In part 1 of this experiment we used a spectrometer and 7 samples of a solution in order to make a c

In part 1 of this experiment we used a spectrometer and 7 samples of a solution in order to make a c

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In part 1 of this experiment we used a spectrometer and 7 samples of a solution in order to make a calibration curve which was used in part 2. To do this the instructor measured the absorbance of the different samples using a spectrometer then made the calibration curve using excel, setting absorbance as the y-axis and concentration as the x- axis. In part 2 of this experiment we measured the absorbance of 5 different solutions of different concentrations of Fe(NO3)3, KSCN, and HNO3 using the spectrometer. Using these absorbances we calculated the equilibrium concentration of Fe(SCN)2+
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Unformatted text preview: using the calibration curve found in part 1. Then using that we determined the equilibrium concentrations of Fe3+ and SCN- then found the equilibrium constant, K, for the solution. Possible sources of error may have arisen from having waited too long and the solution heating up, giving a false absorption value. Also having set up the spectrometer wrong could have given incorrect absorption values and thus thrown off the entire experiment. Balanced equation: Fe3+ + SCN- -> Fe(SCN)2+ Equilibrium constant: [Fe(SCN)2+]/([Fe3+][SCN-])...
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This note was uploaded on 03/14/2010 for the course CHEM 109A 109A taught by Professor Aue during the Spring '09 term at UCSB.

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