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Unformatted text preview: solution is diluted. The first part we added a strong base, NaOH. The pH only increased .11 because the solution is buffered. Then the strong acid was added, HCl. Again the pH only dropped slightly, from 4.66 to 4.5, because the solution is buffered. Then NaOH was added until the buffer capacity was exceeded. Because of the low amount of acetic acid in the solution it only took a very small amount of NaOH to exceed the buffer. The capacity was found by taking the difference between final pH and initial pH and dividing by two. This gave the midpoint in the difference. Then the midpoint was added to the initial to find the buffer capacity. The final part water was added to acetic acid. The pH decreased which means that more H+ was formed. This is because more acetic acid dissociated when there was more water to break the bonds in the acid....
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This note was uploaded on 09/07/2010 for the course CHEM 1310 taught by Professor Cox during the Fall '08 term at Georgia Tech.
- Fall '08