ANALYTICAL CHEMISTRY WITH LABORATORY

Gibbs free energy, chemical potential, activity. Equilibrium constants. Ionic strength. Debye-Huckel theory, activity coefficients. Factors affecting the equilibrium constant. Temperature dependence. K_T and Kst.

Acid-base theories. The ionic product of water. pH. Strength of acids and bases. Strong acids and bases: pH calculation. Solving solution equilibria problems. Mass and charge balance equations, proton condition. Weak acids and bases: degree of dissociation, pH calculation. Buffer solutions: pH calculation and buffer capacity. Polyprotic acids. Distribution diagrams. Amphoteric species. Acid-base titrations.

Solubility equilibria. Solubility product. Dependence on temperature and ionic strength. Effect of the common-ion, pH and complex formation on the solubility.

Complex formation equilibria. Species distribution and competition with the proton. EDTA, conditional formation constants, minimum pH for effective titrations. Complexometric titrations.

Laboratory. Calibration of volumetric glassware. Analytical balance. Volumetric analysis. Acid-base titrations. Standard solutions, acid-base indicators. Potentiometric titrations. Galvanic cells, reference and work electrodes, glass electrode, calibration of a glass electrode, determination of the end-point of a titration. Complexometric titrations. Metallochromic indicators. EDTA titrations and determination of copper(II). Spectrophotometric determination of iron(II).

1. H. Freiser, Q. Fernando, “Gli Equilibri Ionici nella Chimica Analitica", Piccin Editore, Padova

2. Daniel C. Harris, “Chimica Analitica Quantitativa”, Zanichelli Editore, Bologna

3. I. M. Kolthoff, E. B. Sandell, E. J. Meehan, S. Bruckenstein, “Analisi Chimica Quantitativa”, Piccin Editore, Padova