002 kscn and 10 ml of water and last with 50 ml 0002

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mL 0.002 KSCN and 1.0 mL of water, and last with 5.0 mL 0.002 KSCN. The solutions were then put in cuvettes, and the absorbance was measured using the spectrophotometer at a wavelength of 450 nm. In conclusion, using the values/equation on the given calibration curve, we were able to find the moles of FeSCN2+ present, we used our knowledge of the m1v1=m2v2 equation to
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determine amount of reactants, and then we used the Kc equation with the ICE table as demonstrated in lecture to find the Kc values for each reaction. Next, we were able to average all of the calculated Kc values, and find the standard deviation using our knowledge of the equation, which showed us that because Kc is a relatively large number, most of the starting materials have reacted into products. Data: All measurements at 450 nm wavelength. Trial 1 2 3 4 5 Fe(NO3)3 in HNO3 (mL) 5 5 5 5 5 mL water 4 3 2 1 0 mL KSCN 1 2 3 4 5 Absorbance 0.23 0.36 0.52 0.56 0.78 Calculations: Using the calibration curve 2 + ¿ / 10 5 M X FeSC N ¿ + 0.0154 absorbance = 0.027 ¿ we can plug in our measured absorbance to find the x value, which is the estimated amount of 2 + ¿ FeSC N ¿ . So, we do this for all 5 of our measured absorbance values: 1.) 2 + ¿ 10 5 M X FeSC N ¿ + 0.0154 0.23 = 0.027 ¿ 2 + ¿ 10 5 M X FeSC N ¿ 0.2146 = 0.027 ¿ 2 + ¿ 10 5 M 7.94815 = X FeSC N ¿ 2.) 2 + ¿ 10 5 M X FeSC N ¿ + 0.0154 0.36 = 0.027 ¿
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2 + ¿ 10 5 M X FeSC N ¿ 0.3446 = 0.027 ¿ 2 + ¿ 10 5 M 12.763 = X FeSC N ¿ 3.) 2 + ¿ 10 5 M
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  • Fall '06
  • Goddfried
  • Chemistry, Potassium Thiocyanate

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