Analytical Chemistry
A.Y. 2019/2020
Learning objectives
The primary objective of this course is to introduce the basic concepts, principles and techniques of analytical chemistry
that will be better examined and experimentally applied in the following courses with teaching chemistry lab.
Students will be especially provided with principles and techniques of classical qualitative and quantitative inorganic analysis and with basic concepts instrumental analysis. The aim is to provide students with an analytical mind shape and with skills to solve different analytical problems such as identification and quantification of several components in medications.
that will be better examined and experimentally applied in the following courses with teaching chemistry lab.
Students will be especially provided with principles and techniques of classical qualitative and quantitative inorganic analysis and with basic concepts instrumental analysis. The aim is to provide students with an analytical mind shape and with skills to solve different analytical problems such as identification and quantification of several components in medications.
Expected learning outcomes
On successful completion of this course, students will be able to:
1)set the chemical reactions and mathematical equations in order to solve analytical problems,
2)understand and discern different analytical methods, both classical and instrumental methods, to be employed in the following teaching laboratory courses,
3)understand the importance of analytical chemistry in medications and to practice as pharmacists.
1)set the chemical reactions and mathematical equations in order to solve analytical problems,
2)understand and discern different analytical methods, both classical and instrumental methods, to be employed in the following teaching laboratory courses,
3)understand the importance of analytical chemistry in medications and to practice as pharmacists.
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
Linea AL
Responsible
Lesson period
Second semester
Course syllabus
Introduction - Significant figures and rounding. Ionic strenght. Activity and activity coefficients. Debye-Hückel equation.
Ionic equilibria - Acid-base equilibria (Strong and weak acids and bases. Polyprotic acids. Buffer solutions. Distribution diagrams). Solubility equilibria (Solubilities vs. solubility products. Common ion effect. Ionic strenght vs. solubility. Simultaneous equilibria in precipitation. Simple and complex precipitation). Simultaneous solubility-acidity equilibria (Solubility relation on pH). Complexation equilibria (Review on ligands and chelating agents. Formation and dissociation constants. Ion masking). Simultaneous solubility-complexation and acidity-complexation equilibria (Conditional-formation constants. Replacing reactions). Redox equilibria (Oxidizing and reducing agents. Galvanic cells. Standard redox potentials. Nernst equation. Formal redox potentials).
General methods in quantitative chemical analysis - Gravimetric analysis (Basic principles. Crystalline and colloidal precipitates). Volumetric analysis (Basic principles. Acid-base titrations. Precipitation titrations with Ag+. EDTA titrations. Redox titrations. Calculated values in a titration curve. Equivalence and final titration points. Chemical indicators).
Instrumental quantitative chemical analysis - Electrochemical methods (Potentiometry. Direct potentiometric measurements. Reference electrodes. Indicators electrodes. Glass electrode. Ion-selective electrodes. Calibration line. Added solutions method. Potentiometric titrations.). Spectroscopic methods (Properties of light, absorption and emission of radiation. Transmittance and adsorbance. Lambert-Beer's law. Atomic spectroscopy).
Ionic equilibria - Acid-base equilibria (Strong and weak acids and bases. Polyprotic acids. Buffer solutions. Distribution diagrams). Solubility equilibria (Solubilities vs. solubility products. Common ion effect. Ionic strenght vs. solubility. Simultaneous equilibria in precipitation. Simple and complex precipitation). Simultaneous solubility-acidity equilibria (Solubility relation on pH). Complexation equilibria (Review on ligands and chelating agents. Formation and dissociation constants. Ion masking). Simultaneous solubility-complexation and acidity-complexation equilibria (Conditional-formation constants. Replacing reactions). Redox equilibria (Oxidizing and reducing agents. Galvanic cells. Standard redox potentials. Nernst equation. Formal redox potentials).
General methods in quantitative chemical analysis - Gravimetric analysis (Basic principles. Crystalline and colloidal precipitates). Volumetric analysis (Basic principles. Acid-base titrations. Precipitation titrations with Ag+. EDTA titrations. Redox titrations. Calculated values in a titration curve. Equivalence and final titration points. Chemical indicators).
Instrumental quantitative chemical analysis - Electrochemical methods (Potentiometry. Direct potentiometric measurements. Reference electrodes. Indicators electrodes. Glass electrode. Ion-selective electrodes. Calibration line. Added solutions method. Potentiometric titrations.). Spectroscopic methods (Properties of light, absorption and emission of radiation. Transmittance and adsorbance. Lambert-Beer's law. Atomic spectroscopy).
