2.  Binary acid (i.e. H & a non-metal) ◦ the prefix hydro is used ◦ the root of the anion is used ◦ the suffix -ic is used ◦ the word acid is used as the second word of the name  Example ◦ HCl = hydrochloric acid ◦ HBr = hydrobromic acid ◦ HI = hydroiodic acid ◦ HF = hydrofluoric acid

3.  Polyatomic acids ◦ oxyacids: (acids with oxygen in the polyatomic anion) ◦ change suffix of –ate with -ic OR ◦ change suffix -ite to -ous ◦ These acids have the general formula H a X b O c where X = an element other than Hydrogen or Oxygen  Examples ◦ HNO 3 (nitrate) (-ate  -ic) ◦ HSO 3 (sulfite) (-ite  -ous) ◦ H 2 SO 4 (sulfate) (-ate  -ic) Nitric acid Sulfurous acid Sulfuric acid

4.  Strong Acid: ◦ an acid that completely dissociates into ions. ◦ (100 molecules of HCl → 100 H + ions)  The six strong acids to be memorized ◦ HCl ◦ HBr ◦ HI ◦ H 2 SO 4 ◦ HNO 3 ◦ HClO 4 (Perchloric acid)

5.  Strong Bases ◦ a base that completely dissociates into ions. ◦ (100 formula units of NaOH → 100 OH - ions) ◦ When combined with the OH _ (hydroxide) ion, elements found in group 1 (IA) and 2 (IIA) form strong bases  Examples ◦ KOH ◦ CsOH ◦ Ba(OH) 2 ◦ Ca(OH) 2

6.  H + (Hydrogen ion) indicates strong acid ◦ pH scale with a value of 2 or less  OH - (Hydroxide ion) indicates strong base ◦ pH scale with a value of 12 or more

7.  Read p.271-273 Questions: P.273 #’s 29-33

8.  Current Assumption ◦ When strong acid and strong base are combined, all H + and OH - ions join to form HOH (H 2 O)

9.  Neutralization reaction is a double displacement  Example ◦ For NaOH and HCl  Predict the products of the reaction  balance the equation ◦ NaOH (aq) + HCl (aq)  NaCl + HOH ◦ Use solubility rules to confirm whether each product will be aqueous, solid or liquid ◦ NaOH (aq) + HCl (aq)  NaCl ( aq) + HOH (l) ◦ Write the total ionic equation, showing all ions that are in solution

10.  Na + (aq) + OH - (aq) + H + (aq) + Cl - (aq) → Na + (aq) + Cl - (aq) + H 2 O (l)  Cancel the spectator ions and write the net ionic equation  OH - (aq) + H + (aq) → H 2 O (l)

11.  Example ◦ Write the molecular, ionic, net ionic equations for  Sulfuric acid & potassium hydroxide H 2 SO 4 (aq) + KOH (aq) → K 2 SO 4 + HOH 2 H + (aq) + SO 4 2- (aq) + 2 K + (aq) + 2 OH - (aq) → 2 K + (aq) + SO 4 2- (aq) +2 HOH (l) 2 H + (aq) + 2 OH - (aq) → + 2 HOH (l) Simplify H + (aq) + OH - (aq) → + HOH (l) (aq)(l) 22

12.  Recall: ◦ Concentration is calculated as moles per litre  mol/L MM ◦ [NaOH] refers to the concentration of sodium hydroxide  Equation ◦ [ ] =mol/L

13.  In the reaction of 35.0 mL of liquid drain cleaner containing NaOH, 50.08 mL of 0.409 mol/L HCl must be added to neutralize the base. What is the concentration of the base in the cleaner? ◦ Write a balanced equation and the chart NaOH (aq) + HCl (aq) → H 2 O (l) + NaCl (aq) Mm mol V m [ ] 0.0350L0.05008L 0.409M 0.0205mol 0.586M

14.  Calculate the volume of 0.256 mol/L Ba(OH) 2 that must be added to neutralize 46.0 mL of 0.407 mol/L HClO 4. Ba(OH) 2(aq) + 2 HClO 4(aq) → BaCl 2(aq) + 2H 2 O (l) Mm mol V m [ ] 0.256M0.407M 0.0460L 0.0187mol0.00935mol 0.0365L

15.  P. 614 ◦ #’s 30-31  P. 616 ◦ #’s 32-33, 36-37  Aqueous Reactions Worksheet #1 ◦ #’s 5-7  Aqueous Reactions Worksheet #2