Acids and Bases: Concepts, Reactions, and Calculations

This set of flashcards covers key vocabulary and concepts related to acids and bases, their reactions, and the relevant calculations necessary for understanding their properties.

Brønsted–Lowry

A theory that defines acids as proton donors and bases as proton acceptors.

Ionization

The process by which a compound breaks down into ions when dissolved in water.

Ka

The equilibrium constant for acid dissociation, indicating the strength of an acid.

Buffer

A solution that resists changes in pH upon addition of small amounts of acids or bases.

pH

A measure of the acidity or basicity of a solution, calculated as -log[H+].

pOH

A measure of the basicity of a solution, calculated as -log[OH-].

Kw

The ionization constant of water, which is equal to the product of the concentrations of H+ and OH- ions in water.

Neutralization Reaction

A chemical reaction where an acid and a base react to form water and a salt.

Conjugate Acid-Base Pair

A pair that consists of an acid and a base that differ by a single proton.

Strong Acid

An acid that completely ionizes in solution, resulting in a high concentration of H3O+.

Weak Acid

An acid that only partially ionizes in solution, resulting in a lower concentration of H3O+.

Hydronium Ion (H3O+)

The ion formed when an acid donates a proton to water.

Hydroxide Ion (OH-)

The ion formed in basic solutions, resulting from the dissociation of bases in water.

Hydrogen Ion (H+)

An ion that represents a proton and is responsible for the acidic properties of a solution.

Amphoteric

A substance that can act as both an acid and a base.

Solubility Rules

Guidelines used to determine the solubility of ionic compounds in water.

Equilibrium Constant Expression

A mathematical expression that describes the ratio of products to reactants at equilibrium.

Henderson-Hasselbalch Equation

A formula used to calculate the pH of a buffer solution based on the concentration of the acid and its conjugate base.

Acid-Base Equilibrium

The state in which the rates of acid dissociation and recombination of the base are equal, resulting in constant concentrations of H+ and the conjugate base.

Acidic Solution

A solution where [H+] is greater than [OH-], resulting in a pH less than 7.

Basic Solution

A solution where [OH-] is greater than [H+], resulting in a pH greater than 7.