Description

Theory
1

Theory/Practice
3

Instructors

M Teresa Oliva Teles

Contents

1- Periodic Table.
2- Chemical bonding.
3- Stoichiometry
4- Chemical equilibrium. The equilibrium constant. Le Chatelier?s principle.
Equilibrium in liquid solution. Activity coefficients. Mean ionic activity coefficients. Ionic strength. Debye- Huckel law.
5- Acids and bases. Acid and basic ionization constants. pH. Quantitative calculations of pH in different solutions: strong acid, strong base, weak acid, weak base, mixtures of conjugate acid and base pair, amphoteric compounds, polyprotic acids and bases. Quantitative pH calculations: mixtures of acids and bases. Buffer solutions. Applications.
6-Precipitation reactions. Heterogeneous equilibrium. Solubility products. Solubility of salts. Effects of different factors in the solubility of precipitates. Applications.
7-Equilibrium of complexation. Formation constants.
8- Oxidation-reduction reactions. Oxidation number. Oxidizing agent and reducing agent. Redox equations balance. Nernst equation. Standard cell potentials.

Learning Outcomes

OB1: Apply basic chemistry concepts to analyse and solve problems related to chemical processes and engineering applications.

OB2: Calculate solution concentrations and perform quantitative chemical analysis.

OB3: Perform stoichiometric calculations to solve chemical reaction problems.

OB4: Calculate solubility, pH of aqueous solutions, and the electromotive force of electrochemical cells.

OB5: Identify and explain the types of interatomic and intermolecular bonds.

OB6: Apply scientific reasoning and critical thinking to analyse chemical phenomena and solve problems.