1. I. Introduction to Acids & Bases Ch. 19 – Acids & Bases

2. Review – Acid Nomenclature

4. Review – Naming Acids  HCl H2SH2S  H 2 SO 4  H 2 SO 3  HNO 3  HNO 2  HBr  Hydrochloric acid  Hydrosulfuric acid  Sulfuric acid  Sulfurous acid  Nitric acid  Nitrous acid  Hydrobromic acid

5. A. Properties  electrolytes  turn litmus red  sour taste  react with metals to form H 2 gas  slippery feel  turn litmus blue  bitter taste  vinegar, milk, soda, apples, citrus fruits  ammonia, lye, antacid, baking soda

6. B. Definitions HF H 3 PO 4 H 2 SO 4 H +  Monoprotic – an acid with one H + – an acid with more than one H +  Polyprotic – an acid with more than one H + Diprotic – an acid with 2 H +Diprotic – an acid with 2 H + Triprotic – an acid with 3 H +Triprotic – an acid with 3 H + monoprotic triprotic diprotic polyprotic

7. B. Definitions  Arrhenius HCl + H 2 O  H 3 O + + Cl – Acids contain hydrogenAcids contain hydrogen AcidsAcids form hydronium ions (H 3 O + ) in aqueous solution H HHHH H Cl OO – + acid

8. B. Definitions  Arrhenius Bases contain a hydroxide groupBases contain a hydroxide group BasesBases form hydroxide ions (OH - ) in aqueous solution NaOH  Na + + OH - base H2OH2O

9. B. Definitions  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

10. B. Definitions  Brønsted-Lowry HBr + NaOH  NaBr + H 2 O Conjugate AcidsConjugate Acids are the result after a base accepts a hydrogen ion Conjugate BasesConjugate Bases are the result after an acid donates a hydrogen ion conjugate acid conjugate base baseacid

11. B. Definitions H 2 O + HNO 3  H 3 O + + NO 3 – CBCAAB H 2 O + NH 3  NH 4 + + OH - CACB B A – can be an acid or a base  Amphoteric – can be an acid or a base

12. B. 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 +

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

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

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

16. 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

17. Ch. 19 – Acids & Bases II. pH (p. 644 – 658)

18. A. Ionization of Water H 2 O + H 2 O H 3 O + + OH - Self-Ionization of Water

19. Ion Product Constant for Water For all aqueous solutions, the product of the hydrogen-ion concentration and the hydroxide-ion concentration equals 1.0 x 10 -14 The ion production of water, K w = [H 3 O + ][OH – ] Pure water contains equal concentrations of H + and OH – ions, so [H 3 O + ] = [OH – ] A. Ionization of Water K w = [H 3 O + ][OH - ] = 1.0  10 -14

20. A. Ionization of Water  Find the hydroxide ion concentration of 3.0  10 -2 M HCl. [H 3 O + ][OH - ] = 1.0  10 -14 [3.0  10 -2 ][OH - ] = 1.0  10 -14 [OH - ] = 3.3  10 -13 M HCl → H + + Cl - 3.0  10 -2 M

21. A. Ionization of Water  Find the hydronium ion concentration of 1.4  10 -3 M Ca(OH) 2. [H 3 O + ][OH - ] = 1.0  10 -14 [H 3 O + ][2.8  10 -3 ] = 1.0  10 -14 [H 3 O + ] = 3.6  10 -12 M Ca(OH) 2 → Ca 2+ + 2 OH - 1.4  10 -3 M 2.8  10 -3 M

22. pH = -log[H 3 O + ] B. pH Scale 0 7 INCREASING ACIDITY NEUTRAL INCREASING BASICITY 14 pouvoir hydrogène (Fr.) “hydrogen power”

23. B. pH Scale pH of Common Substances

24. B. pH Scale pH = -log[H 3 O + ] pOH = -log[OH - ] pH + pOH = 14

25. B. pH Scale  What is the pH of 0.050 M HNO 3 ? pH = -log[H 3 O + ] pH = -log[0.050] pH = 1.30 Acidic or basic? Acidic

26. B. pH Scale  What is the pH of 0.050 M Ba(OH) 2 ? [OH-] = 0.100 M pOH = -log[OH - ] pOH = -log[0.100] pOH = 1.00 pH = 13.00 Acidic or basic? Basic

27. B. pH Scale  What is the molarity of HBr in a solution that has a pOH of 9.60? pH + pOH = 14 pH + 9.60 = 14 pH = 4.40 Acidic pH = -log[H 3 O + ] 4.40 = -log[H 3 O + ] -4.40 = log[H 3 O + ] [H 3 O + ] = 4.0  10 -5 M HBr

28. C. pH Worksheet #6 A swimming pool has a volume of one million liters. How many grams of HCl would need to be added to that swimming pool to bring the pH down from 7.0000 to 4.0000? (Assume the volume of the HCl is negligible) 7 = -log[H+] -7 = log[H+] [H+] = 1 x 10 -7 M -4 = log[H+] [H+] = 1 x 10 -4 M = 100 mol H+ 1,000,000L Sol’n 1x10 -4 mol H+ 1 L soln = 0.1 mol H+ 1,000,000L Sol’n 1x10 -7 mol H+ 1 L soln

29. C. pH Worksheet #6 100 mol H+ – 0.1 mol H+ = 99.9 mol HCl = 3642 g HCl 99.9 mol HCl 36.46 g HCl 1 mol HCl A swimming pool has a volume of one million liters. How many grams of HCl would need to be added to that swimming pool to bring the pH down from 7.0000 to 4.0000? (Assume the volume of the HCl is negligible)

30. D. pH Sig Figs  For the pH, the number of sig figs is shown by the # of decimal places [H+] = 2.26 x 10 -4 M =>  For the molarity from the pH, check decimal places in the pH pH = 4.25 => pH = 3.646 5.6 x 10 -5 M