1. Acid/Base

2. Properties of Acids ·Sour taste, Change color of dyes, Conduct electricity in solution, React with many metals, React with bases to form salts

3. Properties of Bases ·Bitter taste, Feel slippery, Change color of dyes, Conduct electricity in solution, React with acids to form salts

4. Arrhenius ·Acids: release H + or H 3 O + in solution ·Bases: release OH - in solution

5. Arrhenius ·Acid: HA --> H + + A - ·HCl --> H + + Cl - ·Base: MOH --> M + + OH - ·NaOH -->Na + + OH -

6. Bronsted-Lowry ·Acid: Proton donor ·Base: Proton Acceptor

7. Bronsted-Lowry ·HA + H 2 O --> H 3 O + + A - ·HI + H 2 O --> H 3 O + + I - ·Acid Base CA CB ·NH 3 + H 2 O --> NH 4 + + OH - ·Base Acid CA CB

8. Lewis Acid/Base ·Acid: Electron Acceptor ·Base: Electron Donor

9. Lewis Acid/Base ·H 3 N: + BF 3 --> H 3 N-BF 3 ·Base Acid Neutral

10. Common Names ·H + Hydrogen ion ·H 3 O + Hydronium ion ·H - Hydride ion ·OH - Hydroxide ion ·NH 3 Ammonia ·NH 4 + Ammonium ion

11. Amphoterism ·Can act like an acid or a base ·Can donate or accept protons

12. Define acids & bases by each of the three methods

13. Naming Acids ·All acids are H-anion ·If the anion is: ·-ides  hydro___ic acids ·-ates  ___ic acids ·-ites  ___ous acids

14. Naming Bases ·Almost all bases are metal hydroxides ·Name by normal method ·Ammonia (NH 3 ) as well as many amines are bases

15. Strong Acids or Bases ·Strong acids or bases ionize 100 % in solution ·Weak acids or bases ionize <100 % in solution

16. Strong Acids ·HClO 4 Perchloric acid ·H 2 SO 4 Sulfuric acid ·HNO 3 Nitric acid ·HClHydrochloric acid ·HBrHydrobromic acid ·HIHydroiodic acid

17. Strong Bases ·All column I hydroxides ·Ca(OH) 2 Calcium hydroxide ·Sr(OH) 2 Strontium hydroxide ·Ba(OH) 2 Barium hydroxide

18. Name & give the formula for at least 4 each of strong acids & strong bases

19. Binary Acids ·Acids containing only 2 elements ·HClHydrochloric acid ·H 2 SHydrosulfuric acid

20. Ternary Acids ·Acids containing 3 elements ·H 2 SO 4 Sulfuric acid ·H 2 SO 3 Sulfurous acid ·HNO 3 Nitric acid

21. Monoprotic Acids ·Acids containing only one ionizable hydrogen ·HBr Hydrobromic acid ·HCNHydrocyanic acid ·HC 2 H 3 O 2 Acetic acid

22. Diprotic Acids ·Acids containing 2 ionizable hydrogens ·H 2 SO 4 Sulfuric acid ·H 2 SO 3 Sulfurous acid ·H 2 CO 3 Carbonic acid

23. Triprotic Acids ·Acids containing 3 ionizable hydrogens ·H 3 PO 4 Phosphoric acid ·H 3 PO 3 Phosphorus acid ·H 3 AsO 4 Arsenic acid

24. Polyprotic Acids ·Acids containing more than one ionizable hydrogens ·H 2 SO 4 Sulfuric acid ·H 4 SiO 4 Silicic acid ·H 2 CO 2 Carbonous acid

25. Monohydroxic Base ·A base containing only one ionizable hydroxide ·NaOHSodium hydroxide ·KOHPotassium hydro. ·LiOHLithium hydroxide

26. Neutralization Rxn ·A reaction between an acid & a base making salt & H 2 O ·HA (aq) + MOH (aq)  MA (aq) + H 2 O (l)

27. Neutralization Rxn HCl (aq) + NaOH (aq)  NaCl (aq) + H 2 O (l)

28. Drill: Identify: acid, base, CA, & CB HCO 3 - + H 2 O H 2 CO 3 + OH -

29. Work problems 1 – 6 on page 395

30. Titration ·A method of determining the concentration of one solution by reacting it with a standard solution ·M A V A = M B V B for monoprotics

31. Standard Solution ·A solution with known concentration

32. Titration ·When titrating acids against bases, the end point of the titration is at the equivalence point

33. Make Calculations ·Calculate the molarity of 25.0 mL HCl when it’s titrated to its equivalence point with 50.0 mL 0.200 M NaOH

34. Equivalence Point ·The point where the H + concentration is equal to the OH - concentration

35. Indicator ·An organic dye that changes color when the pH changes

36. Make Calculations ·Calculate the mL of 12.5 M HCl required to make 2.5 L of 0.200 M HCl

37. Molarity ·Moles of solute per liter of solution (M)

38. Normality ·Number of moles of hydrogen or hydroxide ions per liter of solution (N)

39. Titration Formula ·N A V A = N B V B ·Elliott’s Rule: ·# H M A V A = # OH M B V B

40. Make Calculations ·Calculate the molarity of 30.0 mL H 2 CO 3 when it’s titatrated to its equivalence point with 75.0 mL 0.200 M NaOH

41. Make Calculations ·Calculate the molarity of 40.0 mL H 3 PO 4 when it’s titatrated to its equivalence point with 30.0 mL 0.20 M Ba(OH) 2

42. Calculate the volume of 0.250 M HCl needed to titrate 50.00 mL 0.200 M NaOH to its equivalence point

43. Calculate the molarity 25.0 mL H 3 PO 4 that neutralizes 50.00 mL 0.200 M Ca(OH) 2 to its equivalence point

44. Drill: Calculate the volume of 0.10 M H 3 PO 4 that neutralizes 50.00 mL 0.200 M Ca(OH) 2 to its equivalence point

45. pH ·The negative log of the hydrogen or hydronium ion concentration ·pH = -log[H + ] ·pOH = -log[OH - ]

46. Calculate the pH of: 1) [H + ] = 0.040 M 2) [HCl] = 0.0025 M 3) [HBr] = 0.080 M

47. Calculate the pOH of: 1) [OH - ] = 0.030 M 2) [KOH] = 0.0025 M 3) [NaOH] = 4.0 x 10 -5 M

48. Titration Curve: Strong acid vs strong base

50. Titration Curve: Strong acid vs strong base; then weak acid vs strong base

53. Titration Curve: Strong base vs strong acid; then weak base vs strong acid