ANALYTICAL CHEMISTRY I WITH LABORATORY

Course objectives

Lectures have the aim of providing students with the elemental conceptual means by which they can comprehend the meaning of the most common practice in qualitative chemical analysis performed by classical methods. Such conceptual means allow to foresee and evaluate the results by application of the principia governing chemical equilibria in solution. Laboratory experiences aim at providing the knowledge of the most elementary laboratory operations and developing the capacity to apply the theoretical concepts to the experimental activity. Dublin Descriptor 1 (knowledge and understanding): at the end of the course the student is provided with the basic knowledge, both theoretical and of laboratory practice, to comprehend the meaning of the most common operations in the qualitative chemical analysis by classical methods, i.e. by exploiting in solution and heterogeneous equilibria. Dublin Descriptor 2 (applying knowledge and understanding): at the end of the course the student is enabled to understand and practically deal with phenomena related to the most important chemical equilibria (acid-base, complexation and precipitation equilibria), as well as to apply the knowledge about solubilisation and precipitation to the qualitative determination of chemical species and their transformations. Dublin Descriptor 3(making judgements): at the end of the course the student has developed the capacity of critically evaluating the adequacy of data obtained from a numerical exercise or from the result of a laboratory experiment. Such capacity is developed by educational exercises explained during lectures and laboratory experiences. Dublin Descriptor 4 (communication skills): at the end of the course the student has developed the capacity of communicating, by written or oral reports, the knowledge acquired and the experimental data from laboratory experiences, by using the appropriate language, a logical exposure sequence and synthesis capacity. Dublin Descriptor 5 (learning skills): at the end of the course the student is stimulated to further delve into the investigated topics, also creating links among different subjects.

Channel 1
ANNA LAURA CAPRIOTTI Lecturers' profile
Channel 2
CHIARA CAVALIERE Lecturers' profile

Program - Frequency - Exams

Course program
Analytical Problems and Their Solutions - Protocol Basic concepts regarding the role of analytical chemistry and its applications. Analytical work protocol: method selection, sampling, pre-measurement analytical methodology (sample attack and separation). Analytical work protocol. Classic and instrumental tests. Treatment of obtained data. Solution equilibria, kinetic aspects, and thermodynamics (3 h) Redox Reactions and Acidity Homogeneous phase equilibria (acid-base, redox). Nernst equation. Factors influencing the kinetics of a chemical reaction. Redox reactions and acidity. Selective recognition of halides with permanganate. Case study of the nitrite/nitric oxide pair. Disproportionation and pH (case study of halogens and hydrogen peroxide). (4 h) Complexes, Acidity, and Redox Reactions A brief overview of complexes. Factors influencing the stability of a complex (dilution, medium, ionic strength). pH effect on complexes derived from weak acids. Changes in redox properties due to complex formation. Influence of instability constant on potential. The potential of a pair of ions, both complexing. Case study of manganese (III). (3 h) Precipitation, Solubility, and Acidity Equilibria Heterogeneous phase equilibria. Concept of solubility product, relationship between Ksp and solubility. Factors influencing the solubility of a slightly soluble compound (ionic strength, activity, medium, dilution, pH, common ion effect). Solubility of a slightly soluble compound from a weak monoprotic acid. Chemistry of sulfates, carbonates, oxalates. Chemistry of sulfides, calculation of the precipitation pH of a sulfide. Dissolution of a sulfide. Dissolution of sulfides via formation of salts and thio-salts, dissolution via acid-base and redox mechanisms. Solubility of a generic sulfide at any pH value. Hydroxide chemistry, the case of aluminum hydroxide (amphoteric) and zinc hydroxide. Amphoterism of hydroxides. Causes of amphoterism. Solubility of amphoteric hydroxides as a function of pH. Precipitate formation. Formation of colloidal precipitates, adsorption rules, aging of precipitates, post-precipitation. (10 h) Solubility and Complexes Precipitation of an insoluble compound from a complex. Reactions of thio-compounds. Dissolution of a precipitate via complex formation. (2 h) Precipitation and Redox Reactions Oxidations and precipitations. The case of the Fe2+/Fe3+ pair. Variation of redox properties due to salt precipitation. Stabilization of an oxidation state via precipitation (mercury chemistry). Complexes and precipitation. Disproportionation induced by the formation of a precipitate. (2 h) Classification of Separation Methods Liquid-liquid extraction. Phase distribution and Nernst's law: concept of distribution constant, distribution ratio. Theoretical principles of extraction. Efficiency and selectivity of an extraction. Factors involved in extraction equilibria. Extractability of weak acids and bases. Separation techniques and related physicochemical principles. Extractability of a cation, pH dependence. Logarithmic curves. (4 h) Laboratory Activities Safety in the laboratory. Explanation of experiments and discussion of observed phenomena (2 h) Laboratory Exercises 5 CFU
Prerequisites
It is important to have acquired basic knowledge of chemical language and basic knowledge of acid-base reactions, the concept of pH, the concept and calculation of oxidation numbers, redox reactions, and balancing redox reactions from previous courses. It is also useful to know the distinction between electrolytes and non-electrolytes, between strong and weak electrolytes, and to have basic notions regarding the description of a chemical equilibrium, through the respective equilibrium constant and Le Chatelier's principle.
Frequency
Attendance at lectures is not mandatory for taking the exam but is strongly recommended. Attendance at laboratory exercises is mandatory
Exam mode
At the end of the course, students will undergo an oral exam, which must be booked through the INFOSTUD website: https://stud.infostud.uniroma1.it/Sest/Log/. The exam session dates are determined at the beginning of each academic year. Exams begin after the teaching activities of individual courses have concluded. To pass the exam, students must achieve a grade not lower than 18/30. The final grade is unique and guarantees the acquisition of 9 CFU. The assessment method involves evaluating the student's ability to solve chemical problems, such as the separation of multiple inorganic analytes in a complex mixture, using the knowledge provided by the instructor. The evaluation takes into account laboratory attendance and, most importantly, the student's reasoning ability in addressing an analytical chemistry problem (logic followed by the student in solving the problem; correctness of the procedure identified for solving the problem; adequacy of the proposed solution with the skills that the student is expected to have acquired by the end of the course; appropriate use of language. In evaluating the exam, the final grade considers the following elements: 1. Reasoning ability; 2. Clarity and completeness in the oral presentation of the program content; 3. Ability in writing and balancing chemical reactions and in solving analytical problems; 4. Ability to critically evaluate the results of experimental procedures; 5. Ability to make connections. To achieve a score of 30/30 cum laude, the student must demonstrate excellent knowledge of all topics covered during the course, but most importantly, must be able to integrate them logically and coherently.
Lesson mode
The course is conducted through traditional teaching methods. Frontal teaching not only aims to provide basic knowledge in the field of analytical chemistry but also includes the ability to apply the provided knowledge to the study of both theoretical and practical reactions. These latter objectives are achieved through the completion of exercises, the explanation of educational case studies, and laboratory activities. Laboratory exercises also aim to visualize and apply the concepts learned.
Channel 3
STEFANO MATERAZZI Lecturers' profile

