Preparing a Pure Organic Solid (Oxford AQA International A Level Chemistry)
Revision Note
Written by: Philippa Platt
Reviewed by: Stewart Hird
Required Practical 10: Pure Organic Solid Preparation
Prepare a pure organic solid and test its purity
To prepare a sample of aspirin
HOOCC6H4OH + (CH3CO)2O → HOOCC6H4OCOCH3 + CH3COOH
Apparatus
Preparation of aspirin
salicylic acid
100 cm3 conical flask
10 cm3 measuring cylinder
ethanoic anhydride
concentrated sulfuric acid
400 cm3 beaker
tripod, gauze and Bunsen burner
thermometer
250 cm3 beaker
Buchner funnel
filter paper
stirring rod
deionised or distilled water in a wash bottle
spatula
Recrystallisation and testing the purity
25 cm3 measuring cylinder
boiling tube
ethanol
thermometer
deionised or distilled water in a wash bottle
100 cm3 conical flask
stirring rod
kettle
digital mass balance (reading to 2 decimal places)
thermometer (0 oC to 250 oC)
melting point apparatus
tripod, gauze and Bunsen burner
rubber rung to attach melting point tube to the thermometer
melting point tubes
watch glass
spatula
Method - preparation
6.00 g of salicylic acid is added to a conical flask along with 10 cm3 of ethanoic anhydride and 5 drops of concentrated sulfuric acid
The mixture is swirled and held in a warm water bath around 60 oC for about 20 minutes
The flask is then allowed to cool and the contents are added to 75 cm3 cold water in a beaker at which point the aspirin crystallises out
The aspirin is recovered using Buchner filtration and left to dry
Diagram
Method - recrystallisation
Measure out 15 cm3 of ethanol into a boiling tube using a 25 cm3 measuring cylinder
Half-fill a beaker with hot water at a temperature of 75 oC
Use a spatula to add the crude aspirin to the boiling tube and place the tube in the beaker of hot water
Do not scrape the filter paper in this step
Stir until the aspirin dissolves into the ethanol
Pour this solution containing dissolved aspirin into roughly 40 cm3 of water in a 100 cm3 conical flask and gently warm the contents of the flask until the solution is complete
Allow the solution to cool in an ice bath
Crystals of aspirin will begin to form
Filter the purified solid using a Buchner funnel and allow to dry on the filter paper
Record the mass of the dry purified solid
Diagram
Method - melting point test
Powder a sample of the prepared sample by crushing with a spatula
Fill three melting point tubes with the organic solid to a depth of 0.5 cm
Transfer this to the melting point apparatus
Heat the oil bath gently and observe the temperature at which the solid melts
Record the temperature and repeat with the two other tubes
These readings can be taken more slowly as the approximate value recorded from the first reading is approached
On the basis of the recorded temperatures, deduce the melting point of your solid
Diagram
Practical tip
During recrystallisation, scratching the inside of the beaker will help crystals to form
Results
Calculate the theoretical yield which can be formed from 6.00 g of salicylic acid
Use this value to calculate the percentage yield
Compare the melting point recorded to that of the data book value of 136 oC
The proximity of a melting point to the actual data book value can express purity
Impurities tend to lower the melting point of a solid
Evaluation
The proximity of a melting point to the actual data book value can express purity
Impurities tend to lower the melting point of a solid
Worked Example
4.13 g of aspirin was obtained after purification from 6.00 g of salicylic acid and excess ethanoic anhydride.
Calculate the percentage yield.
HOOCC6H4OH + (CH3CO)2O → HOOCC6H4OCOCH3 + CH3COOH
Mr salicylic acid = 138.1
Mr aspirin = 180.1
Answer:
Theoretical yield of aspirin = x 180.1 = 7.82 g
Percentage yield = x 100 = 52.8 %
Examiner Tips and Tricks
Always quote a melting point as a range + or - and reference a data book value if you have one.
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