A solution is made by mixing 100mL Fe ³⁺ solution of 1.00 x 10 ^-3 M and 100 mL A ^- ion solution of 1.00 x 10 ^-3 M. The mixture has a deep blue color, indicating the formation of a complex between Fe ³⁺ and A ^- . By a spectrophotometric analysis, we find that 30.0% of Fe ³⁺ is in the form of the complex and there are two probable products which are FeX ²⁺ or FeX ³

Balance the following equations and calculate the concentrations of the remaining species

(i) Fe ³⁺ + A ^- <--> FeA ²⁺

(ii) Fe ³⁺ + A ^- <--> FeA ³

Assuming that the final state reached equilibrium, write the equilibrium expressions and calculate the equilibrium constants for both cases in (a)

Answer rating: 100% (QA)

Molarity moles volume in liters So no of moles molarityvolume in liters Solution 1 100 mL 01 L of 0001 M Fe 3 solution Soinitial moles of Fe 3 000101 ... View the full answer