1. Day 1 Acid-Base

2. Review of naming acids

3. Determine Name: H 2 SO 3 H 2 SO 4 H 2 S HClO 3 HCl HClO 2

4. Determine Name: H 2 SO 3 H 2 SO 4 H 2 S HClO 3 HCl HClO 2

5. Determine Formula Hydrofluoric acid Carbonic acid Nitrous acid Hydroselenic acid

6. Determine Formula Hydrofluoric acid HF Carbonic acid Nitrous acid Hydroselenic acid

7. Characteristics of Acids & Bases

8. Acids are Characterized by: O Sour taste O  color of indicator O Release of H 2 gas O Reacts with bases  salt( ionic compound) & H 2 O

9. Bases are Characterized by: O Bitter taste O Feels slippery O  color of indicator O Reacts with acid  salt( ionic compound) & H 2 O O Conducts electric current ( its an ionic compound)

10. What does ionization mean?

11. Ionization O Adding or removing electrons (e-) O Making a cation or anion

12. Strong Acids O Ionizes completely = breaks up completely O Conducts electric current (remember electrolyte demo & PhET)

13. Strong Acids Examples: O Hydrochloric Acid (HCl) O Sulfuric Acid (H 2 SO 4 ) O Nitric Acid (HNO 3 )

14. Strong Base O Ionizes completely = breaks up completely O Examples: group 1 hydroxides – sodium hydroxide, potassium hydroxide, etc.

15. Neutralization Reaction HCl + NaOH  NaCl + HOH Strong + Strong  Salt + Water Acid Base HNO 3 + KOH  KNO 3 + HOH

16. Neutralization Reaction Is a double replacement rxn b/w … strong acid + strong base  a salt (ionic compound) + water

17. pH Scale Determining strength of an Acid or Base

18. pH scale 0-14 O neutral pH = 7.0 O acidic pH <7.0 O basic pH > 7.0

19. pH Scale

21. Calculating pH & [H + ] pH = -log[H + ] Inverse of log 10 is 10 ^( ) [H + ] = 10 ^(-pH)

22. Calculating pOH & [OH - ] pH = -log[OH - ] Inverse of log 10 is 10 ^( ) [OH - ] = 10 ^(-pOH)

23. Relationship between pH & pOH pH + pOH = 14

27. Now you try…

28. Answer

29. Try on your own…

32. Practice

33. Now you try

34. Answer

35. Try on your own..

36. Answers

37. Other methods of determining pH

38. If molarity is not known, pH can be determined by… O Acid-Base Indicators O pH meter O Titration

39. Indicator Solutions O Change color depending on pH of test solution

40. Indicators

43. Problems with indicator solutions: O If you have a colored solution O Approx pH value not exact O Temperature affects color 

44. pH meter

45. O consists of a measuring probe O electronic meter: measures & displays the pH reading O have to calibrate probe

46. Titration O Use Buret, Erlenmeyer flask, indicator O Use M 1 V 1 = M 2 V 2 to determine molarity of unknown

47. Titration

49. Answer the following questions while watching the video clips: 1. Where do you read/How do you read a burette? 2. What hand do you use to swirl the Erlenmeyer flask? 3. What hand do use to adjust the burette? 4. When do you know you are getting close to the endpoint? 5. How is the standard solution added as you get close to the endpoint? 6. When do you know you have achieved the endpoint?

50. O Titration Video Clip #1 (3:15) Titration Video Clip #1 O Titration Video Clip # 2 ( 6:07) Titration Video Clip # 2

51. Now, do the titration pre-lab