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Unformatted text preview: 7.30 by use of the Henderson Hasselbach equation: pH = pKa + log [A- / AH] pKa = pH log [A- / AH] = 8 log[ .5 / .1 ] total buffer range 1 2 3 4 5 6 7 8 9 10-4-3-2-1 1 2 3 mmol acid added pH Series1 From the graph of the total range of the buffer solution it can be determined that the range was up to 2.4 mmol acid and 3 mmol base. Discussion: The goal of this experiment was accomplished because the pKa of a buffered solution was found to be 7.3 by and the buffered capacity of the solution was found to be that the buffered solution works for up to 2.4 mmol of acid and 3.0 mmol of base because the pH range remains steady and only changes +/- 1 within these boundaries. . By looking at the graphs is can be determined that unknown 5 was a weak base because it formed a buffered solution when mixed with a strong acid....
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- Spring '08