(Solved): Heya, need help with this titration worksheet. I'll include the data tables first. The last image wi ...

Heya, need help with this titration worksheet. I'll include the data tables first. The last image will be the questions I need help with. Thank you very much!

Table 1: Reagents Used. \begin{tabular}{|c|c|c|c|c|c|} \hline NAME & FORMULA & STRENGTH & QUALITATIVE Observations & MOLARITY (M) & VOLUME (mL) \\ \hline sodium hydroxide & \( \mathrm{NaOH} \) & Strong Base & Transparent Liquid, more dense than water & \( 1.00 \) & see Table 2 Average \\ \hline ethanoic acid & \( \mathrm{CH} \mathrm{COOH}_{3} \) & Weak Acid & Transparent liquid, strong vinegar smell. & \( ? \) & \( 100 \mathrm{ml} \) \\ \hline \end{tabular} Table 2: Titration Observations. NALYSIS: 1. Use the data you collected from the titration to determine the experimental acid equilibrium constant, ( \( \mathrm{K}_{\mathrm{a}} \) ) for the ethanoic acid. To complete the calculation you will need to do the following: [5T, 5T] A) Calculate the unknown molarity of the ethanoic acid in solution using the titration data collected for its neutralization reaction with the solution of sodium hydroxide. B) Use this molarity and the initial \( \mathrm{pH} \) of the ethanoic acid to calculate the equilibrium molarities of all materials for the ethanoic acid in water equilibrium system and calculate \( \mathrm{K}_{\mathrm{a}} \). 2. At SATP, the theoretical \( \mathrm{K}_{\mathrm{a}} \) value for ethanoic acid is \( 1.8 \times 10^{-5} \mathrm{in} \) pure water: \( [2 \mathrm{~T}, 1 \mathrm{C}, 1 \mathrm{C}] \) A) Calculate percent error of the \( \mathrm{K}_{\mathrm{a}} \) you determined to this standard value. \[ \text { o/ Error }=\left|\frac{\text { Theoretical Value - Experimental Value }}{\text { Theoretical Value }}\right| \times 100 \] B) Identify one potential source of error that may have affected the constant value you determined. (You cannot list human error as a source, assume you performed the experiment properly and in person.) C) Explain how the source of error either increased or decreased \( \mathrm{K}_{\mathrm{a}} \) that was derived from experimental data. XTENSION: 3. The phenolphthalein indicator (HIn) that is used during the titration is actually a weak acid so it sets up its own equilibrium system in the water. A) Write the equilibrium dissociation equation for HIn and the equilibrium law expression, \( \left(\mathrm{K}_{\mathrm{a}}\right) \). [2T]