Chem II - Chapter 20

Properties of Acids

Electrolytes, sour, red litmus paper

Properties of Bases

Electrolytes, bitter, slippery, blue litmus paper

Acid

A compound that produces hydrogen ions when dissolved in water for an acid of the general form HX

Base

A compound that produces hydroxide ions when dissolved in water

Hydroxide Ion

The negative ion formed when a water molecule loses a hydrogen ion

Hydronium Ion

The positive ion formed when a water molecule gains a hydrogen ion

Self-Ionization of Water

Reaction in which two water molecules produce ions

Acidic Solution

pH < 7

Neutral Solution

pH = 7

Basic Solution

pH > 7

pH

The negative logarithm of the hydrogen ion concentration

pOH

The negative logarithm of the hydroxide ion concentration

Acid-Base Indicator

An acid or base that shows different colors in a known pH range

Arrhenius Acid

Hydrogen containing compound that ionizes to give H+ ions in an aqueous solution

Monoprotic Acid

Acid with one ionizable hydrogen

Diprotic Acid

Acid with two ionizable hydrogens

Triprotic Acid

Acid with three ionizable hydrogens

Arrhenius Base

Compound that ionizes to give OH- ions in aqueous solution

Bronsted-Lowry Acid

Hydrogen ion donor

Bronsted-Lowry Base

Hydrogen ion acceptor

Conjugate Acid

The particle formed when a base gains a hydrogen ion

Conjugate Base

The particle that remains when an acid has donated a hydrogen ion

Conjugate Acid-Base Pair

Two substances that are related by the loss or gain of a single hydrogen ion

Amphoteric

A substance that can act as either an acid or a base

Lewis Acid

A substance that can accept a pair of electrons to form a covalent bond

Lewis Base

A substance that can donate a pair of electrons to form a covalent bond

Strong Acids

Acids that are nearly 100% ionized in aqueous solutions

Weak Acids

Acids that slightly ionize in aqueous solutions

Acid Dissociation Constant (Ka)

The ratio of the concentration of the dissociated form to the undissociated form: Ka = ([H+][X-])/[HX]

Strong base

Base that completely dissociates metal ions and hydroxide ions in solution

Weak base

React with water to form the hydroxide ion and the conjugate acid of the base

Base dissociation constant (Kb)

The ratio of the concentration of the conjugate acid times the concentration of the hydroxide ion to the concentration of the conjugate base

pH(OH) to molarity

10^(-x)

Molarity to pH(OH)

log