Chem II - Acids and Bases

Arrhenius definition: Acids vs. Bases

Acids: Produce H+ in solution and associate with H2O

Base: Produces OH- in solution

Bronsted-Lowry definition: Acids vs. Bases

Acids: Proton donor

Bases: Proton acceptor (must have a lone pair)

Hydrochloric Acid

HCl

Hydrobromic Acid

HBr

Hydroiodic Acid

HI

Nitric Acid

HNO3

Perchloric Acid

HClO4

Sulfuric Acid

H2SO4

pH Formula

-log [H3O+]

[H3O+] Formula

= 10^-pH

Binary Acid

Acid H+ is attached to a nonmetal atom

Oxyacid

Acid H+ is attached to an oxygen atom

Amphoteric

A substance acting as an acid or a base because they have both a transferrable H+ and a lone pair.

Conjugate Pair

An acid that becomes a conjugate base in the reverse rxn, or a base that becomes a conjugate acid in the reverse rxn.

Strong Bases

1. Group 1 + OH

2. Ca, Sr, Ba + (OH)2

Strong Acids (6)

1. HCl

2. HI

3. HBr

4. HNO3

5. HClO4

6. H2SO4