Changing the pH from 2 to 6 in the redox reaction between Fe2+ and MnO4- in acidic solution will affect the equilibrium position of the reaction. The balanced redox reaction in acidic solution is:5 Fe2+ + MnO4- + 8 H+ 5 Fe3+ + Mn2+ + 4 H2OAs we can see, the reaction involves H+ ions protons , which are directly related to the pH of the solution. A lower pH indicates a higher concentration of H+ ions, while a higher pH indicates a lower concentration of H+ ions.When the pH is increased from 2 to 6, the concentration of H+ ions in the solution decreases. According to Le Chatelier's principle, the equilibrium will shift to counteract this change. In this case, the equilibrium will shift to the left to produce more H+ ions, favoring the reduction of Fe3+ to Fe2+ and the oxidation of Mn2+ to MnO4-.In summary, increasing the pH from 2 to 6 in the redox reaction between Fe2+ and MnO4- in acidic solution will shift the equilibrium position to the left, favoring the reduction of Fe3+ and the oxidation of Mn2+.