Lab Report - Introduction: Aspirin, one of today's most...

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Introduction: Aspirin, one of today’s most common esters, or organic compounds known for their smells, can be created through the simple combination of acetic acid and alcohol. However, because the reaction does not generally come to a completion when acetic acid is used, it is a better choice to use acetic anhydride in its place in a laboratory setting. Using the anhydride will produce water, but at the same time will also react with the water being produced, causing the reaction to be driven to the right and create more successful results. Once the reaction has come to a completion, the sold aspirin is easy to gather because it is insoluble in water and has a large molecular weight. The aspirin produced through this experiment will be extremely impure due to the leftover, water-insoluble salicylic acid. On the contrary, one can assume that the impurity is probably not the acetic acid because the acetic acid is soluble in water and can therefore be cleansed out of the aspirin. When the Aspirin is added in with Fe (III), magenta-colored water will form. The amount of salicylic acid present in the aspirin can be determined through the amount of light absorbed by the
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This lab report was uploaded on 04/16/2008 for the course CHEM 006L taught by Professor Miller during the Spring '08 term at Westmont.

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Lab Report - Introduction: Aspirin, one of today's most...

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