\"You will learn about acetic acid (CH3COOH) and how to determine the concentrat
ID: 1026467 • Letter: #
Question
"You will learn about acetic acid (CH3COOH) and how to
determine the concentration of acetic acid in vinegar
through titration. You will explore the concepts of
stoichiometric equilibrium, concentration, molarity,
indicators, and mass percent."
A) What challenges would you encounter with the titration if you had used apple cider vinegar or balsamic vinegar as the analyte instead of white vinegar?
B) How would your results have differed if the tip of the titrator was not filled with NaOH before the initial volume reading was recorded? Explain your answer.
C) How would your results have differed if you had over-titrated (added drops of NaOH to the analyte beyond the stoichiometric equivalence point)?
Explanation / Answer
Answer (A) Other vinegar contain other chemicals that may have interfered or negated results while white vinegar contains only acetic acid. Additionally, balsamic and apple cider vinegar are dark in color which would make it difficult to identify a color change. These reasons make white vinegar teh best option for use.
Answer (B) If the tip of the titrate was not filled withnNaOH before the initial volume reading was recorded then the initial volume reading wouild likely subsequently be inaccurate. This would the skew all the subsequent readings afterwards. While it did not take a very noticeable amount to fill the stopcock, the measurements were down to the tenth of an mL and it took at least 3-4 10ths to clear the air at the start of the experiment. This was more than enough to skew the result of the experiment.
Answer (C) The results would have differed as the percentage of acetic acid that was calculated would have been greater than the actual percentage within the sample. The data recorded would have indicated a large amount of NaOH required to neutralize the acid within the vinegar.
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