Acid-Base Titrations and Solubility Equilibria

These flashcards cover fundamental concepts and vocabulary from the lecture on acid-base titrations and solubility equilibria, helping students prepare for their exam.

Titration

A quantitative analysis method used to determine the concentration of an unknown solution by reacting it with a solution of known concentration.

Equivalence Point

The point in a titration at which the amount of titrant added is stoichiometrically equivalent to the amount of analyte in the sample.

pH

A measure of the acidity or basicity of a solution, defined as the negative base 10 logarithm of the hydrogen ion concentration.

Ksp (Solubility Product Constant)

An equilibrium constant used to describe the solubility of a sparingly soluble ionic compound.

Strong Acid

An acid that completely ionizes in solution, releasing protons (H+) and resulting in a low pH.

Weak Acid

An acid that partially ionizes in solution, resulting in a higher pH compared to strong acids.

Neutralization Reaction

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

Conjugate Base

The species that remains after an acid donates a proton (H+).

Titration Curve

A graph that plots the pH of a solution against the volume of titrant added during a titration.

Common Ion Effect

A decrease in the solubility of an ionic compound when a common ion is added to the solution.

ICE Table

A table used to calculate the concentrations of reactants and products at equilibrium for a reversible reaction.

Spontaneous Process

A process that occurs without the need for external energy, often characterized by an increase in entropy.

Gibbs Free Energy (ΔG)

A thermodynamic potential used to predict whether a process will occur spontaneously at constant temperature and pressure.

Standard Entropy (S°)

The absolute entropy of a substance at 1 atm pressure and a specified temperature, usually 25°C.

Solubility Equilibrium

The dynamic equilibrium established when the rate of dissolution of a solid into its ions is equal to the rate of precipitation of the solid from its ions.

Molar Solubility

The number of moles of solute that can be dissolved in a liter of solution at equilibrium.

Precipitation Reaction

A reaction in which soluble ions combine to form an insoluble compound that precipitates out of the solution.

Le Chatelier's Principle

A principle stating that if an external change is applied to a system at equilibrium, the system will adjust to counteract the change.

Weak Base

A base that does not completely ionize in solution, resulting in a relatively higher pH.

Thermodynamic State Functions

Properties of a system that depend only on its current state and not on the path taken to reach that state.

ΔU (Change in Internal Energy)

The change in internal energy of a system resulting from heat transfer and work done on or by the system.