Unit 11: Acids, Bases, and Salts

Flashcards covering key concepts related to acids, bases, and salts.

Acids

Substances that donate protons (H+) in solution and have a pH less than 7.

Bases

Substances that accept protons (H+) in solution and have a pH greater than 7.

pH scale

A scale that measures how acidic or basic a solution is, ranging from 0 (acidic) to 14 (basic), with 7 being neutral.

Strong acid

An acid that completely dissociates in solution (e.g., HCl, HNO3).

Weak acid

An acid that partially dissociates in solution (e.g., acetic acid, HF).

Strong base

A base that completely dissociates in solution (e.g., NaOH, KOH).

Weak base

A base that partially dissociates in solution (e.g., ammonia, NH3).

Neutralization

A chemical reaction between an acid and a base to produce a salt and water.

Dissociation

The process in which a compound separates into its constituent ions in solution.

Amphoteric substances

Compounds that can act as either an acid or a base depending on the environment (e.g., water, NH3).

Bronsted-Lowry acid

A substance that donates a proton (H+) during a reaction.

Bronsted-Lowry base

A substance that accepts a proton (H+) during a reaction.

Buffer

A solution that resists changes in pH when small amounts of acid or base are added.

Hydronium ion (H3O+)

The ion formed when an acid donates a proton to water.

Hydroxide ion (OH-)

The ion formed when a base accepts a proton from water.

pKa

A measure of the strength of an acid in solution; it is the negative logarithm of the acid dissociation constant (Ka).

Equivalence point

The point in a titration where the amounts of acid and base have reacted completely.

Indicator

A substance that changes color at a particular pH range, used to determine the endpoint of a titration.

Titration

An analytical technique used to determine the concentration of an unknown solution by reacting it with a standard solution.

Ionization

The process of forming ions in solution, particularly for weak acids and bases.