Question

Suppose you had titrated your vinegar sample with barium hydroxide instead of sodium hydroxide:

Ba(OH)₂ (aq) + 2HC₂H₃O₂ (aq) = Ba(C₂H₃O₂)₂ (aq) + 2H₂)(l)

What volume (in mL) of 0.586 M Ba(OH)2 (aq) must be added to a 5.00mL sample of vinegar to reach the equivalence point?

Answer 1

To determine the volume of 0.586 M Ba(OH)2 needed to titrate a 5.00 mL sample of vinegar, the concentration of acetic acid in vinegar is required. Without it, the calculation cannot proceed.

Step-by-step explanation:

To calculate the volume of 0.586 M Ba(OH)2 needed to neutralize a 5.00 mL sample of vinegar (acetic acid, HC2H3O2), we need to use the stoichiometry of the reaction given: Ba(OH)2 (aq) + 2HC2H3O2 (aq) → Ba(C2H3O2)2 (aq) + 2H2O(l).

First, as the reaction shows, one mole of Ba(OH)2 reacts with two moles of HC2H3O2. To find the moles of acetic acid in the vinegar sample, we would need to know the concentration of vinegar. However, since the concentration is not provided, we cannot calculate an exact volume without this information. Generally, in titration calculations, the volume of titrant can be found by using the molarity of the titrant and the stoichiometry of the reaction.

If the concentration of acetic acid in the vinegar were given, you could calculate the number of moles of acetic acid in 5.00 mL and then use the molar ratio to find the moles of Ba(OH)2 needed. The volume of Ba(OH)2 can then be calculated using its molarity by dividing the moles of Ba(OH)2 by the molarity of the Ba(OH)2 solution.