1. Reactions in Aqueous Solution: Acids (section 4.3)

2. Build the following molecules using the plastic molecular models: Nitric Acid Perchloric Acid Hydrochloric Acid 3 or 4 water molecules

3. Find meanings for these: Amphoteric Bronsted-Lowry Aqueous Conjugate Hydronium

4. What is an ACID? Acid Characteristics: Taste: Indicator:

5. Acid Definitions: Bronsted-Lowry Arrhenius: Acids put H+ into water Bases put OH- into water Bronsted-Lowry Acids: “ADP” Acids donate protons Bases accept protons The Bronsted-Lowry definition is broader (more inclusive) than the Arrhenius definition.

6. Strong Acids Strong Acids Ionize completely in water. (100%) HCl (aq)  H + (aq) + Cl - (aq) The strong ACIDS are: 1. HCl 2. HBr 3. HI 4. HNO 3 5. H 2 SO 4 6. HClO 4 Give formula and name of the 6 strong acids.

7. Weak Acids Weak acids ionize partially in water. Less than 10%, usually much less than 1% ionization. General formula: Double arrow means reversible or it does not go to completion. The equilibrium includes both products AND reactants.

8. Strong Bases Strong Bases Ionize Completely in water. (100%) NaOH  Na + + OH - Always soluble hydroxides and Ca, Ba, Sr hydroxides are strong bases. Including: LiOH KOH Ca(OH) 2 Sr(OH) 2 Ba(OH) 2

9. Weak Bases Produce OH - ions by reacting with the water. Less than 100% ionized. NH 3 aq + H 2 O aq   NH 4 + aq + OH - aq Include: ammonia NH 3 amides R-NH 2

10. Acid-Base Reactions 3 TYPES: 1 Strong ACID - Strong BASE 2 Weak ACID – Strong BASE 3 Strong ACID – Weak BASE

11. Strong ACID + Strong BASE “Neutralization” Reaction The products are water, and an aqueous salt. (ions)

12. Weak Acid – Strong Base Weak acid only partially ionized. Strong base fully ionized. The H+ and OH- combine to form water. All H + gets “used up” (reacted). The anion (salt of the weak acid is not used up or reacted).

13. Strong ACID – Weak BASE The weak base gets “protonated” (H + added to the base) Ammonia and Hydrochloric Acid NH 3 + H + + Cl -  NH 4 + + Cl - Cross out the spectators Methylamine and Nitric Acid CH 3 NH 2 + H + + NO 3 -  CH 3 NH 3 + + NO 3 - Cross out the spectators

14. Johnny finding life a bore, drank some H 2 SO 4. Johnny's father, an M.D., gave him CaCO 3. Johnny's neutralized, it's true, But now he's full of CO 2.

15. Find meanings for these: Amphoteric Bronsted-Lowry Aqueous Conjugate Hydronium

16. Acid Base Titration An standardized acid (known concentration) may be used to determine the unknown strength of a base. (or visa- versa) Using an indicator (solution that changes color) you can know when the added solution is exactly equal to the unknown. this is known as the EQUILVALENCE POINT.

17. Acid-Base titration Objective: Determine the equivalence point. Equivalence point n OH - = n H + If 25.00mL of 0.0800M NaOH is needed to react with 10.00 mL of HCl. What is the molarity of HCl? 1.Write the reaction 2.Use M 1 V 1 =M 2 V 2 In this case the formula could be written M OH - V OH - = M H + V H +