Preparing a Pure Organic Solid (Oxford AQA International A Level Chemistry)

Revision Note

Philippa Platt

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

  1. 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

  2. The mixture is swirled and held in a warm water bath around 60 oC for about 20 minutes

  3. 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

  4. The aspirin is recovered using Buchner filtration and left to dry

Diagram

Preparation of aspirin, downloadable AS & A Level Chemistry revision notes
The preparation of aspirin using a hot water bath

Method - recrystallisation

  1. Measure out 15 cm3 of ethanol into a boiling tube using a 25 cm3 measuring cylinder

  2. Half-fill a beaker with hot water at a temperature of 75 oC

  3. 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

  4. Stir until the aspirin dissolves into the ethanol

  5. 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

  6. Allow the solution to cool in an ice bath

    • Crystals of aspirin will begin to form

  7. Filter the purified solid using a Buchner funnel and allow to dry on the filter paper

  8. Record the mass of the dry purified solid

Diagram

Recrystallisation and Buchner filtration, downloadable AS & A Level Chemistry revision notes
Recrystallisation and Buchner filtration

Method - melting point test

  1. Powder a sample of the prepared sample by crushing with a spatula

  2. Fill three melting point tubes with the organic solid to a depth of 0.5 cm

  3. Transfer this to the melting point apparatus

  4. Heat the oil bath gently and observe the temperature at which the solid melts

  5. 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

  6. On the basis of the recorded temperatures, deduce the melting point of your solid

Diagram

Melting point using an oil bath, downloadable AS & A Level Chemistry revision notes
Melting point test using an oil bath

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 = fraction numerator 6.00 over denominator 138.1 end fractionx 180.1 = 7.82 g

Percentage yield = fraction numerator 4.13 over denominator 7.82 end fraction 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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Philippa Platt

Author: Philippa Platt

Expertise: Chemistry

Philippa has worked as a GCSE and A level chemistry teacher and tutor for over thirteen years. She studied chemistry and sport science at Loughborough University graduating in 2007 having also completed her PGCE in science. Throughout her time as a teacher she was incharge of a boarding house for five years and coached many teams in a variety of sports. When not producing resources with the chemistry team, Philippa enjoys being active outside with her young family and is a very keen gardener

Stewart Hird

Author: Stewart Hird

Expertise: Chemistry Lead

Stewart has been an enthusiastic GCSE, IGCSE, A Level and IB teacher for more than 30 years in the UK as well as overseas, and has also been an examiner for IB and A Level. As a long-standing Head of Science, Stewart brings a wealth of experience to creating Topic Questions and revision materials for Save My Exams. Stewart specialises in Chemistry, but has also taught Physics and Environmental Systems and Societies.