Problem: The formation constant of [M(CN)2]- is 5.30 x 1018, 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?

FREE Expert Solution

M⁺ + 2 CN^- ⇌ [M(CN)₂]^-

$\boxed{{\mathbf{K}}_{\mathbf{f}}\mathbf{ }\mathbf{=}\frac{\mathbf{products}}{\mathbf{reactants}}\mathbf{=}\frac{\left[M{{\left(\mathrm{CN}\right)}_2}^{-}\right]}{\mathbf{\left[}{\mathbf{M}}^{\mathbf{+}}\mathbf{\right]}{\mathbf{\left[}{\mathbf{CN}}^{\mathbf{-}}\mathbf{\right]}}^{\mathbf{2}}}}$

Step 1: Construct ICE table for the reaction