Program - Frequency - Exams

Course program
Analytical problems and their solutions Description of the role of analytical chemistry and its applications in science. Description of the steps in a general analytical workflow: method choice, sampling, sample preparation and other operations before analysis (sample solubilisation, analyte separation), sample analysis by classical and instrumental assays, data analysis. Thermodynamic and kinetic considerations on in solution chemical equilibria. (2h). Redox reactions and acidity Outlines on homogeneous equilibria (acid-base, redox equilibria). Nernst equation. Factors affecting the kinetics of a chemical reaction. Effect of pH on redox reactions. Selective recognition of halides (chlorides, bromides and iodides) by permanganate. The redox couple nitrite/nitric oxide. Disproportionation and pH (study case of halogens and hydrogen peroxide). (4h) Complexes, acidity and redox reactions Definition of complexes. Factors affecting the stability of a complex (dilution, solvent medium, ionic strength). Effect of pH on complexes constituted by ligands which are conjugate bases of weak acids. Variations of the redox potential due to complex formation. Influence of the instability constant on the redox potential. Effect of complexation on the potential of a redox couple. Stabilization of an unstable redox state by complexation (case study, Mn (III)) (3h). Precipitation equilibria, solubility and pH Heterogeneous equilibria. Definition of solubility product, relation between Kps and solubility. Factors which affect the solubility of slightly soluble compounds (ionic strength, activity, solvent medium, dilution, pH, common ion effect). Solubility of a slightly soluble compound deriving from weak monoprotic acid. Chemistry of sulfates, carbonates, oxalate. Calculation of the precipitation pH of a sulfate. Sulfates dissolution. Sulfates dissolution by formation of salts and thiosalts, acid-base and redox reactions. Sulfate solubility and pH. Hydroxide chemistry and the case study of aluminium hydroxide (amphoteric oxide) and of zinc hydroxide. Hydroxide amphoterism and related causes. Solubility of amphoteric hydroxides as a function of pH. Precipitate formation. Colloidal precipitates. Adsorption, aging of precipitates, postprecipitation (10 h). Solubility and complexation Precipitation of an insoluble compound from a complex. Reactions of thiocompounds. Dissolution of a precipitate by complexation (1h). Precipitation and redox reactions Oxidation and precipitation. The case study of Fe2+/Fe3+. Variation of the redox properties by salt precipitation. Stabilization of an oxidation state by precipitation (case study of mercury chemistry). Complexes and redox reactions. Disproportionation induced by precipitation (2h). Classification of separation methods Liquid-liquid extraction. Phase distribution and Nernst equation. Definition of distribution constant and distribution ratio. Theoretical principles on extraction. Extraction efficiency and selectivity. Factors which affect extraction equilibria. Extractability of acids and bases. Separation techniques and related physico-chemical principles. Extractability of cations, pH dependence. Logarithmic curves (2h). Laboratory activity (with description of the practical activities) The laboratory actives are usually held in groups of 50 students and are organized according to the following experiences: 1-assignment of the position and the required labware and glassware. Description of how to employ a centrifuge (time required ~ 1.5 h) 2-Experience 1: solubility in strong acids (nitric acid, hydrochloric acid, sulphuric acid). (time required ~ 3 h) 3-Experience 2: solubility in bases (sodium hydroxide and ammonia) (time required ~ 3 h) 4-Experience 3: oxidation and pH (selective oxidation of halides by permanganate) (time required ~ 4 h) 5-Experience 4: solubility equilibria as a function of pH and complexation. Reactivity test and recognition of Al3+, Fe2+, Fe3+ e Cr3+ (time required ~ 3 h) 6-Experience 5: solubility equilibria as a function of pH and complexation (time required ~ 3 h) 6- Experience 6: separation of Ag+, Zn2+ and Mn+2 by precipitation at controlled pH (time required ~ 4 h) 7-Experience 7: separation of Cu2+, Hg2+, As3+, Ni2+ and Co+2 by precipitation at controlled pH (time required ~ 4 h) 8-Unknown ion assay (time required ~ 4 h) 9- Unknown ion assay 2 (time required ~ 4 h) 10-Restitution of labware and glassware (time required ~ 1 h)
