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4.81 mL of 0.00200 M Fe(NO3)3, 2.85 mL of 0.00200 M KSCN and 2.34 mL of...

4.81 mL of 0.00200 M Fe(NO3)3, 2.85 mL of 0.00200 M KSCN and 2.34 mL of distilled water were mixed. The resulting solution was allowed to attain equilibrium at 24 oC. The absorbance of the equilibrium solution was recorded, and the [FeSCN2+] was determined graphically to be 7.58 x 10-5 M.

Part A: Calculate the number of moles of Fe3+ initially added to the solution.

Part B: Calculate the number of moles of FeSCN2+ formed in the solution at equilibrium.

Part C: Calculate the final number of moles of Fe3+ present in the solution at equilibrium.

Part D: Calculate the concentration of Fe3+ in the solution at equilibrium.

Part E: Calculate the concentration of SCN- in the solution at equilibrium.

Part F: Calculate the equilibrium constant (Kc) for the equilibrium reaction

Fe3+ (aq) + SCN- (aq)      <------>      FeSCN2+ (aq)

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