1. Monday May 18 Objective: Calculate the pH of any solution. Checkpoint:
Write the dissociation equations for the following acids and bases:
HCO3- 
NaOH 
Calculate the pH of the following solutions:
An HCl solution that is 1.0 x 10-3 M.
[HBr] = 1.0 x 10-5 M.
[H+] = 6.32 x 10-4 M
Homework:
pH worksheet (due Tuesday)

2. Arrhenius Acids and Bases
Acid: increases [H+] in solution.
Base: increases [OH-] in solution
Checkpoint:
HCO3- 
NaOH  H+ +
CO32-
Na+ +
OH-

3. pH = -log[H+] pH = -log[1.0 x 10-3] pH = -(-3) pH = 3, acidic
What is the pH of a solution of an HCl solution that is 1.0 x 10-3 M?
pH = -log[1.0 x 10-3]
pH = -(-3)
pH = 3, acidic

4. pH = -log[H+] pH = -log[1.0 x 10-5] pH = -(-5) pH = 5, acidic
What is the pH of [HBr] = 1.0 x 10-5 M?
pH = -log[1.0 x 10-5]
pH = -(-5)
pH = 5, acidic

5. pH = -log[H+] pH = 3.2, acidic pH = -log[6.32 x 10-4 ]
What is the pH of [H+] = 6.32 x 10-4 M?
pH = -log[6.32 x 10-4 ]
pH = 3.2, acidic

6. 5/5 with color, 4/5 without color
pH poster due today
5/5 with color, 4/5 without color

7. HCl  H+ + Cl- NaOH  Na+ + OH- Strong Acids and Bases 100 100 100 100
1000
1000
1000
1000
1000
1000
1,000,000
1,000,000
1,000,000
1,000,000
1,000,000
1,000,000

8. HCN  H+ + CN- NH3 + HOH  NH4 + + OH- Weak Acids and Bases 100 5 5 50
5% dissociation
HCN  H CN-
100 5 5 50
1000 50
1% dissociation
NH3 + HOH  NH OH-
100 1 1
1,000,000
10,000
10,000

9. pH = -log[H+] pH = -log[0.012] pH = 1.92, acidic =
What is the pH of a solution that is made from dissolving 0.87 grams HCl into 2.0 L of water?
0.87 grams
1 mol
M = mol / 2.0 L
= M = x
0.024 mol
36.46 g
pH = -log[0.012]
pH = 1.92, acidic

10. pOH = -log[OH-] pH + pOH = 14
What is the pH of a solution that has 1.0 x 10-3 M NaOH concentration? Is it acidic, basic, or neutral?
pOH = -log[1.0 x 10-3]
pOH = -(-3)
pH + 3 = 14
pH = 11, basic

11. pOH = -log[OH-] pH + pOH = 14
What is the pH of a solution that has 1.0 x 10-2 M KOH concentration? Is it acidic, basic, or neutral?
pOH = -log[1.0 x 10-2]
pOH = -(-2)
pH + 2 = 14
pH = 12, basic

12. pOH = -log[OH-] pH + pOH = 14
What is the pH of a solution that has [OH-] = 3.4 x 10-5 Is it acidic, basic, or neutral?
pOH = -log[3.4 x 10-5]
pOH = 4.47
pH + (4.47) = 14
pH = 9.53, basic

13. pH = -log[H+] pH = -log[0.20] pH = 0.70, acidic 2.0 x 0.10 = 0.20 M
What is the pH of a solution that has 2.0 M of HF, a weak acid? Assume 10% dissociation. Is it acidic, basic, or neutral?
2.0 x 0.10 = 0.20 M
[H+] = 0.20 M
pH = -log[0.20]
pH = 0.70, acidic

15. “Having fun with pH” answer key
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