Aqueous Ionic Equilibria

These flashcards cover key concepts from aqueous ionic equilibria, focusing on buffer solutions, titrations, and solubility equilibria.

What is a buffer solution?

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

Why is blood considered a buffered solution?

Blood maintains a pH of 7.4, an essential condition for many physiological processes.

What are the two components required for a buffer solution?

An acid component and a base component that do not neutralize each other.

What is the Henderson-Hasselbalch equation used for?

To calculate the pH of a buffer solution using the concentrations of the acid and its conjugate base.

What defines the buffer capacity?

The amount of acid or base that a buffer can neutralize before its pH changes appreciably.

What happens to solubility equilibrium in the presence of a common ion?

It shifts to the left, decreasing solubility.

What is the pH range of an effective buffer?

Approximately 2 pH units centered around the pKa of its acid component.

How does the addition of a strong acid or base affect a buffer?

It requires two steps: neutralization calculation and new pH calculation using the Henderson-Hasselbalch equation.

What is the equilibrium constant for the solubility of a salt?

The solubility product constant (Ksp), which describes the equilibrium between a solid solute and its ions in a saturated solution.