Analytical Chemistry
A.Y. 2026/2027
Learning objectives
The course aims to provide students with the general foundations of Analytical Chemistry by providing both theoretical and applied knowledge to operate correctly in an analytical chemistry laboratory. The course aims to introduce students to the understanding of equilibria in solution and the main methods of analysis. The course also aims to provide students with critical skills in evaluating the accuracy and precision of experimental data using statistical methods, the ability to solve analytical problems related to complex equilibria in solution and quantitative analysis of compounds. The course also includes laboratory exercises conducted at individual workstations, aimed at acquiring the knowledge necessary for conducting chemical analyses correctly, including basic safety protocols for handling and disposing of chemicals. These exercises focus on learning the fundamentals of volumetric analysis (titration).
Expected learning outcomes
At the end of the course, the student will have acquired the knowledge of analytical chemistry necessary for the knowledge of the principles on which the most commonly used analytical techniques in the chemical, chemical-toxicological and food fields are based; the knowledge of the procedures for processing and evaluating experimental data; the knowledge of the main complex chemical equilibria in solution and the ability to autonomously solve simple analytical problems ranging from sampling, sample treatment, up to the type of analytical method chosen (among those studied) for the quantification of the analytes, taking into account the uncertainty of measurement; the ability to use the specific language proper to Analytical Chemistry this to describe and comment on an analytical method and to report the result correctly and unambiguously. Attendance at the laboratory will enable the student to be able to operate safely in chemical laboratories and to perform standard laboratory procedures for the recognition and quantification of simple analytical species.
Lesson period: Second semester
Assessment methods: Esame
Assessment result: voto verbalizzato in trentesimi
Single course
This course cannot be attended as a single course. Please check our list of single courses to find the ones available for enrolment.
Course syllabus and organization
Single session
Responsible
Lesson period
Second semester
Course syllabus
Sampling and analytical methods: sampling, sample representativeness, sampling strategies and techniques, sample preservation and treatment. Standardization and calibration of analytical methods.
Statistical treatment and evaluation of data: errors in chemical analysis (systematic, random, and gross errors), sources and treatment of error in the analytical process, characteristics of an analytical method (accuracy and precision), significant figures, and error propagation. Mean, variance, standard deviation, relative standard deviation (RSD), and standard deviation of the mean. Normal distribution and Student's t-distribution. Confidence intervals and their interpretation. Effect of degrees of freedom and confidence level on the value of Student's t. Pooling of multiple data sets (data pooling) for the estimation of pooled standard deviation. Statistical tests for data evaluation, including the Shapiro-Wilk normality test, Dixon's Q-test for outlier detection, Student's t-test for the identification of systematic errors, Student's t-test for the comparison of two experimental means, and the F-test for comparing the precision of two analytical methods or two sets of measurements.
Acid-base equilibria: pH calculations for strong and weak acids and bases. Amphiprotic species and pH calculations. Buffer solutions, the Henderson-Hasselbalch equation, approximations in pH calculations, and buffer capacity. Introduction to acid-base titrations and acid-base indicators.
Effect of electrolytes on chemical equilibria: ionic strength and its calculation. Activities and activity coefficients. Relationship between activity and concentration. Influence of ionic strength on activity coefficients and chemical equilibria. Equilibrium constants expressed in terms of concentrations and activities. Differences between thermodynamic equilibrium constants and concentration equilibrium constants. Effect of ionic strength on acid-base, precipitation, and complexation equilibria. Numerical exercises involving ionic strength calculations, activities, and equilibrium constants corrected for ionic strength.
Precipitation equilibria: solubility and solubility product constant. Common ion effect and the influence of competing equilibria. Precipitation reactions and fractional precipitation separations. Calculation of the solubility of salts whose anion is the conjugate base of a weak acid at a given pH. Introduction to precipitation titrations and precipitation indicators. Precipitation reactions in solutions at constant pH.
Complexation equilibria: formation and instability constants, stepwise and overall formation constants. Systematic treatment of complexation equilibria. Predominant species as a function of ligand concentration. Distribution functions and distribution diagrams of complex species, and the influence of formation constants on distribution diagrams. Calculation of the concentration of species in solution and of the solubility of sparingly soluble compounds in the presence of complexation equilibria. Stability of complexes and the effect of pH. Conditional formation constants. Analytical applications of complexes, including colored complexes, solubilization, masking, and demasking. Multidentate ligands: metal-EDTA complexes, conditional formation constants, and the main analytical applications of EDTA. Introduction to complexometric titrations and metallochromic indicators.
Redox equilibria: similarities and differences between acid-base, complexation, precipitation, and redox equilibria. Oxidation-reduction potentials, the Nernst equation, and factors affecting redox equilibria. Redox indicators, auxiliary oxidizing and reducing agents, Jones and Walden reducers. Introduction to redox titrations.
Tutorial sessions: problem-solving activities covering the topics discussed during the course, with particular emphasis on statistical data treatment, confidence interval calculations, application of statistical tests, ionic strength and activity calculations, acid-base, precipitation, complexation, and redox equilibria, as well as their corresponding titration methods.
Laboratory module: basic instructions for safe operation in the analytical chemistry laboratory and for carrying out the scheduled experiments. Use and calibration of volumetric glassware (burettes, pipettes, pipette fillers, and volumetric flasks). Acid-base titrations using indicators (HCl versus NaOH, determination of acetic acid content in vinegar). Complexometric titration for the determination of total water hardness using EDTA. Applications of EDTA in water treatment and remediation processes.
