Titration for Acetic Acid in Vinegar
Hands-On Labs, Inc.
Version 42-0208-00-02 Lab Report Assistant
This document is not meant to be a substitute for a formal laboratory report. The Lab Report
Assistant is simply a summary of the experiment’s questions, diagrams if needed, and data
tables that should be addressed in a formal lab report. The intent is to facilitate students’
writing of lab reports by providing this information in an editable file which can be sent to an
instructor. Exercise 1: Determining the Concentration of
Acetic Acid
Data Table 1. NaOH Titration Volume. Trial 1
Trial 2
Trial 3 Initial NaOH
Final NaOH
Total volume of
Volume (mL)
Volume (mL)
NaOH used (mL)
9 mL
.2 mL
8.8 mL
10 mL
1.1mL
8.9 mL
10 mL
1.2 mL
8.8 mL
Average Volume of NaOH Used (mL) : 8.8 mL Data Table 2. Concentration of CH3COOH in Vinegar.
Average volume of
NaOH used (mL)
8.83 ml Concentration CH3COOH
in vinegar (mol/L)
.88 mol/L % CH3COOH in vinegar
5.31% Questions
A. The manufacturer of the vinegar used in the experiment stated that the vinegar contained
5.0% acetic acid. What is the percent error between your result and the manufacturer’s
statement?
5.302-5
.302 (.302/5.0)
.0604 (.0604*100)
=6.04% B. 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?
Other vinegars 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 while vinegar the best option for use. C. How would your results have differed if the tip of the titrator were not filled with NaOH
before the initial volume reading was recorded? Explain your answer.
If the tip of the titrate was not filled with NaOH before the initial volume
reading was recorded then the initial volume reading would likely subsequently be
inaccurate. This would then 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. D. How would your results have differed if you had over-titrated (added drops of NaOH to the
analyte beyond the stoichiometric equivalence point)?
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 larger amount of NaOH required to neutralize
the acid within the vinegar.
E. If a 7.0 mL sample of vinegar was titrated to the stoichiometric equivalence point with 7.5
mL of 1.5M NaOH, what is the mass percent of CH3COOH in the vinegar sample?
M=. 0075L(1.5mol/1L)(1mol/1mol)(1/. 0075)=1.5
%=(1.5/1)(1/1000)(1/1)(60.05/1)(100)
= 9.008% F. Why is it important to do multiple trials of a titration, instead of only one trial?
It is imperative to the accuracy of trials to perform multiple trials as this will
minimize error and reduce the risk of human error as you will have a better idea of
what to do the more times you try the experiment. Multiple trials will also offer an
average of results as opposed to simply 1 and this will result in a greater level of final
accuracy.

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