Acids and Bases mini unit

Arrhenius theory

bases dissociate to yield OH^-, acids dissociate to yield H⁺ , not as complete as the Bronsted - Lowry theory

Bronsted Lowry theory

Acids are proton donors (give away H⁺ ions), Bases are proton acceptors (receive H⁺ ion)

Amphiprotic

a substance that can act either as an acid or base (either donate or accept H+ ions). One such substance is water

Conjugate base

an acid that lost its hydrogen ion. (an acid on one side will be the conjugate base on the other side)

Conjugate acid

A base on the other side of th reaction that gains a proton (base and conjugate acid are a pair)

Neutral

pH of 7

Weakly Acidic

pH of 3-6

Strongly Acidic

pH of 0-3

Weakly Alkali (Weak base)

pH of 8-11

Strongly Alkali (strong base)

pH of 11 - 14

Lewis theory

Acids are electron acceptors, Bases are electron donors

Perchloric Acid

HClO₄

Hydrochloric acid

HCl

Hydrobromic Acid

HBr

Hydroiodic acid

HI

nitric acid

HNO₃

Sulfuric Acid

H₂SO₄

6 Strong Acids

Perchloric acid, hydrochloric acid, hydrobromic acid, hydroiodic acid, nitric acid, sulfuric acid

Lithium hydroxide

LiOH

Sodium Hydroxide

NaOH

Potassium hydroxide

KOH

Calcium hydroxide

Ca(OH)₂

Strontium hydroxide

SR(OH)₂

Barium Hydroxide

Ba(OH)₂

6 strong bases

Lithium hydroxide, sodium hydroxide, potassium hydroxide, calcium hydroxide, strontium hydroxide, barium hydroxide

Sulfurous Acid

H₂SO₃

Methanoic Acid

HCO₂H

Phosphoric Acid

H₃PO₄

Nitrous Acid

HNO₂

Hydrofluoric Acid

HF

5 Weak Acids

Sulfurous Acid, Methanoic Acid, Phosphoric Acid, Nitrous Acid, Hydrofluoric Acid

Ammonia

NH₃

ethylamine

C₂H₅NH₂

pyridine

C₅H₅N

aniline

C₆H₅NH₂

ammonium hydroxide

NH₄OH

5 Weak Bases

ammonia, ethylamine, pyridine, aniline, ethylamine,

Acid and base neutralization

forms salt and water

neutralization of acid and carbonates/hydrogen carbonates

salt, carbon dioxide, and water

neutralization of acid with ammonia

ammonium salt

Acid reaction with metals

produce hydrogen and salt