Prerequisites for admission
Basic knowledge of physics and mathematics. In-depth knowledge of all the topics covered in the course of General and Inorganic Chemistry..
Teaching methods
The course is conposed of classroom lectures and exercises. The topics are illustrated with slides and by carrying out exercises on the blackboard. During the course of the exercises, the method of discussion and the tutorial approach, with targeted questions, will also be used in order to stimulate students and to make the learning of the exposed concepts more interactive and personalized.
Teaching Resources
Recommended textbooks:
- D.C. Harris, Quantitative Chemical Analysis, 9th Edition, 2016, W.H. Freeman and Co.
- D.A. Skoog, D.M. West, F.J. Holler, S.R. Crouch, Foundamentals of Analytical Chemistry, 9th Edition, 2014, Brooks/Cole.
- exercise book:
Silvia Araneo, Esercizi per la Chimica Analitica con richiami di teoria. Soc. Ed. Esculapio, 2° edizione 2018.
Reference books:
- General and Inorganic Chemistry and Stoichiometry course textbooks.
- A. Araneo, Chimica Analitica Qualitativa. Ed.C.E.A. (3° ed.)
- Pastore, Di Marco, Bombi, Chimica analitica. Trattazione algebrica e grafica degli equilibri chimici in soluzione acquosa. EdiSES
- Farmacopea Ufficiale della Repubblica Italiana,(F.U.)
- D.C. Harris, Quantitative Chemical Analysis, 9th Edition, 2016, W.H. Freeman and Co.
- D.A. Skoog, D.M. West, F.J. Holler, S.R. Crouch, Foundamentals of Analytical Chemistry, 9th Edition, 2014, Brooks/Cole.
- exercise book:
Silvia Araneo, Esercizi per la Chimica Analitica con richiami di teoria. Soc. Ed. Esculapio, 2° edizione 2018.
Reference books:
- General and Inorganic Chemistry and Stoichiometry course textbooks.
- A. Araneo, Chimica Analitica Qualitativa. Ed.C.E.A. (3° ed.)
- Pastore, Di Marco, Bombi, Chimica analitica. Trattazione algebrica e grafica degli equilibri chimici in soluzione acquosa. EdiSES
- Farmacopea Ufficiale della Repubblica Italiana,(F.U.)
Assessment methods and Criteria
The exam consists on a written test, lasting about 2.5 houres, in which the student is asked to solve 4/5 exercises and to answer 1/2 open questions regarding the theoretical part of the course. By solving the exercises, the student will have to demonstrate able to set chemical reactions and mathematical equations, to solve analytical problems and to understand and to recognize the different analytical methods, both traditional and instrumental, describing them correctly. A short discussion concerning the written test closes the exam.
CHIM/01 - ANALYTICAL CHEMISTRY - University credits: 8
Practicals: 32 hours
Lessons: 48 hours
Lessons: 48 hours
Professor:
Araneo Silvia Rosa
Shifts:
-
Professor:
Araneo Silvia RosaLinea MZ
Responsible
Lesson period
Second semester
Course syllabus
Introduction - Significant figures and rounding. Ionic strenght. Activity and activity coefficients. Debye-Hückel equation.
Ionic equilibria - Acid-base equilibria (Strong and weak acids and bases. Polyprotic acids. Buffer solutions. Distribution diagrams). Solubility equilibria (Solubilities vs. solubility products. Common ion effect. Ionic strenght vs. solubility. Simultaneous equilibria in precipitation. Simple and complex precipitation). Simultaneous solubility-acidity equilibria (Solubility relation on pH). Complexation equilibria (Review on ligands and chelating agents. Formation and dissociation constants. Ion masking). Simultaneous solubility-complexation and acidity-complexation equilibria (Conditional-formation constants. Replacing reactions). Redox equilibria (Oxidizing and reducing agents. Galvanic cells. Standard redox potentials. Nernst equation. Formal redox potentials).
General methods in quantitative chemical analysis - Gravimetric analysis (Basic principles. Crystalline and colloidal precipitates). Volumetric analysis (Basic principles. Acid-base titrations. Precipitation titrations with Ag+. EDTA titrations. Redox titrations. Calculated values in a titration curve. Equivalence and final titration points. Chemical indicators).
