CHIMICA GENERALE ED INORGANICA II E LABORATORIO 1

This course aims to both round out the topics covered in General and Inorganic Chemistry I and introduce new concepts—such as ionic equilibria in aqueous solution, electrochemistry, and an overview of inorganic chemistry—that will serve as a foundation for subsequent courses. As the second course in General and Inorganic Chemistry, it provides students with the tools to consolidate their general chemistry knowledge; by examining the chemistry of elements from the early periods of the periodic table, students will be able to apply everything learned so far regarding electron configuration, chemical reactivity, oxidation states, metallic character, and bond types.

By exploring chemical processes in aqueous solution—such as the dissociation of sparingly soluble salts, solubility, the pH of strong and weak acid/base solutions, buffer solutions, and electrochemistry—the course will give students insight into the role of chemistry in society and everyday life.

Laboratory exercises will be conducted to reinforce classroom concepts and provide practical experience in a chemical laboratory setting. Students will learn how to organize and perform chemical experiments and how to use glassware and basic laboratory instruments (such as pH meters and testers).

By the end of the course, students will have acquired the essential skills to address and solve problems involving quantitative calculations for equilibrium reactions; determine the pH of strong and weak acid/base solutions, salt solutions, and buffers; calculate the solubility of sparingly soluble salts; calculate the quantity of elements deposited at electrodes following the electrolysis of molten salts or solutions; and determine the direction of a reaction based on standard reduction potentials under both standard and non-standard conditions.

The course aims to foster the reasoning skills necessary to approach the study of chemical phenomena using analytical and numerical methods (applying knowledge and understanding).

Specific learning objectives:

To understand aqueous solution equilibria regarding the properties of strong and weak acids and bases, as well as salt solubility. To understand the relationship between the structure and strength of an acid. To understand the operating mechanism of a buffer solution. To understand electrochemistry, specifically the operation of galvanic cells and electrolysis. To understand the significance of standard reduction potentials and the competition between elements during electrolysis. To acquire a general overview of inorganic chemistry, with a more detailed look at the reactivity of elements in the first three periods of the periodic table.

Furthermore, in relation to the so-called Dublin Descriptors, this course contributes to the acquisition of the following transversal skills:

Knowledge and understanding:

Capacity for inductive and deductive reasoning. Ability to outline a chemical reaction in qualitative and quantitative terms. Ability to

formulate a problem using appropriate relationships between physicochemical quantities and to solve it using analytical methods.

Applying knowledge:

Ability to apply acquired knowledge to describe chemical phenomena by rigorously employing the scientific method. Ability to perform quantitative calculations regarding reactants and products in equilibrium chemical reactions.

Making judgments:

Capacity for critical reasoning. Ability to identify the most suitable solutions for chemical problems. Ability to determine the predictions of a theory or model.

Communication skills:

Ability to describe a scientific topic—explaining its rationale and results—both orally and in writing, using appropriate language and precise terminology. Information for students with disabilities and/or specific learning disorders (SLD)

To ensure equal opportunities and in compliance with current regulations, interested students may request a personal meeting to arrange any necessary compensatory and/or dispensatory measures, based on educational objectives and specific needs.

The course comprises 36 hours of lectures (21 hours of theory and 15 hours of classroom exercises) and 30 hours of laboratory work, during which experiments will be conducted to facilitate the understanding of key course concepts.

Students are expected to have fully mastered the concepts learned in the General Chemistry I course. It should be noted that the topics covered in this second part are new and present greater conceptual challenges.

Attendance at lectures, practical exercises, and laboratory sessions is a mandatory requirement for passing the exam. Upon completion of the laboratory work, students are required to submit reports; these will be graded by the instructor, and the assessment will contribute to the final grade. Students who, due to force majeure, are compelled to miss more than one session must pass a practical laboratory exam before being permitted to take the oral exam.

