CHEM 104 Module 16: Additional Aqueous Equilibria

These flashcards cover key concepts from the CHEM 104 Module 16 on additional aqueous equilibria, focusing on acid-base buffer systems, titrations, and chemical equilibrium.

Buffer Solutions

Solutions that resist changes in pH when small amounts of acid or base are added.

Conjugate Acid-Base Pair

A pair consisting of an acid and its corresponding base that differ by one proton.

Henderson-Hasselbalch Equation

An equation used to calculate the pH of a buffer solution, given by pH = pKa + log(rac{[A^-]}{[HA]}) where [A^-] is the concentration of the base and [HA] is the concentration of the acid.

pH

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

Strong Acid

An acid that completely dissociates in water, releasing all its hydrogen ions.

Strong Base

A base that completely dissociates in water, producing hydroxide ions.

Titration Curve

A plot of pH versus volume of titrant added during a titration, showing the changes in pH throughout the reaction.

Ksp (Solubility Product Constant)

An equilibrium constant for the dissolution of a sparingly soluble salt in water.

Common Ion Effect

The decrease in the solubility of a salt when a common ion is added to the solution.

Saturated Solution

A solution in which no more solute can dissolve at a given temperature and pressure.

Unsaturated Solution

A solution that can still dissolve more solute at a given temperature and pressure.

Equivalence Point

The point in a titration at which the amount of titrant added is enough to completely neutralize the analyte solution.

Reaction Quotient (Q)

A measure used to determine the direction of a chemical reaction at any point, calculated similarly to K but using non-equilibrium concentrations.