(Solved): Part B. Analysis of Vinegar 1. Determine the volume of the vinegar sample used by subtracting the f ...

Part B. Analysis of Vinegar 1. Determine the volume of the vinegar sample used by subtracting the final burette volume from the initial burette volume. 2. Determine the volume of \( \mathrm{NaOH} \) used by subtracting the final burctte volume from the initial burette volume. 3. Determine the moles of \( \mathrm{NaOH} \) used (and thus the moles of acetic acid present) by multiplying the volume of \( \mathrm{NaOH} \) solution used, in liters, by the average molarity of the \( \mathrm{NaOH} \) solution from Table 21-1. 4. Calculate the molarity of acctic acid in the vinegar by dividing the moles of aceric acid in the sample by the sample volume, in liters. 5. Record the results of all calculations in Table 21-2. Table 21-2. Questions 1. Since molarity is a concentration unit used mainly by chemists, the concentrations of commercial solutions are normally measured by the percentage of solute in the solution. Household vinegar is a \( 5 \% \) (by volume) solution of acetic acid in water. Assuming that the density of your vinegar is \( 1.0055 \mathrm{~g} \mathrm{~mL}^{-1} \) and the density of acetic acid is \( 1.05 \mathrm{~g} \mathrm{~mL}^{-1} \), use the molarity you measured in the experiment to determine the volume percent of acetic acid in your vinegar sample. 2. Why is the \( 6 \mathrm{M} \mathrm{NaOH} \) selution diluted before titrating the vinegar sample? How might your results be affected if you used the \( 6 \mathrm{M} \) solution rather than the \( 0.3 \mathrm{M} \mathrm{NaOH} \) ? 3. Suppose that instead of a \( 6 \mathrm{M} \) solution, only \( 2 \mathrm{M} \mathrm{NaOH} \) was available in the laboratory to prepare the \( 0.3 \mathrm{M} \mathrm{NaOH} \) needed for your titration. Describe how you would prepare \( \approx 0.3 \mathrm{M} \mathrm{NaOH} \) from a \( 2 \mathrm{M} \mathrm{NaOH} \) solution. 4. You are interested in determining the amount of citric acid present in a sample of 7UP. Will your results be different if you use a sample that has been open for an hour instead of a freshly opened bottle? Explain.