1. I. Introduction to Acids & Bases (p. 453 - 473) Ch. 15 & 16 - Acids & Bases

2. 15-1 Properties of Acids and Bases  electrolytes  turn litmus red  sour taste  react with metals to form H 2 gas  slippery feel  turn litmus blue  bitter taste ChemASAP  vinegar, milk, soda, apples, citrus fruits  ammonia, lye, antacid, baking soda

3. Properties of Acids  Aqueous Solutions of Acids have a sour taste. Citric Acid – Fruit  Acids change the color of Acid/Base indicators. Litmus paper, pH paper, indicators…

4. Properties of Acids  Some metals react with metals to release hydrogen gas. Use activity series to predict, pg. 266  Acids react with bases to produce “salts” and water. “Neutralization” HCl(aq) + NaOH(aq)  NaCl(aq) + H 2 O(l)

5. Properties of Acids  Acids conduct an electric current. “Electrolytes”

6. Nomenclature  “Binary Acids” – an acid that contains only two different elements. HCl HBr HF HI H 2 S

7. Nomenclature  How to name? Binary acids begin with “hydro-” Root name of the second element. Binary acid ends in “-ic”

8. Nomenclature  “Oxyacids”-an acid that is a compound of H and O + another element. H 2 SO 4 HNO 3 HC 2 H 3 O 2 Name based on root of anion.

9. Industrial acids  Know the common uses of the industrial acids on pgs. 456-457

10. Properties of Bases  Aqueous Solutions of bases taste bitter. Ex. Soap.  Bases change the color of acid/base indicators. Ex. pH paper, litmus paper, indicators…

11. Properties of Bases  Feel slippery. Soap.  Bases react with acids to produce salts and water. “neutralization”  Bases conduct electric current. “electrolytes”

12. Definitions  “Arrhenius Acid” – a chemical compound that increases the concentration of H+ ions in aqueous solution.  “Arrhenius Base” – a chemical compound that increases the concentration of OH- ions in aqueous solution.

13. Definitions  Arrhenius - In aqueous solution… HCl + H 2 O  H 3 O + + Cl – AcidsAcids form hydronium ions (H 3 O + ) H HHHH H Cl OO – + acid

14. Definitions  Arrhenius - In aqueous solution… BasesBases form hydroxide ions (OH - ) NH 3 + H 2 O  NH 4 + + OH - H H H H H H N NO O – + H H H H base

15. Definitions  Know Strong Acids and Bases and Weak Acids and Bases Pg. 460 and 461

16. ø 15-2 Brønsted-Lowry Acids and Bases  Brønsted-Lowry HCl + H 2 O  Cl – + H 3 O + AcidsAcids are proton (H + ) donors. BasesBases are proton (H + ) acceptors. conjugate acid conjugate base baseacid

17. Definitions H 2 O + HNO 3  H 3 O + + NO 3 – CBCAAB

18. Definitions - can be an acid or a base.  Amphoteric - can be an acid or a base. NH 3 + H 2 O  NH 4 + + OH - CACBBA

19. Definitions F - H 2 PO 4 - H2OH2O HF H 3 PO 4 H 3 O +  Give the conjugate base for each of the following: - an acid with more than one H +  Polyprotic - an acid with more than one H +

20. Definitions Br - HSO 4 - CO 3 2- HBr H 2 SO 4 HCO 3 -  Give the conjugate acid for each of the following:

21. B. Definitions  Lewis AcidsAcids are electron pair acceptors. BasesBases are electron pair donors. Lewis base Lewis acid

22. C. Strength  Strong Acid/Base 100% ionized in water strong electrolyte - + HCl HNO 3 H 2 SO 4 HBr HI HClO 4 NaOH KOH Ca(OH) 2 Ba(OH) 2

23. C. Strength  Weak Acid/Base does not ionize completely weak electrolyte - + HF CH 3 COOH H 3 PO 4 H 2 CO 3 HCN NH 3