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

Thin layer chromatography experiment to determine which analgesic tablets contain caffeine.

Extracts from this document...

Introduction

The Experiment to determine which analgesic tablets contain caffeine. Thin layer chromatography (TLC) is a technique to determine the quantity of unknown substances in a mixture. It is based on the principle that each substance has a unique molecular weight and size which determines the distance that it travels via capillary action through a stationary phase. In the case of TLC, the stationary phase is a thin, absorbent layer, applied to a glass, metal or plastic plate. A solution of many compounds - such as prepared orange peel solution - can be separated to reveal each component using this method. http://www.ehow.com/ Equipments needed: > Thin layer chromatography plate > Large beaker > Tin foil > Micropipettes > Ruler > Pencil > notebook > two types of aspirin tablets (A and B) > safety glasses to be worn at all times > 50/50 ethanol/ethyl ethanoate solvent for dissolving sample A and B > Grinder for crushing tablet aspirin tablets A and B > Distilled water for washing and paper towels for drying > UV lamp Process Hazard risk of procedure Severity of risk Control measures and precautions Attain 1 TLC plates. ...read more.

Middle

If skin burned place effected area under cold water for few minutes. Make sure to grip the firmly with one hand and grind the the piece with the other. If fingers still end being squashed then place affected area under cold water for few minutes. Do not take the caffeine in by mouth and hands must be washed afterwards. Straightaway Spot the TLC plate with the Aspirin sample A. Label it at the top as A. Make the spot as small as possible Too much of the solution on the TLC plate has the risk of running over the TLC plate and ruin it. If too much pressure put on the hand when labeling contains the risk of piercing through the TLC plate. Low Place the TLC plate on a table and proceed with low pressure force labeling. Use a micropipette to spot the Caffeine on to the TLC plate Squash a little piece of tablet B using a grinder and add a VERY small amount of solvent (50/50 ethanol solvent for dissolving sample A). ...read more.

Conclusion

Gently place the TLC plate in the beaker, touching only the edges of the plate. Inhaling the solution which is contained inside the beaker can cause headache. Dropping the TLC plate into the solution will ruin the TLC plate. Moderate Re-cover the beaker with the tin foil cap and let the plate develop. Take out the TLC plate when the line of developing solution has approximately reached the top of the plate. Mark this line with the pencil and ruler. Let the TLC plate dry. Inhaling the solution which is contained inside the beaker can cause headache. Moving the still Wet TLC plate can cause into ripping the TLC plate Moderate Re-cover the beaker with the tin foil cap after having removed the TLC plate. Dry the plate with a hairdryer on place. Expose the spots on the TLC plate by putting the plate under UV light. Gently outline each spot with a pencil. Draw a diagram of the plate in to a notebook, noting the size and location of each spot. Looking directly into the UV light can harm the eyes. Moderate Avert facing directly into the UV light. Wear protective eye wear all throughout the experiment. ...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 Organic 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 Organic Chemistry essays

  1. Marked by a teacher

    Experiment to determine the ethanol content of wine

    5 star(s)

    Mass of ethanol (g) Density (g/cm3 ) 0 46.285 26.583 0.9975 1 46.224 26.522 0.9952 2 46.197 26.495 0.9942 3 46.168 26.466 0.9931 4 46.120 26.418 0.9913 5 46.086 26.384 0.9900 6 46.048 26.346 0.9886 7 46.014 26.312 0.9873 8 45.984 26.282 0.9862 9 45.947 26.245 0.9848 10 45.915 26.213 0.9836 11 45.867 26.165 0.9818 12 45.843

  2. Marked by a teacher

    Experiment to Determine Acidities of Wine. The purpose of this experiment is to ...

    5 star(s)

    At the start of the titration, the pH was read after every 3cm3 of NaOH was added, but as this came closer to the equivalence point of pH 8.2 this was read more often. A titration curve of volume against pH could then be plotted and the volume for the wine to reach a pH of 8.2 was determined.

  1. Peer reviewed

    Making Aspirin

    5 star(s)

    The mass of silver chloride is = 0.2542 g (practical) with filter paper and the mass of filter paper is 0.1425 g, so the mass of silver chloride is = (0.2542 - 0.1425 ) g = 0.1117 g. Calculations: Step 1: Now we are going to calculate the moles of silver nitrate from its mass.

  2. Synthesis of Aspirin

    * After few moments, the crystals were filtered off by Vacuum filtration apparatus. The mixture was poured into a Buchner funnel with a filter paper first and sucked. * 10cm3 of distilled water was used to wash the sucked production and dried in a filter funnel.

  1. the analysis of aspirin tablet

    The burette was filled with standard sulphuric acid. 5) The initial reading on the burette was recorded. 6) 25 cm3 of diluted sodium hydroxide was transferred to a 250 cm3 conical flask by a pipette. 7) 2-3 drops of phenol red was added to the solution inside the conical flask.

  2. F336- aspirin individual Investigation

    CHEMISTRY REVIEW PROJECT PAGE Possible impurities If the reaction is incomplete or if you mix the reagents in the wrong proportion, your aspirin will be contaminated with unreacted salicylic acid. It might also contain ethanoic acid or the acid catalyst.

  1. The aim of this experiment is to produce Aspirin. This is an estrification in ...

    Into a weighing bottle 2.00g of solid sodium hydroxide was weighed accurately and the mass was then recorded. An analytical balance was used to weigh the solid because they are very accurate. A clean beaker was rinsed with distilled water and the solid was transferred from the weighing bottle into the beaker.

  2. investigating the amount of ascorbic acid present in fruit

    Working Out the Amount of Vitamin C Present: The chemical equation for this reaction is: C6H8O6 + C4H4BrNO2 ---> C6H6O6 + C4H5NO2 + HBr The word equation for this reaction is: Ascorbic Acid + N-Bromosuccinimide ---> Dehydroascorbic Acid + Succinimide + Hydrogen Bromide From this equation I can see that all the compounds have 1 mole.

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