Final answer:
Without the exact concentration of acetic acid in the vinegar, it's not possible to determine the precise volume of 0.25 M NaOH needed to react with it. We need equivalent moles of NaOH to react with the acetic acid, following a 1:1 stoichiometry.
Step-by-step explanation:
To calculate the volume of 0.25 M NaOH needed to react completely with the acetic acid in an 8.3 mL vinegar sample, we must first know the concentration of acetic acid in the vinegar. Vinegar typically contains 5% acetic acid by volume, so we can assume that the 8.3 mL of vinegar is equivalent to 8.3 mL of a 0.5 M acetic acetic acid solution. However, since we are not given the exact concentration of acetic acid in the vinegar sample, determining the precise volume of NaOH needed is not possible without that information.
Nevertheless, the idea is that the reaction follows a 1:1 stoichiometry:
CH3COOH + OH- → CH3COO- + H2O
Therefore, equivalent moles of acetic acid would react with equivalent moles of NaOH. In theory, we would use the molarity of acetic acid and the volume of vinegar to find the moles of acetic acid. Then, we would use the number of moles and the molarity of the NaOH solution to find the required volume of NaOH.