In the presence of CN–, Fe3+ forms the complex ion Fe(CN)63–. The equilibrium concentrations of Fe3+and Fe(CN)63– are 8.5 ⨯ 10–40 M and 1.5 ⨯ 10–3 M, respectively, in a 0.11 M KCN solution.
Fe3+(aq) + 6CN–(aq) ⇌ Fe(CN)63–
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A. Write the formation constant (Kf) expression.
B. Calculate the value for the overall formation constant, Kf and dissociation constant, Kd of Fe(CN)63-
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“ In the presence of CN–, Fe3+ forms the complex ion Fe(CN)63–. The equilibrium concentrations of Fe3+and Fe(CN)63– are 8.5 ⨯ 10–40 M and 1.5 ⨯ 10–3 M, respectively, in a 0.11 M KCN solution. Fe3+(aq) + 6CN–(aq) ⇌ Fe(CN)63– A. Write the formation constant (Kf) expression. B. Calculate the value for the overall formation constant, Kf and dissociation constant, Kd of Fe(CN)63-In the presence of CN–, Fe3+ forms the complex ion Fe(CN)63–. The equilibrium concentrations of Fe3+and Fe(CN)63– are 8.5 ⨯ 10–40 M and 1.5 ⨯ 10–3 M, respectively, in a 0.11 M KCN solution. Fe3+(aq) + 6CN–(aq) ⇌ Fe(CN)63– A. Write the formation constant (Kf) expression. B. Calculate the value for the overall formation constant, Kf and dissociation constant, Kd of Fe(CN)63- ”
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