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
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Related questions
The saturated calomel electrode, abbreviated SCE, is often used as a reference electrode in making electrochemical measurements. The SCE is composed of mercury in contact with a saturated solution of calomel Hg2Cl2. The electrolyte solution is KCl. ESCE is +0.242 V relative to standard hydrogen electrode.
Calculate the potential for each of the galvanic cells containing a saturated calomel electrode and the given half-cell components at standard conditions. In each case indicate whether the SCE is the cathode or the anode. Standard reduction potentials are found in table:
| Electrode |
SCE |
a) Cu2+ + 2e- → Cu | b) Fe3+ + e- → Fe2+ | c) AgCl + e- → Ag + Cl- | d) Al3+ + 3e- → Al | e) Ni2+ + 2e- → Ni |
| Eo |
+0.242 V |
+ 0.339 V | + 0.771 V | + 0.223 V | - 1.677 V | - 0.257 V |
