1. Review of Acids, Bases, & Salts

2. Arrhenius Acid Has H in the formula Produces H + as the only positive ion in solution

3. Formula of an Acid Inorganic – formula starts with H Organic – formula ends with COOH

4. Properties of Acids Sour Taste Electrolytes React with bases to form a salt + H 2 O Turn litmus RED React with most metals to produce H 2 (g)

5. Ionization of an Acid HCl  H + + Cl - HCl + H 2 O  H 3 O + + Cl - or

6. Arrhenius Base Has OH in the formula Produces OH - as the only negative ion in solution

7. Formula of a Base Has format MOH M is a metal

8. Properties of Bases Bitter Taste Slippery Feel Electrolytes React with acids to form a salt + H 2 O Turn litmus BLUE

9. Ionization of a Base NaOH  Na + + OH -

10. Ionization of NH 3 NH 3 + H 2 O  NH 4 + + OH -

11. Formula of a Salt Metal + Nonmetal

12. Write the formula of potasium sulfate K + & (SO 4 ) 2- K 2 SO 4

13. Electrolytes Solutions conduct – they contain ions Acids (HX), bases (MOH), & salts (MX) are electrolytes

14. NONelectrolytes Solutions of covalent compounds (all nonmetals). They do NOT conduct.

15. Identify the electrolytes LiOH CH 3 COOH C 6 H 12 O 6 NaNO 3 H 2 SO 4 CH 3 OH Ca(OH) 2 HCl C 8 H 18 Al(OH) 3 HNO 3 CH 3 CH 2 COOH K 2 SO 4 CH 3 CHOHCH 3 CH 3 OCH 3 H 3 PO 4 Mg(OH) 2 CH 3 CH 2 OH Yes - B Yes - A No Yes - S Yes - A No Yes - B Yes - A No Yes - B Yes - A Yes - S No No Yes - A Yes - B No

16. pH scale 0-14 Acidic: 0 to 7, Neutral: 7 Basic: 7-14

17. Most acidic on pH scale pH = 0

18. Most basic on pH scale pH = 14

19. OH - Hydroxide ion

20. H+H+H+H+ Hydrogen ion or Proton

21. H3O+H3O+H3O+H3O+ Hydronium ion. Interchangeable with H +.

22. Acidic Solution [H + ]  [OH - ]

23. Basic Solution [OH - ]  [H + ]

24. If the pH changes from 3 to 5, how does the [H + ] change? The pH changes by 2, so the [H + ] changes by 10 2 or 100X. Since the pH went up, it became LESS acidic. The new solution has a [H + ] 100 times less than the original solution.

25. How can pH be safely tested? Instrumental – use pH meter Indicators – use a series of indicators to narrow down the pH range NOT Test acids with metals (NOT Cu, Ag, or Au)

26. Bronsted-Lowry Acid Proton Donor

27. Bronsted-Lowry Base Proton Acceptor

28. Bronsted-Lowry Acids & Bases HCl + H 2 O  H 3 O + + Cl -

29. Strong Acids & Bases Complete or almost complete ionization.

30. Weak Acids & Bases Ionization occurs only to a slight extent, a few percent.

31. Reactions of Acids with Metals Metal + Acid  H 2 (g) + salt

32. Zn(s) + HCl  ? Zn(s) + 2HCl  H 2 (g) + ZnCl 2

33. Al(s) + HCl  ? 2Al(s) + 6HCl  3H 2 (g) + 2AlCl 3

34. Neutralization Reactions Acid + Base  Salt + H 2 O

35. Net Ionic Equation for Neutralization Reactions H + + OH -  H 2 O

36. At neutralization Moles H + = Moles OH -

37. Molarity (M) Molarity = Moles solute Liters of soln

38. Titration Equation M a V a = M b V b This equation works when the number of H’s on the acid EQUALS the number of OH’s on the base!

39. Titration Equation n a M a V a = n b M b V b This equation works when the number of H’s on the acid does NOT equal the number of OH’s on the base! n a = number of acidic H’s in acid. n b = number of OH’s in base.

40. pH -log[H + ] or –log[H 3 O + ]

41. pOH -log[OH - ]

42. pOH + pH = 14

43. [OH - ] X [H + ] = 1.0 X 10 -14

44. If the [H + ] = 1 X 10 -3 1.The pH = 2.The pOH = 3.The [OH - ] =3 11 1 X 10 -11

45. Indicator Substance that changes color over a narrow pH range.

46. Molarity H 2 SO 4 Vs. Molarity H + H 2 SO 4  2H + + SO 4 2- [H + ] = 2[H 2 SO 4 ] 2M H 2 SO 4  4M H +

47. What is the concentration of a hydrochloric acid solution50.0 mL 0.250 M KOH 20.0 mL of the HCl solution What is the concentration of a hydrochloric acid solution if 50.0 mL of a 0.250 M KOH solution are needed to neutralize 20.0 mL of the HCl solution of unknown concentration? M a V a = M b V b X(20.0 mls) =.250M(50.0mls)

48. Acid 1.50 M Base ? M Final Volume 16.0724.25 Initial Volume 5.454.05 Amount Used (1.50 M)(10.62 mls) = X(20.20 mls) 10.6220.20