metimes equilibria for complex ions are described in terms of dissociation constants, Kd. For the complex ion Fe(CN)64−, the dissociation reaction is as follows. Fe(CN)64− Fe2+ + 6 CN− Kd = [Fe2+ ] · [CN− ]6 [Fe(CN)64− ] = 1.3 ✕ 10−37 Calculate the value of the formation constant, Kf, for Fe(CN)64−.
metimes equilibria for complex ions are described in terms of dissociation constants, Kd. For the complex ion Fe(CN)64−, the dissociation reaction is as follows. Fe(CN)64− Fe2+ + 6 CN− Kd = [Fe2+ ] · [CN− ]6 [Fe(CN)64− ] = 1.3 ✕ 10−37 Calculate the value of the formation constant, Kf, for Fe(CN)64−.
Chapter11: Dynamic Electrochemistry
Section: Chapter Questions
Problem 8P
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Sometimes equilibria for complex ions are described in terms of dissociation constants, Kd. For the complex ion Fe(CN)64−, the dissociation reaction is as follows.
Fe(CN)64− <equalibrium arrow> Fe2+ + 6 CN−
Kd =
= 1.3 ✕ 10−37
[Fe2+ ] · [CN− ]6 |
[Fe(CN)64− ] |
Calculate the value of the formation constant, Kf, for Fe(CN)64−.
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