1. Acid/Base Titration Buffers

2. Buffers A mixture composed of a weak acid and its conjugate base (acidic buffer) OR weak base and its conjugate acid (basic buffer) Allow small amounts of acids and bases into a solution without a huge change in the solution’s pH Buffer capacity—trait of buffers indicating how much strong acid/base can be tolerated before a solution’s pH changes drastically.

3. Why are buffers important to us? Buffers present in our body keep fluids within a certain pH range. Blood has a pH range of approximately 7.3-7.4. A buffer involving H 2 CO 3 /HCO 3 - maintains the blood pH

4. Titration Used to determine UNKNOWN concentrations of solutions through a solution of KNOWN concentration. An acidic or basic solution of KNOWN concentration is added to an acidic/basic solution of UNKNOWN concentration. Indicators such as phenolphtalein display a change when all of the acid or base has been neutralized.

6. Titration Terminology End Point: point in a titration where a change is observed due to indicator. Equivalence Point: point in a titration where enough base or acid is present to neutralize the acidic or basic solution. We can plot a titration on a graph—titration curve

10. Calculations M a V a = M b V b Where M is the molarity & V is the volume Used to determine final concentration vs original concentration. Solve like you would dilution problems.

11. Example 1: If 20.0ml of 0.0100M aqueous HCl is required to neutralize 30.0ml of an aqueous solution of NaOH, determine the molarity of the NaOH solution.

12. Example 2 A 15.5 ml sample of 0.215M KOH solution required 21.2ml of aqueous acetic acid solution in a titration experiment. Calculate the molarity of the acetic acid (CH 3 COOH) solution.

13. Example 3: If 29.96 ml of a solution of Ba(OH) 2 requires 16.08 ml of a 2.303M solution of HNO 3 for complete titration, what is the molarity of the Ba(OH) 2 solution?

14. Homework Titration Problem Set # 1