Question
If BaCl2(aq) + Na2CO3 (aq) react , do precipitate formed? If sure then write the balanced net ionic equation for the precipitate formed.
Answers
GPT-4o mini
When barium chloride (BaCl₂) and sodium carbonate (Na₂CO₃) react in an aqueous solution, a double displacement (or metathesis) reaction occurs. In this reaction, barium carbonate (BaCO₃), which is insoluble in water, precipitates out of the solution, while sodium chloride (NaCl) remains dissolved in the aqueous phase.
First, we can write the balanced molecular equation for the reaction:
\[
\text{BaCl}_2 (aq) + \text{Na}_2\text{CO}_3 (aq) \rightarrow \text{BaCO}_3 (s) + 2 \text{NaCl} (aq)
\]
Next, we need to break the soluble compounds into their ions to write the complete ionic equation:
**Complete Ionic Equation:**
\[
\text{Ba}^{2+} (aq) + 2 \text{Cl}^- (aq) + 2 \text{Na}^+ (aq) + \text{CO}_3^{2-} (aq) \rightarrow \text{BaCO}_3 (s) + 2 \text{Na}^+ (aq) + 2 \text{Cl}^- (aq)
\]
Now, we can identify the spectator ions. The sodium ions (Na⁺) and the chloride ions (Cl⁻) do not participate in the formation of the precipitate and are present on both sides of the equation.
**Net Ionic Equation:**
Removing the spectator ions, we get the net ionic equation:
\[
\text{Ba}^{2+} (aq) + \text{CO}_3^{2-} (aq) \rightarrow \text{BaCO}_3 (s)
\]
This equation indicates that barium ions and carbonate ions react to form solid barium carbonate, which precipitates out of the solution. Therefore, a precipitate is formed in this reaction.
First, we can write the balanced molecular equation for the reaction:
\[
\text{BaCl}_2 (aq) + \text{Na}_2\text{CO}_3 (aq) \rightarrow \text{BaCO}_3 (s) + 2 \text{NaCl} (aq)
\]
Next, we need to break the soluble compounds into their ions to write the complete ionic equation:
**Complete Ionic Equation:**
\[
\text{Ba}^{2+} (aq) + 2 \text{Cl}^- (aq) + 2 \text{Na}^+ (aq) + \text{CO}_3^{2-} (aq) \rightarrow \text{BaCO}_3 (s) + 2 \text{Na}^+ (aq) + 2 \text{Cl}^- (aq)
\]
Now, we can identify the spectator ions. The sodium ions (Na⁺) and the chloride ions (Cl⁻) do not participate in the formation of the precipitate and are present on both sides of the equation.
**Net Ionic Equation:**
Removing the spectator ions, we get the net ionic equation:
\[
\text{Ba}^{2+} (aq) + \text{CO}_3^{2-} (aq) \rightarrow \text{BaCO}_3 (s)
\]
This equation indicates that barium ions and carbonate ions react to form solid barium carbonate, which precipitates out of the solution. Therefore, a precipitate is formed in this reaction.