1. ABC’s of pH Acids and Bases Revised 10-03-2006

2. Homeostasis Chemical reaction in the body are very sensitive to changes in pH.

3. pH values in Body Gastric Juices1.2 - 3.0 Urine 4.6 – 8.0 Saliva6.35 - 6.85 Blood7.35 – 7.45 Spinal Fluid7.4 Pancreatic Juice7.1 – 8.2 Bile7.6 – 8.6

4. pH pH is based on the relative concentration of hydrogen ions (H + or H 3 O + ) in a solution. Water ionizes into H + and OH - H 2 O H 3 O + + OH -

5. Scientists measure the pH of solutions using a pH meter The meter reads the H+ ion concentration in solution indicating the pH of the solution.

6. Mathematically it is pH is based on the relative concentration of hydrogen ions in a solution. pH = -log [H + ] Water at 25 o C contains 1/10,000,000 mole of H + ions = 10 -7 moles/liter pH = -log [10 -7 ] pH = 7

7. pH

8. logarithmic a pH of 6 is ten times more acidic than distilled water. Also, a solution that has a pH of 8 is ten times more basic (alkaline) than distilled water. Likewise, a solution that has a pH of 4 is 100 times more acidic than one which has a pH of 6.

9. The pH scale is logarithmic (that's what the "p" stands for; the "H" is short for hydrogen); therefore, a solution that has a pH of 6 is ten times more acidic than distilled water. Also, a solution that has a pH of 8 is ten times more basic (alkaline) than distilled water. Likewise, a solution that has a pH of 4 is 100 times more acidic than one which has a pH of 6.

10. Properties of Acids Substances with a pH below 7 are acids. An acid is any substance that ionizes (release charged particles when dissolved) in water to produce H+ hydrogen ions or free protons in water. Acids tend to taste sour. Change blue litmus paper to red. React with metals to release hydrogen gas. Neutralize bases, forming water and salts Acidic solutions have concentrations of H 3 O + above 1 X 10 -7

11. Acid Examples stomach juiceshydrochloric acid HCl  H + + Cl - battery acidsulfuric acid H 2 SO 4  2H + + SO 4 2- vinegar acetic acid CH 3 COOH  H + + CH 3 COO -

12. Measuring Acidity Added acids increase [H 3 O + ] In acid solutions [H 3 O + ] > 1 x 10 -7 M pH scale measures acidity without using exponential numbers.

13. Acid pH Calculations [H 3 O + ]=1 x 10 -5 M, pH = ? 5 (acidic) [H 3 O + ]=2.6 x 10 -5 M, pH = ? 4.59 (acidic) [H 3 O + ]=7.8 x 10 -3 M, pH = ? 2.11 (acidic)

14. Properties of Bases have a pH greater than 7. A base is a substance that ionizes in water solution to produce OH - hydroxide ions. Bases tend to feel slippery to the skin. Bases accept protons Bitter taste Bases turn red litmus paper blue. Neutralize acids, forming water and salts. Basic solutions have H 3 O + concentrations less than 1 X 10 -7

15. Base Examples Milk of Magnesia Mg (OH) 2  2OH - + Mg 2+ Mylanta Mg (OH) 2 + Al(OH) 3  5OH - + Mg 2+ + Al 3+ Maalox Mg (OH) 2 + Al(OH) 3  5OH - + Mg 2+ + Al 3+

16. Measuring Acidity Added bases increase [OH - ]. In basic solutions [OH - ] > 1 x 10 -7 M [H 3 O + ] < 1 x 10 -7 M pH scale measures acidity without using exponential numbers.

17. Base pH Calculation [H 3 O + ] to ph [H 3 O + ]=1 x 10 -10 M, pH = ? 10 (basic) [H 3 O + ]=6.3 x 10 -9 M, pH = ? 8.20 (basic) What if the number is not 1?

18. pH Calculations pH to [H 3 O + ]? –inverse log of negative pH –orange juice, pH 3.5 [H 3 O + ]=? [H 3 O + ] = 10 -3.5 = 3.2 x 10 -4 M –saliva, pH 6.2 [H 3 O + ]=? [H 3 O + ] = 10 -6.2 = 6.3 x 10 -7 M

19. Strong acids ionize completely in water Weak acids ionize only partially in water Strong bases ionize completely in water. Weak bases ionize only partially in water. Strong and Weak Acids and Bases

20. Neutralization Acids and bases can neutralize each other by forming water and salt. Salt - a crystalline compound composed of the negative ion of an acid and the positive ion of a base. H + A - + B + OH -  H 2 0 + A - B + (salt)

21. Examples Stomach acid + Milk of Magnesia  H 2 0 + salt Hydrochloric Acid + Magnesium Hydroxide  H 2 0 + salt 2HCl + Mg(OH) 2  2 H 2 0 + MgCl 2 Stomach acid + Mylanta  H 2 0 + salt Hydrochloric Acid + Magnesium Hydroxide and Aluminum Hydroxide  H 2 0 + salt 5HCl + Mg(OH) 2 and Al(OH) 3  5H 2 0 + MgCl 2 + AlCl 3

22. Hard and Soft Water A solution of Ca 2+ and Mg 2+ ions is called hard water because soap does not lather up very well in it. –The Ca 2+ and Mg 2+ replace the sodium or potassium ions in the soap and become insoluble

23. Buffer Buffers act as a reservoir for hydrogen ions, donating or removing them from solution as necessary. a solution that can receive moderate amounts of either acid or base without the significant change in its pH.

