A potentiometric measurement of 15 mL of a 0.1500 Cu2+ 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).
a. What is the ½ cell potential of the solution relative to a standard hydrogen electrode?
b. What cell potential would be measured in this experiment?
c. If 25.00mL 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 ½ cell
potential be? For CuY2-, assume K=10^18 and a4 for EDTA=1*10^-7 , pH =4.5
d. What cell potential would be measured relative to the SCE?
e. Diagram the cell using the conventional cell notation (i.e., not a picture with beakers, etc.)
f. If the pH were made more basic, would the potential measured relative to the SCE increase, decrease, or stay the same? Why
A potentiometric measurement of 15 mL of a 0.1500 Cu2+ 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).
a. What is the ½ cell potential of the solution relative to a standard hydrogen electrode?
b. What cell potential would be measured in this experiment?
c. If 25.00mL 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 ½ cell
potential be? For CuY2-, assume K=10^18 and a4 for EDTA=1*10^-7 , pH =4.5
d. What cell potential would be measured relative to the SCE?
e. Diagram the cell using the conventional cell notation (i.e., not a picture with beakers, etc.)
f. If the pH were made more basic, would the potential measured relative to the SCE increase, decrease, or stay the same? Why