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Experiment #3: Distillation
Giana Coach
Giana Coach and Amara Kincaid
February 21, 2024
February 28, 2024
Distillation Experiment #3
Abstract:
Distillation is used to separate liquids from nonvolatile solids. There are four types of distillation:
fractional, vacuum, simple, and steam. This experiment will use simple distillation to distillate the
chemical compound, acetone. Simple distillation is used to purify liquids that contain either
nonvolatile impurities (like salts) or very small amounts of high/low boiling liquids. When trying to
distillate acetone, multiple factors were noted during the experiment. The primary tool that was used
for this experiment was a simple distillation apparatus, which consisted of a 19.22 round bottom
flask, a graduated cylinder, a hose, a water spout (this will serve as the source of water), a hot plate, a
clamp, a condenser, a thermometer, rubber bands, and the distillation apparatus itself. Using these
tools, the apparatus can be set up, and the acetone will begin to boil. When a continuous stream of
bubbles appears from the flask, it will begin to condensate and start distilling the acetone. Following
this guideline, a conclusion was made that a compound’s distillation point will correlate with it’s
boiling point. Acetone has an average boiling point of 56 °C, whereas the distillation point (the
highest temperature recorded from the apparatus) was 54 °C. The proximity of temperatures will help
justify why distillation is heavily dependent on a compound’s boiling point.
Introduction:
Distillation is a technique used to separate and purify liquids. This technique is crucial in laboratory
procedures because it helps purify volatile liquids. This technique is essential in certain laboratory
procedures because it helps purify volatile liquids and estimate their boiling points. With the use of a
simple distillation apparatus and a hot plate, we can get a more in-depth analysis of the distillation
process as we observe the acetone boil, condense, and eventually distillate. Furthermore, it’s
important to know that acetone has an average boiling point of 56 °C, so this means the distillation
point will fall in that temperature range.
:
Experimentation:
Name
Acetone
Average Mass
58.079 Da
Molecular Formula
C₃H₆O
Molecular Weight
58.08 g/mol
Melting Point
-95 ℃
Boiling Point
56 ℃
Solubility
193 g/L
Density
0.79 g/mL
Appearance
Colorless liquid with “sweet” odor
Hazard?
Yes (highly volatile)
Flash Point
-18 ℃
Before any data can be obtained, the simple distillation apparatus must be set up. Obtain a 19.22
round bottom flask, a graduated cylinder, a clamp, a condenser, a distillation apparatus, a few rubber
bands, and a thermometer. Plug in the hot plate, set it to the highest temperature possible, and pour
30 milliliters of acetone into the flask using the graduated cylinder. Obtain a crucible and place the
sand in it; this will serve as the sandbag. Lower the flask into the crucible and lock it in place using
the clamp. Set up the apparatus and observe the flask. Grab a hose and hook one end to the water
sprout and the other end to the apparatus; once the hose is secured, turn the water on and make sure it
flows at a steady rate. Observe the apparatus until the flask is nearly empty, and closely monitor the
thermometer. Once the acetone boils, make sure it distills at one drop per second, and closely monitor
the flask until it is nearly empty. Once the flask has a small amount of acetone left, record the highest
temperature on the thermometer. Let the flask and crucible cool and begin the disposal process.
Disassemble the apparatus and turn off the hot plate. Dispose of the acetone via waste disposal and
place the lab equipment back into their respective places.
Results/Discussion:
From the experiment, we could see that the distillation point of acetone was almost equal to the
boiling point of acetone. After observing the acetone boil, condensate, and distillate, the distillation
point was 54 °C. The hot plate was set to 500 °C, and the acetone hit its boiling point about an hour
into the experiment.
From the experiment, we could see that the acetone took an extremely long time to boil, even though
the hot plate was turned to the highest temperature. It took at least an hour for the acetone to boil, and
it took even longer for it to condensate and distillate. From the experiment, we came to the
conclusion that distillation is directly related to the boiling point of a compound. This is evident if we
take a look at the temperatures in the experimentation table and the results table.
Acetone is the simplest of all ketones and a very weak acid. Acetone is primarily used as a chemical
remover and can be used to remove nail polish, paint, varnish, and much more. By looking at the
structural formula of acetone, we can see it has all the elements of a ketone. Ketones are usually
weak acids that can be found in the body. If ketone levels become too high (too acidic), it can lower
the pH of blood and cause ketoacidosis. Like the previous experiment, we are not sure which acetone
we are using, but it can be assumed that this acetone and the previous acetone are the same. This is
more evident if you take a look at how the distillation point was nearly identical to the average
boiling point of acetone. Therefore, distillation is dependent on a substance’s boiling point.
:
Acetone
Temperature of Hot Plate
500 °C
Highest Temperature Obtained
54 °C
Conclusion:
Using the distillation apparatus, thermometer, and hot plate, the acetone was tested, and the
distillation point was nearly identical to the boiling point of acetone. Upon observation of the
distillation process, we noticed that the temperature increases at a slightly slower rate in comparison
to the boiling point process. What we did notice and record was that the distillation point (54°C) was
close to the average boiling point of acetone (56 °C).This leads us to believe that the distillation and
boiling point methods are directly linked to each other and completely dependent on one another.
:
References:
1. National Library of Medicine, “PubChem Compound Summary for Acetone,”
PubChem,
https://pubchem.ncbi.nlm.nih.gov/compound/Acetone
2. The American Chemical Society and Division, “ACS Publications Recycling of Waste
Acetone by Fractional Distillation,”
ACS Publications,
https://pubs.acs.org/doi/10.1021/ed2001158
3. Department of Climate Change, Energy, Environment, and Water, “DCCEWW Acetone
General Information and Volatility,”
DCCEEW,
:
https://www.dcceew.gov.au/environment/protection/npi/substances/factsheets/acetone#:~:text=It%20is%20highly%20flammable.,by%20the%20National%20Polluta
nt%20Inventory.
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