Experiment V. Equilibrium Constant Lab Report ( 50 pts) Calibration Curve 1. Record the absorbance for each of the standard solutions in the table below. Calculate the concentration of FeSCN)” in each of the standard solutions and record the values in the table below. Show a sample calculation (for A2) of your work in the space below the table. Solution Absorbance [Fe(SCN)” A-1 A-2 A-3 0.000 0.390 0.535 0.713 0.835 0.898 1. 102 11.0x104M 1.48104 M 1.8 X 10-4 M 22 x 10-4 M 268104 M 3.0 x104 M A-5 A-6 II. Determination of the equilibrium constant 1. Record the absorbance values for each of the equilibrium solutions in part II and calculate the [Fe(SCN) , concentration for each of the solutions using the obtained calibration curve in part 1. Show your work in the space provided below. Solution Absorbance [Fe(SCN) B-1 B-2 B-3 3-4 0.114 0.260 0.359 0.537 0.623 1.82 X 10-4 3.648164 5.45 8 10 4 7.24 8104 9.09×104 B-5 2. Determine the equilibrium concentrations of each of the reactants and products in solution B-1 using the table provided below (ICE table). Fill in all blank values [Fe] (SCN) [Fe(SCN) Initial Concentration Change in Concentration Equilibrium Concentration 3. Determine the equilibrium concentrations of each of the reactants and products in solution B-2 using the table provided below (ICE table). Fill in all blank values Fes [SCN) [Fe(SCN)?”) Initial Concentration Change in Concentration Equilibrium Concentration

II. Determination of the equilibrium constant A. For only your lab group, prepare the following solutions: Solution Volume of 0.002 M Fe3+ Volume of 0.002 M SCN B-1 5.0 mL 1.0 mL B-2 5.0 mL 2.0 mL B-3 5.0 mL 3.0 mL 5.0 mL 4.0 mL B-5 5.0 mL 5.0 mL Volume of H2O 5.0 mL 4.0 mL 3.0 mL 2.0 mL 1.0 mL B-4