1. ½ sheet of paper and Chemistry book out About ¼-½ a page Use your own words to describe acids and bases. –Give examples of acids and bases. –What is pH? –(Mr. B Note, do this as a class discussion. K of a KWL)

2. ½ sheet of paper and Chemistry book out My example: Chicken bone in vinegar. Acids such as Pop absorb the calcium out of bones and make the bones weak and rubbery. That’s why pop is not sold in many schools. Can skip pH demo and go to slide 8.

3. Record this order HCl, NaOH, H 2 SO 4, HC 2 H 3 O 2, KOH, LiOH, HNO 3 Make observations when the phenolphthalein is added.

4. Record this order HCl, NaOH, H 2 SO 4, HC 2 H 3 O 2, KOH, LiOH, HNO 3 Make observations when the phenolphthalein is added. Predict what will happen when phenolphthalein is added to the last 2 solutions.

5. Record this order HCl, NaOH, H 2 SO 4, HC 2 H 3 O 2, KOH, LiOH, HNO 3 Make observations when the phenolphthalein is added. Predict - What will happen when phenolphthalein is added to the last 2 solutions? Predict – What will happen when a solid chunk of NaOH is added to water? HCl?

6. Record this order HCl, NaOH, H 2 SO 4, HC 2 H 3 O 2, KOH, LiOH, HNO 3 Explain, create a theory, about why some solutions turn pink.

8. Acids and Bases

9. Acids taste sour, become less acidic when mixed with bases. Bases feel slippery and are bitter, become less basic when mixed with acids.basesacids

11. What is the common name of a hydrogen ion?

12. What is the common name of a hydrogen ion? What are the atomic parts of a hydrogen atom? Hydrogen Ion?

13. What is the common name of a hydrogen ion? What are the atomic parts of a hydrogen atom? Proton and electron Hydrogen Ion? Proton What did you see at the start of all the acid formulas? (repeated next slide)

15. Arrhenius definition of: acid: generates [H + ] in solution (HCl) base: generates [OH - ] in solution (NaOH) Some textbooks call acids a Hydrogen donor instead of a proton donor. HCl + H 2 O = H + (aq) + Cl - (aq) NaOH(s) + H 2 O  NaOH(aq) NaOH(aq) = Na + (aq) + OH - (aq)

16. Arrhenius definition of: acid: generates [H + ], Often Positive base: generates [OH - ] Often Negative But they are not always positive and negative. Often but NOT ALWAYS! For example, Sometimes they are neutral and have no charge. The can both be negative or positive, but the acid is always less negative or the more positive.

17. Arrhenius definition of: acid: generates [H + ], Often Positive base: generates [OH - ] Often Negative So look at the signs and the one that is “more positive” is always the acid because it has the [H + ].

18. Common Bases. What do you notice common in their formulas? Typical Acid Reaction in Water, H+ gets lonely and often combines with water.

19. Is water an acid or base? So if acids begin with H and bases end with OH, What is the correct chemical formula for water?

20. Is water an acid or base? Both So if acids begin with H and bases end with OH, What is the correct chemical formula for water? HOH (not H 2 0)

21. Oldest or original definition: Copy the following into your powerpoint notes: Acid Neutral Base (Water) pH 1 pH 7 pH 14 Strong Weak Weak Strong Protons Hydroxide H + HOH OH - H + meet with OH - in the middle to form HOH

22. Bronsted-Lowry: acid: anything that donates a H + ion (proton donor) base: anything that accepts a H + ion (proton acceptor) Means a base does not have to have OH - This definition is the most commonly used in industry. HCl + Mg  MgCl 2 + H 2 Flashback: How do you balance this?

23. Lewis: acid= accept a pair of electrons to form a covalent bond Base= e- donor Acid with Covalent Bond: H : Cl H + + Cl - = H:Cl H accepts e- from Cl OH – as a base, donating an e- to H + H + + OH - = H:OH HCl + Mg  MgCl 2 + H 2 Mg has formed a 2 + ion losing 2 electron H + have each gained an electron forming H 2

24. Remember all 3 definitions for the test:

25. Remember for test: When an acid and base react, they produce salt and water HCl + NaOH  H + + Cl - + Na + + OH - HCl + NaOH  NaCl + HOH

26. Conjugate acid / Conjugate base pair: they are acid/base on the right or product side of a reversible reaction (acid and base are reactants, Conjugates are always Proton transfer, never OH). Proton transfers. acid + 1 + base - 2  base - 1 + acid + 2 acid + 1 loses proton to become base - 1 base - 2 gains proton to become acid + 2. Proton transfers back acid + 1 + base - 2  base - 1 + acid + 2 When the proton is returned, the process reverses or goes back the other direction.

