This topic covers the chemical reactions that occur between acids and bases.
Acids and Bases: Basic introduction and definition of acids and bases along with their properties.
pH and pOH: Explanation of pH and pOH scales, and their relevance in acid-base reactions.
Strong and Weak Acids/Bases: Difference between strong and weak acids/bases and their ionization potentials.
Bronsted-Lowry Theory: Acid-Base theory based on proton transfer, and explanation on conjugate acid-base pairs.
Lewis Acids and Bases: Acid-Base theory based on electron-pair exchange, and explanation of coordination complexes.
Acid/Base Equilibria: Concept of acid-base equilibria, dissociation constants, and equilibria expressions.
Common Ion Effect: Effect of adding or removing an ion to the reaction mixture, and its impact on the equilibrium position.
Neutralization Reactions: Concept of neutralization reactions, and the formation of salt and water in the chemical reaction.
Titration: Method for determining the concentration of an acid or base using a standard solution, and calculation of equivalence point and half-equivalence point.
Buffer Solutions: Solutions that resist changes in pH upon addition of acid or base, and explanation of buffer capacity and buffer range.
Acid-Base Indicators: Substances that change color at a certain pH, and their use in acid-base titration.
Hydrolysis: Chemical reaction involving the reaction between ions of a salt and water, and its role in pH control.
Acid-Base Strength: Factors that influence acid/base strength, and comparison between different classes of acids/bases.
Acid-Base Reactions in Biological Systems: Acid-base reactions involved in biochemical pathways, and their relationship to human physiology.
Acid-Base Catalysis: Reaction process involving the participation of an acid/base catalyst, and impact on reaction rates.
Neutralization reactions: Occur when an acid and a base react to form a salt and water. The acid and the base cancel each other out, resulting in a neutral solution.
Redox reactions: Occur when an acid reacts with a reducing agent, or a base reacts with an oxidizing agent. These reactions involve a transfer of electrons, and the acid or base is reduced or oxidized in the process.
Acid-base substitution reactions: Occur when a hydrogen ion or a metal ion in an acid is substituted with another metal ion or hydrogen ion from another acid or base.
Hydrolysis reactions: Occur when water interacts with either an acid or a base. The acid or base is split into its component ions, which then react with the water molecules.
Proton transfer reactions: Occur when a hydrogen ion (proton) is transferred from an acid to a base.
Lewis acid-base reactions: Involve the transfer of a lone pair of electrons from a nucleophile to an electrophile.
Conjugate Acid-Base Pairs: Are related pairs of acids and bases that differ only by the loss or gain of a proton.
Amphiprotic and amphoteric substances: Are substances that can act both as acids and bases, depending on the conditions.
Bronsted-Lowry acid-base reactions: Involve the transfer of protons from an acid to a base. This is the most widely used definition of acids and bases.
Lewis acid-base reactions: Involve the transfer of electrons from a Lewis base to a Lewis acid. This definition is more inclusive than the Bronsted-Lowry definition and includes interactions between non-proton donors and acceptors.