Review of Acids

HCl Strong Acid HCl  H+ + Cl- 0.10 M 0.10 M pH = -Log[H+] = 1.0 No ICE HF Weak Acid HF ⇌ H+ + F- I 0.10 M 0 0 C x x x E 0.10 - x x x small Ka x2 = 3.5 x 10-4 x = 0.005916 M 0.10 pH = -Log[0.005916] = 2.23

NaOH Strong Base NaOH  Na+ + OH- 0.20 M 0.20 M pOH = -Log[OH-] = 0.70 No ICE NH3 Weak Base NH3 + H2O ⇌ NH4+ + OH- I 0.20 M 0 0 C x x x E 0.20 - x x x small Kb x2 = Kb = Kw = 1.0 x 10-14 = 1.786 x 10-5 0.20 Ka 5.6 x 10-10 x = 0.001890 M pOH = -Log[0.001890] = 2.73 pH = 11.27

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 NH4+ + H2O ⇌ H3O+ + NH3 hydrolysis

Fe(H2O)63+ ⇌ H+ + Fe(H2O)5(OH)2+ hydrolysis- copy off chart! FeCl3 acidic salt Fe(H2O)63+ ⇌ H+ + Fe(H2O)5(OH)2+ hydrolysis- copy off chart! Know the pH scale 0 7 14 HCl HF NaCl NH3 NaOH Assuming 1M

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

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 = 4.8 + 6.0 = 5.4 2 Ka = [H+] = 10-5.4 = 4 x 10-6

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 10-14 = 1.7 x 10-13 5.9 x 10-2 acid

Is NH4CH3COO an acid or base? Ka (NH4+) = 5.6 x 10-10 Kb (CH3COO-) = 1.0 x 10-14 = 5.6 x 10-10 1.8 x 10-5 neutral

100. 0 mL 0. 100 M H2SO4 is mixed with 220. 0 mL of 0. 100 M NaOH 100.0 mL 0.100 M H2SO4 is mixed with 220.0 mL of 0.100 M NaOH. What is the pH of the resulting solution? H2SO4 + 2NaOH 0.1000 L x 0.100 mole 0.2200 L x 0.100 mole 1 L 1 L I 0.0100 mole 0.0220 mole C 0.0100 mole 0.0200 mole E 0 mole 0.0020 mole [NaOH] = 0.0020 mole = 0.00625 M 0.320 L pOH = 2.20 pH = 11.80

Complete the reaction and state if the reactants or products are favoured. HCO3- + HSO3- Base Acid HCO3- + HSO3- ⇌ H2CO3 + SO32- weaker weaker stronger stronger base acid acid base Reactants are favoured

Know the Equations E + H2O ⇌ H+ + OH- Kw = [H+][OH-] = 1.0 x 10-14 pH = -Log[H+] pOH = -Log[OH-] [H+] = 10-pH [OH-] = 10-pOH pH + pOH = pKw = 14 @ 25 oC @ other temperatures pure water is always neutral & [H+] = [OH-] & pH = pOH  7