1. WARM UP 1. Write the equation for the neutralization reaction between sulfuric acid (H 2 SO 4 ) and ammonium hydroxide (NH 4 OH).

2. Acid/Base Titration

3. Titrations

4. Find concentration of unknown acid or base – Add standard solution of acid/base (known concentration) to neutralize unknown – Calculate moles of OH - /H + in standard added Use molarity and liters – Moles of standard = moles of unknown – Calculate molarity of unknown Use moles and liters of unknown

5. WRAP UP Describe why an indicator is helpful in finding the equivalence point.

6. WARM UP 128 mL of.650 M LiOH was required to completely neutralize 50 mL of nitric acid (HNO 3 ) solution. What was the concentration of the nitric acid solution?

7. WRAP UP 128 mL of.650 M Ba(OH) 2 was required to completely neutralize 50 mL of nitric acid (HNO 3 ) solution. What was the concentration of the nitric acid solution?

8. WARM UP 1.List 5 reasons water can be considered both an acid and a base.

9. WRAP UP 1.Calculate the H + concentration in a.01M solution of potassium hydroxide.

10. WARM UP Determine the pH of a.73M HCl solution. Determine the pH of a.92M NaOH solution.

11. WRAP UP Calculate the OH concentration in a solution with a pH of 12.4.