2B: Acids and Bases

arrhenius acis

produces H+ ions in aqueous solutions

arrhenius bases

produces OH- ions in an aqueous solution

limitations of arrhenius theory

1. doesnt explain why certain subspaces dissolve to form basic soln BUT dont contain OH ions

2. same as above for certian acidic solns

3. does not explain acid-base rxns outside aqueous solution

bronsted lowry acid

H+ donor

bronsted lowry base

proton acceptor

lewis acid

electron pair acceptor

lewis base

electron pair donor

amphoteric substances

can act as an acid or a base (ex. H20)

Autoionization of H2O

• water is amphoteric

• dissociates into ions

dissociation of strong acids/ bases

St. A/B dissociate fully/ are strong electrolytes

wk A/B’s and dissociation

partial dissociation/ weak electrolytes

High Ka = __[H3O+] = __Acid = __pKa

high, strong, low

low Ka = __ dissociation = weaker

less

anions are (neutral/ basic/ acidic)

neutral / basic

cations are (neutral/ basic/ acidic)

acidic

salts that yield neutral solutions

anion of St Acid/ cation of St. Base

salts that yield basic solutions

anion of Wk. Acid/ Cation of St. Base

salts w conj acids and bases

anion of W acid/ cation of WB

polyprotic acids

several protons which could be donates

leveling effect

St. Acids all exhibit same strength in water