1. The Chemistry of Acids and Bases

2. Acids and Bases: Define and Calculate pH/pOH At the conclusion of our time together, you should be able to: 1. Define pH and pOH 2. Explain the pH scale and what it means 3. Change any pH reading to pOH 4. Convert pH to concentration of hydronium ion concentrations, hydronium ion concentrations to pH

3. Law of Probability  -The probability of being watched is directly proportional to the stupidity of your act

4. The pH scale is a way of expressing the strength of acids and bases. This scale is defined by: pH = - log [H+] Under 7 = acid 7 = neutral Over 7 = base What is pH???

5.  p = count  H = Hydronium ion  (H 3 O + )  In 1 Liter of water, (55+ moles of water), how many moles of hydronium ions are there???  Understanding pH gives me this number!!!  If there was 1 mole of H 3 O + in 1 Liter of water, (55+ moles of water), this count would be 1 mole.

6. What is pH???  Remember: pH = - log [H+]  pH = -log[1]  Therefore, by definition, the pH of this solution is  = 0

7. What is the pH of water???  H 2 O + H 2 O ---> H 3 O + + OH -  <===  This equation indicates that most water molecules stay as molecules, very few will form hydronium ions  If we count the number of hydrogen ions in one liter of water (pH) we would get: .0000001 moles of H 3 O + /liter of water  or 10 -7 moles of H 3 O + /liter of water  What is the pH of water??  pH = 7

8. What is the pOH of water???  H 2 O + H 2 O ---> H 3 O + + OH -  <===  This equation indicates that most water molecules stay as molecules, very few will form hydroxide ions  If we count the number of hydroxide ions in one liter of water (pOH) we would get: .0000001 moles of OH - /liter of water  or 10 -7 moles of OH - /liter of water  What is the pOH of water??  pOH = 7

9. How High is the pH Scale??  Since 1 mole of OH- in one Liter of water would be a pOH = 0  And the pH and pOH of water is 7 or neutral,  Therefore, the pH of a strong base with a pOH of 0 would be?  pH = 14  Therefore, the pH scale goes from 0-14  Also, any pH can be converted to pOH by?  Subtracting from 14.

10. pH- The Amount Of H + Ions In A Solution. ACID extra H +1 ions (protons) BASE fewer H +1 ions. extra OH -1 ions. 1 2 3 4 5 6 7 8 9 10 11 12 13 14

11. Where Do You Find a Dog With No Legs?  Right Where You Left Him.

12. Let’s Try Some Calculations by Not Using Calvin’s Approach to Math in Chemistry:

13. Examples of Converting pH  If an acid has a pH of 3, what would be the pOH?  14 – 3 =  11  If an base has a pOH of 2, what would be the pH?  14 – 2 =  12

14. Calculating the pH pH = - log [H+] (Remember that the [ ] mean Molarity) Example: If [H + ] = 1 X 10 -10 pH = - log 1 X 10 -10 pH = 10 Example: If [H + ] = 1.80 X 10 -5 pH = - log 1.80 X 10 -5 pH = 4.7

15. Try These! Find the pH of these: 1) A 0.15 M solution of Hydrochloric acid 2) A 3.00 X 10 -7 M solution of Nitric acid pH = 0.82 pH = 6.5

16. But Why Only 2 Significant Figures?? 2) A 3.00 X 10 -7 M solution of Nitric acid pH = 6.5 Remember, we are working with logarithms. Therefore, we will use the pHAD principle. Add significant figures after the Decimal Point for pH.

17. pH Calculations – Solving for H + If the pH of Coke is 3.12, [H + ] = ??? Because pH = - log [H + ] then - pH = log [H + ] - pH = log [H + ] Divide both sides by log or Take antilog (10 x ) of both sides and get 10 -pH = [H + ] 10 -3.12 = [H + ] = 7.6 x 10 -4 M *** to find antilog on your calculator, press “Shift” or “2 nd function” and then the log button *** to find antilog on your calculator, press “Shift” or “2 nd function” and then the log button

18. pH Calculations – Solving for H+  A solution has a pH of 3.78. What is the concentration of hydrogen ions in the solution? (#1 on handout) pH = -log [H + ] 3.78= -log [H + ] -3.78= log [H + ] Inverse log -3.78 = inverse log (log [H + ]) 10 -3.78 = [H + ] 1.66 x 10 -4 = [H + ]

