what is the total ionic equation for the following reaction? hcn + lioh → o h⁺ + oh⁻ → h₂o o cn⁻ + li⁺ → li⁺…

what is the total ionic equation for the following reaction? hcn + lioh → o h⁺ + oh⁻ → h₂o o cn⁻ + li⁺ → li⁺ + cn⁻ o h⁺ + cn⁻ + li⁺ + oh⁻ → li⁺ + cn⁻ + h₂o done

what is the total ionic equation for the following reaction? hcn + lioh → o h⁺ + oh⁻ → h₂o o cn⁻ + li⁺ → li⁺ + cn⁻ o h⁺ + cn⁻ + li⁺ + oh⁻ → li⁺ + cn⁻ + h₂o done

Answer

Explanation:

Step1: Identify strong and weak electrolytes

HCN is a weak acid and does not fully - ionize. LiOH is a strong base and fully ionizes into $Li^{+}$ and $OH^{-}$.

Step2: Write the ionization of reactants and products

LiOH(aq) $\rightarrow$ $Li^{+}$(aq)+$OH^{-}$(aq). HCN(aq) remains mostly as HCN molecules but partially ionizes into $H^{+}$ and $CN^{-}$. The product $LiCN$ is a soluble salt and ionizes into $Li^{+}$ and $CN^{-}$, and water is a non - electrolyte. The overall reaction in total ionic form shows all the ions present in the solution. So, HCN(aq)+LiOH(aq) gives $H^{+}$(aq)+$CN^{-}$(aq)+$Li^{+}$(aq)+$OH^{-}$(aq) $\rightarrow$ $Li^{+}$(aq)+$CN^{-}$(aq)+$H_{2}O$(l).

Answer:

$H^{+}+CN^{-}+Li^{+}+OH^{-}\rightarrow Li^{+}+CN^{-}+H_{2}O$