Quantitative analytical chemistry (full program)
Prof. dr hab. Jacek Gliński
Laboratory: 60 hours
Tutorials: 30 hours
Self-study: 30 hours
ECTS points: 10
Level of course: fundamental.
Objective of the course:
Knowledge of foundations of analytical chemistry, application of simple calculations on
chemical equilibria in laboratory practice, practical knowledge of fundamental analytical
reactions and techniques of classical quantitative analysis.
Course contents:
Laboratory: 7 simple classical analyses and 4 instrumental analyses. Except NaOH, all other
titrants will be prepared by the laboratory staff or by weighing. Titrants: 0.1 M NaOH, 0.1 M
Na2S2O3 and 0.02 M KMnO4 prepared using commercial concentrated volumetric solution
(Fixanal® or similar).
Classical analyses: (Alkacymetry 1) Determination of the mass of ascorbinic acid (vitamin C)
or acetylosalicylic acid in tablets; (Alkacymetry 2) Analysis of H3PO4 (classical with two
titration end-points); (Alkacymetry 3) pH-metric titration of H3PO4 pure sample or in CocaCola/Pepsi, or citric acid in citron juice; (Gravimetry) Analysis of Ni gravimetrically (with
dimethylglyoxime); Redoxometry) Analysis of Cu iodometrically; Analysis of Fe
manganometrically; (Precipitation analysis) Analysis of Cl argentometrically (by Mohr
method); (Complexometry) Analysis of Ca+Mg complexonometrically (preferably in a
carbonate rock).
Instrumental analyses: Turbidimetry (analysis of sulphates or chlorides); Colorimetry
(analysis of phosphates or iron); Extraction (analysis of fat content in food); Densimetry
(determination of alcohol content in beverages); plus one or two analyses chosen from the
following: electrogravimetry, conductometric titration of sulphates, spectrophotometry of
natural dyes (this list can be expanded).
Theory: Reactions of proton transfer, acid/base equilibrium, calculating pH of solutions:
acids, bases, buffers, ampholites. Titration curve, indicators. Reactions with electron transfer:
redox reactions, redox equilibrium. Reactions of transfer of ions and molecules, coordination
compounds, complex formation equilibrium. Heterogenic equilibria, processes influencing
these equilibria: the “common ion” effect and salt effect. The basis of selected instrumental
methods of analysis.
Assessment methods:
Partial tests concerning laboratory works, positive results of the analyses, final exam (oral).
Literature:
Douglas A. Skoog, Donald M. West, F. James Holler, Stanley R. Crouch, Fundamentals of
Analytical Chemistry, Thomson Brooks/cole (2000).