Statistical treatment and evaluation of data: errors in chemical analysis (systematic, random, and gross errors), sources and treatment of error in the analytical process, characteristics of an analytical method (accuracy and precision), significant figures, and error propagation. Mean, variance, standard deviation, relative standard deviation (RSD), and standard deviation of the mean. Normal distribution and Student's t-distribution. Confidence intervals and their interpretation. Effect of degrees of freedom and confidence level on the value of Student's t. Pooling of multiple data sets (data pooling) for the estimation of pooled standard deviation. Statistical tests for data evaluation, including the Shapiro-Wilk normality test, Dixon's Q-test for outlier detection, Student's t-test for the identification of systematic errors, Student's t-test for the comparison of two experimental means, and the F-test for comparing the precision of two analytical methods or two sets of measurements.
Acid-base equilibria: pH calculations for strong and weak acids and bases. Amphiprotic species and pH calculations. Buffer solutions, the Henderson-Hasselbalch equation, approximations in pH calculations, and buffer capacity. Introduction to acid-base titrations and acid-base indicators.
Effect of electrolytes on chemical equilibria: ionic strength and its calculation. Activities and activity coefficients. Relationship between activity and concentration. Influence of ionic strength on activity coefficients and chemical equilibria. Equilibrium constants expressed in terms of concentrations and activities. Differences between thermodynamic equilibrium constants and concentration equilibrium constants. Effect of ionic strength on acid-base, precipitation, and complexation equilibria. Numerical exercises involving ionic strength calculations, activities, and equilibrium constants corrected for ionic strength.
Precipitation equilibria: solubility and solubility product constant. Common ion effect and the influence of competing equilibria. Precipitation reactions and fractional precipitation separations. Calculation of the solubility of salts whose anion is the conjugate base of a weak acid at a given pH. Introduction to precipitation titrations and precipitation indicators. Precipitation reactions in solutions at constant pH.
Complexation equilibria: formation and instability constants, stepwise and overall formation constants. Systematic treatment of complexation equilibria. Predominant species as a function of ligand concentration. Distribution functions and distribution diagrams of complex species, and the influence of formation constants on distribution diagrams. Calculation of the concentration of species in solution and of the solubility of sparingly soluble compounds in the presence of complexation equilibria. Stability of complexes and the effect of pH. Conditional formation constants. Analytical applications of complexes, including colored complexes, solubilization, masking, and demasking. Multidentate ligands: metal-EDTA complexes, conditional formation constants, and the main analytical applications of EDTA. Introduction to complexometric titrations and metallochromic indicators.
Redox equilibria: similarities and differences between acid-base, complexation, precipitation, and redox equilibria. Oxidation-reduction potentials, the Nernst equation, and factors affecting redox equilibria. Redox indicators, auxiliary oxidizing and reducing agents, Jones and Walden reducers. Introduction to redox titrations.
Tutorial sessions: problem-solving activities covering the topics discussed during the course, with particular emphasis on statistical data treatment, confidence interval calculations, application of statistical tests, ionic strength and activity calculations, acid-base, precipitation, complexation, and redox equilibria, as well as their corresponding titration methods.
Laboratory module: basic instructions for safe operation in the analytical chemistry laboratory and for carrying out the scheduled experiments. Use and calibration of volumetric glassware (burettes, pipettes, pipette fillers, and volumetric flasks). Acid-base titrations using indicators (HCl versus NaOH, determination of acetic acid content in vinegar). Complexometric titration for the determination of total water hardness using EDTA. Applications of EDTA in water treatment and remediation processes.
Prerequisites for admission
Knowledge of basic mathematics, knowledge of general chemistry and stoichiometry
Teaching methods
The course consists of three teaching units: lectures, classroom exercises, and practical laboratory exercises
Teaching Resources
Analytical Chemistry and Quantitative Analysis (D. S. Hage and J. D. Carr) Publisher: Piccin;
Fundamentals of Analytical Chemistry (Skoog & West) Publisher: EdiSES;
Analytical Chemistry (V. Di Marco, P. Patore, G. G. Bombi) Publisher: EdiSES. Lecturer's handouts.
Fundamentals of Analytical Chemistry (Skoog & West) Publisher: EdiSES;
Analytical Chemistry (V. Di Marco, P. Patore, G. G. Bombi) Publisher: EdiSES. Lecturer's handouts.
Assessment methods and Criteria
The written exam, with a total duration of three hours, includes open-ended questions of varying length, as well as short exercises and problems covering the topics addressed during the course. Honors (cum laude) in the final grade will be awarded only to students who demonstrate both an excellent theoretical understanding and achieve full marks in the laboratory component.
Students are allowed to take the written exam only if they have previously submitted the Laboratory Reports. The Laboratory Reports will be included in the final evaluation.
Students are allowed to take the written exam only if they have previously submitted the Laboratory Reports. The Laboratory Reports will be included in the final evaluation.
CHEM-01/A - Analytical Chemistry - University credits: 6
Exercises: 16 hours
Tutorials: 16 hours
Lessons: 32 hours
Tutorials: 16 hours
Lessons: 32 hours
Professor:
Comite Valeria
Professor(s)