Understanding how to work with acidic and basic solutions, identifying the acid and base, calculating pH, and balancing acid-base reactions.
Acids and Bases: Understanding the concepts of acids and bases, their definitions, properties, and differences.
Chemical reactions: Understanding the basics of chemical reactions, including reactants, products, and equations.
Stoichiometry: The quantitative relationships between the amounts (moles) of reactants and products in a chemical equation.
Molarity: A concentration unit that measures the number of moles of solute in a given volume of solution.
pH scale: A measure of the acidity or basicity of a solution, ranging from 0 to 14, with 7 being neutral.
Acid-base titrations: A laboratory technique for determining the concentration of an acid or base solution by adding a known amount of the opposite solution until the reaction is complete.
Buffer solutions: Solutions that resist pH changes upon addition of acids or bases, consisting of a weak acid and its conjugate base, or a weak base and its conjugate acid.
Acid-base indicators: Substances that change color depending on the pH of a solution, often used in titrations to indicate the endpoint of the reaction.
Neutrality: The concept of neutralization, in which an acid reacts with a base, resulting in the products of a salt and water.
Strong and weak acids and bases: Understanding the differences between strong acids and bases that undergo complete ionization in a solution and weak acids and bases that undergo partial ionization.
Equilibrium: The state of a chemical reaction in which the rates of the forward and reverse reactions are equal, and the concentrations of reactants and products are constant.
Acid and base dissociation constants: The equilibrium constants that describe the strength of an acid or base, and determine the pH of a solution.
Lewis acids and bases: The concept of Lewis acids as electron pair acceptors and Lewis bases as electron pair donors, broader than the Bronsted-Lowry theory of acid-base reactions.