• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

The purpose of this experiment was to prepare a sample of Aspirin and measure its boiling point

Extracts from this document...


12th October 2015 Preparation of Aspirin Abstract The purpose of this experiment was to prepare a sample of Aspirin and measure its boiling point. Reacting salicylic acid with acetic anhydride in excess with the presence of a catalyst sulphuric acid. Through a sequence of heating, filtering and recrystallizing the end product of making aspirin was positive and the measuring of its boiling point was successful. The sample was purified and the percentage yield was calculated to be 61.2% and to measure the purity of the sample the melting point was considered which came to be 122°c. Introduction The chemical name for Aspirin is Acetylsalicylic acid. Aspirin is known to relieve pain and is an over the counter drug. Salicylic acid was first found in the bark of the willow tree, which used to be used for treating fever and a variety of illnesses. However scientists soon began to realise that the acid used to thin the stomach lining and burn throats. (Ling, 1994) Not long after a German scientist, Felix Hoffman, derived a pain reliever that did not produce the same side effects as salicylic acid, and is credited for the finding of Aspirin. (Ling, 1994) Uses of Aspirin Another use of aspirin is people having to take it to thin the blood, which reduces the chance of unnecessary blood clots to form; therefore in the long term taking an aspirin everyday will prevent heart attacks and strokes in high risk patients. ...read more.


Lastly measure the yield and the melting point of the crystals. Diagram of experiment: On paper. Hazard and Risk Analysis Risks Hazards Precautions Salicylic acid If the acid comes to contact with skin, there can be risk of burns. Swallowing can cause major internal disruptions, vomiting and diarrhoea, dizziness etc. The acid could be inhaled as well which could also cause problems with the respiratory tract. To keep toxic fumes from getting inhaled do all steps in a fume cupboard. To prevent the acid touching any skin, gloves, suitable clothing and lab coats must be warn at all times. In addition goggles must be worn to prevent eye damage. Acetic anhydride Very corrosive and causes severe burns. Allowing eye or skin contact would cause irritation, redness and burns. Inhaling the substance can cause shortness of breath and inflammation. The more serious case can cause blistering. Use in fume cabinet as it is a very toxic smelling gas. If unknowingly toxic gases are released make sure the area is being well ventilated. Precautions such as wearing protective goggles, lab coats and disposable gloves. Rinse all lab equipment after use, to ensure other colleagues use contaminated equipment. Sulfuric acid A clear colourless liquid, highly corrosive, very toxic, fatal if inhaled, highly reactive, reacts violently with water. ...read more.


The equipment used will have left over product on them, which would be a potential source of error and a low the yield. Such as trying to transfer all the sample from the round bottom flask in to the beaker, or residue left on the glass rod. Again some errors are unavoidable and are just minimised as in this situation. Measuring the melting point came to 135°C (Haynes, 2014) but the experimental melting point was 122°C. The melting points show a small range, but a larger difference between the theoretical and actual melting points. There can be many reasons as to why there was a difference between the melting points. As the yield is not 100% some of the product may have been lost when transferring the product from one container to another. All reactants may not have all reacted. Conclusion The experiment as a whole was successful and the reactants react together to form Aspirin, however if the experiment was to be done again a way to increase the percentage yield would make it feasible would make the experiment more commendable. For example when measuring the melting point the temperature there should be more control over the temperature and humidity of the surroundings, and kept at a minimum to stop the reactants reacting with vapour in the air. ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our AS and A Level Inorganic Chemistry section.

Found what you're looking for?

  • Start learning 29% faster today
  • 150,000+ documents available
  • Just £6.99 a month

Not the one? Search for your essay title...
  • Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

See related essaysSee related essays

Related AS and A Level Inorganic Chemistry essays

  1. Peer reviewed

    Determining the concentration of acid in a given solution

    5 star(s)

    If I didn't swirl the solution then the area in the middle of the conical flask where the sulfuric acid was falling would turn pink first as the OH- particles and H+ particles in that part of the solution would have reacted.

  2. Analysis of Commercial Aspirin Tablets

    was titrated using standard 0.05M sulphuric acid with phenol red as indicator. The titration was repeated twice and data obtained was drawn into a table. Results Calculation 1. The initial no. of moles of NaOH before hydrolysis = 1.00M*25cm3*1/1000 =0.025mol 2.

  1. Determination of Chemical Oxygen Demand (COD) of a Given Sample of Waste Water

    of moles of FAS solution in titrant = 4.17 x 10-4 mol x 6 = 0.002502 mol The molarity of FAS solution= no. of moles x 1000/ volume in ml = 0.002502 x 1000/ 10= 0.2502M By standardization, the molarity of the FAS solution is 0.2502M 2.

  2. Determination of DO & BOD in a water sample

    The difference between 2 DO is defined as BOD5. Data Analysis Concentration of standard Na2S2O3 at the first day: 0.0149 M Volume of 0.0149M Na2S2O3 used = 40.00 - 26.75 = 13.25 cm3 Amount of 0.0149M Na2S2O3 used = 13.25 x 0.0149 = 0.1974 mmol Amount of I2 generated = 1/2 (0.1974)

  1. Finding Out how much Acid there is in a Solution

    I will add four drops of methyl orange indicator to this and place it under the burette, on a white tile to make it easier to see the colour change.

  2. The preparation, analysis, and reactions of an ethanedioate complex of iron

    Then few more drops of tin(II) chloride were added . Once the solution was cooled to room temperature, one portion 10cm3 of mercury(II) chloride solution was added quickly. 10cm3 of 40% phosphoric acid and 10 drops of barium diphenylamine sulphonate indicator solution were added to the reduced solution.

  1. Synthesis of Aspirin

    Mass/g Weighing boat + 3 salicylic acid 4 Weighing boat after transfer 1.06 2-hydroxybenzoic 3 Melting Point apparatus Thermometer Estimation (�C) Electrical Measurement (�C) Start collapsing 120 124 Melting Point 125 129 16.32 Petri dish + Filter paper + Aspirin - 15.25 Petri dish + Filter paper = 1.07 Aspirin

  2. An Environmental Case Study - Acid Rain: Causes, Effects and Solutions

    Dry deposition occurs in the absence of precipitation. This has been calculated to be responsible for up to 60% of acid deposition in some areas. Here, particle and gases such as NOx and SO2 stick to the ground, trees and buildings.

  • Over 160,000 pieces
    of student written work
  • Annotated by
    experienced teachers
  • Ideas and feedback to
    improve your own work