The standard reduction potential for the reactions: Ag^+ + e^– - Ag and Ag(NH3)2^+ + e^– - Ag + 2NH3 are +0.79 V and +0.37 V, respectively. From these values and the Nernst equation, what should be

Question

The standard reduction potential for the reactions: Ag^+ + e^– -> Ag and Ag(NH3)2^+ + e^– -> Ag + 2NH3 are +0.79 V and +0.37 V, respectively. From these values and the Nernst equation, what should be Kf for the Ag(NH3)2^+ ion? [Given: 2.303RT/F = 0.06]

Prashant Kotian · Accepted Answer

Correct answer: B. Reverse the second reaction and add it to the first to get the complexation reaction: Ag^+ + 2NH3 -> Ag(NH3)2^+. E°_cell = 0.79 - 0.37 = 0.42 V. Using E°_cell = (0.06/n) * log(Kf), we get 0.42 = 0.06 * log(Kf). Thus, log(Kf) = 7, giving Kf = 10^7. Therefore, correct answer is B.

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