Given the following standard reduction potentials Ag^+(a q)+e^- ⟶Ag(s) E^0=0.799 V Ag(CN)2

step 1 So given the following standard reduction potentials, we are asked to find the KF for AG CN2 min

Given the following standard reduction potentials Ag^+(a...

Given the following standard reduction potentials $$ \begin{gathered} \mathrm{Ag}^{+}(a q)+e^{-} \longrightarrow \mathrm{Ag}(s) \quad E^0=0.799 \mathrm{~V} \\ {\mathrm{Ag}(\mathrm{CN})_2^{-}+e^{-} \longrightarrow \mathrm{Ag}(s)+2 \mathrm{CN}^{-}(a q) \quad E^e=-0.31 \mathrm{~V}}^{\longrightarrow} \end{gathered} $$ find $K_f$ for $\mathrm{Ag}(\mathrm{CN})_2{ }^{-}(a q)$ at $25^{\circ} \mathrm{C}$.

Given the following standard reduction potentials
$$
\begin{gathered}
\mathrm{Ag}^{+}(a q)+e^{-} \longrightarrow \mathrm{Ag}(s) \quad E^0=0.799 \mathrm{~V} \\
{\mathrm{Ag}(\mathrm{CN})_2^{-}+e^{-} \longrightarrow \mathrm{Ag}(s)+2 \mathrm{CN}^{-}(a q) \quad E^e=-0.31 \mathrm{~V}}^{\longrightarrow}
\end{gathered}
$$
find $K_f$ for $\mathrm{Ag}(\mathrm{CN})_2{ }^{-}(a q)$ at $25^{\circ} \mathrm{C}$.

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Key Concepts

Complex Ion Formation (Stability) Constant

The formation constant (Kf) quantifies the stability of a complex ion, reflecting the equilibrium between the free metal ion and ligands versus the resulting complex. In many cases, it is derived indirectly from thermodynamic or electrochemical measurements. A large Kf indicates a highly stable complex, as the reaction strongly favors the formation of the complex ion.

Standard Reduction Potentials

Standard reduction potentials measure the inherent tendency of a chemical species to be reduced under standard conditions (25°C, 1 M concentration, 1 atm pressure). They serve as a basis for predicting the direction of redox reactions and are used to calculate the overall cell potential when two half?reactions are combined.

Relationship Between ?G° and Equilibrium Constants

The connection between redox potentials and thermodynamics is established through the relationship ?G° = -nFE°. This relation links the standard free energy change (?G°) of a process with its electrical work, allowing one to determine the equilibrium constant via lnK = nFE°/RT. This concept is fundamental when using electrochemical data to derive equilibrium properties.

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