pre lab model 6
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Dec 6, 2023
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Uploaded by MajorGuineaPig1298
CHM 1046L U12
Kaylyn Keith TA
Date: 9/25/23
Volumetric Analysis Part 2
Purpose:
How to determine the concentration of a HCl solution and the percentage of Acetic Acid in
Commercial Vinegar.
Introduction:
Hydrochloric Acid is an aqueous solution of hydrogen chloride. is a powerful, colorless mineral
acid with numerous industrial applications. (cameochemicals). After formic acid, acetic acid is
the second-simplest carboxylic acid. It is a crucial industrial chemical and reagent. (Wikipedia).
Any species that raises the concentration of protons or H+ ions in an aqueous solution is
considered an Arrhenius acid. Any species that raises the concentration of H+ is Arrhenius acid.
Any species that raises the concentration of OH+ is an Arrhenius base. (khanacademy.org). Like
Arrhenius acid, a Bronsted-Lowry acid is a substance that decomposes in solution to produce an
H+. The base produces OH+. In Lewis Acid The attacking electron pair is accepted by the
Hydronium ion's H+ atom, forming a connection. Lewis Base Hydroxide contributes an electron
pair to H+ to form a bond. (leah4sci).
Procedures:
A 100 mL beaker was washed and prepared well. And rinsed with an unknown HCl solution.
Then it was filled with the HCl solution and labeled. A 10mL volumetric pipet was rinsed with
DI water then with small amount of HCl solution. The rinsed HCl was pipetted into a 50mL
beaker and disposed in the waste container. 10mL volumetric pipet was used to deliver 10mL
aliquots of HCl solution into three numbered 250 ml Erlenmeyer flasks. Then a phenolphthalein
indicator was added to every flask and titrated with NaOH until the end point. All data was
recorded in the table.
The Molarity, deviation from the average, the average deviation, and the relative average
deviation (RAD) in ppt of HCl were calculated. The RAD should have been precisely less than
or equal to 5.0 ppt before moving to the next part of the experiment. If it was obtained more than
5.0 ppt the more performs should have done to get that precision.
A 10 mL aliquot of commercial vinegar was pipetted into a 100 mL volumetric flask and diluted
to the mark with DI water. Shaked well. Three 10 mL aliquots of the diluted vinegar were titrated
against the standard NaOH solution using the indicator phenolphthalein. All data were recorded.
The average molarity of the diluted vinegar solution was calculated accordingly.
The RAD
should have been precisely less than or equal to 5.0 ppt before moving to the next part of the
experiment. If it was obtained more than 5.0 ppt the more performs should have done to get that
precision.
The molarity of the undiluted sample was calculated using the average molarity of the diluted
vinegar solution that was calculated, Assuming the density of the vinegar is 1 g/mL. The molarity
of acetic acid was converted to grams of acetic acid per liter of solution, then into percent by
weight acetic acid. The bottle of vinegar was consulted and compared the experimental value
with the value listed on the bottle.
Pre-lab questions:
1-
Reaction between hydrochloric acid and sodium hydroxide:
HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)
Reaction between acetic acid and sodium hydroxide:
CH3COOH(aq) + NaOH(aq) → CH3COONa(aq) + H2O(l)
2-
As HCl is a strong acid compared to Acetic acid, it dissociates almost completely, on the
other hand, the Acetic acid does not dissociate completely. As known the greater the
number of free H+, the lower the value of pH for that acid. Inferring from that the second
reaction will have higher pH. (
chem.libretexts.org).
Lab safety precautions:
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When creating diluted solutions, always add acid or base to water rather than the other way
around.
NaOH should be properly weighed on a piece of paper. Clean up all spills, dispose of
any chemicals that are no longer needed in a wash basin, and add cold water for drainage. Avoid
using flame in the lab since phenolphthalein is flammable. Use a fire extinguisher or add sand to
the area to block the oxygen supply in case of fire.
References:
1-
Smith, J. A. Titration Experiment Procedure. Chemistry Lab Resources, 2020.
https://www.examplewebsite.com/titration-experiment-procedure
.
2-
sciencebuddies.org/science-fair-projects/Titration-tutorial: Tips/Tricks for Titrating.
2002-
2023 Science Buddies.
https://www.sciencebuddies.org/science-fair-projects/references/titration-tutorial-tips-
tricks-for-titrating
3-
Royal Society of Chemistry. Acid-Base Titration. (Accessed September 15, 2023).
https://www.rsc.org/learn-chemistry/resources/analytical-chemistry/acids-and-bases/acid-
base-titration
4-
Johnson, M. A. Titration Techniques. Chemistry Lab Help. (Accessed August 15, 2023).
https://www.chemlabhelp.com/titration-techniques
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