176 0.002
0.001
0.006
0.008
0.003
0.007
0.007
0.006
0.005
0.007
4.33E-06
1.17E-06
3.70E-05
6.53E-05
9.49E-06
5.01E-05
5.01E-05
3.70E-05
2.58E-05
5.01E-05
0.272
0.274
0.272
0.271
0.274
0.273
0.270
0.271
0.272
0.262 0.010
0.010
0.012
0.010
0.009
0.012
0.011
0.008
0.009
0.010
1.07E-04
1.07E-04
1.52E-04
1.07E-04
8.71E-05
1.52E-04
1.28E-04
6.95E-05
8.71E-05
1.07E-04
0.350
0.350
0.348
0.348
0.345
0.348
0.350
0.350
0.344
0.347 0.006
0.003
0.003
0.001
0.001
-0.002
0.001
0.003
0.003
-0.003
3.57E-05
8.84E-06
8.84E-06
9.48E-07
9.48E-07
4.11E-06
9.48E-07
8.84E-06
8.84E-06
9.16E-06
Standard 5 11.2 0.427
0.424
0.423
0.420
0.424
0.422
0.421
0.421
0.422
0.415
0.432 -0.005
-0.008
-0.009
-0.012
-0.008
-0.010
-0.011
-0.011
-0.010
-0.017
2.50E-05
6.40E-05
8.10E-05
1.44E-04
6.40E-05
1.00E-04
1.21E-04
1.21E-04
1.00E-04
2.89E-04
Sum ∑ 3.37·10-3
With = 50 and = 2 7.03·10-5
0.008

Calculation of the limit of quantification
= 0.008 µA
B = 0.038 µA·L·mg-1
Limit of detection (LOD) = 3· / B = 0.66 mg/L ≙ 0.028 µA
Limit of quantification (LOQ) = 10· / B = 2.20 mg/L ≙ 0.087 µA
Figure 46: Limit of detection and limit of quantification for the determination of vitamin C.
0.00
0.05
0.10
0.15
0.20
0.25
0.30
0.35
0.40
0.45
0.0 2.0 4.0 6.0 8.0 10.0
I
p
/
µA
Concentration /mg·L-1
Measured values Linear regression LOD LOQ
3·sy
10·sy

Examples
7.2.3 Determination of vitamin C in multivitamin products
Sample Multivitamin effervescent tablet
Vitamin C content: 60 mg/tablet
Sample preparation 1 tablet dissolved in 200 mL ultrapure water.
Measuring solution 10 mL ultrapure water
Calibration curve
Figure 47: Calibration curve for the determination of vitamin C. (Measuring solution: 10 mL H2O + 1 mL
ammonium acetate buffer + ).
/ mL / mL β(vitamin C) / mg·L-1 *
/ µA
0.05 11.05 4.5 0.187
0.10 11.10 9.0 0.355
0.15 11.15 13.5 0.520
0.20 11.20 17.9 0.683
0.25 11.25 22.2 0.841
0.30 11.30 26.5 0.997
0.35 11.35 30.8 1.153
0.40 11.40 35.1 1.297
0.45 11.45 39.3 1.442
0.50 11.50 43.5 1.583
*
Regression parameters: Intercept (A) / µA 0.036
Slope (B) / µA·L·mg-1
0.036
0.0
0.2
0.4
0.6
0.8
1.0
1.2
1.4
1.6
1.8
0.0 20.0 40.0
I
p
/
µA
β(vitamin C) / mg·L-1

Sample with calibration curve
Figure 48: Determination of vitamin C in multivitamin effervescent tablet with calibration curve.
Vitamin C / µA / µA
Replication 1 0.407 0.405
Replication 2 0.403
With regression parameters from calibration curve: Intercept (A) / µA 0.036
0.036
 β(Vitamin C) = 10.3 mg/L
Volume correction:
– Concentration in the measuring solution 10.3 mg/L
– Total volume of the measuring solution 11.5 mL
– Volume of sample in the measuring solution 0.5 mL
– Concentration in the sample β(vitamin C) = 236.5 mg/L
1 tablet dissolved in 200 mL water w(vitamin C) = 47.3 mg/tablet
0.0
0.2
0.4
0.6
0.8
1.0
1.2
1.4
1.6
1.8
0.0 10.0 20.0 30.0 40.0
I
p
/
µA

Examples
Sample with standard addition
Figure 49: Determination of vitamin C in multivitamin effervescent tablet with standard addition.
Vitamin C /
mL
/ mL β(vitamin C) /
mg·L-1
/ µA / µA
Sample 0.0 11.5 0.0 0.407
0.403
0.405
1st
addition 0.1 11.6 8.6 0.666
0.665
0.665
2nd
addition 0.2 11.7 17.1 0.922
0.911
0.916
Linear regression: y = A + B x Intercept (A) / µA 0.406
0.030
for y = 0 it is -x = A / B  β(vitamin C) = 13.6 mg/L
Volume correction:
– Concentration in the measuring solution 13.6 mg/L
– Concentration in the sample β(vitamin C) = 312.1 mg/L
1 tablet dissolved in 200 mL water w(vitamin C) = 62 mg/tablet
0.0
0.2
0.4
0.6
0.8
1.0
-15.0 -10.0 -5.0 0.0 5.0 10.0 15.0 20.0
Ip / µA

