Question
Write the total ionic equation and net ionic equation for the following consider the balance equation as well as stage.
B. Ba(OH)2 (aq) + Fe2(SO4)(aq) =Fe(OH) (s)+BaSO4(aq)
B. Ba(OH)2 (aq) + Fe2(SO4)(aq) =Fe(OH) (s)+BaSO4(aq)
Answers
GPT-4o mini
To write the total ionic equation and the net ionic equation for the given reaction, we first need to ensure that the balanced molecular equation is correct. The reaction appears to be:
\[ \text{Ba(OH)}_2 (aq) + \text{Fe}_2(\text{SO}_4)_3 (aq) \rightarrow 2 \text{Fe(OH)}_3 (s) + \text{BaSO}_4 (aq) \]
### Step 1: Write the Balanced Molecular Equation
1. **Balance the Equation:**
- On the reactant side, we have 2 Fe from Fe₂(SO₄)₃, so we need 2 Fe(OH)₃ on the product side.
- Ba(OH)₂ will produce BaSO₄ as a soluble salt.
The balanced equation is:
\[ \text{3Ba(OH)}_2 (aq) + \text{Fe}_2(\text{SO}_4)_3 (aq) \rightarrow 2 \text{Fe(OH)}_3 (s) + 3\text{BaSO}_4 (aq) \]
### Step 2: Write the Total Ionic Equation
For the total ionic equation, we separate the soluble ionic compounds into their respective ions:
**Total Ionic Equation:**
\[
3 \text{Ba}^{2+} (aq) + 6 \text{OH}^- (aq) + 2 \text{Fe}^{3+} (aq) + 3 \text{SO}_4^{2-} (aq) \rightarrow 2 \text{Fe(OH)}_3 (s) + 3 \text{Ba}^{2+} (aq) + 3 \text{SO}_4^{2-} (aq)
\]
### Step 3: Write the Net Ionic Equation
To derive the net ionic equation, we eliminate the spectator ions (ions that do not change during the reaction). In this case, Ba²⁺ and SO₄²⁻ are spectator ions since they appear on both sides of the equation.
**Net Ionic Equation:**
The remaining species that participate in the reaction are:
\[
2 \text{Fe}^{3+} (aq) + 6 \text{OH}^- (aq) \rightarrow 2 \text{Fe(OH)}_3 (s)
\]
### Conclusion
The final results:
- **Total Ionic Equation:**
\[
3 \text{Ba}^{2+} (aq) + 6 \text{OH}^- (aq) + 2 \text{Fe}^{3+} (aq) + 3 \text{SO}_4^{2-} (aq) \rightarrow 2 \text{Fe(OH)}_3 (s) + 3 \text{Ba}^{2+} (aq) + 3 \text{SO}_4^{2-} (aq)
\]
- **Net Ionic Equation:**
\[
2 \text{Fe}^{3+} (aq) + 6 \text{OH}^- (aq) \rightarrow 2 \text{Fe(OH)}_3 (s)
\]
\[ \text{Ba(OH)}_2 (aq) + \text{Fe}_2(\text{SO}_4)_3 (aq) \rightarrow 2 \text{Fe(OH)}_3 (s) + \text{BaSO}_4 (aq) \]
### Step 1: Write the Balanced Molecular Equation
1. **Balance the Equation:**
- On the reactant side, we have 2 Fe from Fe₂(SO₄)₃, so we need 2 Fe(OH)₃ on the product side.
- Ba(OH)₂ will produce BaSO₄ as a soluble salt.
The balanced equation is:
\[ \text{3Ba(OH)}_2 (aq) + \text{Fe}_2(\text{SO}_4)_3 (aq) \rightarrow 2 \text{Fe(OH)}_3 (s) + 3\text{BaSO}_4 (aq) \]
### Step 2: Write the Total Ionic Equation
For the total ionic equation, we separate the soluble ionic compounds into their respective ions:
**Total Ionic Equation:**
\[
3 \text{Ba}^{2+} (aq) + 6 \text{OH}^- (aq) + 2 \text{Fe}^{3+} (aq) + 3 \text{SO}_4^{2-} (aq) \rightarrow 2 \text{Fe(OH)}_3 (s) + 3 \text{Ba}^{2+} (aq) + 3 \text{SO}_4^{2-} (aq)
\]
### Step 3: Write the Net Ionic Equation
To derive the net ionic equation, we eliminate the spectator ions (ions that do not change during the reaction). In this case, Ba²⁺ and SO₄²⁻ are spectator ions since they appear on both sides of the equation.
**Net Ionic Equation:**
The remaining species that participate in the reaction are:
\[
2 \text{Fe}^{3+} (aq) + 6 \text{OH}^- (aq) \rightarrow 2 \text{Fe(OH)}_3 (s)
\]
### Conclusion
The final results:
- **Total Ionic Equation:**
\[
3 \text{Ba}^{2+} (aq) + 6 \text{OH}^- (aq) + 2 \text{Fe}^{3+} (aq) + 3 \text{SO}_4^{2-} (aq) \rightarrow 2 \text{Fe(OH)}_3 (s) + 3 \text{Ba}^{2+} (aq) + 3 \text{SO}_4^{2-} (aq)
\]
- **Net Ionic Equation:**
\[
2 \text{Fe}^{3+} (aq) + 6 \text{OH}^- (aq) \rightarrow 2 \text{Fe(OH)}_3 (s)
\]