A solution was prepared such that the initial concentrations of Cu²⁺(aq) and CN^-(aq) were 0.0120 M and 0.0400 M, respectively. These ions react according to the following chemical equation:
$\mathrm{Cu}^{2+}(a q) +4 \mathrm{CN}^{-}(a q) \rightleftharpoons \mathrm{Cd}(\mathrm{CN}) _{4}^{2-}(a q)$

$\mathrm{K}_{\mathrm{c}}=1.0 \times 10^{25}$
What will be the concentration of CN^-(aq) at equilibrium

Question

A solution was prepared such that the initial concentrations of Cu²⁺(aq) and CN^-(aq) were 0.0120 M and 0.0400 M, respectively. These ions react according to the following chemical equation:

\mathrm{Cu}^{2+}(a q) +4 \mathrm{CN}^{-}(a q) \rightleftharpoons \mathrm{Cd}(\mathrm{CN}) _{4}^{2-}(a q)

\mathrm{K}_{\mathrm{c}}=1.0 \times 10^{25}

What will be the concentration of CN^-(aq) at equilibrium

Quizplus · Accepted Answer

The Answer of A solution was prepared such that the initial concentrations of Cu²⁺(aq) and CN^-(aq) were 0.0120 M and 0.0400 M, respectively. These ions react according to the following chemical equation: $\mathrm{Cu}^{2+}(a q)+4 \mathrm{CN}^{-}(a q) \rightleftharpoons \mathrm{Cd}(\mathrm{CN})_{4}^{2-}(a q)$ $\mathrm{K}_{\mathrm{c}}=1.0 \times 10^{25}$ What will be the concentration of CN^-(aq) at equilibrium

A Solution Was Prepared Such That the Initial Concentrations of Cu2+(aq)

A Solution Was Prepared Such That the Initial Concentrations of Cu²⁺(aq)