1. "Determination of Anionic Surfactants Using Atomic
Absorption Spectrometry and Anodic Stripping Voltammetry"
John, Richard; Lord, Daniel. J. Chem. Educ. 1999 76 1256.
(September 1999)
An experiment has been developed for our undergraduate analyticalchemistry
course that demonstrates the indirect analysis of anionic surfactants
by techniques normally associated with metal ion determination;
that is, atomic absorption spectroscopy (AAS) and anodic stripping
voltammetry (ASV). The method involves the formation of an extractable
complex between the synthetic surfactant anion and the bis(ethylenediamine)diaqua
copper(II) cation. This complex is extracted into chloroform and
then back-extracted into dilute acid. The resulting Cu(II) ions
are determined by AAS and ASV. Students are required to determine
the concentration of a pre-prepared "unknown" anionic
surfactant solution and to collect and analyze a real sample of
their choice. After the two extraction processes, students typically
obtain close to 100% analytical recovery. Correlation between
student AAS and ASV results is very good, indicating that any
errors that occur probably result from their technique (dilutions,
extractions, preparation of standards, etc.) rather than from
the end analyses.
2. "Using Cyclic Voltammetry and Molecular Modeling
To Determine Substituent Effects in the One-Electron Reduction
of Benzoquinones" Heffner, Janell E.; Raber, Jeffrey
C.; Moe, Owen A., Jr.; Wigal, Carl T. J. Chem. Educ. 1998 75 365.
(March 1998)
An experiment has been developed to teach the principles of molecular
luminescence spectroscopy. This laboratory experiment is designed
for upper-level undergraduates as a less toxic alternative to
current fluorescence experiments. It combines elements of physical
and inorganic as well as analytical chemistry. The experiment
can be performed on a variety of rudimentary fluorescence instrumentation
and still give good analytical figures of merit. The object of
the experiment is to measure the luminescent enhancement that
is achieved when a lanthanide such as Eu(III) or Tb(III) is complexed
with appropriate organic ligands, in this case 2,6 pyridinedicarboxylic
acid. The importance of pH on metal ion coordination is also explored
via luminescence intensity. This approach provides several advantages
over current luminescence experiments. These advantages include
limited toxicity and flammability of the chemicals involved, a
large luminescence linear dynamic range, and low detection limits
(parts per trillion). These low detection limits, achieved using
modest equipment, allow the determination of the europium concentration
in a variety of samples, such as tap water. The narrow lanthanide
luminescent bands also permit incorporation of qualitative analysis
of a mixture of lanthanides.
3. "The use of cyclic voltammetry in the study of the chemistry of metal-carbonyls: An introductory experiment" Carriedo, Gabino A. . J.Chem. Educ. 1988 65 1020.
4. "A cyclic voltammetry experiment using a mercury electrode" Brillas, Enrique; Garrido, Jose A.; Rodriquez, Rosa M.; Domenech, Javier. J. Chem. Educ. 1987 64 189.
5. "Voltammetry as a model for teaching chemical instrumentation" Gunasingham, H.; Ang, K. P. J. Chem. Educ. 1985 62 610.
6. "A cyclic voltammetry experiment for the instrumental analysis laboratory" Baldwin, Richard P.; Ravichandran, K.; Johnson, Ronda K. J. Chem. Educ. 1984 61 820.
7. "Anodic stripping voltammetry: an instrumental analysis experiment" Wang, Joseph. J. Chem. Educ. 1983 60 1074.
8. "Cyclic voltammetry experiment" Van Benschoten, James J.; Lewis, Jane Y.; Heineman, William R.; Roston, Daryl A.; Kissinger, Peter T. J. Chem. Educ. 1983 60 772.
2. "The effect of complex formation upon the redox potentials of metallic ions: Cyclic voltammetry experiments" Ibanez, Jorge G.; Gonzalez, Ignacio; Cardenas, Marco A. J. Chem. Educ. 1988 65 173.
Back to Voltammetry Page
Return to Bioanalytical Homepage