1. pH of Acids and Bases

2. Arrhenius Acid Base
Acids = H+, Bases = OH-

3. Modified Arrhenius
Uses the idea that the substance will react with water to form H3O+ instead of just H+
Acids = H3O+, Bases = OH-

4. [H3O+][OH-] = 1.00x10-14

5. Example 1
What Is the hydroxide ion concentration in a solution with a hydronium ion concentration of 2.59x10-4M?

6. Example 2
If 2.50g of NaOH was dissolved in water to produce 500mL of solution, what would be the concentration of hydronium and hydroxide ions in solution?

7. Sig Figs and pH
The number of significant digits in the concentration is the number of decimal places in the pH

8. Example 3
What is the pH of a solution of 0.159M HCl?

9. Example 4
What is the hydronium and hydroxide ion concentration of a solution with a pH of 2.42?

10. pOH Potency power of hydroxide!!! Used for BASES!! pOH = -log [OH-]
[OH-] = 10-pOH

11. pH + pOH = 14.00

12. Example 5
A solution has a pH of What are the hydronium ion and hydroxide ion concentrations?

13. Example 6
A solution has a hydronium ion concentration of 1.95x10-4M. What are the pH, pOH and [OH-] values?
pH = 3.710
pOH =
[OH-] = 5.13x10-11M

14. Example 7
A solution of Calcium hydoxide was created using 5.673g of solid in mL of solution. What is the pH, pOH, [OH-] and [H3O+]???
[OH-] = M
pOH =
pH =
[H3O+] = 1.633x10-14M