I. Experiment Title : Recrystallization and Making Aspirin II. Day / Date of Experiment : March 22 nd 2013 III. Finish of Experiment : March 26 th 2013 IV. Objective of Experiment : 1. Doing well recrystallization 2. Determining a suitable solvent for recrystallization 3. Eliminate impurities through recrystallization 4. Doing the manufacture of aspirin by acetylation of the phenol 5. Doing recrystallizing aspirin synthesis with good results V. Basic Theory Recrystallization Recrystallization is one way of purifying solids plural is used, where such substances or solids are dissolved in a solvent and then crystallized again. This method relies on the solubility of a substance in a particular solvent at a time when the temperature increased. Since the total concentration impuriti usually smaller than the concentration of the purified, when cold, the concentration of low impuriti but the temporary solution of high concentration products will precipitate. (Arsyad, 2001). Recrystalitation is routinely used for the purification of compounds synthesized or collation of result from natural ingredients, preanalized further, for example by
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I. Experiment Title : Recrystallization and Making Aspirin
II. Day / Date of Experiment : March 22nd 2013
III. Finish of Experiment : March 26th 2013
IV. Objective of Experiment :
1. Doing well recrystallization
2. Determining a suitable solvent for recrystallization
3. Eliminate impurities through recrystallization
4. Doing the manufacture of aspirin by acetylation of the phenol
5. Doing recrystallizing aspirin synthesis with good results
V. Basic Theory
Recrystallization
Recrystallization is one way of purifying solids plural is used, where such substances or
solids are dissolved in a solvent and then crystallized again. This method relies on the
solubility of a substance in a particular solvent at a time when the temperature increased.
Since the total concentration impuriti usually smaller than the concentration of the purified,
when cold, the concentration of low impuriti but the temporary solution of high concentration
products will precipitate. (Arsyad, 2001).
Recrystalitation is routinely used for the purification of compounds synthesized or
collation of result from natural ingredients, preanalized further, for example by
spectrophotometry (UV, IR, MR, and MS). (Tim Dosen Kimia Organik UNESA, 2013)
Recrystallization is an important method for the purification of organic solvent
component. There are seven methods of recrystallization are: selecting the solvent, the solute
dissolves, color removal solution, remove solids, crystallizing solution, collecting and
washing the crystals, dry products (results) (Williamson, 1999).
Salicilic acid is an acid bifungsional containing two-OH groups and-COOH. Therefore
salicylic acid may be subject to two different types of reactions the reaction of acids and
bases. Salicylic acid (pure) will turn purple if FeCl3 is added, because salicylic acid has a
phenol group that will react with FeCl3. The melting point of salicylic acid is 159 C.
Making of Aspirin
Aspirin is an ester of acetic acid with salicylic acid. Therefore, this compound can be prepared by reacting salicylic acid with acetic anhydride using sulfuric acid as a catalyst. With reaction :
(Tim Dosen Kimia Organik Unesa, 2013)
In the manufacture of aspirin, salicylic acid (o-hydroxy benzoic acid) serves as the alcoholic and the reaction takes place on the hydroxyl group. The purity of aspirin could diuiji using iron (III) chloride. Before the purified aspirin do recrystallized aspirin beforehand in order to have a pure. Aspirin is used as a fever-lowering drugs, antibiotics, and pain relievers (analgenetika). Aspirin is usually sold as a sodium salt, which is sodium acetyl salicylate (Irdoni, 2010)
The purity of aspirin can be determined by testing the melting point, which should be pure aspirin melting point is 136 ° C. The purity of aspirin can also be tested using iron (III) chloride. Iron (III) chloride reacts with the phenol group of salicylic acid to form a purple complex. Iron (III) chloride is a yellow solution, if the sample is not a remaining salicylic acid sample pure of aspirin) then it will not react with salicylic acid, or color of sample is yellow, like the color of a solution of iron (III) chloride when added Iron (III) chloride.
