1. Acid or Alkali
and the relationship
Of pH
Type notes here

2. Acid - a material that has a pH of 1 to 6.9
Terms:
Acid - a material that has a pH of 1 to 6.9
Base - a material that has a pH of 7.1 to 14.
Alkaline – an adjective that describes a material meaning the material has a pH greater than 7.
Alkali – a base.
Type notes here

3. Terms:
5. Ion - a molecule or atom that has an electric charge and is reactive. H+ OH- are the ions involved in pH.
6. Acidic - an adjective that describes a material meaning the material has a pH LESS than 7
Type notes here

4. 7. Neutral – a pH = 7
8. pH- potential of hydrogen ions in a solution. (you can think of this as a percentage) Pure water has a pH of 7
Type notes here

5. Video \\Ranchoviejolx1\apps\USERS\Teachers\Jventule\My Videos\PhySci\Elements_of_Chemistry__Acids__Bases__and_Salts.mov

6. A pH is expressed as a number from 1 to 14
(there is a rare scientific exception with pH range -0 to % of the time, the scale is referred as 1 to 14, and that is the reference in school)
Type notes here

7. How do we measure pH?

8. Water is neutral as it contains equal amounts of OH – and H + ions

9. The mathematical formula to determine pH is: The number of H + ions in solution is expressed in exponent form. The number of the pH is the exponent.

10. A pH of 1 has H ions in solution at a % of 0.1%
0.1= 1x10-1 = pH 1
Type notes here

11. A pH of 2 has H ions in solution at a % of 0.01% .1 = pH 1
.01 = 1x10-2 pH 2
Type notes here

12. A pH of 3 has H ions in solution at a % of 0.001% .1 = pH 1 .01 = pH 2
Type notes here

13. A pH of 4 has H ions in solution at a % of 0.0001% .1 = pH 1
Type notes here

14. A pH of 5 has H ions in solution at a % of 0.00001% .1 = x10-1 pH 1
Type notes here

15. A pH of 7 has a % of H ions in solution of 1 x10-7 or .0000001%
Type notes here

16. A pH of 14 has H ions in a solution with a concentration of%
1x10-14
Type notes here

17. have more OH ions than H ions in solution.
Alkali compounds
have more OH ions than H ions in solution.
Type notes here

18. The more OH ions, the fewer the H ions. Thus the pH increases.
As H+ increases,
As H+ decreases, pH
rises, & OH- increases
pH decreases
and
H ions lessen
OH- decreases H+
OH- H+
OH-

20. 2. turns blue litmus paper to red 3. corrosive-wears away metal
Standard 5a
Reactions
Acids and Bases
Property of Acids
1. tastes sour
2. turns blue litmus paper to red
3. corrosive-wears away metal
4. Acids produce hydrogen ions (H+) in water
HCl H+ + Cl-

21. 1. Tastes bitter & feels slippery 2. turns red litmus paper to blue
Standard 5a
Reactions
Property of Bases
1. Tastes bitter & feels slippery
2. turns red litmus paper to blue
3. Base produces hydroxide ions
(OH-) in water
NaOH  Na+ + OH-

22. Strengths of Acids and Bases
Standard 5a
Reactions
Strengths of Acids and Bases
1. pH scale- determines if it is an acid (0-6) or a base (8-14)
<----Acid Base--->
0 < > 14
Strong acid Neutral Strong base
2. pH= 5 would be an _____
3. pH =9 would be a _____

23. 67
Standard 5a
Reactions
Thursday
March 17
Acids and Bases
Neutralization (~pH 7)
1. In neutralization, an acid reacts with a base to always produce salt and water
HCl + NaOH NaCl + H2O
Acid Base Salt Water

24. Video https://www.youtube.com/watch?v=ujkuW-0cpNw

25. Importance of pH in Biology
pH is important in regulating the nature and rate of chemical reactions necessary to support life.

26. In endothermic organisms (regulate body temperature with metabolic heat: like humans), pH is maintained within a very narrow range.

27. In ectothermic organisms ("cold-blooded") that use behavioral means of regulating body temperature) pH varies inversely with body temperature.

28. Some examples:
pH ultimately controls the rate at which you breathe;
pH determines the dissociation of oxygen and carbon dioxide from hemoglobin (relative to breathing and metabolic process)

29. pH determines the dissociation of chemicals and helps regulate chemical reactions in the body, especially buffer systems and enzymes.

30. pH determines the balance of reactions which occur in aquatic systems relative to things like carbon dioxide, bicarbonates; sulfur.

31. pH induced problems in livestock
Acidosis : change in pH from normal range to acid. Causes: ingestion of acidic feeds; formation of lactic acids; lung problems; suffocation. Symptoms: seizures, confusion, severe muscle pain, nausea, loss of consciousness, coma, death

32. Alkalosis: change in pH from normal range to alkali
Alkalosis: change in pH from normal range to alkali. Causes: hyperventilation, prolonged vomiting, severe dehydration, and eating/drinking alkali plants, liquids or other materials. Symptoms: muscle weakness, severe cramps, tetany, death.

33. pH induced problems in plants
Nutrient shortages.
Increase in toxic minerals able to be absorbed by plant.
Preferences by plants to specific pH ranges (azaleas love pH 5.5-6) )
pH affects pesticide and fertilizer applications, tying up or releasing same

34. An Azalea

35. pH is involved in inorganic chemistry
Reactions between metals (batteries) to form electricity
Swimming pool maintenance – incorrect pH increases algae growth, calcium deposits on pool tile.

36. Measuring pH
1. Indicators - change color based on pH reaction.
2. Electric meter - meter reads based on electrical conductivity

38. pH Measurement Laboratory