Result discussion
The specified amount of vitamin C in the effervescent tablet is 60 mg. With the calibration curve a
content of 47.3 mg/tablet is determined, which corresponds to 78.8 % of the specified amount.
With the standard addition technique a content of 62 mg/tablet is determined, which corresponds to
103.3 % of the specified amount. The result obtained with the standard addition technique is much
closer to the specified amount of vitamin C in the tablet. The reasons are the compensation of matrix
and electrode effects. These are two of the main advantages of the standard addition technique over
the calibration curve. Therefore the standard addition technique would be the calibration technique
of choice to determine vitamin C in multivitamin products. Advantages and disadvantages of the two
calibration techniques are summarized below.
Calibration curve technique
Advantage Disadvantage
 Fast for large number of samples, since only
one measurement in the sample is required
once the calibration curve is established.
 New calibration curve required when a new
electrode is used (not feasible when the
electrode only lasts for a few
measurements).
 Sometimes outdated calibration curves are
not recognized.
 Matrix effects
- Influence of the matrix on the result
difficult to detect.
- Incorrect results due to matrix effects.
- Difficult to overcome matrix effects.
Standard addition technique
 Calibration in each determination.
 Matrix effects minimized.
 Effects from differing sensitivity of different
electrodes eliminated.
 Relatively slow, since at least one
measurement in the sample plus the
measurement of one addition are necessary.
For reliable results the measurement of two
additions is recommended.

Examples
Experiment 8: Quantification of mercury
8.2.1 Initial preparation of the electrode
Figure 50: Example for the change in the base line during the conditioning of the gold electrode. Displayed is
the 1st
, 10th
and 20th
replication (conditioning solution: 11 mL H2O + 0.1 mL HClO4).
Concentration standard: β(Hg) = 10 mg/L
/
mL
/
mL
β(Hg) / µg·L-1 *
/ µA
0.04 11.04 36.2 1.317
0.08 11.08 72.2 2.960
0.12 11.12 107.9 4.354
0.16 11.16 143.4 5.797
0.20 11.20 178.6 7.317
0.24 11.24 213.5 8.428
*
Concentrations outside the linear working range are marked
gray.
Figure 51: Linear working range for the determination of mercury. (Measuring solution: 10 mL ultrapure water
+ 1 mL supporting electrolyte + ). mean of 2 replications.
1st

10th

20th


Figure 52: Linear working range for the determination of mercury.
Calibration curve for the determination of LOD and LOQ
Figure 53: Example for curves recorded for the determination of LOD and LOQ for mercury. (Measuring
solution: 10 mL H2O + 1 mL supporting electrolyte + ).
0
1
2
3
4
5
6
7
8
9
0.0 50.0 100.0 150.0 200.0
Ip / µA
c(Hg) / µg·L-1
0.0
0.5
1.0
1.5
2.0
2.5
3.0
3.5
0.0 20.0 40.0 60.0 80.0
Ip /µA
Concentration /µg·L-1
Linear working range Hg

Examples
Solution /
mL
/ mL β(Hg) / µg·L-1 *
/ µA ̂ / µA
Blank 0.000 11.000 0.0 0.047 -0.182
Standard 1 0.020 11.020 18.1 0.486 0.471
Standard 2 0.040 11.040 36.2 1.114 1.123
Standard 3 0.060 11.060 54.2 1.756 1.772
Standard 4 0.080 11.080 72.2 2.418 2.418
Standard 5 0.100 11.100 90.1 3.073 3.063
*
Regression parameters: Intercept (A) -0.182 µA
Slope (B) 0.036 µA·L·µg-1
∑
( ̂ )
(Eq. 6)
Solution β(Hg) / µg·L-1
/ µA ̂ / µA ̂ ( ̂ )
Blank 0.0 0.031
0.139
0.040
0.041
0.025
0.031
0.040
0.026
-0.182 0.213
0.321
0.222
0.223
0.207
0.213
0.222
0.208
4.56E-02
1.03E-01
4.95E-02
4.99E-02
4.30E-02
4.56E-02
4.95E-02
4.35E-02
Standard 1 18.1 0.499
0.455
0.483
0.517
0.494
0.500
0.455
0.484
0.471 0.028
-0.016
0.012
0.046
0.023
0.029
-0.016
0.013
7.69E-04
2.64E-04
1.38E-04
2.09E-03
5.17E-04
8.26E-04
2.64E-04
1.62E-04
Standard 2 36.2 1.079
1.135
1.087
1.132
1.125
1.135
1.087
1.132
1.125 -0.044
0.012
-0.036
0.009
0.002
0.012
-0.036
0.009
1.92E-03
1.49E-04
1.28E-03
8.49E-05
4.91E-06
1.49E-04
1.28E-03
8.49E-05
Standard 3 54.2 1.725
1.743
1.760
1.756
1.796
1.725
1.743
1.796
1.774 -0.047
-0.029
-0.012
-0.016
0.024
-0.047
-0.029
0.024
2.18E-03
8.25E-04
1.37E-04
2.47E-04
5.90E-04
2.18E-03
8.25E-04
5.90E-04

