A potentiometric measurement of 15 mL of a 0.1500 M Cu^2+ solution with a pH = 4.5 was made using a saturated calomel electrode (SCE) as a reference. The saturated calomel electrode has a reduction potential of 0.244 relative to a standard hydrogen electrode (SHE). What is the 1/2 cell potential of the solution relative to a standard hydrogen electrode? What cell potential would be measured in this experiment? If 25.00 mL of a 0.120 M solution of EDTA was added to the copper solution and the resulting solution had a pH = 4.5, what would the new 1/2 cell potential be? For CuY^2-, assume K = 10^18 K and a_4 for EDTA = 1 times 10^-7, pH = 4.5 What cell potential would be measured relative to the SCE? Diagram the cell using the conventional cell notation (i.e., not a picture with beakers, etc.) If the pH were made more basic, would the potential measured relative to the SCE increase, decrease, or stay the same? Why?