Instrumental quantitative chemical analysis - Electrochemical methods (Potentiometry. Direct potentiometric measurements. Reference electrodes. Indicators electrodes. Glass electrode. Ion-selective electrodes. Calibration line. Added solutions method. Potentiometric titrations.). Spectroscopic methods (Properties of light, absorption and emission of radiation. Transmittance and adsorbance. Lambert-Beer's law. Atomic spectroscopy).
Ionic equilibria - Acid-base equilibria (Strong and weak acids and bases. Polyprotic acids. Buffer solutions. Distribution diagrams). Solubility equilibria (Solubilities vs. solubility products. Common ion effect. Ionic strenght vs. solubility. Simultaneous equilibria in precipitation. Simple and complex precipitation). Simultaneous solubility-acidity equilibria (Solubility relation on pH). Complexation equilibria (Review on ligands and chelating agents. Formation and dissociation constants. Ion masking). Simultaneous solubility-complexation and acidity-complexation equilibria (Conditional-formation constants. Replacing reactions). Redox equilibria (Oxidizing and reducing agents. Galvanic cells. Standard redox potentials. Nernst equation. Formal redox potentials).
General methods in quantitative chemical analysis - Gravimetric analysis (Basic principles. Crystalline and colloidal precipitates). Volumetric analysis (Basic principles. Acid-base titrations. Precipitation titrations with Ag+. EDTA titrations. Redox titrations. Calculated values in a titration curve. Equivalence and final titration points. Chemical indicators).
Instrumental quantitative chemical analysis - Electrochemical methods (Potentiometry. Direct potentiometric measurements. Reference electrodes. Indicators electrodes. Glass electrode. Ion-selective electrodes. Calibration line. Added solutions method. Potentiometric titrations.). Spectroscopic methods (Properties of light, absorption and emission of radiation. Transmittance and adsorbance. Lambert-Beer's law. Atomic spectroscopy).
Prerequisites for admission
Basic knowledge of physics and mathematics and in-depth knowledge of all the topics covered in the course of General and Inorganic Chemistry
Teaching methods
The course is divided into classroom lectures and exercises. The topics are illustrated with slides and by carrying out exercises on the blackboard. During the course of the exercises, the method of discussion and the tutorial approach, with targeted questions, will also be used in order to stimulate students and to make the learning of the exposed concepts more interactive and personalized
Teaching Resources
Recommended textbooks:
- D.C. Harris, Quantitative Chemical Analysis, 9th Edition, 2016, W.H. Freeman and Co.
- D.A. Skoog, D.M. West, F.J. Holler, S.R. Crouch, Foundamentals of Analytical Chemistry, 9th Edition, 2014, Brooks/Cole
Reference books:
- General and Inorganic Chemistry and Stoichiometry course textbooks.
- A. Araneo, Chimica Analitica Qualitativa. Ed.C.E.A. (3° ed.)
- Pastore, Di Marco, Bombi, Chimica analitica. Trattazione algebrica e grafica degli equilibri chimici in soluzione acquosa. EdiSES
- Farmacopea Ufficiale della Repubblica Italiana,(F.U.)
- D.C. Harris, Quantitative Chemical Analysis, 9th Edition, 2016, W.H. Freeman and Co.
- D.A. Skoog, D.M. West, F.J. Holler, S.R. Crouch, Foundamentals of Analytical Chemistry, 9th Edition, 2014, Brooks/Cole
Reference books:
- General and Inorganic Chemistry and Stoichiometry course textbooks.
- A. Araneo, Chimica Analitica Qualitativa. Ed.C.E.A. (3° ed.)
- Pastore, Di Marco, Bombi, Chimica analitica. Trattazione algebrica e grafica degli equilibri chimici in soluzione acquosa. EdiSES
- Farmacopea Ufficiale della Repubblica Italiana,(F.U.)
Assessment methods and Criteria
The exam consists on a written test, lasting about 2.5 houres, in which the student is asked to solve 4/5 exercises and to answer 1/2 open questions regarding the theoretical part of the course. By solving the exercises, the student will have to demonstrate able to set chemical reactions and mathematical equations, to solve analytical problems and to understand and to recognize the different analytical methods, both traditional and instrumental, describing them correctly
CHIM/01 - ANALYTICAL CHEMISTRY - University credits: 8
Practicals: 32 hours
Lessons: 48 hours
Lessons: 48 hours
Professor:
Panigati Monica
Shifts:
-
Professor:
Panigati MonicaProfessor(s)