Standard 4 72.2 2.347
2.355
2.424
2.468
2.579
2.347
2.355
2.468
2.420 -0.071
-0.063
0.006
0.050
0.161
-0.071
-0.063
0.050
5.09E-03
4.01E-03
3.24E-05
2.47E-03
2.58E-02
5.09E-03
4.01E-03
2.47E-03
Standard 5 90.1 3.024
2.985
3.079
3.151
3.086
3.024
3.151
3.086
3.064 -0.039
-0.078
0.016
0.088
0.023
-0.039
0.088
0.023
1.49E-03
6.02E-03
2.70E-04
7.82E-03
5.49E-04
1.49E-03
7.82E-03
5.49E-04
Sum ∑ 5.22·10-1
With = 40 and = 2 1.37·10-2
0.117
Calculation of the limit of quantification for mercury
= 0.117 µA
B = 0.036 µA·L·µg-1
Limit of detection (LOD) = 3· / B = 8.1 µg/L ≙ 0.108 µA
Limit of quantification (LOQ) = 10· / B = 26.9 µg/L ≙ 0.786 µA
Figure 54: Limit of detection and limit of quantification for the determination of mercury.
-0.5
0.0
0.5
1.0
1.5
2.0
2.5
3.0
3.5
0.0 10.0 20.0 30.0 40.0 50.0 60.0 70.0 80.0 90.0
I
p
/
µA
3·sy
10·sy

Examples
8.2.4 Determination of mercury in air
Sample Polluted air
Since no contamination with mercury could be detected in ambient and
workplace air the following setup was chosen to simulate polluted air.
Approx. 100 g of mercury were filled into a 500 mL sample container. The
container was closed tightly and kept at room temperature to allow the
evaporation of mercury. After 1 day the air from the sample container was
sampled with the described setup.
Sample preparation Sampling:
Shortly before the sampling the flame-sealed ends of the sorbent tube
were broken off using a glass cutter. The sorbent tube was connected to
the air pump as shown in Figure 55 and the air was sampled with the
following conditions:
Air flow 120 L/h
Sampling time 60 min
After the sampling time the sorbent tube was disconnected from the
sampling unit and both ends were closed with the included sealing caps.
Figure 55: Schematic setup for the sampling of mercury in air.
Extraction:
After removing the glass wool from the sorbent tube, the sorbent was
completely transferred into a 10 mL volumetric flask. 2 mL w(HNO3) =
65 % were added and thoroughly mixed with the sorbent. Then 2 mL
w(HCl) = 30 % were carefully added. Attention, vigorous reaction with
intensive gas formation! After the reaction the volumetric flask was firmly
closed and placed for 1 hour in a water bath at 50 °C. When cooled down
to room temperature the test solution was made up to the mark with
ultrapure water.
Measuring solution 10 mL H2O
flow meter
sorbent tube
air pump
connecting tube
air flow
glass wool
sorbent

Calibration curve
Figure 56: Calibration curve for the determination of mercury. (Measuring solution 10 mL H2O + 1 mL
supporting electrolyte + )
/ mL / mL β(Hg) / µg·L-1 *
/ µA
0.040 11.040 36.2 1.317
0.060 11.060 54.2 2.076
0.080 11.080 72.2 2.960
0.100 11.100 90.1 3.649
0.120 11.120 107.9 4.354
0.140 11.140 125.7 5.023
0.160 11.160 143.4 5.797
0.180 11.180 161.0 6.585
0.200 11.200 178.6 7.317
*
Regression parameters: Intercept (A) / µA -0.156
Slope (B) / µA·L·µg-1
0.042
0.0
1.0
2.0
3.0
4.0
5.0
6.0
7.0
8.0
0.0 50.0 100.0 150.0 200.0
I
p
/
µA
β(Hg)/ µg·L-1

Examples
Sample with calibration curve
Figure 57: Determination of mercury air with calibration curve.
Hg / µA / µA
Replication 1 2.057 2.083
Replication 2 2.108
With regression parameters from calibration curve: Intercept (A) / µA -0.156
0.042
 β(Hg) = 53.6 µg/L
Volume correction:
– Concentration in the measuring solution 53.6 µg/L
– Volume of test solution in the measuring solution 0.5 mL
– Concentration in the test solution β(Hg) = 1.23 mg/L
With
Concentration of mercury in the test solution β(Hg) = 1.23 mg/L
Total volume of test solution 10 mL = 0.01 L
Gas flow 120 L/h = 0.12 m3
/h
Sampling time 1 h
βair(Hg) = 0.10 mg/m3
0.0
1.0
2.0
3.0
4.0
5.0
6.0
7.0
8.0
0.0 50.0 100.0 150.0 200.0
Ip / µA
β(Hg) / µg·L-1

Assuming the mercury in the test tube is only deriving from the mercury vapor in the sample
container, the concentration of mercury in the air space of the sample container is:
Total volume of the sample container 620 mL = 0.62·10-3
m3
Sample with standard addition
Figure 58: Determination of mercury in air with standard addition.
Hg /
mL
/ mL β(Cd) / µg·L-1
/ µA / µA
Sample 0.000 11.500 0.0 2.057
2.108
2.083
1st
addition 0.025 11.525 21.7 2.946
3.058
3.002
2nd
addition 0.050 11.550 43.3 3.993
3.995
3.994
0.044
for y = 0 it is -x = A / B  β(Hg) = 46.9 µg/L
0.0
1.0
2.0
3.0
4.0
5.0
-50.0 -30.0 -10.0 10.0 30.0 50.0
Ip / µA
β(Hg)/ µg·L-1

