How To Neutralise Aspirin

The coated aspirin took less drops of sodium hydroxide than the uncoated aspirin because to neutralize an acid you need a base and the coated aspirin was covered in a base compound that partially neutralize the acidity of the acetylsalicylic acid making it not need as many drops of sodium hydroxide.

For someone who must take Aspirin on a regular basis the acid-reduced Aspirin is a better choice because regular Aspirin is more acidic than the acid-reduced Aspirin and can cause painful ulcers. The acid-reduced Aspirin is more gentle on the stomach so it is safer choice for regular use.

In this investigation phenolphthalein was used as an indicator. When added to the Aspirin solution it was colourless but as you add sodium hydroxide and solution turns into a base, it becomes pink. The solution is neutralized when the next drop of sodium hydroxide will make the solution a base, turning the solution pink. …show more content…
Crushing the tablets is similar to the tablets being digested and the warm water serves as stomach acid making this investigation more realistic.

To verify that a sample of extra-strength aspirin contains more pain-relievers than regular-strength aspirin i would repeat steps 2 to 4 with the extra-strength aspirin. Then continue with the rest of the procedure and compare the number of drops of sodium hydroxide that it took to neutralize the extra-strength aspirin and the regular-strength aspirin. To prove that the extra-strength aspirin contains more pain relievers it should take more sodium hydroxide to neutralize the solution than the regular aspirin.

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