Evaluating the Equilibrium Constant for the Reaction of Iron

Evaluating the Equilibrium Constant for the Reaction of...

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Evaluating the Equilibrium Constant for the Reaction of Iron (III) Ion with Thiocyanate Ion Jerrin Raju Miss. Vagmita Pabuwal Chemistry 104, Section 57 Date performed: March 19, 2010 Date Submitted: April 2, 2010
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Purpose The purpose of this laboratory experiment is to evaluate the equilibrium constants of the Iron (III) ion and thiocyanate ion reactions. The experiment focuses on performing an initial experiment with known variable to find ratios with based on which the concentrations of products and reactants vary. Using spectroscopy, the individual performing the experiment can attain an equation to find the equilibrium constant under conditions that are varied and more unknown. Procedure Attain 6 beakers, each of them will have 10 mL. of 0.2 M Fe 3+ solutions poured into them. Five of the beakers have to be filled with 1 to 5 mL. of 0.002 M SCN - solutions. The remaining test tube must be filled with HNO 3 solutions till they have 50 mL. per beaker. Attain some cuvettes and fill two of them with the solution containing no SCN - . These will be used as blanks on the spectrometer. Now fill the cuvettes with the rest of the solutions and perform spectroscopic analysis on these samples. Record the data. Plot a chart with the absorption of the solutions on the y-axis and concentration of the FeNCS solutions on the x-axis. Find the equation for the line of best fit from this graph. Now perform a second experiment where there has to be 5 mL. of 0.002 M Fe 3+ solutions each in 6 beakers; 0 to 5 mL. of 0.00230 M SCN - solutions in the beakers, and the rest of the solution must be filled with HNO 3 till there is 10 mL. in each beaker. Now find the absorbance of these solutions using the 0 mL. SCN - solution as a blank. Use the equation from the previous graph to find the equilibrium constant for these reactions.
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