Question
If BaCl2(aq) + NaCl (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 (BaClâ‚‚) reacts with sodium chloride (NaCl) in aqueous solution, all the reactants and products remain in the ionic form because they are both soluble in water. Therefore, no precipitate is formed in this reaction.
The reaction can be written as follows:
\[ \text{BaCl}_2(aq) + 2 \text{NaCl}(aq) \rightarrow \text{BaCl}_2(aq) + 2 \text{NaCl}(aq) \]
When we look at the dissociated ions in solution:
- \( \text{Ba}^{2+}(aq) + 2 \text{Cl}^-(aq) + 2 \text{Na}^+(aq) + 2 \text{Cl}^-(aq) \)
All ions remain in solution and no new solid product is formed, meaning there is no net ionic reaction.
If we attempt to cancel out the spectator ions, which in this case are simply the sodium and chloride ions, we find that the remaining components do not yield a net ionic equation since they do not change:
\[
\text{No precipitate is formed and there is no net ionic equation.}
\]
Thus, the conclusion is that no precipitate forms when BaClâ‚‚ reacts with NaCl in solution.
The reaction can be written as follows:
\[ \text{BaCl}_2(aq) + 2 \text{NaCl}(aq) \rightarrow \text{BaCl}_2(aq) + 2 \text{NaCl}(aq) \]
When we look at the dissociated ions in solution:
- \( \text{Ba}^{2+}(aq) + 2 \text{Cl}^-(aq) + 2 \text{Na}^+(aq) + 2 \text{Cl}^-(aq) \)
All ions remain in solution and no new solid product is formed, meaning there is no net ionic reaction.
If we attempt to cancel out the spectator ions, which in this case are simply the sodium and chloride ions, we find that the remaining components do not yield a net ionic equation since they do not change:
\[
\text{No precipitate is formed and there is no net ionic equation.}
\]
Thus, the conclusion is that no precipitate forms when BaClâ‚‚ reacts with NaCl in solution.