A change in pH can affect the equilibrium position of a redox reaction between iron III and iodide ions. The redox reaction between iron III and iodide ions can be represented as follows:2Fe + 2I 2Fe + IThe Nernst equation can be used to predict the effect of pH on the equilibrium position of this redox reaction. The Nernst equation is given by:E = E - RT/nF lnQwhere E is the cell potential, E is the standard cell potential, R is the gas constant, T is the temperature, n is the number of electrons transferred, F is the Faraday constant, and Q is the reaction quotient.In this reaction, the number of electrons transferred n is 2. The reaction quotient Q can be expressed as:Q = [Fe][I] / [Fe][I] Since the reaction involves H ions, a change in pH will affect the concentrations of the species involved in the reaction. For example, an increase in pH i.e., a decrease in H concentration will cause the reaction to shift towards the products, while a decrease in pH i.e., an increase in H concentration will cause the reaction to shift towards the reactants.To support this answer with experimental data and calculations, let's assume the following hypothetical data:At pH 1:[Fe] = 0.1 M[Fe] = 0.01 M[I] = 0.1 M[I] = 0.001 MAt pH 3:[Fe] = 0.01 M[Fe] = 0.1 M[I] = 0.01 M[I] = 0.1 MUsing the Nernst equation, we can calculate the cell potential E at both pH values:At pH 1:Q = 0.01 0.001 / 0.1 0.1 = 0.0001E = E - RT/2F ln 0.0001 Assuming E = 0.77 V, R = 8.314 J/molK, T = 298 K, and F = 96485 C/mol:E = 0.77 - 8.314 298 / 2 96485 ln 0.0001 0.84 VAt pH 3:Q = 0.1 0.1 / 0.01 0.01 = 100E = E - RT/2F ln 100 E = 0.77 - 8.314 298 / 2 96485 ln 100 0.70 VAs predicted, the cell potential E decreases with an increase in pH, indicating that the reaction shifts towards the products. This demonstrates that the Nernst equation can be used to predict the effect of pH on the equilibrium position of a redox reaction between iron III and iodide ions.