Acids Bases - Lesson 3 - pH & pOH
Transcript of Acids Bases - Lesson 3 - pH & pOH
![Page 1: Acids Bases - Lesson 3 - pH & pOH](https://reader034.fdocuments.us/reader034/viewer/2022052410/547ab71eb4af9fd3158b4bd6/html5/thumbnails/1.jpg)
Acids & Bases Equilibria
pH & pOH
![Page 2: Acids Bases - Lesson 3 - pH & pOH](https://reader034.fdocuments.us/reader034/viewer/2022052410/547ab71eb4af9fd3158b4bd6/html5/thumbnails/2.jpg)
What is the [H3O+] of a solution which has a [OH-] of 1.0 x 10-9 M at 25oC? Is this solution acidic or basic?
Kw = [H3O+][OH-]
1 x 10-14 = [H3O+][1 x 10-9]
[H3O+] = 1 x 10-5 M
![Page 3: Acids Bases - Lesson 3 - pH & pOH](https://reader034.fdocuments.us/reader034/viewer/2022052410/547ab71eb4af9fd3158b4bd6/html5/thumbnails/3.jpg)
Expressing acidity or basidity by moles per liter takes a long time!!
So we use the pH & pOH scale.
Recall pH of:
0 – 7 is acidic 7 – 14 is basic
Opposite for pOH: 0 – 7 is basic 7 – 14 is acidic
![Page 4: Acids Bases - Lesson 3 - pH & pOH](https://reader034.fdocuments.us/reader034/viewer/2022052410/547ab71eb4af9fd3158b4bd6/html5/thumbnails/4.jpg)
pH = - log [H+]
pOH = - log [OH-]
pH + pOH = 14
![Page 5: Acids Bases - Lesson 3 - pH & pOH](https://reader034.fdocuments.us/reader034/viewer/2022052410/547ab71eb4af9fd3158b4bd6/html5/thumbnails/5.jpg)
What is the pH of a solution with a [H3O+] of 1 x 10-5 M?
pH = - log (1 x 10-5)
pH = - log [H+]
pH = 5
![Page 6: Acids Bases - Lesson 3 - pH & pOH](https://reader034.fdocuments.us/reader034/viewer/2022052410/547ab71eb4af9fd3158b4bd6/html5/thumbnails/6.jpg)
What is the pH of a solution that contains 1.0 x10–2 M of H+?
pH = - log (1 x 10-2)
pH = - log [H+]
pH = 2
![Page 7: Acids Bases - Lesson 3 - pH & pOH](https://reader034.fdocuments.us/reader034/viewer/2022052410/547ab71eb4af9fd3158b4bd6/html5/thumbnails/7.jpg)
What is the pH of a solution that contains 5.0 x10–12 M of H+?
pH = - log (5 x 10-12)
pH = - log [H+]
pH = 11.30
![Page 8: Acids Bases - Lesson 3 - pH & pOH](https://reader034.fdocuments.us/reader034/viewer/2022052410/547ab71eb4af9fd3158b4bd6/html5/thumbnails/8.jpg)
What is the pH of a solution that contains 1.0 x10–7 M of H+? pOH?
pH = - log (1 x 10-7)
pH = - log [H+]
pH = 7
pH + pOH = 14
pOH = 7
![Page 9: Acids Bases - Lesson 3 - pH & pOH](https://reader034.fdocuments.us/reader034/viewer/2022052410/547ab71eb4af9fd3158b4bd6/html5/thumbnails/9.jpg)
What is the pOH of a solution that contains 6.4 x10–10 M of OH-? pH?
pOH = - log (6.4 x 10-10)
pOH = - log [OH-]
pOH = 9.19
pH = - log [H+]
pH = - log (1.56 x 10-5)
pH = 4.81
![Page 10: Acids Bases - Lesson 3 - pH & pOH](https://reader034.fdocuments.us/reader034/viewer/2022052410/547ab71eb4af9fd3158b4bd6/html5/thumbnails/10.jpg)
A solution of 0.25M HCN is prepared in water at 25oC. What is the pH of the solution? pOH?
pH = - log (0.25)
pH = - log [H+]
pH = 0.60
pH + pOH = 14
pOH = 13.40
HCN + H2O H3O+ + CN-
ACID BASE
![Page 11: Acids Bases - Lesson 3 - pH & pOH](https://reader034.fdocuments.us/reader034/viewer/2022052410/547ab71eb4af9fd3158b4bd6/html5/thumbnails/11.jpg)
What is the pH of black coffee at 25oC if [OH-] is 2.0 x 10-10 M?
pOH = - log (2.0 x 10-10)
pOH = - log [OH-]
pOH = 9.70
pH = - log [H+]
pH = - log (5 x 10-5)
pH = 4.30
pH + pOH = 14
![Page 12: Acids Bases - Lesson 3 - pH & pOH](https://reader034.fdocuments.us/reader034/viewer/2022052410/547ab71eb4af9fd3158b4bd6/html5/thumbnails/12.jpg)
A solution of 0.09M NH3 is prepared in water at 25oC. What is the pH?
pOH = - log (0.09)
pOH = - log [OH-]
pOH = 1.05
pH + pOH = 14
pH = 12.95
NH3 + H2O NH4+ + OH-
BASE
![Page 13: Acids Bases - Lesson 3 - pH & pOH](https://reader034.fdocuments.us/reader034/viewer/2022052410/547ab71eb4af9fd3158b4bd6/html5/thumbnails/13.jpg)
What is the [H+] of a solution if the pH is 3.7?
[H+] = 1.995 x 10-4 M
[H+] = 10- pH
[OH-] = 10 - pOH
[H+] = 10- 3.7
![Page 14: Acids Bases - Lesson 3 - pH & pOH](https://reader034.fdocuments.us/reader034/viewer/2022052410/547ab71eb4af9fd3158b4bd6/html5/thumbnails/14.jpg)
What is the [H+] solution if the pH is 9.62?
[H+] = 2.40 x 10-10 M
[H+] = 10- pH
[H+] = 10- 9.62
This makes sense, because the [H3O+] < [OH-] so basic &
pH is basic
![Page 15: Acids Bases - Lesson 3 - pH & pOH](https://reader034.fdocuments.us/reader034/viewer/2022052410/547ab71eb4af9fd3158b4bd6/html5/thumbnails/15.jpg)
What is the [OH-] of a solution if the pOH is 5.4? pH? [H+]?
[OH-] = 3.98 x 10-6 M
[OH-] = 10- pOH
[OH-] = 10-5.4
pH + pOH = 14
pH = 8.6
[H+] = 10- pH
[H+] = 10-8.6
[H+] = 2.51 x 10-9 M
Does [H+] x [OH-] = Kw?
![Page 16: Acids Bases - Lesson 3 - pH & pOH](https://reader034.fdocuments.us/reader034/viewer/2022052410/547ab71eb4af9fd3158b4bd6/html5/thumbnails/16.jpg)