1. Acids and Bases

2. Types of Acids Binary Acids (contains H & 1 other element) HCl-hydrochloric acid Oxyacids (contain H, O, & other elements) H 2 SO 4 H 2 SO 3

3. Common Acids Sour milk (lactic acid) Vinegar (acetic acid) Carbonated beverages (phosphoric acid) Lemons, oranges (citric acid) Apples (malic acid) Grape Juice (tartaric acid)

4. Sulfuric Acid Most commonly used product in the world Petroleum Automobile batteries Dehydration agent Metallurgy Refining

5. Nitric Acid Stains proteins yellow Suffocating odor Stains skin Causes burns Explosives Rubber Plastics Dyes Pharmaceuticals

6. Phosphoric Acid Manufacturing fertilizers for plants and animal feed Flavoring agent in beverages Cleaning agent for dairy equipment

7. Hydrochloric acid Produced in the stomach Cleaning agent Maintain acidity in pools

8. Common Properties of Acids Sour taste Produce hydronium H 3 O + ions Change the color of acid-base indicators React with active metals to release hydrogen gas React with bases to produce salts and water Conduct electric current

9. Bases

10. Common Bases Lye (sodium hydroxide) Milk of magnesia (magnesium hydroxide) Antacids (aluminum hydroxide)

11. Common Properties of Bases Taste bitter Produce hydroxide OH - ions Change the color of acid-base indicators Feel slippery React with acids to produce salts and water Conduct electric current

12. Specific Definitions of Acids/Bases

13. Arrhenius Acids and Bases Arrhenius acid-increases H+ ions (H 3 O+) H 2 SO 4 + H 2 O  H 3 O + +HSO 4 - Arrhenius base-increases OH- ions Ca(OH) 2  Ca +2 + 2OH -

14. Weak/Strong Weak acid-weak electrolyte (end in -COOH) Strong acid-ionizes completely, strong electrolyte (HCl) Alkaline-base completely dissociates in water to yield OH- ions NaOH  Na + + OH - Strong bases-completely dissociates, strong electrolyte (end in OH)

15. Bronsted-Lowry Bronsted-Lowry Acid-proton donor Bronsted-Lowry Base-proton acceptor HCl + NH 3  NH 4 + + Cl - Monoprotic acid-donates one proton HCl Diprotic acid-donates two protons H 2 SO 4 Triprotic acid-donates three protons H 3 PO 4

16. Conjugate Acids and Bases Conjugate base-the species that remains after a Bronsted-Lowry acid has given up a proton HF + H 2 O  F - + H 3 O + Acid Conj. Base Conjugate acid-the species that is formed when a Bronsted-Lowry base gains a proton HF + H 2 O  F - + H 3 O + Base Conj. Acid

17. Strength of Acid/Conj. Base Strong acid  weak conjugate base Weak acid  strong conjugate base

18. Amphoteric compound-any species that can react as either and acid or a base Neutralization-the reaction of hydronium ions and hydroxide ions to form water molecules and salt Self-ionization of water H 3 O + + OH -  2H 2 O or H 2 0 + H 2 O  H 3 O + + OH - Salt-an ionic compound composed of a cation from a base and an anion from an acid

19. Titration Practice Problems

20. Ex 1 A 30.mL volume of HCl is titrated with 23mL of 0.20M NaOH. What is the molarity of HCl in this solution?

21. Answer 0.15M

22. Ex 2 A 26mL volume of NaOH is titrated with 23mL of 0.20MHCl. What is the molarity of NaOH in this solution?

23. Answer 0.18M

24. Ex 3 A 40.mL volume of H 2 SO 4 is titrated with 38mL of 0.24M NaOH. What is the molarity of H 2 SO 4 in this solution?

25. Answer 0.11M