Examples
Volume correction:
– Concentration in the test solution β(Hg) = 1.08 mg/L
With
Gas flow 120 L/h = 0.12 m3
/h
Sampling time 1 h
Assuming the mercury in the test tube is only deriving from the mercury vapor in the sample
container, the concentration of mercury in the air space of the sample container is:
Total volume of the sample container 620 mL = 0.62·10-3
m3
Result discussion
Referring to the air volume which was sampled in 1 hour, the concentration of mercury found with
the calibration curve technique was 0.10 mg/m3
and with the standard addition curve 0.09 mg/m3
.
The fact that the two results are quite similar indicates that there is no significant interference from
the sample matrix. Therefore both calibration techniques can be used for this application.
Nevertheless standard addition should be preferred because of the advantages and disadvantages
summarized below.
A quite interesting result is obtained if the result is not calculated with respect to the total volume of
air sampled in 1 hour but only with respect to the available air space in the sample container which
would represent the concentration of mercury vapor in the closed sample container. The
concentration was found to be βair(Hg) = 19.84 mg/m3
by calibration curve and βair(Hg) = 17.42
mg/m3
by standard addition. These values are in a good agreement with the mass concentration of
mercury in air at equilibrium that can be found in the literature (21)
:
β(Hg) = 13.6 mg/m3
at 20 °C
β(Hg) = 29.6 mg/m3
at 30 °C

Calibration curve technique
 Fast for large number of samples, since only
one measurement in the sample is required
once the calibration curve is established.
 New calibration curve required when a new
electrode is used (not feasible when the
electrode only lasts for a few
measurements).
 Sometimes outdated calibration curves are
not recognized.
 Matrix effects
- Influence of the matrix on the result
difficult to detect.
- Incorrect results due to matrix effects.
- Difficult to overcome matrix effects.
Standard addition technique
 Calibration in each determination.
 Matrix effects minimized.
 Effects from differing sensitivity of different
electrodes eliminated.
 Relatively slow, since at least one
measurement in the sample plus the
measurement of one addition are necessary.
For reliable results the measurement of two
additions is recommended.

Examples
Experiment 9: Quantification of cadmium and lead
9.2.1 Preparation of the mercury film
Figure 59: Example for the potential scan after the plating of the mercury film (measuring solution: 12 mL Hg
plating solution), signal at -0.6 V is due to lead impurities in the plating solution.

9.2.2 Deposition potential
Edep / V (Cd)*
/ µA (Pb)*
/ µA
-0.5 0.940 0.817
-0.6 0.975 1.287
-0.7 0.912 4.677
-0.8 1.192 5.851
-0.9 7.905 6.324
-1.0 8.197 6.491
-1.2 8.426 6.299
-1.4 8.138 6.136
*
Figure 60: Example for the influence of the deposition potential on the peak height. (Measuring solution: 10 mL
H2O + 1 mL buffer pH 4.4 + 0.1 mL Cd standard solution (β(Cd) = 10 mg/L) + 0.1 mL Pb standard solution
(β(Pb) = 0.1 mg/L)).
Figure 61: Pseudo-polarogram for cadmium and lead.
Result discussion
The so-called «pseudo-polarogram» shows the peak height of the stripping signal as a function of the
deposition potential. At potentials more positive than the peak potential of the Me/Me2+
system
(Cd/Cd2+
at approx. -0.8 V or Pb/Pb2+
at approx. -0.6 V) no deposition of metal can be observed. The
peak height reaches the maximum at a deposition potential of approx. 200 mV more negative than
the peak potential. Applying a more negative potential does not further increase the peak height. It
can be concluded that -1.0 V or better yet -1.2 V would be suitable deposition potentials for the
determination of cadmium and lead at the mercury film electrode.
0
2
4
6
8
10
-1.5 -1.3 -1.1 -0.9 -0.7 -0.5
Ip / µA
Edep / V
Cd
Pb

Examples
Cadmium
Concentration standard: β(Cd) = 10 mg/L
/
mL
/ mL β(Cd) /
µg·L-1
*
/ µA
0.050 11.100 45.0 4.934
0.100 11.200 89.3 9.880
0.150 11.300 132.7 14.756
0.200 11.400 175.4 18.724
0.250 11.500 217.4 22.662
0.300 11.600 258.6 26.026
0.350 11.700 299.1 28.100
0.400 11.800 339.0 29.243
*
marked gray.
Figure 62: Linear working range for the determination of cadmium. (Measuring solution 10 mL H2O + 1 mL
buffer pH 4.4 + ).
Figure 63: Linear working range for the determination of cadmium.
0
5
10
15
20
25
30
0 50 100 150 200 250 300 350
Ip / µA
c(Cd) / µg·L-1
Linear working range Cd

Lead
Concentration standard: β(Pb) = 10 mg/L
/
mL
/ mL β(Pb) /
µg·L-1
*
/ µA
0.050 11.100 45.0 3.024
0.100 11.200 89.3 6.094
0.150 11.300 132.7 9.317
0.200 11.400 175.4 12.041
0.250 11.500 217.4 15.186
0.300 11.600 258.6 18.106
0.350 11.700 299.1 19.887
0.400 11.800 339.0 21.228
*
marked gray.
Figure 64: Linear working range for the determination of lead. (Measuring solution 10 mL H2O + 1 mL buffer
pH 4.4 + ).
Figure 65: Linear working range for the determination of lead.
0
5
10
15
20
25
0 50 100 150 200 250 300 350
Ip / µA
c(Pb) / µg·L-1
Linear working range Pb

