Write an overall net ionic equation and calculate $K$ for the reaction where $\mathrm{CuCl}\left(K_{s p}=1.9 \times 10^{-7}\right)$ is dissolved by $\mathrm{NaCN}$ to form $\left[\mathrm{Cu}(\mathrm{CN})_{2}\right]^{-}$ $\left(K_{f}=1.0 \times 10^{16}\right)$.
Added by Lorenzo R.
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Step 1: Write the overall net ionic equation for the reaction: $\mathrm{CuCl_{2(s)} + 4NaCN_{(aq)} \rightarrow [Cu(CN)_{4}]^{2-}_{(aq)} + 4NaCl_{(aq)}}$ Show more…
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