Lab 6 Discussion

# Lab 6 Discussion - The amount of Fe3 was constant in this...

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In part one, we used a spectrophotometer to determine the absorption of seven different solutions. We used the same wavelength when measuring all seven solutions. Then, we found the concentrations for [Fe(SCN)2+] by multiplying .00200 M KSCN by the amount of KSCN mL present, and dividing that by the total amount of mL present. In part two, we sought to determine the equilibrium constant K and Pk. Again, we started by using the spectrophotometer to determine each solutions absorption. Each solution had a different amount of mL and we needed to use the equation M1V1=M2V2 in order to find the amount of SCN-, which we would plug into the equation for K, which is K=[FeSCN2+]/[[Fe3+][SCN-]].
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Unformatted text preview: The amount of Fe3+ was constant in this equation, and it was 9.09*10^-4. However, we used the equation y=770.99x-.0056 and used the measured absorption in part 2 as y in order to find x. This x is the number we used as the FeSCN2+ in the K equation. Once we found K, we took –logK in order to find Pk, and thus we finished all of our calculations. However, we think that the spectrophotometer may have errored in its reading, because when we redid the test some results varied, and if the amount of absorption is off, it is pretty evident that the rest of the experiment would be thrown off since it all depends initially on the measure of absorption....
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## This note was uploaded on 04/09/2008 for the course CHEM 1AL taught by Professor Hooker during the Fall '07 term at UCSB.

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