CHIMICA ANALITICA A - L

-Knowledge and understanding: knowledge of the main chemical and phenomenological aspects relating to the study of equilibria in solution, with particular reference to the calculation of pH, solubility and oxidation-reduction and complexation equilibria.

-Ability to apply knowledge and understanding: being able to develop simple and rigorous calculation approaches for the study of equilibria in solution. Development of useful knowledge and its application for carrying out quantitative determinations.

- Making judgments: developing the ability to critically evaluate the characteristics of the solutions related to their composition.

-Communication skills: develop and/or improve the ability to explain even complex scientific concepts.

-Learning skills: Apply techniques and theoretical models for the study of chemical equilibria.

Lessons and  exercises.

If the course would be at distance, or in presence and at distance at the same time, the necessary and appropriate changes to the statement originally declared will be introduced to comply to the program reported in the syllabus.

Introduction. Definition of Analytical chemistry. Qualitative and quantitative methods. Analyses and determinations. Overall analytical procedure. Application of specific analytical methodologies to the solution of practical problems.Measurements and errors. Accuracy and precision. Classification of errors in Analytical Chemistry: gross, systematic and random errors. Report of the results and propagation error law. Most utilized Statistical Tests in Analytical Chemistry.

Solution equilibria. Definition of chemical equilibrium. Equilibrium constants. Activity and Activity Coefficient. Thermodynamic and Stoichiometric Constants. Ionic Strength. Debye and Hückel theory. Calculation of activity coefficients as a function of the Ionic Strength.

Acid-Base Equilibria. Definition of Acid and Base according to Arrhenius, Brönsted and Lewis. Conjugate acid-base pairs. Strength of Acids and Bases. The concept of pH. Error on the measurement of pH. The Concept of Neutral Solution. Calculation of pH. Electroneutrality of the solutions. Mass Balance, charge balance. Strong Acids and Bases solutions. Monobasic acids. Degree of Dissociation. Weak acid and weak base solutions. Buffer Solutions: buffer power. Polyprotic acids. Poliacidic Bases. Diprotic and polyprotic Acid solutions. Calculation of the species concentrations in polyprotic acid solutions as afunction of pH. Poliacidic bases solutions. Ampholytes Solutions. Acid-base mixtures.

Solubility Equilibria. Quantitative relationship between solubility and solubility product. Common ion effect. Role of Acid-Base reactions on solubility equilibria.

Redox equilibria. Standard potential. Nernst equation. Formal potential. Equilibrium constants as a function of standard potential. Redox indicators.

Complexation equilibria. Definition of a Complex. Monodentate and polydentate ligands. Chelating agents. Effects of Acid-Base reactions on complexation equilibria. Auxiliary ligands. Conditional constants. Minimum Operating pH. Metallochromic indicators.

Theoretical methods of solvent extraction, influence of pH and formation constants, selective extraction. Principles of countercurrent extraction. Theoretical distribution in an extraction process with two solutes.

1. H. Freiser e Q. Fernando Gli Equilibri ionici nella Chimica Analitica.

2. D. C. Harris Chimica analitica quantitativa Zanichelli

3. Skoog - West – Holler Fondamenti di Chimica Analitica- EDISES Editore

4. Kolthoff - Sandell - Meehan - Bruckenstein: Anbalisi Chimica Quantitativa - Piccin Editore, Padova.

Verification of learning will take place through a written test. Problem solving will allow the student to demonstrate his ability to integrate different notions. The entire reasoning will be evaluated, the student will therefore be asked to clearly demonstrate how he performed the exercise. In specific cases the commission reserves the right to carry out a subsequent oral test.