Acid Base Titration Lab Report Discussion

ACID BASE TITRATION OBJECTIVES 1. To demonstrate the basic laboratory technique of titration 2. To learn to calculate molarity based on titrations INTRODUCTION Molarity (M) or molar concentration is a common unit for expressing the concentration of solutions. It is defined as the number of moles of solute per liter of solution (or millimoles of solute per milliliter of solution). The concentration of a basic solution can be determined by titrating it with a volume of a standard acid solution (of known concentration) required to neutralize it. The purpose of the titration is the detection of the equivalence point, the point at which chemically equivalent amounts of the reactants have been mixed. The amount of reactants that have been mixed at
HNO3 and H2SO4 have the same molarity. Why did H2SO4 require about twice the volume of NaOH solution for the titration?

2. Explain the effect of each of the following sources of error on the molarity of NaOH as determined in this experiment stating whether the concentration of NaOH obtained would be too high or too low. a. The buret is contaminated with an acid solution.

b. The buret contains a large air bubble in the tip, which disappears in the course of the titration.

c. A small volume of the acid solution is spilled when you transfer it into the Erlenmeyer flask.

3. Using the molarity of the NaOH solution obtained from your titration, calculate the molarity of a 26.0 mL of CH3COOH solution that requires 32.50 mL of NaOH to reach the