1. 1A + 1B  1C + 1D Calculate the equilibrium concentrations of each species when 150 ml 2.0 M A is mixed with 100.0 ml 2.0 M B. K c = 0.25

2. Acid/Base

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

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

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

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

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

8. 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

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

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

11. Drill: List 3 properties each of both acids & bases

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. Define acids & bases by each of the three methods

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

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

20. 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

21. 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

22. 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

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

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

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

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

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

28. Equivalence Point [ H + ] = [OH - ] Molarity (M) acid =Molarity(M) base

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

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

31. 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

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

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

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

35. 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

36. 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

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

38. 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

39. 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

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

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

42. Calculate the pOH of each of the following: 1) [OH - ] = 0.030 M 2) [KOH] = 0.0025 M 3) [NaOH] = 4.0 x 10 -12 M

43. 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.