The balanced equation for the redox reaction involving Fe2+ and MnO4- is not complete. The complete balanced equation, including the hydrogen ions H+ , is as follows:5Fe2+ + MnO4- + 8H+ 5Fe3+ + Mn2+ + 4H2ONow, let's analyze the effect of increasing the pH on the equilibrium position using Le Chatelier's Principle. Increasing the pH means decreasing the concentration of H+ ions in the solution. According to Le Chatelier's Principle, if a change is applied to a system at equilibrium, the system will adjust itself to counteract the change and restore equilibrium.In this case, when the concentration of H+ ions decreases due to increased pH , the equilibrium will shift to the left to counteract the change and produce more H+ ions. This means that the reaction will favor the reactants Fe2+ and MnO4- over the products Fe3+ and Mn2+ .In conclusion, increasing the pH of the redox reaction involving Fe2+ and MnO4- will shift the equilibrium position to the left, favoring the formation of reactants Fe2+ and MnO4- and decreasing the concentration of products Fe3+ and Mn2+ . This can be explained using Le Chatelier's Principle, as the system adjusts itself to counteract the decrease in H+ ion concentration caused by the increase in pH.