Examples
Cadmium
Figure 66: Example for curves recorded for the determination of LOD and LOQ for cadmium and lead.
(Measuring solution 10 mL H2O + 1 mL buffer pH 4.4 + )
Concentration standard: β(Cd) = 0.2 mg/L
Solution /
mL
/ mL β(Cd) / µg·L-1 *
/ µA ̂ / µA
Blank 0.0 11.0 0.00 0.004 -0.017
Standard 1 0.1 11.1 1.80 0.147 0.157
Standard 2 0.2 11.2 3.57 0.333 0.327
Standard 3 0.3 11.3 5.31 0.506 0.494
Standard 4 0.4 11.4 7.02 0.658 0.659
Standard 5 0.5 11.5 8.70 0.813 0.820
*
Regression parameters: Intercept (A) -0.017 µA
∑
( ̂ )
(Eq. 6)
0.0
0.1
0.2
0.3
0.4
0.5
0.6
0.7
0.8
0.9
0.0 2.0 4.0 6.0 8.0
Ip /µA
Cd


Solution β(Cd) / µg·L-1
/ µA ̂ / µA ̂ ( ̂ )
Blank 4.5 0.003
0.003
0.002
0.008
0.005
0.006
0.008
0.004
0.003
0.004
-0.017 0.020
0.020
0.019
0.025
0.022
0.023
0.025
0.021
0.020
0.021
3.81E-04
3.81E-04
3.43E-04
6.01E-04
4.63E-04
5.07E-04
6.01E-04
4.21E-04
3.81E-04
4.21E-04
0.147
0.149
0.146
0.153
0.148
0.152
0.145
0.152
0.146
0.157 -0.019
-0.010
-0.008
-0.011
-0.004
-0.009
-0.005
-0.012
-0.005
-0.011
3.56E-04
9.71E-05
6.17E-05
1.18E-04
1.49E-05
7.84E-05
2.36E-05
1.41E-04
2.36E-05
1.18E-04
Standard 2 13.5 0.329
0.333
0.335
0.340
0.329
0.336
0.337
0.311
0.330
0.339
0.327 0.002
0.006
0.008
0.013
0.002
0.009
0.010
-0.016
0.003
0.012
3.53E-06
3.46E-05
6.21E-05
1.66E-04
3.53E-06
7.88E-05
9.76E-05
2.60E-04
8.28E-06
1.41E-04
Standard 3 17.9 0.500
0.500
0.506
0.512
0.514
0.506
0.512
0.508
0.497
0.513
0.494 0.006
0.006
0.012
0.018
0.020
0.012
0.018
0.014
0.003
0.019
3.16E-05
3.16E-05
1.35E-04
3.11E-04
3.85E-04
1.35E-04
3.11E-04
1.86E-04
6.89E-06
3.47E-04
Standard 4 22.2 0.646
0.660
0.661
0.663
0.660
0.662
0.651
0.663
0.658
0.649
0.659 -0.013
0.001
0.002
0.004
0.001
0.003
-0.008
0.004
-0.001
-0.010
1.61E-04
1.71E-06
5.32E-06
1.85E-05
1.71E-06
1.09E-05
5.92E-05
1.85E-05
4.81E-07
9.40E-05
Standard 5 26.5 0.810
0.815
0.817
0.815
0.808
0.805
0.816
0.806
0.804
0.796
0.820 -0.010
-0.005
-0.003
-0.005
-0.012
-0.015
-0.004
-0.014
-0.016
-0.024
1.03E-04
2.66E-05
9.95E-06
2.66E-05
1.48E-04
2.30E-04
1.73E-05
2.00E-04
2.61E-04
5.83E-04
Sum ∑ 1.02·10-2
With = 50 and = 2 2.13·10-4
0.015

Examples
Calculation of the limit of quantification for cadmium
= 0.015 µA
B = 0.096 µA·L·µg-1
Figure 67: Limit of detection and limit of quantification for the determination of cadmium.
Lead
Figure 68: Example for curves recorded for the determination of LOD and LOQ for cadmium and lead.
(Measuring solution 10 mL H2O + 1 mL buffer pH 4.4 + )
-0.1
0.0
0.1
0.2
0.3
0.4
0.5
0.6
0.7
0.8
0.9
0.0 1.0 2.0 3.0 4.0 5.0 6.0 7.0 8.0 9.0
I
p
/
µA
3·sy
10·sy
0.0
0.1
0.2
0.3
0.4
0.5
0.6
0.7
0.8
0.9
0.0 2.0 4.0 6.0 8.0 10.0 12.0
Ip / µA
Pb


Concentration standard: β(Pb) = 0.3 mg/L
Solution /
mL
/ mL β(Pb) / µg·L-1 *
/ µA ̂ / µA
Blank 0.0 11.0 0.00 0.010 0.005
Standard 1 0.1 11.1 2.70 0.171 0.186
Standard 2 0.2 11.2 5.36 0.372 0.364
Standard 3 0.3 11.3 7.96 0.554 0.539
Standard 4 0.4 11.4 10.53 0.714 0.710
Standard 5 0.5 11.5 13.04 0.866 0.879
*
Regression parameters: Intercept (A) 0.005 µA
∑
( ̂ )
(Eq. 6)
Solution β(Pb) / µg·L-1
/ µA ̂ / µA ̂ ( ̂ )
Blank 0.00 0.018
0.005
0.016
0.009
0.004
0.003
0.003
0.004
0.006
0.003
0.005 0.013
0.000
0.011
0.004
-0.001
-0.002
-0.002
-0.001
0.001
-0.002
1.76E-04
7.49E-08
1.27E-04
1.83E-05
5.28E-07
2.98E-06
2.98E-06
5.28E-07
1.62E-06
2.98E-06
Standard 1 2.70 0.164
0.176
0.165
0.172
0.177
0.174
0.178
0.184
0.176
0.185
0.186 -0.022
-0.010
-0.021
-0.014
-0.009
-0.012
-0.008
-0.002
-0.010
-0.001
4.78E-04
9.72E-05
4.35E-04
1.92E-04
7.85E-05
1.41E-04
6.18E-05
3.46E-06
9.72E-05
7.38E-07
Standard 2 5.36 0.391
0.359
0.366
0.375
0.371
0.364
0.374
0.369
0.340
0.376
0.364 0.027
-0.005
0.002
0.011
0.007
0.000
0.010
0.005
-0.024
0.012
7.42E-04
2.26E-05
5.03E-06
1.26E-04
5.25E-05
5.91E-08
1.05E-04
2.75E-05
5.64E-04
1.50E-04
Standard 3 7.96 0.569
0.554
0.548
0.547
0.552
0.553
0.548
0.546
0.539 0.030
0.015
0.009
0.008
0.013
0.014
0.009
0.008
9.30E-04
2.40E-04
9.01E-05
7.21E-05
1.82E-04
2.10E-04
9.01E-05
5.92E-05

