Chemistry Equilibrium to Titrations

These flashcards cover key vocabulary and concepts related to equilibrium, acids and bases, dissociation, buffers, neutralization reactions, and titration techniques in chemistry.

Equilibrium

A state where the concentrations of all reactants and products are constant over time.

Le Chatelier’s Principle

If a change is imposed on a system at equilibrium, the position of the equilibrium will shift in a direction that reduces that change.

Dissociation

The process of an acid dissolving in water to produce hydronium ions and an anion.

Monoprotic Acid

An acid that has one acidic hydrogen, such as hydrochloric acid (HCl).

Polyprotic Acid

An acid that has more than one acidic hydrogen, such as sulfuric acid (H2SO4).

pH Scale

A logarithmic scale that measures the concentration of hydronium ions in a solution.

Buffer

A solution that resists changes in pH when an acid or base is added.

Neutralization Reaction

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

Strong Acid

An acid that completely dissociates in water.

Weak Acid

An acid that partially dissociates in water.

Hydronium Ion

An ion formed when a proton (H+) is attached to a water molecule, represented as H3O+.

Conjugate Acid

The species formed when a base gains a proton.

Conjugate Base

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

Titration

A laboratory technique to determine the molarity of an acid or base where one solution is known and the other is unknown.

Endpoint in Titration

The point at which the acid has completely neutralized the base.

pOH

A measure of the hydroxide ion concentration in a solution, related to pH by the equation 14 = pOH + pH.