19. What is the pOH?  If an acid has a pH of 3.78, what would be the pOH? (#1 on handout)  14 – 3.78 =  10.22

20. pH Calculations – Solving for H+  A solution has a pH of 3.78. What is the concentration of hydroxide ions in the solution? (#1 on handout) pOH = - log [OH - ] 10.22 = - log [OH - ] - 10.22 = log [OH - ] Inverse log -10.22 = inverse log (log [OH - ]) 10 -10.22 = [OH - ] 6.03 x 10 -11 = [OH - ]

21. Calculating [H 3 O + ], pH, [OH - ], and pOH Problem 1: What is the [H 3 O + ], [OH - ], and pOH of a solution with pH = 3.78? Is this an acid, base, or neutral? [H 3 O + ] = 1.66 x 10 -4 M pOH = 10.22 [OH - ] = 6.03 x 10 -11 M Acid

22. Calculating the pOH pOH = - log [OH-] (Remember that the [ ] mean Molarity) Example #4 on handout: If [OH - ] = 4.88 x 10 -6 pOH = - log (4.88 x 10 -6 ) pOH = 5.31

23. Calculating [H 3 O + ], pH, [OH - ], and pOH Problem 2: A chemist dilutes concentrated hydrochloric acid to make: 0.000 389 M HCl. Calculate the pH, [OH - ], and pOH pH = 3.41 pOH = 10.59 [OH - ] = 2.57 x 10 -11 M Acid

24. [OH - ] [H + ] pOH pH 10 -pOH 10 -pH -Log[H + ] Log[OH - ] -Log[OH - ] 14 - pOH 14 - pH 1.0 x 10 -14 [OH - ] [OH - ] 1.0 x 10 -14 [H + ] [H + ]

25. pH [H + ] [OH - ] pOH

26. Acids and Bases: Define and Calculate pH/pOH Let’s see if you can: 1. Define pH and pOH 2. Explain the pH scale and what it means 3. Change any pH reading to pOH 4. Convert pH to concentration of hydronium ion concentrations, hydronium ion concentrations to pH

27. The American Medical Association announced today that the Universal Choking Sign has been revised:

28. Old Sign:

29. New Sign:

30. Get Your Clicker!!!

31. The “p” in pH stands for? 1. Priority 2. Count 3. Number 4. Molarity 5. Not listed

32. The “H” in pH stands for? 1. House 2. Hydrogen ions 3. Acid 4. Concentration 5. Not listed

33. If a solution has a pH of 6.5, what is the pOH of that same solution? 1. 4.5 2. 7.5 3. 6.5 4. 0.0 5. 12.5 6. Not listed

34. If a solution has a pH of 6.2, what is the [H + ] of that solution? 1. 6.2 2. 6.3 x 10 -7 3. 1.0 x 10 6.2 4. 1.0 x 10 7.8 5. 7.8 6. Not listed

35. If a solution has a pOH of 9.44, what is the [OH - ] of that same solution? 1. 0.98 2. 1.00 x 10 9.44 3. 3.63 x 10 -10 4. 4.56 5. 9.44 6. Not listed

36. Let’s kick back and relax!!

37. The Chemistry of Acids and Bases

38. Acids and Bases: Strength and Indicators At the conclusion of our time together, you should be able to: 1. Determine the relative strength of acids and bases and the reason for the strengths 2. List the 3 basic types of indicators 3. Explain each indicator’s strengths and weaknesses 4. Use an appropriate indicator to determine the pH of a substance

39. Remember: the pH scale is a way of expressing the strength of acids and bases. Under 7 = acid 7 = neutral Over 7 = base What makes an acid strong or weak??

40. HNO 3, HCl, H 2 SO 4 and HClO 4 are among the only known strong acids. Strong or Weak Acids/Bases The strength of an acid (or base) is determined by the amount of IONIZATION.

41. Strong Acids Generally divide acids and bases into STRONG or WEAK ones. STRONG ACID: HNO 3 (aq) + H 2 O (l) ---> H 3 O + (aq) + NO 3 - (aq) HNO 3 is about 100% dissociated in water.

