To determine the total ionic equation for the reaction between HCN and LiOH, we need to carefully consider the individual ions involved and their behavior in the solution. Let’s break down the steps to arrive at the total ionic equation.
### Step 1: Dissociate the Reactants
First, we need to understand how HCN and LiOH dissociate in an aqueous solution:
- HCN (Hydrogen cyanide) partially ionizes to form:
[tex]\[ \text{HCN} \leftrightarrow \text{H}^+ + \text{CN}^- \][/tex]
- LiOH (Lithium hydroxide) fully dissociates into its ions:
[tex]\[ \text{LiOH} \rightarrow \text{Li}^+ + \text{OH}^- \][/tex]
### Step 2: Write the Ionization Reactions
We can now write the ionization reactions of the involved species:
- HCN dissociates to give:
[tex]\[ \text{HCN} \rightarrow \text{H}^+ + \text{CN}^- \][/tex]
- LiOH dissociates to give:
[tex]\[ \text{LiOH} \rightarrow \text{Li}^+ + \text{OH}^- \][/tex]
### Step 3: Combine the Ionized Species
Next, we combine all the ionized species in our reaction mixture:
- From HCN, we get:
[tex]\[ \text{H}^+ \text{ and } \text{CN}^- \][/tex]
- From LiOH, we get:
[tex]\[ \text{Li}^+ \text{ and } \text{OH}^- \][/tex]
### Step 4: Identify the Reactions that Occur
Examine the reactions occurring between these ions in the solution:
1. Acid-Base Neutralization:
[tex]\[ \text{H}^+ + \text{OH}^- \rightarrow \text{H}_2\text{O} \][/tex]
2. Other Ions:
The [tex]\(\text{CN}^-\)[/tex] and [tex]\(\text{Li}^+\)[/tex] ions remain in the solution:
[tex]\[ \text{CN}^- + \text{Li}^+ \rightarrow \text{Li}^+ + \text{CN}^- \][/tex]
### Step 5: Write the Total Ionic Equation
To construct the total ionic equation, we can combine the ions that are originally present in the solution and show the chemical process occurring:
[tex]\[
\text{H}^+ + \text{CN}^- + \text{Li}^+ + \text{OH}^- \rightarrow \text{Li}^+ + \text{CN}^- + \text{H}_2\text{O}
\][/tex]
### Step 6: Verify Spectator Ions
Finally, identify and confirm any spectator ions (ions that do not participate in the reaction and remain unchanged):
- [tex]\(\text{Li}^+\)[/tex]
- [tex]\(\text{CN}^-\)[/tex]
These ions don’t change during the reaction, confirming that the equation is accurate.
Thus, the total ionic equation for the reaction is:
[tex]\[
\text{H}^+ + \text{CN}^- + \text{Li}^+ + \text{OH}^- \rightarrow \text{Li}^+ + \text{CN}^- + \text{H}_2\text{O}
\][/tex]
