Welch Valdez
07/05/2024 · High School
Given the reaction: \( \mathrm{Ba}(\mathrm{NO} 3) 2(\mathrm{aq})+2 \mathrm{KCl}(\mathrm{aq})-->\mathrm{BaCl} 2(\mathrm{~s})+2 \mathrm{KNO} 3(\mathrm{aq}) \) What is the net ionic equation?
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Step-by-step Solution
The given reaction is a precipitation reaction, which means that a solid precipitate is formed. In this case, the precipitate is barium chloride (\( \mathrm{BaCl} 2 \)).
To write the net ionic equation, we need to identify the spectator ions, which are ions that are present on both sides of the equation and do not participate in the reaction. In this case, the spectator ions are potassium (\( \mathrm{K}^+ \)) and nitrate (\( \mathrm{NO} 3^- \)) ions.
We can remove the spectator ions from the equation to obtain the net ionic equation:
\( \mathrm{Ba}^{2+}(\mathrm{aq}) + 2 \mathrm{Cl}^{-}(\mathrm{aq}) \rightarrow \mathrm{BaCl} 2(\mathrm{~s}) \)
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The net ionic equation for the given reaction is:
\( \mathrm{Ba}^{2+}(\mathrm{aq}) + 2 \mathrm{Cl}^{-}(\mathrm{aq}) \rightarrow \mathrm{BaCl} 2(\mathrm{~s}) \)
Quick Answer
\( \mathrm{Ba}^{2+}(\mathrm{aq}) + 2 \mathrm{Cl}^{-}(\mathrm{aq}) \rightarrow \mathrm{BaCl} 2(\mathrm{~s}) \)
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