VI. Tools and Materials
Recrystallization
Tools:
a. Erlenmeyer flask
b. Spatula
c. Buchner funnel
d. pippete
e. electric stove
f. Thermometer
Materials :
a. Salicilic acid
b. Aquades
c. Norit
1 gram salicylic acid
Result
Entered into Erlenmeyer flask 125 mLAdded 5 mL aquadestBoiled and shakedAdded some aquades until crystall is dissolved
Result
- Filtered using Buchner funnel in hot conditions- Cooled
- Filtered back with Buchner funnel- Dried in eksikator- Weighed
Mass =
- Measured the melting pointTemperature =
- Added drops of FeCl3Result
Making Aspirin
Tools:
a. Erlenmeyer flask
b. Spatula
c. Buchner funnel
d. Thermometer
Materials:
a. Salicilic acid
b. Anhidrate salisilic acid
c. concentrated sulfuric acid
d. Ethanol 96%
e. FeCl3 solution
f. Aquades
VII. Procedure
Recrystallization
2,5 gram Salicilic acidAlumunium
Result
- Put in a 125 mL Erlenmeyer- Added 3.75 grams of acetic acid anhydride- Added 3 drops of concentrated H2SO4- Stirred until homogeneous- Heated bath above 50o - 60o C while stirring 5 minutes- Cooled while stirring
- Added 37.5 mL of distilled water
- Filtered with Buchner funnel- Added 7.5 mL of 96% ethanol- Added 25 mL of distilled water- recrystallized- dried in eksikator
Result
Result
weighedMass =
Measures the melting pointTemperature =
Added drops of FeCl3
Result
Making Aspirin
VIII. Observation table
Recrystallization
Treatment Hypothesis Result ConclussionBefore After- Adding aquadest to salicylic acid and
boiled.
- Filtering the solution using Buchner
funnel
- Cooling the colorless filtrate
- Filtering the filtrate using Buchner funnel
- Weighing the crystall
- Measuring the melting point of crystall
- Adding FeCl3 to crystall
Salicylic acid dissolve in aquadest form colorless solution
We get residue and colorless filtrate.
Will form white crystal
The crystal left in filter paper
Mass of crystal is less than sample (<1gram)
The melting point of crystal is ± 159C
Crystal will reacts with FeCl3.The color of crystal changes to dark purple.3 C7H6O3 (aq) + FeCl3 (aq) ------> Fe(C7H5O3)3 (aq) + 3 HCl (aq)
Salicylic acid is white
crystal
The solution is colorless
The solution is colorless
We have colorless solution and crystal in it
Color of crystal = white
Color of FeCl3 = yellow
Form homogeneous
mixture (colorless) with
aquadest
There is little bit residue
and colorless filtrate
There is white crystall in solution
The white crystal left in filter paper
Mass = 0.8 gram
Temperature = 150C
The color of crystall changes to dark purple
The result is suitable with hypothesisWe get pure compound of salicylic acid
Making of Aspirin
Treatment Hypothesis Result ConclussionBefore After- Adding acetic anhydride acid and H2SO4
to salicylic acid and stirred.
- Boilliing the solution untill 50-60C
- Adding aquadest
- Filtering using Buchner funnel
- Recrystalizing the filtrate
- Weighing the crystal
- Measuring the melting point of aspirin
- Adding FeCl3 to crystal
Salicylic acid reacts with acetic anhydride acid form aspirin
The solution become white crystal
The crystal will dissolve form colorless solution
Will get residue and colorless filtrate
Will get white sharp crystal of aspirin
The mass of crystal is less than initial sample (<2.5gram)The melting point of aspirin is 136C
Aspirin is not react with crystal, so the color of crystal still white and FeCl3 solution is yellow
Salicylic acid is white
crystal
The solution is colorless
There is white crystal
The solution is colorless
There is colorless filtrate
Color of crystal = white
Color of FeCl3 = yellow
Form homogeneous
mixture react with acetic
anhydride acid
The solution become
white crystal
Crystal dissolve in water and form colorless solution
We get litlle bit residue and colorless filtrate
Formed white sharp crystal
Mass = 2.021 gram
Temperature = 134C
There is no color changing
The result is suitable with hypothesisWe get pure compound of aspirin
IX. Analysis
Recrystallization
The purpose of this experiment is to purifying salicylic acid from impurities by recrystallization. Firstly, We put 1 gram of crystal salicylic acid into Erlenmeyer flask and add 5 mL aquadest. Initially the crystal does not dissolve, but when we boil and stir it the crystal dissolve and form homogeneous mixture. And then we filter the solution using Buchner funnel and filter paper in hot condittion. We get little bit residue in filter paper and colorless solution as filtrate. It indicates the impurities left in filter paper.
Next step, we let the filtrate cool. And we can see the crystal formed in solution. We filter again the filtrate to get the crystal using Buchner funnel. So we get the white crystal in filter paper and we dry it in desiccator for three days.