Examples
0.537
0.545
-0.002
0.006
2.27E-06
4.22E-05
Standard 4 10.53 0.734
0.713
0.708
0.720
0.697
0.699
0.685
0.707
0.682
0.685
0.710 0.024
0.003
-0.002
0.010
-0.013
-0.011
-0.025
-0.003
-0.028
-0.025
5.67E-04
7.90E-06
4.80E-06
9.62E-05
1.74E-04
1.25E-04
6.35E-04
1.02E-05
7.95E-04
6.35E-04
Standard 5 13.04 0.882
0.876
0.863
0.863
0.844
0.836
0.854
0.832
0.840
0.840
0.879 0.003
-0.003
-0.016
-0.016
-0.035
-0.043
-0.025
-0.047
-0.039
-0.039
9.69E-06
8.34E-06
2.52E-04
2.52E-04
1.22E-03
1.84E-03
6.19E-04
2.20E-03
1.51E-03
1.51E-03
Sum ∑ 1.81·10-2
With = 50 and = 2 3.77·10-4
0.019
Calculation of the limit of quantification for lead
= 0.019 µA
B = 0.067 µA·L·µg-1
Figure 69: Limit of detection and limit of quantification for the determination of lead.
0.0
0.1
0.2
0.3
0.4
0.5
0.6
0.7
0.8
0.9
0.0 2.0 4.0 6.0 8.0 10.0 12.0
I
p
/
µA
Concentration/ µg·L-1
3·sy
10·sy

9.2.5 Determination of cadmium and lead in articles of daily use
Sample Decanter made from lead glass
Sample preparation The decanter was filled to the top with extraction solution (w(acetic acid) =
4 % v/v). After 24 hours at room temperature (approx. 23 °C) the complete
extraction solution was transferred into a clean storage container.
Measuring solution 10 mL H2O
1 mL buffer pH 4.4
1 mL extraction solution
Cadmium
Figure 70: Determination of cadmium in extraction solution from lead glass by standard addition.
Concentration standard: β(Cd) = 0.5 mg/L
Cd /
mL
/ mL β(Cd) / µg·L-1
/ µA / µA
Sample 0.0 12.0 0 0.065
0.068
0.067
1st
addition 0.1 12.1 4.1 0.471
0.466
0.469
2nd
addition 0.2 12.2 8.1 0.891
0.898
0.895
0.101
for y = 0 it is -x = A / B  β(Cd) = 0.6 µg/L
0.0
0.2
0.4
0.6
0.8
1.0
-1.0 1.0 3.0 5.0 7.0 9.0
Ip / µA
β(Cd)/ µg·L-1
Cd


Examples
Volume correction:
– Volume of sample in the measuring solution 1 mL
– Concentration in the sample β(Cd) = 7.2 µg/L
Lead
Figure 71: Determination of lead in extraction solution from lead glass by standard addition.
Concentration standard: β(Pb) = 1 mg/L
Pb /
mL
/ mL β(Pb) / µg·L-1
/ µA / µA
Sample 0.0 12.0 0.0 0.602
0.591
0.597
1st
addition 0.1 12.1 8.3 1.12
1.131
1.126
2nd
addition 0.2 12.2 16.4 1.675
1.714
1.695
0.067
for y = 0 it is -x = A / B  β(Pb) = 8.8 µg/L
0.0
0.2
0.4
0.6
0.8
1.0
1.2
1.4
1.6
1.8
-10.0 -5.0 0.0 5.0 10.0 15.0 20.0
Ip / µA
β(Pb) / µg·L-1
Pb


Volume correction:
– Volume of sample in the measuring solution 1 mL
– Concentration in the sample β(Pb) = 105.4 µg/L
Result discussion
The concentrations for cadmium and lead found in the extraction solution are β(Cd) = 7.2 µg/L and
β(Pb) = 105.4 µg/L. These values are far below the tolerable limits e.g. in Germany β(Pb) = 4.0 mg/L
and β(Cd) = 0.3 mg/L (as specified in EU directive 84/500/EEC(22)
and adopted by German regulation
BedGgstV(23)
). As far as the measured concentration of Cd is concerned, it has to be kept in mind
that the concentration in the measuring solution is only β(Cd) = 0.6 µg/L which is below the limit of
quantification of β(Cd) = 1.5 µg/L. Therefore a rather large error has to be expected for this result.

