Aqueous Equilibria

These flashcards cover key concepts related to aqueous equilibria and are designed to help students understand the principles of buffer solutions, titrations, equilibrium and the relationships in acid-base chemistry.

Buffer Solutions

A solution containing both a weak acid and its conjugate base, capable of resisting changes in pH.

Henderson–Hasselbalch Equation

An equation used to calculate the pH of buffer solutions based on the concentration of the weak acid and its conjugate base.

Titration

A method to determine the concentration of a substance by adding a solution of known concentration until the reaction reaches its equivalence point.

pKa

The negative logarithm of the acid dissociation constant (Ka), used to describe the strength of an acid.

Solubility Product Constant (Ksp)

An equilibrium constant for the solubility of a sparingly soluble ionic compound.

Common-Ion Effect

The suppression of the ionization of a weak acid or base in the presence of a strong electrolyte that has a common ion.

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 Indicator

A substance that changes color at a certain pH level, used to signify the endpoint of a titration.

Polyprotic Acids

Acids that can donate more than one proton (H+) per molecule.

Molar Solubility

The number of moles of a solute that can dissolve in one liter of solution, usually in the context of saturated solutions.

Weak Acid

An acid that does not fully dissociate in solution, characterized by a moderate value of Ka.

Weak Base

A base that does not fully dissociate in solution, characterized by a moderate value of Kb.