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

Analysis of Aspirin Tablets.

Extracts from this document...

Introduction

Analysis of Aspirin Tablets Background Information Aspirin is a well-known drug, which is analgesic and antipyretic. Analgesic drugs are those that relieve pain. Antipyretics are ones that lower body temperature. The main component of aspirin tablets is: 2 - Ethanoylhydroxybenzoic acid CH3COOC6H4COOH After aspirin is swallowed, it is unchanged in the acidic conditions of the stomach, but is hydrolysed by the alkali juices in the intestines. Hydroxybenzoates lower body temperature quickly and very effectively in fever patients, but they have little or no effect if the temperature is normal. They are also analgesics, which relieve pain, such as headaches. The toxic dose from hydroxybonzoates is relatively large; their uncontrolled use could be dangerous. Aspirin, one of the first drugs to come into common usage, is still mostly the widely used in the world - approximately 35,000 metric tonnes are produced and consumed annually, enough to make over 100 billion standard aspirin tablets every year. Aspirin is analgesic, anti-inflammatory, antipyretic and is an inhibitor of platelet aggregation. It inhibits fatty acid cyclo-oxygenase by acetylation of the active site of enzyme and the pharmacological effects of aspirin are due to the inhibition of the formation of cyclo-oxygenase products including prostglandins, thromboxanes and prostacyclin. ...read more.

Middle

* To hydrolyse the aspirin acid - heat it gently for 10 minutes. SAFETY: eye protection must be worn. * Cool the mixture and transfer (with washings) to a 250 cm�-graduated flask. Fill up to the blue mark with distilled water. Part 3 - Estimating the quantity of unused NaOH after hydrolysis * Put 25 cm� of the hydrolysed solution (from part 2) into a conical flask using a pipette. * Put a couple of drops of Phenolphthalein indicator in the solution. It should go purple. * Titrate this against 0.1-mol dm-3 HCl acid (which is in the Burette). * Carry out the titration until the solution goes colourless (keep shaking the beaker whilst releasing the HCl acid). Results Part 1: Titration Rough Accurate 1 Accurate 2 Final reading (cm�) 25.65 25.25 25.30 Initial reading (cm�) 0.00 0.00 0.00 Amount of HCl acid added (t1) 25.65 25.25 25.30 Average (t1) = (25.25 + 25.30) 2 = 25.275 cm� of HCl acid Part 2: Mass of aspirin tablets = 1.66 g Part 3: Titration Rough Accurate 1 Accurate 2 Final reading (cm�) 7.90 15.80 23.65 Initial reading (cm�) 0.00 8.00 16.00 Amount of HCl acid added (t2) ...read more.

Conclusion

Burette: This is accurate to 0.05 cm�. If the reading has to be rounded because the scale on the Burette is not big enough to be exact, this will also cause an error. Graduated Flask: If the volume of the flask is 250 cm�, the bottom of the meniscus is on the calibration line, the error is 0.1 cm�. Pipette: Once again, the scale is not extremely accurate and may cause an error. Procedural errors: It could have been difficult to spot the endpoint of the reaction. Despite the solution being purple, and the colour looked for was colourless - it may be hard to get the exact amount of HCl added to go colourless. This is because the releaser of the Burette may release too much of the HCl acid when you know you only need a small amount of it for the solution to go colourless. The equipment may not have washed well (drying is also very important). Some of the HCl acid may have got onto the side of the conical flask and not reacted with the hydrolysed aspirin. If an acid-base titration had been carried out, it would not have been a good idea to put too much indicator in, because the indicator itself is a weak acid. ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our GCSE Aqueous 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 GCSE Aqueous Chemistry essays

  1. Preparation Of Aspirin.

    * Apply suction using a filter pump and wash the crystals with ice cold water. * Dry the crystals and carefully weigh them * Transfer the crystals into a beaker and add 8cm3 ethanol stir the mixture and warm gently to dissolve the crystals.

  2. Indigestion Tablets Investigation

    The first (black x) results was from my first experiment. I had been supplied with a short delivery tube. The experiment was fine until the 2-minute mark when the delivery tube came out of the measuring cylinder. The result of this was that the gas produced by the reaction escaped rather than being collected in the measuring cylinder.

  1. Determine the percent aspirin in an aspirin tablet and to compare this with the ...

    Using the relationship given in the equation: 1 mole aspirin is hydrolysed by 2 moles NaOH It is then possible to calculate the number of moles of acetyl salicylic acid that has been hydrolysed. This answer can then be compared to the label stating the aspirin content.

  2. Preparation of aspirin - The chemical background This is the overall reaction that ...

    Weak alcohol acts as nucleophile, attacks like carbonyl carbon. After a proton transfer a water molecule is released The acid catalyst is regenerated. When Ethanoic acid is involved in esterification the process is sometimes known as ethanoylation. The ? OH group in phenol is less reactive to esterification than the ?

  1. Investigating different types of aspirin and making aspirin.

    Both qualitative and quantitative data can be obtained. Modern high performance techniques can identify trace impurities in samples. Chromatography can also be used to separate mixtures on a large scale. There is a range of related techniques. All work on the same principle. A delivery system supplies a mobile phase, which is moved through a stationary phase.

  2. Analysis of the content in Aspirin Tablet

    1 Pipette filler X 1 White tile X 1 Stand X 1 Clamp X 1 Filter funnel X 1 Glass rod X 1 Dropper X 1 Bunsen burner X 1 Matchbox X 1 Tripod X 1 wire gauge X 1 Bench mat X 1 75 cm3 beaker X 3 6)

  1. Indigestion - find out the composition of tablets which are for indigestion and compare ...

    Contains 0.47g sucrose per tablet, unsuitable for people with sugar intolerance. Setlers antacid tablets can be used during pregnancy and whilst breast- feeding. Setlers Antacid Peppermint ( 30 tablets - 3 rolls ) Price: �1.69Including VAT at 17.5% Andrews antacid Andrews antacid gives fast effective relief from acid indigestion and

  2. How much Iron (II) in 100 grams of Spinach Oleracea?

    Place the conical flask containing the hot solution on a white tile. 16) Titrate the Potassium Manganate (VII) (aq) into the hot spinach extract solution until a pink colour appears. 17) Continue to add the Potassium Manganate (VII) (aq)

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