The study of the properties and reactions of acids and bases.
pH and pOH: The measurement of the acidity or basicity of a solution through pH and pOH scales, respectively.
Acid and base definitions: Understanding the characteristics of acids and bases and their behavior in solution.
Bronsted-Lowry theory: Defining acids as proton (H+) donors and bases as proton acceptors.
Lewis theory: Defining acids as electron pair acceptors and bases as electron pair donors.
Strong and weak acids and bases: Understanding the differences between strong and weak acids and bases in terms of their dissociation constants and strength of acidity or basicity.
Acid-base titrations: The process of determining the concentration of an acid or base through titration with a known concentration of the opposite substance.
Buffer solutions: Understanding the role and function of buffer solutions in maintaining a constant pH in a system.
Acid-base equilibria: Understanding the concept of equilibrium in acid-base reactions and the factors that influence it.
Indicators: The use of indicators to determine the endpoint of an acid-base titration.
Acid-base reactions: The different types of acid-base reactions, including neutralization, hydrolysis, and proton transfer.
Henderson-Hasselbalch equation: The use of the Henderson-Hasselbalch equation to calculate the pH of buffer solutions.
Acid-base properties of salts: Understanding how salts can act as acids or bases in solution.
Common ion effect: The effect of adding an ion to a solution to shift the equilibrium between an acid and its conjugate base, or a base and its conjugate acid.
Solubility equilibria: Understanding the relationship between solubility, pH, and acid-base equilibria.
Acid-base catalysis: The role of acids and bases as catalysts in chemical reactions.
Arrhenius theory: This theory states that an acid is a substance that releases hydrogen ions (H+) in aqueous solution, while a base is a substance that releases hydroxide ions (OH-) in aqueous solution.
Bronsted-Lowry theory: This theory defines an acid as any substance that can donate a hydrogen ion (H+) and a base as any substance that can accept a hydrogen ion.
Lewis theory: This theory defines an acid as any substance that can accept a pair of electrons, while a base is any substance that can donate a pair of electrons.
Acid-base equilibrium: This is a dynamic process in which acid and base species are constantly interconverting. At equilibrium, the concentrations of the acid and its conjugate base are determined by the equilibrium constant.
Proton transfer reactions: These reactions involve the transfer of a hydrogen ion from one molecule to another, resulting in the formation of a new acid or base.
Neutralization reactions: These reactions involve the reaction of an acid and a base to form a salt and water.
Acid-base titrations: These are experimental methods that determine the concentration of an acid or base by adding a standard solution of the opposite type until the equivalence point is reached.
Buffer systems: These are solutions that resist changes in pH by reacting with added acid or base, and keeping the pH relatively constant.
Acid-base indicators: These are colored compounds that exhibit a different color in acidic and basic solutions and are used to determine the endpoint of an acid-base titration.
Acid rain: This refers to rainwater that has a pH of less than 5.6, which is caused by the dissolution of acidic pollutants in the atmosphere.
Strong acids and bases: These are substances that completely dissociate in water to form H+ and OH- ions, respectively.
Weak acids and bases: These are substances that only partially dissociate in water, resulting in an equilibrium between the parent acid or base and its conjugate.
Amphiprotic species: These are substances that can act as both an acid and a base, such as water and amino acids.