Question

1. Why is a direct titration of the acetlysalicylic acid in the tablet with sodium hydroxide not performed?

	a. Acetylsalicylic acid is a diprotic acid, so a single end point is not possible
	b. Acetylsalicylic acid is a weak acid and does not react very well with sodium hydroxide.
	c. Acetylsalicylic acid is unstable in the presence of sodium hydroxide and will undergo decomposition releasing toxic benzene - to which we do not want our students exposed.
	d. Acetylsalicylic acid undergoes more than one reaction with sodium hydroxide and will not react fast enough in a normal titration.

2. The HCl solution you are using needs to be standardized with Na₂CO₃. If 23.5 mL of HCl is required to react with 0.1127g Na₂CO₃, then what is the concentration of HCl.

3. According to the bottle that the aspirin tablets came in, they contain 325 mg of acetylsalicylic acid (C₉H₈O₄). Determine the number of moles of acetylsalicylic acid in each tablet.

4. How many mL of 0.100 M NaOH is required to react completely with the 325 mg of acetylsalicylic acid in the tablet?

5. If 50.0 mL of 0.100 M NaOH is added to the tablet, how many mL of the HCl (molarity found in question 1) will be required to react with the excess NaOH

6. In the experiment, phenol red will be used as the indicator. What color will phenol red be in a basic solution?

Red

Yellow

Orange

Clear

7. In the experiment, phenol red will be used as the indicator. What color will phenol red be in an acidic solution?

Red

Yellow

Orange

Clear