Question

In the Determination of an Equilibrium Constant lab, you will react acetic acid with ethanol in the presence of sulfuric acid until equilibrium is established. Then, you will titrate the equilibrium mixture with NaOH to determine the acetic acid concentration. Suppose you determine that the added sulfuric acid requires 2.97 mL of NaOH to be neutralized in a blank solution. The equilibrium mixture requires 12.92 mL of NaOH to reach the endpoint. What volume of NaOH should you use to calculate the acetic acid concentration at equilibrium

Answer 1

9.95mL is the volume of NaOH that you must use

Step-by-step explanation:

In the problem, you have in your blanck the presence of an acid as sulfuric acid. That means the blank requires an amount of NaOH to neutraliz its solution.

The volume required for the sample will be:

Volume of the sample - Volume of the blank

Beacuse we don't have to take into account the acidity of the blanck

12.92mL - 2.97mL =

9.95mL is the volume of NaOH that you must use