1. Review of
Acids

2. HCl Strong Acid HCl  H+ + Cl-
0.10 M 0.10 M
pH = -Log[H+] = No ICE
HF Weak Acid HF ⇌ H F-
I 0.10 M 0 0
C x x x
E x x x
small Ka
x2 = 3.5 x x = M
0.10
pH = -Log[ ] = 2.23

3. NaOH Strong Base NaOH  Na+ + OH-
0.20 M M
pOH = -Log[OH-] = No ICE
NH3 Weak Base NH3 + H2O ⇌ NH4+ + OH-
I 0.20 M
C x x x
E x x x
small Kb
x2 = Kb = Kw = x = x 10-5
Ka x
x = M
pOH = -Log[ ] = 2.73
pH = 11.27

4. CaO Basic Anhydride CaO + H2O  Ca(OH)2
SO2 Acid Anhydride SO2 + H2O  H2SO3
Salts
NaCl neutral salt NaCl  Na Cl-
KCN basic salt
CN H2O ⇌ HCN OH-
hydrolysis
NH4Cl acidic salt
NH H2O ⇌ H3O NH3
hydrolysis

5. Fe(H2O)63+ ⇌ H+ + Fe(H2O)5(OH)2+ hydrolysis- copy off chart!
FeCl3 acidic salt
Fe(H2O) ⇌ H+ + Fe(H2O)5(OH)2+
hydrolysis- copy off chart!
Know the pH scale
HCl HF NaCl NH NaOH
Assuming 1M

6. Buffers Maintain the pH
Weak Acid Salt ( conjugate)
HF KF
HF ⇌ H F-
High Low High
Indicator Change colour with pH
HInd ⇌ H Ind-
Acid Low Basic

7. Indicators Change colour with pH
methyl red
HInd ⇌ H Ind-
red yellow page 7
@ trans pt [HInd] = [Ind-] colour is orange
and Ka = [H+]
pH = = 5.4 2
Ka = [H+] = = 4 x 10-6

8. Acid Rain SO2 NO2 pH  5
Normal Rain CO2 pH = 6
Amphriprotic H2C2O4 acid
HC2O4- ampriprotic
C2O42- base
Is HC2O4- an acid or base?
Ka (HC2O4-) = 6.4 x 10-5
Kb (HC2O4-) = 1.0 x = 1.7 x
5.9 x acid

9. Is NH4CH3COO an acid or base?
Ka (NH4+) = 5.6 x 10-10
Kb (CH3COO-) = 1.0 x = x 10-10
1.8 x neutral

10. 100. 0 mL 0. 100 M H2SO4 is mixed with 220. 0 mL of 0. 100 M NaOH
100.0 mL M H2SO4 is mixed with mL of M NaOH. What is the pH of the resulting solution?
H2SO NaOH
L x mole L x mole
1 L L
I mole mole
C mole mole
E 0 mole mole
[NaOH] = mole = M
0.320 L pOH = 2.20
pH =

11. Complete the reaction and state if the reactants or products are favoured.
HCO HSO3-
Base Acid
HCO HSO3- ⇌ H2CO SO32-
weaker weaker stronger stronger base acid acid base
Reactants are favoured

12. Know the Equations
E H2O ⇌ H+ + OH-
Kw = [H+][OH-] = 1.0 x
pH = -Log[H+] pOH = -Log[OH-]
[H+] = 10-pH [OH-] = 10-pOH
pH + pOH = pKw = @ 25 oC
@ other temperatures pure water is always neutral
& [H+] = [OH-] & pH = pOH  7