ACID BASE EQUILIBRIA | 4.2

ACIDS (Increase H* in solution). BASES (Increases OH-)

Arrhenius Definition of ACID and BASES

ACIDS (proton H* donor). BASES (proton H* acceptor)

Brønsted-Lowry definition of ACIDS and BASES 

ACIDS (electron pair acceptor). BASES (electron par donor)

Lewis Definition of ACIDS and BASES

Arrhenius

Brønsted-Lowry

acid

BASE

must have a pair of non bonding electron (ex. NH3,H20)

Amphiprotic Species (or Amphoteric)

Brønsted-Lowry Acids and Bases

which acid definition has base, acid, conju acid, and conju base

Conjugate Base

the species produced when an acid gives off its acidic

proton (H+)

Conjugate Acid

the species produced when a base accepts a proton given

off by the acid

Lewis Acid

Lewis Base

P functions

pH – Measure of Acidity

NEUTRAL

[H3O+] = [OH-]

[H3O+] = 1 x 10-7

pH = 7

ACIDIC

[H3O+] > [OH-]

[H3O+] > 1 x 10-7

pH < 7

BASIC

Strong acids and bases

ionize

completely in water.

Weak acids and bases

ionize

only to a limited extent in WATER

Weak Acids & Bases

Strong Acids and Bases

↓strength of its

conjugate base

↑strength acid

Ka

acid dissociation constant

↑higher the Ka value, the stronger the acid

Kb

base dissociation constant

↑higher the Kb value, the stronger the base

Percent Ionization

BUFFER SOLUTION

solutions that resist drastic changes in pH upon addition of

small amounts of acids or bases

Acidic Buffer:

weak acid + salt containing the

conjugate base

Basic/Alkaline Buffer:

weak base + salt containing the

conjugate acid