Examples
Experiment 10: The principle of a glucose sensor
β(glucose) / mg·L-1 *
/ µA *
/ µA·s
200 0.552 21.807
400 1.166 46.276
600 1.716 71.561
800 2.173 89.561
1000 2.527 106.075
*
Mean of 5 injections
marked gray.
Figure 72: Curves recorded to evaluate the linear working range for the determination of glucose on a GOx
modified electrode. (Carrier solution: phosphate buffer pH 5.2).
Figure 73: Linear working range for the determination of glucose on a GOx modified electrode.
0.0
20.0
40.0
60.0
80.0
100.0
0 200 400 600 800 1000
Ap / µA·s
β(glucose) / mg·L-1
Linear working range

10.2.4 Interferences
/ µA / µA·s
β(glucose) = 400 mg/L 1.051 38.128
β(vitamin C) = 10 mg/L 1.274 46.290
Figure 74: Interference of vitamin C in the determination of glucose on a GOx modified electrode. (Carrier
solution: phosphate buffer pH 5.2).
Result discussion
No interference can be observed from other sugars. Even the disaccharide sucrose which contains
one molecule of glucose does not show a signal in the measurement. However, at the potential of
0.5 V, which is used to oxidize the hydrogen peroxide, also vitamin C is oxidized. β(Vitamin C) =
10 mg/L would feign a concentration of approx. β(glucose) = 500 mg/L. Conversely this means, that
the expected error of the glucose result will be less than 10 % if the concentration of vitamin C is not
more than 0.2 % of the concentration of glucose.
One possibility to overcome the interference of vitamin C could be the optimization of the oxidation
potential. Depending on the electrolyte, the oxidation potential of vitamin C begins in the range of
+0.2 V to +0.4 V (see experiments 5 and 7). The oxidation of hydrogen peroxide starts at around 0 V.
Choosing a potential between 0 V and +0.2 V for the amperometric detection should allow the
determination without the interference of vitamin C, but this hypothesis needs confirmation by
experimental data.
10.2.5 Determination of glucose in different food products
Sample Fruit juice: apple juice, grape juice
Beverages: iced tea, cola soft drink
Honey
Sample solution
juices and beverages
0.1 mL of the particular sample was pipetted into a 10 mL volumetric flask
and made up to the mark with phosphate buffer.
Honey stock solution 1.144 g honey was weight in, transferred into a 25 mL volumetric flask
and dissolved and made up to the mark with phosphate buffer.
Sample solution
honey
An aliquot of 0.1 mL honey stock solution was pipetted into a 10 mL
volumetric flask and made up to the mark with phosphate buffer.

β(vitamin C) = 10 mg/L


Examples
Recovery test
solution 1
0.1 mL honey stock solution and 0.075 mL of glucose stock solution
(β(glucose) = 10 g/L) was pipetted into a 10 mL volumetric flask and made
up to the mark with phosphate buffer.
Recovery test
solution 2
0.1 mL honey stock solution and 0.15 mL of glucose stock solution
(β(glucose) = 10 g/L) was pipetted into a 10 mL volumetric flask and made
up to the mark with phosphate buffer.
Calibration curve
Figure 75: Calibration curve for the determination of glucose on a GOx modified electrode. (Carrier solution:
phosphate buffer pH 5.2).
β(glucose) / mg·L-1 *
/ µA *
/ µA·s
50 0.132 4.783
100 0.255 9.173
200 0.513 18.745
300 0.751 27.619
400 0.986 36.586
500 1.199 44.897
600 1.380 52.719
*
Mean of 3 injections
Regression parameters: Intercept (A) / µA·s 0.796
Slope (B) / µA·s·L·mg-1
0.088
0.0
10.0
20.0
30.0
40.0
50.0
0 200 400 600
A
p
/
µA·s

Samples with calibration curve
Apple juice made from concentrate
Figure 76: Determination of glucose in apple juice with calibration curve (apple juice diluted 1:100 with
Glucose / µA·s / µA·s
Injection 1 16.230 16.250
Injection 2 15.980
Injection 3 16.540
With regression parameters from calibration curve: Intercept (A) / µA·s 0.796
0.088
 β(glucose) = 175.8 mg/L
Volume correction:
– Concentration in the sample solution 175.8 mg/L
– Total volume of the sample solution 10 mL
– Volume of sample in the sample solution 0.1 mL
– Concentration in apple juice β(glucose) = 17.6 g/L
0.0
10.0
20.0
30.0
40.0
50.0
0 100 200 300 400 500 600
Ap / µA·s

Examples
Grape juice
Figure 77: Determination of glucose in grape juice with calibration curve (grape juice diluted 1:100 with
Injection 1 47.454 46.849
Injection 2 46.913
Injection 3 46.180
0.088
Volume correction:
– Concentration in grape juice β(glucose) = 52.4 g/L
0.0
10.0
20.0
30.0
40.0
50.0
0 100 200 300 400 500 600
Ap / µA·s

Iced tea
Figure 78: Determination of glucose in iced tea with calibration curve (iced tea juice diluted 1:100 with
Injection 1 27.824 28.413
Injection 2 28.669
Injection 3 28.747
0.088
Volume correction:
– Concentration in iced tea β(glucose) = 31.4 g/L
0.0
10.0
20.0
30.0
40.0
50.0
0 100 200 300 400 500 600
Ap / µA·s

Examples
Cola soft drink
Figure 79: Determination of glucose in cola soft drink with calibration curve (cola soft drink diluted 1:100 with
Injection 1 41.541 41.407
Injection 2 41.385
Injection 3 41.294
0.088
Volume correction:
– Concentration in cola soft drink β(glucose) = 46.2 g/L
0.0
10.0
20.0
30.0
40.0
50.0
0 100 200 300 400 500 600
Ap / µA·s