Prerequisites
From the previous courses the student should already have acquired basic knowledge of the chemical language and the basic knowledge about acid-base equilibria, pH, oxidation number definition and calculation, redox reactions and their balancing. For the aim of the course, it is also useful to have previous knowledge about the distinction between electrolytes and non-electrolytes, strong and weak electrolytes, and basic knowledge on the description of chemical equilibria by means of equilibria constants and Le Chatelier principle.
Books
-Araneo A. “Chimica Analitica Qualitativa: Nuovo Metodo Periodale”, Casa Editrice Ambrosiana Milano -Douglas A.Skoog, Donald M. West, F. James Holler. “Fondamenti di Chimica Analitica”, EdiSES S.r.l. Napoli
Teaching mode
The course is held by a traditional didactic teaching method, which does not only provide the basic knowledge of analytical chemistry, but it also provides the means by which the theoretical knowledge can be applied to the study of reactions, at both a practical and theoretical level. These latest aims are reached by explanation of selected exercises, study cases and by the laboratory experiences, which include the writing of a report.
Frequency
Lesson attendance is not mandatory for the exam, but laboratory experiences are
Exam mode
In order to take the exam, the student must book a proper date on the INFOSTUD site: https://stud.infostud.uniroma1.it/Sest/Log/ The period in which exams take place is decided at the beginning of every academic year. Exam sessions begin at the end of the teaching activity of each course. The exam is made up two parts, i.e. a practical experiment at the end of the didactic laboratory and an oral exam. To pass the exam, the final mark must not be less than 18/30. Passing the exam provides 9 CFU. During the exam, the capacity of the student to solve problems of analytical chemistry will be evaluated, such as the separation of different inorganic analytes in a complex mixture, so to selectively isolate them by applying the knowledge provided in the course. The attendance to the didactic laboratory is considered for evaluation, and more importantly the reasoning capacity in the solution of an analytical problem (logic of the proposed solution, correctness of the solution compared to the knowledge the student is supposed to possess at the end of the course, language correctness). More specifically, in the choice of the final mark the following features are considered: 1. reasoning capacity; 2. clarity and completeness in the oral presentation of the contents of the course; 3. mastery in the writing and balancing of chemical equations and in the solving of analytical chemistry problems; 4. critical evaluation capacity of exercise results and of the experimental procedures; 5. capacity of linking contents from different topics.
Lesson mode
The course is held by a traditional didactic teaching method, which does not only provide the basic knowledge of analytical chemistry, but it also provides the means by which the theoretical knowledge can be applied to the study of reactions, at both a practical and theoretical level. These latest aims are reached by explanation of selected exercises, study cases and by the laboratory experiences, which include the writing of a report.
Channel 4
SUSY PIOVESANA Lecturers' profile
ALDO LAGANA' Lecturers' profile
  • Lesson code1020315
  • Academic year2024/2025
  • CourseChemical Sciences
  • CurriculumSingle curriculum
  • Year1st year
  • Semester2nd semester
  • SSDCHIM/01
  • CFU9
  • Subject areaDiscipline Chimiche