M^{+} + 2 CN^{-} ⇌ [M(CN)_{2}]^{-}

$\overline{){{\mathbf{K}}}_{{\mathbf{f}}}{\mathbf{}}{\mathbf{=}}\frac{\mathbf{products}}{\mathbf{reactants}}{\mathbf{=}}\frac{\left[M{{\left(\mathrm{CN}\right)}_{2}}^{-}\right]}{\mathbf{\left[}{\mathbf{M}}^{\mathbf{+}}\mathbf{\right]}{\mathbf{\left[}{\mathbf{CN}}^{\mathbf{-}}\mathbf{\right]}}^{\mathbf{2}}}}$

Step 1: Construct ICE table for the reaction

The formation constant of [M(CN)_{2}]^{- }is 5.30 x 10^{18}, where M is a generic metal.

A 0.160-mole quantity of M(NO3) is added to a liter of 0.710 M NaCN solution. What is the concentration of M^{+} ions at equilibrium?

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Based on our data, we think this problem is relevant for Professor Vickrey's class at UNL.