27. Conjugate acid / Conjugate base pair: they are acid/base on the right or product side of a reversible reaction (acid and base are reactants) Ammonia plus water makes ammonium plus hydroxide

28. Note: any question that asks about conjugate means Conjugate on the right acid/base always means left side. HOWEVER! If the word conjugate is NOT in the problem, then the acid or base may be on either side of the equation. HCl (l) + H 2 O (l) H 3 O + (aq) + Cl - (aq)

29. Label the acid/base and conjugate acid/base HCl (l) + H 2 O (l) H 3 O + (aq) + Cl - (aq) Acid:_________ Base:_________ Conjugate Acid:_____________ Conjugate Base:_____________

30. Water reacts with the H + in solution and forms the hydronium ion H 3 O +

31. Self-ionization of water H 2 O ↔ H + + OH -

32. New Concept: Water, acids, and bases have both H + and OH - in them at the same time. It probably appeared that acid only has H + but it actually has both of them. Bases also have both.

33. Remember for test: All water contains all three of the following: Water Molecules, Hydronium ions, and Hydroxide Ions. Hydronium Ion is H 3 0 + Hydroxide Ion is OH - Know ion formula and charge.

34. Important. REMEMBER THIS! ion-product constant for water (Kw): Where have we seen that 14 before?

35. Important. REMEMBER THIS! ion-product constant for water (Kw): [concentrations] : Brackets around a element means concentration. What do we measure concentration in?

36. [concentrations] : are measured In Molarity = moles/L of Solution (remember: solute + solvent = solution)

37. acidic solution = [H + ] is greater than [OH - ]; but solutions have both H + and OH - in them (and water molecules). [H + ] of an acidic solution is greater than 1 x 10 -7 M NOTES: ACIDS: [H + ] > 1 x 10 -7 M

39. How concentrated is the acid? The acidity is defined most typically by the pH value, pH= -log[H + ] (added my me) pH is the exponent on the 10 (made positive). pH 2 means 1.0 x 10 -2 Molarity of [H + ]

40. [H + ]pHExample Acids1 X 10 0 0HCl 1 x 10 -1 1Stomach acid 1 x 10 -2 2 Lemon juice 1 x 10 -3 3 Vinegar 1 x 10 -4 4Soda 1 x 10 -5 5Rainwater 1 x 10 -6 6Milk Neutral1 x 10 -7 7Pure water Bases1 x 10 -8 8Egg whites 1 x 10 -9 9Baking Soda 1 x 10 -10 10Tums ® antacid 1 x 10 -11 11Ammonia 1 x 10 -12 12Mineral Lime - Ca(OH) 2 1 x 10 -13 13 Drano ® 1 x 10 -14 14NaOH

41. The pH scale is a measure of the concentration of H + in solution the higher the H + concentration the lower the pH number pH means probability of Hydrogen.

42. The pH scale is a measure of the concentration of H + in solution the higher the H + concentration the lower the pH number pOH?

43. pOH scale. Note that it is just the reverse of pH. Add pink line to your pH notes: Acid Neutral Base (Water) pOH 14 pOH 7 pOH 1 Strong Weak Weak Strong Protons Hydroxide H + HOH OH - H + meet with OH - in the middle to form HOH

44. Know these Equations for the test: pH + pOH = 14 pH= -log[H + ] pOH= -log[OH - ] 10 -pH = [H + ] 10 -pOH = [OH - ] (Discuss how to do on calculator. Point out the opposites. 2 and 4, 3 and 5.)

45. Examples of last slide, how to use calculator. Given pH = 2.6, find pOH. Use pH + pOH = 14 Answer: 14 - 2.6 = 11.4 Given Molarity of H + = [H + ] =.0023 M Find pH. Use: pH= -log[H + ] Put in Calculator: -log[.0023] Answer: pH = 2.6 (2.638227) Given pH = 2.6, find Molarity of H + = [H + ] Use10 -pH = [H + ] Put in Calculator: 10 -2.638227 Answer:.0023 or 2.3 x 10 -3 M (or.0025) (note: The bottom 2 equations or examples are opposites.)

