lab 9 dis

lab 9 dis - ions in solutions. To obtain the Ka we measured...

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Liana Raineault Chem 1B Exp 9 Josh Kurzman Thurs 6-10 Discussion In part one of this experiment we titrated NaOH with acetic acid in order to obtain the pH at the equivalence and half equivalence point and volume to find the dissociation constant. We measured and calculated a dissociation constant of 2.51 * 10^(-5) which is close to the accepted value of 1.76 * 10^(-5). The discrepancy between the two values could be due to us not measuring the volume of NaOH exactly at the equivalence point because the indicator color changed quickly. In the next part of the experiment we calculated the dissociation constant again through using the different concentrations of
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Unformatted text preview: ions in solutions. To obtain the Ka we measured pH and deduced the hydrogen ion concentration from that and then used an equation to find the Ka. We calculated very similar dissociation constants from these solutions as we had in part one. In part three we observed how buffer solutions work to keep pH much more constant. The first solution we mixed the pH changed dramatically while in the buffer solution it fluctuated only .2 degrees of a pH. Possible sources of error for the experiment were solution measurements, making sure the pH meter was calibrated correctly and cleaned in between readings and rounding in calculations....
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This note was uploaded on 04/07/2008 for the course CHEM 1B taught by Professor Watts during the Winter '08 term at UCSB.

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