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Aspirin Purity Titration Resource

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when testing the purity of aspirin, why is titration helpful? what does the titration show? is a smaller titre value or a larger titre value indicative of a purer sample? etc thanks fed i am dissolving the aspirin in ethanol and then titrating against NaOH (0.1moldm-3)

rje102 replied: "What are you titrating it against? Another method would be to use melting point apparatus. You can measure the melting point accurately and compare it to the known. It your sample melts over a range of temperatures it indicates it is not very pure!"

Alec replied: "Aspirin is an organic acid, and therefore it can be titrated against a strong base like NaOH. You know the molecular weight of acetylsalicylic acid (aspirin), and you know how many moles of acid you should have. Once you titrate it, it will show if your sample contained 100% aspirin. You will never have more than 100% aspirin, so if the titration shows that you have more acid that you have calculated - then either you did the titration inoccrectly, or you have another acidic impurity present. Most likely you will have less than the calculated/throretical amount based on the titration, and the will indicate how much of the mass you're titrating is other stuff - non-acidic impurities."

Is salicylic acid the main component of aspirin? (titration)? salicylic acid -->C6 H4 (OCOCH3 )COOH Is that the main component of aspirin ? I did a lab on aspirin titration, and I'm just confused how salicylic acid should be used to determine the purity of the aspirin; Thank you Thank you for your answers! Akeem: " (Remember the base ONLY reacts with the aspirin in the tablet BUT there's other substances in the tablet i.e. the impurities.) " I've been trying to understand that; how does that affect my result.. or does it affect it at all? I did use NaOH for the titration; I have calculated and found the purity; so does it means that the greater the amount of salicylic acid, higher the percentage of purity? And the final "% of purity" I have calculated.. that would be considered slightly inaccurate (slightly higher) because of the impurities.. is that what you're saying?

James replied: "Aspirin is Acetylsalicylic Acid, or ASA. So, to answer your question, Salicylic acid is the main component of aspirin, with a single acetyl group added on. It would be used in a electrophoresis or a simple chromatography test along-side a sample of aspirin to determine how pure the aspirin sample was. This works because Salicylic acid is a smaller molecule, and will travel further through the gel/filter paper than the aspirin would, since it has the additional acetyl group weighing it down. If the aspirin is not very pure, it will contain lots of salicylic acid, which would separate, and you would see two samples, one right beside the salicylic acid sample and one not quite as far down."

Akeem replied: "Yes aspirin is the main component.In the lab you most likely reacted the crush tablets with a base of known concentration(e.g. NaOH). The volume of base required to completely react with the aspirin in the tablet can be used to find out the number of moles of the aspirin in the tablet. Convert this number of moles to mass. (Remember the base ONLY reacts with the aspirinn in the tablet BUT there's other substances in the tablet i.e. the impurities.) The mass of the tablets used should have been weighed before hand also. To determine the % impurity: Mass of Aspirin/Mass of tablet used x 100"

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when testing the purity of aspirin, why is titration helpful?
Aspirin is an organic acid, and therefore it can be titrated against a strong base like NaOH. ... more than 100% aspirin, so if the titration shows that you ...