1. WARM UP
For the reaction Br2(aq) + I2(aq) IBr(aq), equilibrium concentrations are .108M for Br2, .34M for I2, and .472M for IBr. What is K? Is the reaction product-favored or reactant-favored?
Using the same reaction equation, if you begin with 2.5 M of each reactant, and have 1.1 M remaining at equilibrium, how much product would you have formed?

2. Acid/Base Ionization

3. Strong vs. Weak Strong acids and bases
Completely ionize (dissociate) in water
HCl  H+ + Cl-
Every bit of reactant becomes acid or base
2 M HCl = 2M H+ (acid)

4. Strong vs. Weak Weak acids and bases Do not completely ionize
Equilibrium between reactant and products
CH3COOH H+ + CH3COO-
Smaller than expected amount of acid or base
Percent ionization
Ratio of H+ / CH3COOH
K value
Ka (acids) or Kb (bases)

5. Weak Acids/Bases
Calculate K for the ionization if you know concentrations at equilibrium
Ka x Kb = Kw
Greater the K value, stronger the acid or base
More H+ or OH- product
Ex: NH3 + H2O NH4+ + OH-
Kb = [NH4+] [OH-]
[NH3]

6. ICE and K Calculating K Ex: .1 M HCOOH (pH = 2.39)
You often only know pH and Initial concentration
Equilibrium[H+] or [OH-] determined by pH
H+ = 10-pH OH-=10-pOH pH + pOH = 14
ICE Table to get values for K
Ex: .1 M HCOOH (pH = 2.39)

7. WARM UP
A .100 M solution of chloroacetic acid (ClCH2COOH) has a pH of Calculate the Ka for chloroacetic acid.