1. 1A + 2B  1C + 1D Calculate the equilibrium concentrations of each species when 150 mL 2.5 M A is mixed with 100.0 mL 2.5 M B. K c = 2.0 x 10 -10

2. Drill: 1A + 2B  1C + 1D Calculate the equilibrium concentrations of each species when a solution is made with 1.0 M A & 1.0 M B. K c = 2.0 x 10 -12

3. Acid/Base

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

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

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

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

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

9. 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

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

11. Lewis Acid/Base H 3 N: + BF 3  H 3 N-BF 3 Base Acid Neutral

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

13. Amphiprotism ·Can act like an acid or a base ·Can donate or accept protons

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

15. Drill: Name each of the following: KOHHBr Al(OH) 3 H 2 CO 3 HClO 4 NH 3

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

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

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

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

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

21. Strong Acid/Base Ionizes 100 % (1 M) HAH + + A - 1 M – all1 1

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

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

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

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

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

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

28. Monohydroxic Base ·A base containing only one ionizable hydroxide ·NaOHSodium hydroxide ·LiOHLithium hydroxide

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

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

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

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

33. Calculate the pOH of each of the following: 1) [OH - ] = 0.030 M 2) [KOH] = 0.0025 M 3) [NaOH] = 4.0 x 10 -7 M

34. Standard Solution ·A solution with known concentration

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

36. Titration ·A method of determining the concentration of one solution by reacting it with a standard solution

37. Titration Formula for monoprotic solutions M A V A = M B V B

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

39. Equivalence Point ·The point where the concentrations of the two solutions in the titration are equal

40. Acid/Base Equivalence Point The point where the H + concentration is equal to the OH - concentration

41. Titration Fact No changes will be observed when titrating acids against bases; thus, one must use an indicator to see changes

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

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

44. Titration Formula for monoprotic solutions M A V A = M B V B

45. Dilution Formula M 1 V 1 = M 2 V 2

46. ·Calculate the mL of 16.0 M HNO 3 it takes to make 4.0 L of 0.100 M HNO 3

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

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

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

50. Titration Formula for Acid/Base ·N A V A = N B V B ·Elliott’s Rule: ·# H M A V A = # OH M B V B

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

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

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

54. 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

55. Titration Curve: Strong acid vs strong base

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

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

62. 3.2 g HI is dissolved in a 1250 mL aqueous solution. Calculate its pH.

63. 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

64. Drill: Calculate the molarity of 25.00 mL of H 3 PO 4 that was titrated to its equivalence point with 75.00 mL of 0.125 M Ba(OH) 2.