46. Examples of last slide, how to use calculator. Given [H + ] = 2.3 x 10 -3 M find pOH. Put in Calculator: -log[.0023] Gives pH = 2.6 Use pH + pOH = 14 Answer: 14 - 2.6 = 11.4 pOH = 11.4

47. [concentrations] ion-product constant for water (Kw) Important. REMEMBER THIS for test! 10 -14 / [H + ] = [OH - ] 10 -14 / [OH - ] = [H + ]

48. To change an acid to a base: Take away a H + or add OH - Take away a H + Ex: HPO 4 2- = PO 4 3- + H + Add OH - Ex: HCl + OH - = Cl - + HOH Remember to balance charges! To change a base to an acid: Add a H + or take away an OH - Ex: PO 4 3- + H + = HPO 4 2- For Conjugate Acids, take away H + For Conjugate Bases, add H +. Remember to balance charges!

49. Monoprotic Acid Donates 1 H + HCl = H + + Cl - Diprotic Acid Donates 2 H + H 2 SO 4 = 2H + + SO 4 2- Triprotic Acid Donates 3 H + H 3 PO 4 = 3H + + PO 4 3- Note: Number of H + Donated may be different than the number of H. CH 3 COOH only donates 1 H + and is Monoprotic.

50. If the [H + ] in a solution is 1.0 x10 -5 M, is the solution acidic, basic, or neutral? What is the [OH - ] of this solution?

52. If the [H + ] in a solution is 1.0 x10 -5 M, is the solution acidic, basic, or neutral? What is the [OH - ] of this solution? My way: Exp is 5 so pH is 5. 14-5 = 9 = pOH [OH - ] =1.0 x10 -9 M

53. A solution has a [H + ] of 0.0023M what is the pH? What is the pOH. Does this solution contain more H + or OH - ?

54. A solution has a [H + ] of 0.0023M what is the pH? What is the pOH. Does this solution contain more H + or OH - ?

55. A solution has a [H + ] of 0.0023M what is the pH? What is the pOH. Does this solution contain more H + or OH - ?

56. A solution has a [H + ] of 0.0023M what is the pH? What is the pOH. Does this solution contain more H + or OH - ? (error due to rounding on calculator.)

57. A solution has a [H + ] of 0.0023M what is the pH? What is the pOH. Does this solution contain more H + or OH - ?

58. The pH is 4.7, what is the pOH, what is the [H + ] (hydrogen ion concentration)?

59. O

60. You try it. The pOH is 6, what is the pH and what is the [H + ]?

61. The pOH is 6, what is the pH and what is the [H + ]?

62. indicator (HIn) = a weak acid / base that undergoes dissociation in a known pH range (changes colors). [H+] + [In-] WOD: (HIn) Something that changes color to indicate a pH level.

63. Color Indicators

64. Acid dissociation constant (Ka): is the ratio of the concentration of the dissociated (or ionized) form of an acid to the concentration of the undissociated (nonionized) form. Note: Dissolved Ions on top. Undissolved on bottom. WOD in 2 slides.

65. Acid dissociation constant (Ka): HCl  H + + Cl - The HCl and H + + Cl - exist in the water at the same time.

66. Acid dissociation constant (Ka): is the ratio of the molarity of the ions over the molarity of the whole acid. High number means strong acid. For WOD: Also Copy equation below

67. Strong acids/bases completely dissociate in water, so do not have Ka values.. Do not confuse. Ka and Kw.. Ka: How Strong. Kw: How Much.

68. Weak acids/bases only partly dissociate in water

69. If Ka value exists, then the reaction is reversible and the right side is a conjugate acid/base pair.

70. Weak acids have small Ka values. The stronger the weak acid, the larger the Ka value, the more of the solid that dissolves.

71. The words concentrated and dilute indicate how much of an acid or base is dissolved in solution. (Molarity) Not if it is a strong or weak acid/base.

72. The words concentrated and dilute indicate how much of an acid or base is dissolved in solution. (Molarity) Not if it is a strong or weak a strong acid can be concentrated or diluted.

73. A 0.100M solution of methanoic acid is only partially ionized. The [H + ] is 2.0 x 10 -3 M. What is the acid dissociation constant (Ka) of methanoic acid?

74. 1.What are 5 equations from this chapter (pH and pOH)? 2.What is the pH and pOH of a 0.000316M solution of HCl? 3.In your own words describe acids and bases (2-3 sentences). (Give examples, pH…) 4.What is the pH and pOH of a 0.00055M solution of NaOH?

