Strong Acids

HNO₃

H₂SO₄

HCL

HBR

HI

HCLO₄

*sometimes H₃PO₄

Strong Bases

LiOH

NaOH

KOH

RbOH

CsOH

Ca(OH)2

Sr(OH)2

Ba(OH)2

*NH3 = WEAK

arrhenius acid

produces and H+ ion (H3O+)

arrhenius Base

produces OH- ions

Bronsted Lowery Acid

donates a proton (loses H+)

Bronsted Lowry Base

accepts a proton (accepts H+)

Lose of H ions in stronger acids and stronger bases

STRONG acid lose H ions more quickly

STRONGER base hold onto H ions more strongly

Lewis Acid

e- pair donor

Lewis base

e- pair donor

characteristics of Bronsted Lowry rxns

-acid base rxns are not restricted to aqueous solutions

-species can be amphoteric depending on what the other reactant is

streght of attraction in strong/weak acids

-strong acid-weak attraction (completely ionize)

-weak acid-strong attraction (partial ionization)

*stronger acids on products equilib pushes towards reactants

Why is HF not a stron acid?

due to its extremely HIGH electronegativity (does not want to dissociate)

Polarity's effect on bond strenght

-more polar -more pulling e- towards X ( H-X bond) therefore H+ able to leave and dissociate

(strong acids do this easily)

-larger X weaker the bond and greater the acidity

Acidity as you go down a column

Radius INC and H-X bond strength DEC 

bonds become weaker and weaker

INC in acidity

Larger Ka

= smaller pKa

STRONGER acid

Acidity as you go across a row

polarity H-X bonds becomes dominant factor

as electroneg INC polarity INC and acid strenght INC

H3N < H20 < HF

Acidic strength of Oxoacids

H-O-Y....

*polarity depends on rest of molecule

-H alwasy bonded to O

-if Y has LARGE electronegativity O-H bond relativly polar and acidc strengh = greater

HOCl > HOBr > HOT

(CL more electro neg than Br than T)

finding pH of mixtures of Acids

use the stronger acid (neglect the weaker one)