Analytical Chemistry I and Laboratory A - L

Module Module 2

The course aims to provide students with fundamental tools for quantitative analysis based on ionic equilibria in solution through the employment of the most significant gravimetric and volumetric methods in analytical chemistry. The purpose of the course is to give a global vision of the analytical process from the selection of the method of analysis to data processing and critical discussion of the results.

Knowledge and understanding:

Understanding the basic concepts of the classical methods of volumetric and gravimetric analysis as well as of their applications. Knowledge of the basis of statistics for the treatment of experimental data.

Applying knowledge and understanding:

Development of tools for understanding the methods and procedures for quantitative chemical analysis as well as acquisition of the practical skills for volumetric and gravimetric methods through experiments in the laboratory. Development of a critical thinking for the presentation of the analytical data obtained.

Making judgements:

Ability to independently solve an analytical problem using volumetric/gravimetric methods as well as ability to interpret experimental data on the basis of the acquired knowledge and laboratory experiments.

Communication skills:

Acquiring proper language skills and ability to rigorously expose the topics covered in the course.

Learning skills:

Capability to develop tools and skills to successfully undertake further study paths with a high level of autonomy.

Class lectures, exercises, presentation of the lab experiments, treatment of the analytical data. Experiments in laboratory on volumetric and gravimetric analysis.

Should teaching be carried out in mixed mode or remotely, it may be necessary to introduce changes with respect to previous statements, in line with the programme planned and outlined in the syllabus.

Knowledge of fundamental concepts of Mathematics, Physics, and General and Inorganic Chemistry.

Mandatory attendance

Introduction. Elements of statistics. Errors in analytical chemistry. Presentation of data and results. Position and dispersion index. Most common statistical tests.

Analytical measurement instrumentations. Precision, accuracy, sensitivity. Laboratory apparatuses: analytical balance and calibrated glassware.

Volumetric analysis. General principles on titrations. Preparation of standard solutions. Primary standards. Standardization procedures. Acid-base titrations. Acid-base indicators. Acidimetric and alkalimetric determination of sodium tetraborate.

Precipitation titrations. Determination of chloride by Mohr and Fajans methods. Carbonate/chloride separation.

Gravimetric analysis. Analysis by precipitation. Formation, nature and size of precipitates. Gravimetric determination of Ni²⁺ as the bis-dimethylglioximate complex.

Complexometric titrations. EDTA titrations. Metallochromic indicators. Determination of Cu²⁺.

Redox titrations. Methods based on the use of permanganate. Determination of Fe²⁺. Iodometry. Determination of Cu²⁺.

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

2. D. C. Harris, "Chimica Analitica quantitativa", terza ed., Zanichelli, Bologna.

3. F. J. Holler, S. R. Crouch, “Fondamenti di Chimica Analitica”, terza ed., Edises, Napoli.

4. M. Garetto, "Statistica, lezioni ed esercizi", Università di Torino.

5. E. De Simoni, "Chimica Analitica", CUL, Bologna.

Written and oral exams with evaluation of the laboratory reports. 

Written exam will be focused on similar exercises already presented and carried out during the lessons and the classroom exercises. One of these exercises included in the exams will be related to laboratory experiences.

Oral exam will consist of a discussion aimed at verify the level of knowledge of each student on analytical methods dealt with the lessons.

The students have to write the laboratory report in time for each laboratory experience.

The results will consider the reports, written and oral exams.

Examples:

• Calculation of the equilibrium constant and reduction pontential at the equivalent point of the redox titration.
• Describing the standardization protocol for EDTA solution.
• Experimental issues related to use of the permanganate solution.
• Acid-base indicators in the volumetric titration.
• Calculation of relative, absolute errors and the exact concentration of a solution.