• 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...


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.


* 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.


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

    Experimentation A sample of aspirin tablets, a stock solution of sodium hydroxide approximately 1 mol dm -3 and a standardised solution of hydrochloric acid of 0.1 mol dm -3 are supplied. The determination of the exact molarity of the sodium hydroxide solution is carried out by diluting the supplied stock solution by a factor of ten.

  1. Investigation into the efficiency of various indigestion tablets.

    Scientific details Indigestion is caused by excess hydrochloric acid, produced in the lining of the stomach. This can be treated quickly and effectively, using medicines containing chemicals called antacids. Antacids are alkalis that are used to neutralise the acid, turning it into a salt and water.

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

    I also wanted to see how this affected the volume of Iron (II) that I was able to extract from the Spinach Oleracea. The solution was boiled to a temperature of 70 oc as this is hot enough to break up the oxalate complexes around the Iron (II).

  1. Indigestion Tablets Investigation

    If they are stirred or shaken (agitated) then the particles are given more energy and so are more likely to collide. I will not be stirring because I could not guarantee that the agitation given would be identical for all the experiments. Prediction I predict several things will happen 1.

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

    OH of ethanol so it needs a more vigorous reagent to esterify it. A more vigorous ethanoylation agent than Ethanoic acid is Ethanoic anhydride, which is made by eliminating a molecule of water between two Ethanoic acid molecules: Ethanoic anhydride Ethanoic anhydride is often used as an ethanoylating agent because

  1. Analysis of the content in Aspirin Tablet

    16.65 16.25 16.30 16.30 16.35 16.10 Mean volume of H2SO4 used = (16.25 + 16.30 + 16.30 + 16.35) / 4 = 16.30 cm3 8) Calculation/interpretation: Equations of the reaction: CH3COOC6H4COOH(aq) + 2NaOH(aq)�HOC6H4COO-Na+(aq) + CH3COO-Na+(aq) +H2O(l) H2SO4(aq.) + 2NaOH(aq.) � Na2SO4(aq)

  2. Making Aspirin.

    By 1899, though, one of Bayer's top chemists, a scientist named Dreser, had finished demonstrating the usefulness of the potent new medicine and even gave it a new name: aspirin. It is believed that the name comes from a plant relative of a rose that makes salicylic acid (several plants make this compound, not just the willow).

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