Changing the pH of a redox reaction involving copper and zinc can affect the equilibrium position by altering the concentrations of H+ ions in the solution. This, in turn, can influence the reduction potentials of the half-reactions involved.The redox reaction between copper and zinc can be represented by the following half-reactions:1. Cu2+ + 2e- Cu Reduction half-reaction 2. Zn Zn2+ + 2e- Oxidation half-reaction The Nernst equation can be used to determine the effect of pH on the reduction potential of each half-reaction:E = E - RT/nF * ln Q Where E is the reduction potential at a given pH, E is the standard reduction 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 case, the pH affects the H+ ion concentration, which can influence the reaction quotient Q . However, since there are no H+ ions directly involved in the half-reactions for the copper and zinc redox reaction, the pH does not have a significant impact on the equilibrium position.As for which ion is favored, we can compare the standard reduction potentials of the two half-reactions. The standard reduction potential for the Cu2+/Cu half-reaction is +0.34 V, while the standard reduction potential for the Zn2+/Zn half-reaction is -0.76 V. Since the Cu2+/Cu half-reaction has a more positive reduction potential, it is more likely to be reduced, meaning Cu2+ ions are favored in this redox reaction.In summary, changing the pH does not have a significant impact on the equilibrium position of the redox reaction involving copper and zinc, and Cu2+ ions are favored due to their more positive standard reduction potential.