Reaction Predictions

Acids and Bases

Acids

Arrhenius definition Produces H+ ions in aqueous solutions

Some completely dissociate, others partially dissociate in solutions

1) Strong Acids

Completely dissociate into ions in an aqueous solution, only a few acids

Strong electrolytes

[acid] = [ion concentration] in solution, no molecules left

HCl, HBr, HI, HNO3, H2SO4, HClO4 (KNOW THEM!!!)

Ex. HBr

Ex. 1 HBr

2) Weak Acids

Partially dissociate in an aqueous solution

Weak electrolytes

Some molecules break up into ions, other molecules stay together in solution

[weak acid] ≠ [ion]

Ex. CH3COOH

Ex. 2 CH3COOH

Multiple Ionizations

Some acids can donate more than one H+ ion and go through multiple ionizations

H3PO4 and H2SO4

How do we recognize acids in chemical

formulas? 1) H+ ion appears 1st in chemical formula.

Ex. HCl, H2SO4

2) H atom location in structural formula Usually at the end Indicates atom bonded to H Ex. CH3COOH

Bases

Arrhenius definition Produces hydroxide (OH-) ions in aqueous

solutions

Some completely dissociate, others partially dissociate in solutions

1) Strong Bases

Completely dissociate into ions in aqueous solutions

Strong electrolytes, mainly ionic compounds

[strong base] = [ion] in solution

Most Group IA and IIA metals combined with hydroxide ion LiOH, NaOH, KOH, RbOH, CsOH, Mg(OH)2 ,

Ca(OH)2 , Sr(OH)2 , Ba(OH)2 –KNOW THEM ! ! !

2) Weak Bases

Partially dissociate in an aqueous solution

Weak electrolytes, typically molecular compounds

Some molecules break up into ions, other molecules stay together in solution

[weak base] ≠ [ion]

Do not necessarily have hydroxide (OH-) ion in chemical compound

React with water and produce the hydroxide ion as a product.

2) Weak Bases (cont.)

Ex. NH3

How do we recognize bases in a chemical

formula? 1) Ionic Compound with metal cation + hydroxide (OH-) anion

Strong base

2) Molecular compound has OH covalently bound, not existing as OH- ion

Consisting of nonmetals Rely on chemical equation to show ionization Most common weak bases: ammonia (NH3) and

amines (R-NH2)

Neutralization Reactions

Acids and bases cancel each other out, “neutralize” or even out the solution

ACID + BASE SALT + H2O

How do we determine when a solution is neutral? Check pH with litmus paper, color changes Acid/base indicator– compound where its color

is influenced by the [H+] and [OH-] in solution

Special Net-Ionic Equations with Acids

and Bases

NH3

Produces ammonium ion when combined with an acid, slightly basic

Acid-Base reaction, but no OH- ion released

HA + NH3 NH4+