Acids & Bases (Part 1)

These flashcards cover important terms and concepts related to acids and bases as discussed in the lecture.

Strong Acid

An acid that donates a proton and fully dissociates in solution, acting as a strong electrolyte.

Strong Base

A base that accepts a proton and fully dissociates in solution, also acting as a strong electrolyte.

Weak Acid

An acid that partially dissociates in solution, involved in both forward and reverse reactions, and behaves as a weak electrolyte.

Weak Base

A base that does not completely dissociate in solution, also involved in both forward and reverse reactions, acting as a weak electrolyte.

Brönsted-Lowry Acid

A substance that donates a proton (H+ ion) in a chemical reaction.

Brönsted-Lowry Base

A substance that accepts a proton (H+ ion) in a chemical reaction.

Conjugate Acid-Base Pair

A pair of species that differ by the presence or absence of a proton.

Amphoteric

A substance that can act as both an acid and a base.

Ka

The acid dissociation constant that measures the strength of an acid in solution.

Kb

The base dissociation constant that measures the strength of a base in solution.

Hydrolysis Reaction

A reaction in which a salt reacts with water to produce either an acidic or basic solution.

Electrolyte

A substance that dissociates into ions in solution and conducts electricity.

Conjugate Base

The species that remains after an acid donates a proton.

Conjugate Acid

The species that is formed when a base accepts a proton.

pH

A measure of the acidity or basicity of a solution, calculated based on H3O+ ion concentration.

Neutral Salt Solution

A solution that results from the combination of a strong acid and a strong base, having a pH around 7.

Acidic Solution

A solution where the concentration of H3O+ is greater than that of OH-, resulting in a pH less than 7.

Basic Solution

A solution where the concentration of OH- is greater than that of H3O+, resulting in a pH greater than 7.

Successive Ka Values

The multiple dissociation constants for polyprotic acids, indicating strength variations between each proton donation.

Inductive Effect

The effect on acid strength due to electron density shifting through covalent bonds, often impacting acidity.