1. Acids and Bases Chapter 19

2. Review Electrolyte A substance that conducts an electrical current when melted or in solution Ionic compounds Acids and Bases

3. Acid-Base Theories Different definitions of acids and bases Arrhenius Bronsted-Lowry

4. Arrhenius Acid Compounds that ionize to produce hydrogen ions (H + ) in aqueous solutions Examples: HCl, HBr, H 2 SO 4, CH 3 COOH H + (aq) = H 3 O + *Note: CH 3 COOH is an organic acid Acidic H

5. Arrhenius Base Compounds that ionize to produce hydroxide ions (OH - ) in aqueous solutions Examples: KOH, NaOH, LiOH *Note: CH 3 OH is not a base, it’s an organic alcohol

6. Bronsted-Lowry (alternate) Acid Hydrogen ion donor Examples: HCl, HBr, H 3 O + Base Hydrogen ion acceptor Examples: H 2 O, NH 3

7. Acid-Base Theories Arrhenius Bronsted- Lowry

8. Properties of Acids & Bases Acids - Taste Sour Bases - Taste Bitter, Feel Slippery Will change color of acid – base indicator Can be strong or weak electrolytes in an aqueous solution

10. Ionization Electrolytes will dissociate into ions when dissolved in water Strong Electrolytes will completely dissociate Weak Electrolytes will only partially dissociate

11. Ionization HCl (s)  H + (aq) + Cl - (aq) HNO 3(s)  H + (aq) + NO 3 - (aq) NaOH (s)  Na + (aq) + OH - (aq) KOH (s)  K + (aq) + OH - (aq)

12. Polyprotic Acids Acids that have more than one H Can release more than one H + into solution Examples:H 2 SO 4, H 3 PO 4 H 2 SO 4(s)  2H + (aq) + SO 4 2- (aq) Bases can also release more than one OH - into solution Mg(OH) 2(s)  Mg +2 (aq) + 2OH - (aq)

13. Ionization of Water Water can be split into 2 ions H + and OH - Ionization of Water H 2 O  H + + OH - H 2 O + H 2 O  H 3 O + + OH -

15. Neutral Solutions For neutral solutions [H + ] = [OH - ] For all aqueous solutions [H + ] * [OH - ] = 1.0 x 10 -14 [ ] means concentration

16. Measuring Acidity (Alkalinity) Traditionally we measure [H + ] pH = -log [H + ] Neutral solution [H + ] = 1.0 x 10 -7 pH = 7

17. Acidity Acidic SolutionspH < 7.0 [H + ] > 1.0 x 10 -7 Basic SolutionspH > 7.0 [H + ] < 1.0 x 10 -7

19. Measuring pH Litmus paper Red in acid Blue in base pH paper pH Meter Acid – Base Indicators (Table M)

20. Table M

22. Changes in pH pH increases by 1 for every decrease in [H + ] by a magnitude of 10 [H + ]pH 1.0*10 -7 7 1.0*10 -8 8 1.0*10 -9 9 1.0*10 -10 10

23. pH Changes

27. Neutralization Acid + Base  Water + Salt Double Replacement Reaction HA + BOH  HOH + BA

28. Neutralization Examples: HCl + NaOH  H 2 O + NaCl HNO 3 + LiOH  H 2 O + LiNO 3 H 2 SO 4 + 2KOH  2 H 2 O + K 2 SO 4