Alright, let's break down the reaction step-by-step to determine the net ionic equation for the reaction between [tex]\( H_2CrO_4 \)[/tex] (chromic acid) and [tex]\( Ba(OH)_2 \)[/tex] (barium hydroxide).
1. Identify the molecular equation:
First, write the balanced molecular equation for the reaction:
[tex]\[
H_2CrO_4 + Ba(OH)_2 \rightarrow BaCrO_4 + 2H_2O
\][/tex]
2. Dissociation into ions:
The compounds that are strong electrolytes will dissociate into their respective ions in aqueous solution. The chromic acid partially dissociates but we will treat it as a soluble species for the net ionic process:
[tex]\[
H_2CrO_4 \rightarrow 2H^+ + CrO_4^{2-}
\][/tex]
[tex]\[
Ba(OH)_2 \rightarrow Ba^{2+} + 2OH^-
\][/tex]
3. Combine the ions:
When the solutions of [tex]\( H_2CrO_4 \)[/tex] and [tex]\( Ba(OH)_2 \)[/tex] are mixed, they react to form water and the insoluble compound [tex]\( BaCrO_4 \)[/tex]:
[tex]\[
2H^+ + CrO_4^{2-} + Ba^{2+} + 2OH^- \rightarrow BaCrO_4(s) + 2H_2O
\][/tex]
4. Identify spectator ions:
Spectator ions are ions that appear on both sides of the equation in the same form. However, since [tex]\( BaCrO_4 \)[/tex] is a solid formed from the reaction and does not dissociate, there are no spectator ions involving these species. The key reaction here involves the neutralization of [tex]\( H^+ \)[/tex] and [tex]\( OH^- \)[/tex] to form water.
5. Write the net ionic equation:
Remove the spectator ions (if any) and focus on the ions that participate in forming the product. Upon simplification, the net ionic reaction showcases the direct formation of water from hydrogen and hydroxide ions:
[tex]\[
H^+ + OH^- \rightarrow H_2O
\][/tex]
Therefore, the net ionic equation for the reaction between [tex]\( H_2CrO_4 \)[/tex] and [tex]\( Ba(OH)_2 \)[/tex] is:
[tex]\[
H^+ + OH^- \rightarrow H_2O
\][/tex]
This equation succinctly captures the essence of the reaction, showing the fundamental process of neutralization.
