The following electrochemical cell was constructed, S.C.E. II cell solution I Pt

Question

The following electrochemical cell was constructed, S.C.E. II cell solution I Pt(s) with a cell voltage of 0.353 V. With a total volume of 1 L, the cell solution (pH 6.85) was comprised of 0.0025 M Ce(SO_4)_2, 0.0010 M CeCl_3, and 0.0045 M Na_2EDTA Write the reaction for the right half-cell as a reduction and provide its standard reduction potential(E^Degree) Calculate the quotient for the uncomplexed ions, [Ce_3+]/[Ce^4+], in the cell solution.[Ce^3+]/Ce^4+] = Determine the formation constant quotient, K_f(Ce EDTA)/K (CeEDTA)K_1 (CeEDTA)/K_1 (CeEDTA) =

Explanation / Answer

A) Ce4+ + e- ---> Ce3+

Eo = 1.61 V

B) [Ce3+]/[Ce4+] = 0.001/0.0025 = 0.4

C) Kf[CeEDTA]/Kf[CeEDTA-] = (0.0025/0.001] = 2.5

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