24. Buffer A buffer is a mixture of a weak acid with the salt of the acid. If small amounts of acid is added, hydronium ions are neutralized by reacting with the salt in solution If small amounts of base is added, hydroxide ions are neutralized by reacting with the acid.

25. Protein Buffer System Intracellular Fluid Blood Plasma Red Blood Cells –Hemoglobin Blood Plasma –Albumin

26. Protein Buffer Systems carboxyl group (—COOH) amino group (—NH 2 );

27. Protein Buffer Systems carboxyl group (—COOH) –Releases H + ↑pH

28. Protein Buffer Systems amino group (—NH2); –Forms NH 3 + ↓pH

29. 20 Amino Acids

30. Hemoglobin

31. The protein hemoglobin is an important buffer of H+ in red blood cells. As blood flows through the systemic capillaries, carbon dioxide (CO2) passes from tissue cells into red blood cells, where it combines with water (H2O) to form carbonic acid (H2CO3). Once formed, H2CO3 dissociates into H+ and HCO3-.

32. At the same time that CO2 is entering red blood cells, oxyhemoglobin (Hb-O2) is giv­ ing up its oxygen to tissue cells. Reduced hemoglobin (deoxyhe-moglobin) is an excellent buffer of H+, so it picks up most of the H+. For this reason, reduced hemoglobin usually is written as Hb-H. The following reactions summarize these relations

33. Hemoglobin Brown 65,000 Daltons 4 sub units

34. Hemoglobin

35. Carbonic Acid- Bicarbonate Carbonic acid –H 2 CO 3 –weak acid Bicarbonate ion –HCO 3 - –weak base

36. Carbonic acid-bicarbonate buffer system

37. carbonic acid-bicarbonate buffer system

38. Carbonic Acid- Bicarbonate

40. carbonic acid-bicarbonate buffer system

41. Phosphate Buffering System

45. Intracellular Fluid Cytosol Kidneys

46. Exhalation of CO 2

47. Breathing and pH levels

48. Negative Feedback Loop

49. Kidney Excretion of H +

52. Summary of Mechanisms that Maintain pH of Body Fluids MechanismComments Buffer SystemsMost consist of a weak acid and the salt of that acid, which functions as a weak base. They prevent drastic changes in body fluid pH. ProteinsThe most abundant buffers in body cells and blood. Histidine and cysteine are the two amino acids that contribute most of the buffering capacity of proteins. Hemoglobin inside red blood cells is a good buffer.

53. Summary of Mechanisms that Maintain pH of Body Fluids MechanismComments Carbonic acid- bicarbonate Important regulator of blood pH. The most abundant buffers in extracellular fluid (ECF). PhosphatesImportant buffers in intracellular fluid and in urine.

54. Summary of Mechanisms that Maintain pH of Body Fluids MechanismComments Exhalation of CO 2 With increased exhalation of C0 2, pH rises (fewer H+). With decreased exhalation of CO 2, pH falls (more H + ). KidneysRenal tubules secrete H + into the urine and reabsorb HCO 3 - so it is not lost in the urine.

55. pH Summary Acids dissociate in water to increase the concentration of H +. –pH values lower than 7 Bases combine with H + ions when dissolved in water, thus decreasing H + concentration. –pH values above 7 Buffers act as a reservoir for hydrogen ions, donating or removing them from solution as necessary.

56. Calibration of pH Meter Use pH standards –pH 7 –pH 10

57. Calibrate pH Meter

58. Steps: Turn the pH meter on by pressing the “on/off” button. Remove the pH electrode from the green pH 7 solution and rinse the electrode well with distilled water into the “waste” 600ml beaker..

59. Place the electrode into the orange pH 4 solution, and press “cal”. Observe the digital numbers in the readout window, when the numbers stop changing press the “read” button. The display should now read 4.00

60. Rinse Electrode each time

61. Calibrate pH Meter

63. 24 well container

64. Read pH of Solutions

65. Ammonia Predict pH

66. Apple Juice Predict pH

67. Baking Soda Predict pH

68. Berry Juice Predict pH

69. Bleach Predict pH

70. Grapefruit Juice Predict pH

71. Mylanta Predict pH

72. Phillips’ Milk of Magnesia Predict pH

73. Tomato Juice Predict pH

74. Vinegar Predict pH