After three days we weigh the crystal and get the mass of crystal is 0.8 gram, less than the mass of sample. It indicates the impurities have been separated and we get the pure crystal of salicylic acid. But, to prove it we measure the melting point of crystal that we have got. We get the current temperature melting crystals is 150C. The number of melting point our crystal is different with basic theory. And we do confirmation test by add FeCl3 to crystal and the crystal form dark purple solution. it indicates the crystal that we get contain salicylic acid and react with FeCl3 because there is –OH group in the salicylic acid that will react with FeCl3.
The purpose of this experiment is to synthesis aspirin and purifying it from the impurities using cristallization method. Firstly, we put 2.5 gram salicylic acid to Erlenmeyer flask and add acetic anhydride acid and drops of sulfuric acid. The salicylic acid react with acetic anhydride acid form aspirin. Sulfuric acid that we added act as catalyst. We get the colorless solution of aspirin. With reaction :
Next step, we boil the solution in 50-60C for five minutes and let the solution cool. The solution changes to crystal. And then we added aquadest, the crystal dissolve in aquadest and form homogeneous mixture (colorless).
After we get the colorless solution of aspirin, we do recrystallization to separate aspirin from the impurities or salicylic acid that remain. And then we get white taper crystal of aspirin. And we dry it in desiccator for three days.
After three days we weigh the crystal and get the mass of crystal is 2.021 gram, less than the mass of sample. It indicates the impurities have been separated and we get the pure crystal of aspirin. But, to prove it we measure the melting point of crystal that we have got. We get the melting point of crystals is 134C. The number of melting point our crystal is close with the basic theory, 136C. And we do confirmation test by add FeCl3
to crystal, but there is no reaction occur the color of crystal still white and the color of FeCl3 solution still yellow. It indicates the crystal that we get does not contain salicylic acid because FeCl3 just can react with salicylic acid form dark purple solution. So the crystal that we have got is pure of aspirin.
X. Discussion
In this experiment we have difficulty to measuring the melting point of crystal that we have got. Because the crystal is easy to melt with small range of temperature. So, in the first experiment, recrystallization, we get the melting point of salicylic acid is different with basic theory. In basic theory the melting point of salicylic acid is 159C, but we just get 150C for our crystal. It caused by our accuracy in measure the melting point of crystal.
XI. Conclusion
From the data that we have got we can conclude that we got the pure crystal of salicylic acid in the first experiment by recrystallization method. With the melting point of salicylic acid is 150C and percentage of salicylic acid in sample is 80.0 %.
For the second experiment, making of aspirin. We can conclude that we got pure crystal of aspirin after react salicylic acid and acetic anhydride acid and continued with recrystallization process to separate crystal from impurities. The melting point of our crystal (aspirin) is 134C, It is too close with the melting point in basic theory, 136C. With the percentage of aspirin in sample is 80.8 %.
References
- Arsyad, M.Natsir. 2011, Kamus Kimia Arti dan Penjelasan Istilah, Gramedia,
Jakarta
- Irdoni, HS and Nirwana, HZ. 2009, Modul Kimia Organik, Universitas Riau,
Pekanbaru
- Tim Dosen Kimia Organik Unesa. 2013, Panduan Praktikum Kimia Organik, Unesa
Press, Surabaya
- Williamson. 1999, Macroscale and Microscale Organic Experiments, Houghton
Mifflin Company, USA
Attachment
picture explanation
1 gram salicilic acid add with 5 mL H2O
salicilic acid add with some H2O while heating until the salicilic acid dissolve completely
salicilic acid that completely dissolve filt by using buchner funnel
filtrate of salicilic acid that produce cooled in room temperature
filtrate of salicilic acid that have been cooled filt by using buchner funnel
the crystal of salicilid acid after put into desicator in 4 days. Pure of salicilid acid
crystal that produce have shape as needle but in the sort size
the crystal of aspirine after have been around the step of crystalization and put into desicator for 4 days.
the cystal that produce have shape as grains and soft texture.
crystal of aspirine
crystal of salicilid acid
crystal of aspirine in selinder pipe
the color of the top pipe is white
crystal of salicilid acid in selinder pipe
the color of th e top pipe is white
aspirine after occure the melting point test
the color of the top pipe is black
salicilid acid after accure the melting point test