Exam 3 Study Guide - Acid Base Equilibria

Flashcards covering key concepts from the lecture notes about acid-base equilibria.

Arrhenius Acid

A substance that produces H+ ions in water.

Arrhenius Base

A substance that produces OH- ions in water.

Brønsted-Lowry Acid

A proton (H+) donor.

Brønsted-Lowry Base

A proton (H+) acceptor.

Autoionization of Water

The reversible reaction: H2O (l) + H2O (l) ⇌ H3O+ (aq) + OH- (aq).

Kw (Equilibrium Constant for Water)

The value of Kw at 25 degrees Celsius is 1.0 x 10^-14.

Acidic Solution

A solution where [H+] > [OH-].

Basic Solution

A solution where [OH-] > [H+].

Neutral Solution

A solution where [H3O+] = [OH-] = 1.0 x 10^-7 M.

pH Scale

A measure defined as pH = -log [H+].

Strong Acid

An acid that completely dissociates in water.

Weak Acid

An acid that only partially dissociates in water.

Conjugate Acid-Base Pair

A pair of compounds that differ by a single proton (H+).

Henderson-Hasselbalch Equation

pH = pKa + log[A-]/[HA].

Buffer Solution

A solution that resists changes in pH upon the addition of small amounts of acid or base.

Common-Ion Effect

The reduction in ionization of a weak acid or weak base due to the presence of a common ion.

Titration

The process of analyzing an unknown amount of acid or base by determining the equivalent amount of a known acid or base.

Solubility Product (Ksp)

An equilibrium constant that applies to the solubility of sparingly soluble ionic compounds.