Honey
Figure 80: Determination of glucose in honey with calibration curve (honey diluted with phosphate buffer
pH 5.2).
Injection 1 13.535 13.497
Injection 2 13.376
Injection 3 13.581
0.088
Volume correction:
– Volume of the aliquot of honey stock
solution in the sample solution
0.1 mL
– Concentration in honey stock solution β(glucose) = 14.5 g/L
– Concentration in honey stock solution 14.5 mg/L
– Total volume of the honey stock solution 25 mL
– Amount of sample in the stock solution 1.144 g
– Concentration in honey w(glucose) = 315.8 mg/g
0.0
10.0
20.0
30.0
40.0
50.0
0 100 200 300 400 500 600
Ap / µA·s

Examples
Recovery test solution
Figure 81: Determination of glucose recovery in honey with calibration curve.
Recovery test solution 1
Injection 1 21.236 20.305
Injection 2 19.835
Injection 3 19.845
0.088
( )
– concentration in the recovery test solution 222.0 mg/L
– concentration in the sample solution 144.5 mg/L
– spiked concentration 75 mg/L
Recovery 103.3 %
Injection 1 27.954 27.547
Injection 2 27.899
Injection 3 26.789
0.088
0.0
10.0
20.0
30.0
40.0
50.0
0 100 200 300 400 500 600
Ap / µA·s

( )
– concentration in the recovery test solution 304.4 mg/L
– concentration in the sample solution 144.5 mg/L
– spiked concentration 150 mg/L
Recovery 106.6 %
Result discussion
Recovery in honey
= 75 mg/L 103.3 %
= 150 mg/L 106.6 %
The concentration of glucose in the honey
sample solution was found to be β(glucose) =
144.5 mg/L. Spiking this solution with β(glucose)
= 75 mg/L and β(glucose) = 150 mg/L respectively
shows a recovery of 103.3 % and 106.6 %. This
indicates that there is no significant interference
from the matrix.
Honey
β(glucose) 315.8 mg/g
Nutrition facts(24) Glucose: 22 – 41 %
Vitamin C: 0.026 mg/g
From the concentration in the honey sample
solution a content of β(glucose) = 315.8 mg/g in
honey can be calculated. A comparison with
nutrition facts, which can be found in the
literature, shows that the result of about 31 %
glucose in honey is realistic. The expected
vitamin C content does not affect the result for
the glucose. Doing a rough calculation,
considering the dilution of the honey for the
measurement, the concentration of vitamin C in
the sample solution was about 0.001 mg/L. This
concentration is at least 100 times lower than the
concentration of vitamin C that would trigger a
signal in the measurement.
Sample β(glucose) Sugar
as specified
on the bottle
Apple juice 17.6 g/L 100 g/L
Grape juice 52.4 g/L 160 g/L*
Iced tea 31.4 g/L 80 g/L
Cola soft
drink
46.2 g/L 106 g/L
The table to the left shows the comparison of the
determined concentrations of glucose and the
total amount of sugar specified on the bottles of
the other samples. The fraction of glucose as part
of the sugar represents between 18 % in apple
juice to 44 % in cola soft drink. None of the
samples contained vitamin C as an additive.
*
Carbohydrates, sugar not separately specified

Abbreviations
12 Abbreviations
SI unit
Area of the working electrode cm2
Peak area µA·V or µA·s
A Intercept of a linear regression
AE Auxiliary electrode
B Slope of a linear regression
Concentration mol·L-1
Diffusion coefficient cm2
·s-1
Diffusion coefficient of the reduced species,
corresponds to the anodic signal
cm2
·s-1
Diffusion coefficient of the oxidized species,
corresponds to the cathodic signal
cm2
·s-1
Peak potential V
Peak potential of the anodic signal V
Peak potential of the cathodic signal V
Faraday constant (9.648·104
C·mol-1
)
Peak height µA
Peak height of the anodic signal µA
Peak height of the cathodic signal µA
Standard rate constant for electron transfer cm·s-1
Number of electrons --
PEEK Polyether ether ketone
PTFE Polytetrafluoro ethylene, most common name Teflon
Molar gas constant (8.314 J·mol-1
·K-1
)
RE Reference electrode
Temperature K
Volume L or cm3
w Mass concentration % or mg·g-1
WE Working electrode
Charge transfer coefficient --
β Mass concentration g·L-1
or g·m-3
Scan rate V·s-1
𝜓 Charge transfer parameter --

Bibliography
13 Bibliography
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ISBN 3-527-29275-6.
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anodic stripping voltammetry.
http://www.metrohm.com/com/Applications/literature2/Application_Bulletins.html.
13. ISO 17733:2004. Workplace air - Determination of mercury and inorganic mercury compounds.
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anodic stripping voltammetry using carbon electrodes.
http://www.metrohm.com/com/Applications/literature2/Application_Bulletins.html.
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1: Test method. ISO - International Organization for Standardization. 2000.
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2: Permissible limits. ISO - International Organization for Standardization. 2000.
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Bibliography
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of the laws of the Member States relating to ceramic articles intended to come into contact with
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Verlagsgesellschaft mbH, 2011.
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Akademischer Verlag, 1998. ISBN 3-8274-0135-6.
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Aspect Publications Ltd., 1990. ISBN 1-85529-025-1.

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