1. The pH scale and what does it mean?
Acid/Base Chemistry
The pH scale and what does it mean?

2. pH What is it? What does it mean? How do you measure it?
Can you determine other things from pH?

3. pH an Overview
pH is the measure of the concentration of hydrogen ions is a solution. pH is measured on a log scale.
pH = - log[H+]
pH is used to indicate the degree of acidity or alkalinity (basic) of a solution.
A solution is of a water solvent (polar)

4. When there is a high [H+], the solution is acidic.
On the other hand when the [H+] concentration is low, the solution is basic.
So if there is a high [H+], there must be a low [OH-]
If there is a low [H+], there must be a high [OH-]
So what does H+ and OH- create?
H2O

5. Water
Pure water should have a neutral pH, due to have equal amounts of [H+] & [OH-].
Acid and bases are created by adding polar molecules to water to increase [H+], or increase [OH-]
The pH scale is used to measure the acidity or alkalinity of a solution.

6. Representative pH Values
pH Scale
The pH scale ranges from 0 to being the most acidic and 14 being the most basic.
So what does the pH tell us about [H+] of a solution?
If something has a pH of:
pH 1 = [H+] = 0.1 M
pH 2 = [H+] = 0.01 M
pH 3 = [H+] = 0.001M
pH 4 = [H+] = M
pH 5 = [H+] = M
pH 6 = [H+] = 1X 10-6M
pH 7 = [H+] = 1X 10-7M
pH 8 = [H+] = 1X 10-8M
pH 9 = [H+] = 1X 10-9M
pH 10=[H+] = 1X 10-10M
pH 11=[H+] = 1X 10-11M
pH 12=[H+] = 1X 10-12M
pH 13=[H+] = 1X 10-13M pH 14=[H+] = 1X 10-14M
Representative pH Values
Substance pH
battery acid
0.5
gastric acid
lemon juice
2.4
cola
2.5
vinegar
2.9
orange juice
3.5
acid rain
tea
5.5
milk
6.5
pure water
7.0
saliva
blood
sea water
8.0
soap
ammonia
11.5
household bleach
12.5
lye (sodium hydroxide)
13.5

7. How to Figure it out?
If you were given HCl with a concentration of 0.003M, what would be the pH? pH = -log [H+] pH = -log[0.003M] pH = 2.52 pH will not have a unit!!!

8. How does pH and pOH relate?
pH and pOH relate in the following way pH + pOH = 14 pOH is the measure of the [OH-], in a solution. What would be the pOH of an solution with a pH of 5.75? pOH = pOH = 8.25

9. If given pH
To determine the concentration from pH, one must do the following: [H+] = 10 (-pH) So what is the [H+] of a solution with a pH of 12.05? [H+] = 10 (-12.05) [H+] = 8.91 X M
antilog

10. Sample Problem 1
What is the pH and pOH of an solution with [H+] of 3.33 X 10-9 M? 1st solve for pH pH = -log [H+] pH = - log[3.33 X 10-9 M] pH = nd  solve for pOH pOH = 14 – pH pOH = pOH = 5.52 (acidic)

11. Sample Problem 2
What is the [H+] of a solution with a pOH of 4.14? 1st  determine pH pH = 14 – pOH pH = 14 – 4.14 pH = 9.86 (basic) 2nd determine [H+] [H+] = 10 (-pH) [H+] = 10 (-9.86) [H+] = 1.38 X M

12. Sample Problem 3
What is the pH of a solution with a [OH-] = 2.35 X 10-9? 1st determine pOH pOH = -log [OH-] pOH = -log[2.35X10-9 M] pOH = nd determine pH pH = 14 – pOH pH = pH = 5.37 (acidic)

13. Sample Problem 4 4.57g HCl 1 mol HCl = 0.125 mol HCl 36.46 g HCl
What is the pH of a solution that was made from 4.57g of HCl dissolved in 750 mL of water? 1st  determine moles of HCl
4.57g HCl
1 mol HCl =
0.125 mol HCl
36.46 g HCl

14. Sample 4 ….
2nd determine concentration of [H+], since this is an acid the [H+] would be the same as the concentration of the whole molecule of HCl. We will get [H+] & [Cl-], both with the total of moles each. So concentration will be moles / volume (L) [H+] = moles/ L [H+] = 0.333M

15. Problem 4…
Next determine pH pH = -log [H+] pH = -log [0.333M] pH = 0.48 (very acidic)

16. Your Turn.. What is the [H+] of an acid with a pH of 5.56?
Determine the pH of a M HCl?
Determine pOH of a solution with a pH of 8.65?
What is the pH of a base with an [OH-] of X10-5 M?
Ans:
X 10-6M