1. Chemical Equilibrium. Ionic equilibria in aqueous solution: Water dissociation and pH; acid-base theories (Arrhenius, Brønsted-Lowry, and Lewis); structure-acidity relationship; ampholytes; pH of salt solutions (hydrolysis); buffer solutions; polyprotic acids; acid-base titrations and pH indicators. pH calculations for solutions of acids, bases, salts, and buffers. Heterogeneous equilibria: Salt solubility and solubility product.

2. Electrochemistry: Conductivity of aqueous solutions; electrochemical cells and standard half-cell potentials; use of standard potentials to predict redox reactions; Nernst equation; electrolysis; Faraday's laws; overpotential and discharge potentials.

3. Introduction to Inorganic Chemistry: Hydrogen and elements up to the third period of the s-block and p-block.

4. Exercises:

 - pH calculations for solutions of acids, bases, salts, and buffers. Acid-base reactions.

 - Solubility and solubility product (Definition of the solubility product constant; relationship between salt solubility and solubility product for salts with different stoichiometries). Common-ion effect. Effect of pH on the solubility of certain salts. - Electrochemistry (Calculation of the E° of a redox reaction and the corresponding equilibrium constant; calculation of quantities obtained at electrodes via the electrolysis of saline solutions and molten salts)

5. Laboratory Experiments: 1) Titrations of strong and weak monoprotic acids using an indicator and a pH meter

                                               2) Salt solubility (determination of the solubility product of a sparingly soluble salt and solubility tests of silver halides in ammonia)

                                               3) Construction of a galvanic cell and electrolysis of aqueous solutions

                                               4) Permanganometric titration of hydrogen peroxide and of a detergent containing sodium percarbonate

All topics covered are considered essential for passing the exam.

1.CHEMICAL PRINCIPLES - Atkins, Jones, Laverman

2. Stoichiometry- B I Bhatt-S B Thakore

3. Chemical Reactions and Stoichiometry, R. K. Dave

4. Chemistry: A Molecular Approach (5th edition) Nivaldo J. Tro, Global Edition

5. Chemistry & Chemical Reactivity. Kotz/Treichel/Townsed

Lecture notes

The exam consists of a written test with a maximum duration of 2 hours (the date listed in the official schedule is the date of the written test). The written test involves solving a series of problems similar to those addressed in class during the semester. The oral exam will take place a few days later, as scheduled by the instructor (date and location to be announced), and will assess the laboratory work and the topics covered during lectures.

The final assessment will also take into account the quality of the laboratory reports, which must be submitted at least one week prior to the written test date. Students who have not attended at least 70% of the laboratory sessions will also be required to complete a practical test before the written exam.

During the course, the instructor addresses a range of problem types considered important for the professional development of a chemist-in-training—and which will appear on the written exam—as well as a series of laboratory experiments to be performed.

Any topic covered in the course may be the subject of an exam question. Please note that the exam may also include questions regarding the laboratory experiments; therefore, a thorough review of these experiments is strongly recommended.

Examples of questions:

Buffer solutions; salt hydrolysis; salt solubility; electrochemical cells; electrolysis.

Examples of exercises:

    2.5 g of calcium iodate are completely dissolved in the minimum amount of water. The solution volume is 1.19 liters. Determine the Ksp of calcium iodate (Molar Mass = 389.88). Given solid calcium iodate, calculate how many grams dissolve when washed 10 times with 150 mL of solvent each time.

    Calculate the pH of a solution obtained by dissolving 5.88 g of sodium cyanide (NaCN) in pure water and bringing the solution volume to 250 mL (Molar Mass (NaCN) = 49.01 g/mol; Kb(CN-) = 2.03 × 10⁻⁵).

    Calculate the EMF of the following concentration cell:

       Ag|Ag2SO4 (sat. sol.) || Ag+ (0.100 M)|Ag
         The solubility product of Ag2SO4 is 1.6 × 10⁻⁵. 

Calculate the pH and the concentration of the species in a solution obtained by adding 50.0 mL of 1.60 × 10⁻¹ M NaOH to 30 mL of 1.60 × 10⁻¹ M CH₃COOH. For CH₃COOH, Ka = 1.76 × 10⁻⁵.