75. 1.) pH + pOH = 14 pH= -log[H + ] pOH= -log[OH - ] 10 -pH = [H + ] 10 -pOH = [OH - ] 2.) pH=3.5 pOH= 10.5 3.) Individual Descriptions 4.) pH=3.25 pOH= 10.75

76. Any rain that falls with a pH below 5.6 is considered acid rain

77. Salts = compounds consisting of an anion from an acid and a cation from a base. Ex: HCl = H + + Cl - NaOH = OH - + Na + Cl - is an Anion Na + is a Cation Put the anion and cation together to form a salt.

78. neutralization reactions acids and bases react in water to produce a salt and water (what kind of reaction is this?) When acids and bases react in “equal” quantities to make neutral water. (Equal H+ and OH - )

79. Equivalence point when the number of moles of hydrogen ions equals the number of moles of hydroxide ions (neutralized) What is pH, pOH, [H + ], [OH - ]?

80. How many moles of hydrochloric acid are required to neutralize 0.50 mol of calcium hydroxide?

81. How many moles of hydrochloric acid are required to neutralize 0.50 mol of calcium hydroxide? Step 1.) Make sure equation is balanced. Step 2.) List known. Step 3.) List Unknown. Step 4.) Use dimensional analysis to change known to unknown (multiply by molar ratio.

82. How many moles of hydrochloric acid are required to neutralize 0.50 mol of calcium hydroxide?

85. =1

86. You try it! How many moles of calcium hydroxide are required to neutralize 1.37 mol of hydrochloric acid?

87. How many moles of calcium hydroxide are required to neutralize 1.37 mol of hydrochloric acid?

88. Titration Adding a known amount of base or acid to an unknown to find the pH of the unknown. Uses: Equivalence point, End Point, Neutralization, and Indicators

89. Titration A titration is done to find the molarity of an unknown solution by neutralization. A pH indicator that changes color at 7 is added. A standard solution of a base such as Ca(OH) 2 is added to an acid until the solution changes color. The known pH of the added base is used to find the starting pH of the acid.

90. End Point The point at which the indicator changes color during a titration.

91. Titration Show titration videos Intro: http://www.youtube.com/watch?v=3iuVXHxyB1k&feature=related&safety_mode=true&persist_safety_mode=1&safe=active 2 short samples. http://www.youtube.com/watch?v=g8jdCWC10vQ&safety_mode=true&persist_safety_mode=1&safe=active http://www.youtube.com/watch?v=s1TCH3Vj2RY&feature=related&safety_mode=true&persist_safety_mode=1&safe=active Optional. 6min http://www.youtube.com/watch?v=YDzzMcrdyB4&feature=grec_index&safety_mode=true&persist_safety_mode=1&safe=active Example of caluculations http://www.youtube.com/watch?v=BllRQAc76Y0&feature=related&safety_mode=true&persist_safety_mode=1&safe=active http://www.youtube.com/watch?v=3iuVXHxyB1k&feature=related&safety_mode=true&persist_safety_mode=1&safe=active http://www.youtube.com/watch?v=g8jdCWC10vQ&safety_mode=true&persist_safety_mode=1&safe=activehttp://www.youtube.com/watch?v=s1TCH3Vj2RY&feature=related&safety_mode=true&persist_safety_mode=1&safe=activehttp://www.youtube.com/watch?v=YDzzMcrdyB4&feature=grec_index&safety_mode=true&persist_safety_mode=1&safe=activehttp://www.youtube.com/watch?v=BllRQAc76Y0&feature=related&safety_mode=true&persist_safety_mode=1&safe=active

92. Find the moles needed to make the solution reach the equivalence point

93. 3 steps to solve a titration: 1. Find moles of known or added H + or OH - L x M = n (known) 2. Find moles of unknown. Use equivalent point: moles of unknown = moles of known 3. Find molarity of unknown. n / L = M (unknown)

94. A 33-mL solution of HCl is completely neutralized by 22- mL of 1.0M Ca(OH) 2. What is the concentration (molarity) of the HCl solution?

103. A 50-mL solution of Ca(OH) 2 is completely neutralized by 25- mL of 1.0M HCl. What is the concentration (molarity) of the HCl solution?

104. A 50-mL solution of Ca(OH) 2 is completely neutralized by 25- mL of 1.0M HCl. What is the concentration (molarity) of the calcium hydroxide solution?

109. Buffer is a solution in which the pH remains relatively constant when small amounts of acid or base are added.

110. buffer capacity is the amount of acid or base that can be added to a buffer solution before a significant change in pH occurs.

111. End