Acid and bases

Arrhenius Acid

A substance that, when dissolved in water, increases the concentration of hydrogen ions.

Arrhenius Base

A substance that, when dissolved in water, increases the concentration of hydroxide ions.

Conjugate Acids and Bases

The products of reactions between acids and bases that always yield their conjugate bases and acids.

Amphiprotic

Substances that can donate or accept a proton.

Autoionization of Water

The process where water molecules act as both acids and bases to form hydronium and hydroxide ions.

Ion-Product Constant (Kw)

The equilibrium constant for the autoionization of water, equal to 1.0 × 10^(-14) at 25°C.

pH

The negative base-10 logarithm of the hydronium ion concentration, used to indicate the acidity or basicity of a solution.

pH

A measure of the acidity or alkalinity of a solution, defined as the negative logarithm of the hydrogen ion concentration.

pOH

The negative logarithm of the hydroxide ion concentration in a solution.

Kw

The ion product constant for water, equal to 1.0 x 10^-14 at 25°C.

Litmus paper

A simple pH indicator that changes color in acidic or basic solutions.

pH meter

An instrument used to measure the pH of a solution by detecting the voltage generated by the hydrogen ions in the solution.

Strong acids

Acids that completely dissociate into ions in aqueous solutions, such as HCl, H2SO4, and HNO3.

Strong bases

Bases that completely dissociate into hydroxide ions in aqueous solutions, including alkali metal and heavier alkaline earth metal hydroxides.

Acid-dissociation constant (Ka)

A measure of the strength of an acid, calculated as the ratio of the concentration of products to reactants in an acid dissociation reaction.

Percent Ionization

The percentage of acid molecules that ionize in a solution.

pH

A measure of the acidity or basicity of a solution, defined as the negative logarithm of the hydrogen ion concentration.

Equilibrium Constant Expression

An expression that relates the concentrations of reactants and products at equilibrium for a chemical reaction.

Weak Acid

An acid that only partially dissociates in solution, resulting in a lower concentration of ions compared to a strong acid.

Strong Acid

An acid that completely dissociates in solution, resulting in a high concentration of ions.

Quadratic Equations

Equations involving a single variable to the second power, often used to solve for equilibrium concentrations in acid-base reactions.

Ionized

Refers to the process of forming ions by the dissociation of molecules in a solution.

Acetic Acid

A weak acid with the chemical formula CH3COOH, commonly found in vinegar.

Polyprotic Acids

Acids that have more than one acidic proton available for donation.

Le Châtelier’s Principle

States that if a system at equilibrium is disturbed by a change in temperature, pressure, or concentration, the system will shift its equilibrium position to counteract the effect of the disturbance.

Conjugate Base

The species that remains after an acid has donated a proton.

pH

A measure of the acidity or basicity of a solution, defined as the negative logarithm of the hydrogen ion concentration.

Hydrolysis Reaction

A chemical reaction in which a compound reacts with water to produce ions.

Conjugate Acid

The species that is formed when a base accepts a proton.

Arrhenius Bases

Bases that dissociate in water to release hydroxide ions (OH-) and cations.

Conjugate Acid

The species that is formed when a base accepts a proton.