42.  Weak acids are much less than 100% ionized in water. One of the best known is acetic acid = CH 3 CO 2 H Weak Acids

43. Weak ACID Strong ACID HCl Hydrochloric acid H 2 SO 4 Sulfuric acid HNO 3 Nitric acid CH 3 COOH Acetic acid H 2 CO 3 Carbonic acid Citric acidpH H2OH2OH2OH2O H+H+H+H+0551 15501 255001

44. Strong Base: 100% dissociated in water. NaOH (aq) ---> Na + (aq) + OH - (aq) NaOH (aq) ---> Na + (aq) + OH - (aq) Strong Bases Other common strong bases include KOH and Ca(OH) 2. CaO (lime) + H 2 O --> Ca(OH) 2 (slaked lime) Ca(OH) 2 (slaked lime) CaO

45. Weak base: less than 100% ionized in water One of the best known weak bases is ammonia NH 3 (aq) + H 2 O (l) NH 4 + (aq) + OH - (aq) Weak Bases

47. Strong acids and bases dissolve in water Hydrochloric, Hydrobromic, Hydroiodic, (All Binaries) Nitric, Sulfuric, Perchloric Acids (Ternary Acids with 2 more O than H) Group I hydroxides Strong or Weak Acids/Bases Summary

48. Maybe Our Goals Aren’t the Exact Same, But They’re Similar!!

49. There are Several Ways to Test for pH  There are three basic types:  Paper  pH meter  Liquid indicators  (Some are natural liquid indicators like red cabbage, radishes)

50. Paper Testing  Paper tests like litmus paper and pH paper  Put a stirring rod into the solution and stir.  Take the stirring rod out, and place a drop of the solution from the end of the stirring rod onto a piece of the paper  Read and record the color change. Note what the color indicates.  Use a small portion of the paper. You can use one piece of paper for several tests.

51. pH Paper Blue Litmus paper Red Litmus paper

52. pH Meter  Tests the voltage of the electrolyte  Converts the voltage to pH  Expensive, but very accurate  Must be calibrated with a buffer solution

53. pH Indicators  Indicators are dyes that can be added that will change color in the presence of an acid or base.  Some indicators only work in a specific range of pH  Once the drops are added, the sample is ruined  Some dyes are natural, like radish skin or red cabbage

54. We’ll Chip Away at this a Little at a Time!!

55. pH of Common Substances

56. A Former Student Trying to Apply His Knowledge of Chemistry!!

57. Acids and Bases: Strength and Indicators Let’s see if you can: 1. Determine the relative strength of acids and bases and the reason for the strengths 2. List the 3 basic types of indicators 3. Explain each indicator’s strengths and weaknesses 4. Use an appropriate indicator to determine the pH of a substance

58. Get Your Clicker!!!

59. Red litmus paper will turn what color in an acid? 1. Blue 2. White 3. Red 4. Clear 5. Not listed

60. Which of the following would be the most accurate way to test for pH? 1. pH meter 2. Litmus paper 3. Phenylthalein 4. Cabbage juice 5. Universal indicator 6. Not listed

61. Several liquids are tested for pH. Which of these liquids would be the weakest acid? 1. Liquid a, pH = 1.0 2. Liquid b, pH = 4.5 3. Liquid c, pH = 6.5 4. Liquid d, pH = 8.5 5. Liquid e, pH = 10.5 6. Liquid f, pH = 13.0

62. So – What did you think of today’s class??

63. If a solution has a [H 3 O + ] of 6.20 x 10 -8, what is the pH of that solution? 1. 6.79 2. 8.79 3. 5.21 4. 4.56 5. 7.21 6. Not listed

64. If a solution has a [OH - ] of 1.05 x 10 -3, what is the pH of that solution? 1. 11.02 2. 2.98 3. 1.00 4. 3.02 5. 10.98 6. Not listed

65. Converting pH to pOH  If an acid has a pH of 6, what would be the pOH?  14 – 6 = 8888

66. [H 3 O + ], [OH - ] and pH Page 14:5 What is the pH of the 0.0001 M NaOH solution? [OH - ] = 0.0001 (or 1.0 X 10 -4 M) pOH = - log 0.0001 pOH = - log 0.0001 pOH = 4 pOH = 4 pH = 14 – 4 = 10 pH = 14 – 4 = 10

67. The pOH of rainwater collected in a certain region of the northeastern United States on a particular day was 9.94. What is the H + ion concentration of the rainwater? The OH - ion concentration of a blood sample is 2.88 x 10 -6 M. What is the pH of the blood? Try These! Page 15:9 pH = 4.06 8.91 x 10 -5 pOH = 5.54 14.0 – 5.54 = 8.46 pH

68. I wouldn’t do that if I were you!!!