Question
Write the total ionic and net ionic equation for the following .consider the balance equation as well as stages.
A. HCI (aq) + Na2CO3 (aq) = H2O (l) +CO2 (g) + NaCl (aq)
A. HCI (aq) + Na2CO3 (aq) = H2O (l) +CO2 (g) + NaCl (aq)
Answers
GPT-4o mini
To write the total ionic and net ionic equations for the reaction between hydrochloric acid (HCl) and sodium carbonate (Na2CO3), we first start with the balanced molecular equation and then break it down into its ionic components.
### Step 1: Write the balanced molecular equation
The balanced equation for the reaction is:
\[
2 \, \text{HCl (aq)} + \text{Na}_2\text{CO}_3 \, \text{(aq)} \rightarrow \, H_2O \, \text{(l)} + \, CO_2 \, \text{(g)} + 2 \, \text{NaCl (aq)}
\]
### Step 2: Write the total ionic equation
Next, we convert all the soluble ionic compounds into their respective ions. HCl and Na2CO3 are soluble, while water (H2O) and carbon dioxide (CO2) are not dissociated as they are not strong electrolytes.
The total ionic equation is:
\[
2 \, \text{H}^+ \, \text{(aq)} + 2 \, \text{Cl}^- \, \text{(aq)} + 2 \, \text{Na}^+ \, \text{(aq)} + \text{CO}_3^{2-} \, \text{(aq)} \rightarrow \, H_2O \, \text{(l)} + \, CO_2 \, \text{(g)} + 2 \, \text{Na}^+ \, \text{(aq)} + 2 \, \text{Cl}^- \, \text{(aq)}
\]
### Step 3: Write the net ionic equation
To obtain the net ionic equation, we remove the spectator ions (ions that appear on both sides of the equation without undergoing any change). In this case, Na\(^+\) and Cl\(^-\) ions are spectator ions.
Thus, the net ionic equation is:
\[
2 \, \text{H}^+ \, \text{(aq)} + \text{CO}_3^{2-} \, \text{(aq)} \rightarrow H_2O \, \text{(l)} + \, CO_2 \, \text{(g)}
\]
### Summary
- **Total Ionic Equation**:
\[
2 \, \text{H}^+ \, \text{(aq)} + 2 \, \text{Cl}^- \, \text{(aq)} + 2 \, \text{Na}^+ \, \text{(aq)} + \text{CO}_3^{2-} \, \text{(aq)} \rightarrow \, H_2O \, \text{(l)} + \, CO_2 \, \text{(g)} + 2 \, \text{Na}^+ \, \text{(aq)} + 2 \, \text{Cl}^- \, \text{(aq)}
\]
- **Net Ionic Equation**:
\[
2 \, \text{H}^+ \, \text{(aq)} + \text{CO}_3^{2-} \, \text{(aq)} \rightarrow H_2O \, \text{(l)} + \, CO_2 \, \text{(g)}
\]
### Step 1: Write the balanced molecular equation
The balanced equation for the reaction is:
\[
2 \, \text{HCl (aq)} + \text{Na}_2\text{CO}_3 \, \text{(aq)} \rightarrow \, H_2O \, \text{(l)} + \, CO_2 \, \text{(g)} + 2 \, \text{NaCl (aq)}
\]
### Step 2: Write the total ionic equation
Next, we convert all the soluble ionic compounds into their respective ions. HCl and Na2CO3 are soluble, while water (H2O) and carbon dioxide (CO2) are not dissociated as they are not strong electrolytes.
The total ionic equation is:
\[
2 \, \text{H}^+ \, \text{(aq)} + 2 \, \text{Cl}^- \, \text{(aq)} + 2 \, \text{Na}^+ \, \text{(aq)} + \text{CO}_3^{2-} \, \text{(aq)} \rightarrow \, H_2O \, \text{(l)} + \, CO_2 \, \text{(g)} + 2 \, \text{Na}^+ \, \text{(aq)} + 2 \, \text{Cl}^- \, \text{(aq)}
\]
### Step 3: Write the net ionic equation
To obtain the net ionic equation, we remove the spectator ions (ions that appear on both sides of the equation without undergoing any change). In this case, Na\(^+\) and Cl\(^-\) ions are spectator ions.
Thus, the net ionic equation is:
\[
2 \, \text{H}^+ \, \text{(aq)} + \text{CO}_3^{2-} \, \text{(aq)} \rightarrow H_2O \, \text{(l)} + \, CO_2 \, \text{(g)}
\]
### Summary
- **Total Ionic Equation**:
\[
2 \, \text{H}^+ \, \text{(aq)} + 2 \, \text{Cl}^- \, \text{(aq)} + 2 \, \text{Na}^+ \, \text{(aq)} + \text{CO}_3^{2-} \, \text{(aq)} \rightarrow \, H_2O \, \text{(l)} + \, CO_2 \, \text{(g)} + 2 \, \text{Na}^+ \, \text{(aq)} + 2 \, \text{Cl}^- \, \text{(aq)}
\]
- **Net Ionic Equation**:
\[
2 \, \text{H}^+ \, \text{(aq)} + \text{CO}_3^{2-} \, \text{(aq)} \rightarrow H_2O \, \text{(l)} + \, CO_2 \, \text{(g)}
\]