Unit ANALYTICAL CHEMISTRY
- Course
- Chemistry and technology of drugs
- Study-unit Code
- GP003076
- Location
- PERUGIA
- Curriculum
- In all curricula
- Teacher
- Riccardo Vivani
- Teachers
-
- Riccardo Vivani
- Hours
- 48 ore - Riccardo Vivani
- CFU
- 6
- Course Regulation
- Coorte 2020
- Offered
- 2020/21
- Learning activities
- Affine/integrativa
- Area
- Attività formative affini o integrative
- Academic discipline
- CHIM/01
- Type of study-unit
- Obbligatorio (Required)
- Type of learning activities
- Attività formativa monodisciplinare
- Language of instruction
- Italian
- Contents
- Principia of Analytical Chemistry. Equilibria of precipitation, electron transfer, proton transfer, complexation, in the light of chemical analysis. Separation processes.
Introduction to the statistic treatment of data - Reference texts
- D.C. Harris, Chimica Analitica Quantitativa, Zanichelli, Bologna 2005.
Additional material downloadable from the web site unistudium.unipg.it - Educational objectives
- The course aims to introduce students to the understanding of the principles upon which the chemical analysis in solution and its use in the quantitative analysis of volumetric and gravimetric, in order to provide useful tools for the laboratory courses of the following years.
The main knowledge gained will be:
- Mechanisms of formation of precipitates
- Properties of colloidal state
- Treatment of acid-base equilibria
- Operation of the electrodes for potentiometric measurements
- Ripartition and distribution equilibria between immiscible phases
The main skills (ability to apply knowledge acquired):
- Use of precipitation reactions in chemical analysis
- Use of acid-base reactions in chemical analysis
- Use of complexation reactions in chemical analysis
- Use of redox reactions in chemical analysis
- Introduction to the ripartition and distribution equilibria for the separation and qualitative and quantitative analysis using chromatographic methods - Prerequisites
- In order to understand and achieve the intended learning is important that the student has mastered the topics covered in the teaching of General and Inorganic Chemistry, then has already passed this examination.
In particular the knowledge of the following topics is essential:
- Electronic structure of atoms and chemical bonding
- Polarity of the molecules and intermolecular interactions
- Principles of thermodynamics
- Chemical equilibrium with particular reference to the balance in aqueous solution (solubility equilibria and acid-base equilibria)
Furthermore the knowledge of the following topics is important:
- Coordination compounds
- Basic concepts of chemical kinetics
- Basic concepts of electrochemical and galvanic cells - Teaching methods
- The course is organized as follows:
- Lectures on all the topics of the course. The lessons will be conducted with the help of the blackboard and through slide shows.
- Numerical exercises in the classroom for the solution of numerical exercises guided with the aid of the blackboard.
The teaching material (slides, exercises during numerical exercises, texts of previous written tests, other material) are made available to students on the e-studium platform after registration. - Other information
- At the exam the students are advised to bring student card and proof of identity.
- Essentials allowed for the written exam: periodic table, traditional calculator (scientific), pen.
- Not Allowed: mini computers or PDAs, cell phones, notebooks, books, notes or other information.
- The test must be written in non-erasable pen.
- The student who had not passed a test, can access any of the subsequent tests. - Learning verification modality
- The exam can be taken in two ways: two partial written tests, Partial I, single date, half term, and Partial II, on the dates of the official exam session calendar.
The Partial II is dedicated to students who have already achieved the sufficiency at Partial I.
The final grade will be the average of the two partial partial tests. If a test is not passed, it can be repeated in any of the calendar dates, and in any case only by September 2021. Beyond this date, the exam must be taken in Total mode.
- The Total examination is intended for those who have not obtained the sufficiency in Partial I, or however, those who prefer to take the exam in this way.
The written exam of the Total exam will be held on the official exam dates.
The duration of the partial written tests is about two hours while for the Total one it is about three hours.
They consist of 10-15 open-ended questions, both theoretical and numerical, in which case it must contain the procedure followed to obtain the result. The theoretical questions require a clear answer concise and comprehensive, according to the knowledge transmitted during lectures.
The exams are designed to ascertain the knowledge, understanding, language acquisition own discipline and the ability to display and summary about the theoretical aspects, and ensure the ability to apply the acquired skills to solve numerical problems related to practical cases. - Extended program
- Introduction on Analytical Methods. Classical and itstrumental methods. Sensitivity of analytical methods. Standard solutions. Ionic solids and precipitation reactions. Gravimetric analysis. Precipitate formation mechanism. Saturation degree and crystal growth. The colloidal state. Factors affecting the purity of precipitates. Controlled precipitation and homogeneous precipitation. Precipitation titrations. End-point determination: some methods for chloride analysis.
Protonic transfer reactions in aqueous solution. Outline on the accurate treatment of acid-base equilibria: charge and mass balance. Protonic condition. Graphic representation of acid-base equilibria. Distribution curves and logarithmic diagrams of concentration. Acid-base titration curves. Acid-base indicators. Errors in titrations.
Electron transfer reactions. Standard electrode potential and pH. Redox reactivity of water. Graphic representation of redox equilibria. Pourbaix diagrams of some redox systems. Potentiometric methods. Reference electrodes: calomel and Ag/AgCl electrodes. Indicator electrodes: membrane potential and ion-selective electrodes, some examples. Glass electrode for pH measurements. Electrode calibration. Redox titrations and common redox reagents. Redox indicators. Problems on the calibration of an instrumental method. Complexation reactions. Coordination compounds. Nomenclature. Metal-ligand bond description according to the valence bond model. Monodentate or polydentate ligands. Formation constants. Consecutive and cumulative constants. Chelating effect. EDTA. Effect of pH on the complexation reactions with EDTA. Conditional constant. Complexometric titrations. Metallochromic indicators.
Introduction on separation processes. Ripartition and distribution. Solvent extaction. Effects of pH. Extraction of metals with chelating agents. Generality on chromatography and chromatographic techniques. Treatment of the analytical data. An outline on errors in analytical chemistry.
Introduction to the statistical treatment of experimental data: Significant figures, rounding, propagation of inaccuracies. Systematic and random errors, precision, accuracy, sensitivity, S / N ratio, LOD, LOQ. Gaussian distribution of random errors, characteristics of the Gaussian curve, mean, variance, standard deviation,% RDS, normal Gaussian curve. Statistical tests with the normal Gaussian curve for a large population and Student's t test for a small population. Notes on the use of the t test for the comparison of means and the F test for the comparison of variances. Dixon Q test for suspicious data. Notes on calibration problems, two-point and multi-point calibration (least squares).