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An equilibrium solution is prepared by mixing 2.750 mL of 0.001650 M SCN-, 5.000 mL of...

An equilibrium solution is prepared by mixing 2.750 mL of 0.001650 M SCN-, 5.000 mL of 0.001650 M Fe3+, and 2.750 mL of 0.05000 M HNO3. The equilibrium solution’s absorbance is determined to be 0.9150. Using this absorbance value and a standard curve, you determine that the equilibrium concentration of Fe(SCN)2+ is 0.0001830 M. Prepare an ICE table for the equilibrium mixture. Include the initial concentrations, changes in concentrations, and the equilibrium concentrations of Fe3+, SCN- and Fe(SCN)2+. Using the information in your ICE table, calculate the equilibrium constant. What is the value of the equilibrium constant?

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