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Unformatted text preview: acid CH 3 COOH (aq) ↔CH 3 COO-(aq) +H + (aq) the K a was 3.15E-5. This discrepancy could be because of a not quite mixed solution, causing the pH to be too high. Next we had 5mL of NaA and 30mL of acetic acid. This time the K a was 2.098E-6. This could again be because the solution wasn’t mixed together all the way. In part III we found the buffering capacity of a buffer solution compared to an unbuffered solution. When a strong acid was added to an unbuffered solution the pH decreased from 7 to 1.4 and when a strong base was added the pH went to 12.1. In a buffered solution the pH when acid was added was from 4.5 (sometimes DI water is slightly acidic) to 4.4. And when a strong base was added it went from 4.5 to 4.7. The buffered solution resisted pH change much better than the unbuffered....
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This note was uploaded on 05/03/2008 for the course CHEM 1BL taught by Professor Davis during the Winter '08 term at UCSB.
- Winter '08