To determine the total ionic equation, we carefully observe the dissociation of each substance in aqueous solution and write out all the ions involved in the reaction. Here's a step-by-step breakdown of the process:
1. Dissociation of Reactants in Aqueous Solution:
- Chromic acid ([tex]\( H_2CrO_4 \)[/tex]):
[tex]\[
H_2CrO_4 \rightarrow 2H^+ + CrO_4^{2-}
\][/tex]
- Barium hydroxide ([tex]\( Ba(OH)_2 \)[/tex]):
[tex]\[
Ba(OH)_2 \rightarrow Ba^{2+} + 2OH^-
\][/tex]
2. Total Ionic Equation:
Combine all the dissociated ions from the above reactants on the left side of the equation:
[tex]\[
2H^+ + CrO_4^{2-} + Ba^{2+} + 2OH^- \rightarrow
\][/tex]
3. Formation of Products in Aqueous Solution:
- Barium chromate ([tex]\( BaCrO_4 \)[/tex]) is an insoluble salt and remains undissociated in water, but in this case it is not formed as a product in the given reaction.
- Water ([tex]\( H_2O \)[/tex]) is a molecular compound that does not dissociate in solution.
Therefore, the product side of the equation remains the ions [tex]\( Ba^{2+} \)[/tex] and [tex]\( CrO_4^{2-} \)[/tex] along with the formed water:
[tex]\[
Ba^{2+} + CrO_4^{2-} + 2H_2O
\][/tex]
4. Complete Total Ionic Equation:
Putting these together, the total ionic equation is:
[tex]\[
2H^+ + CrO_4^{2-} + Ba^{2+} + 2OH^- \rightarrow Ba^{2+} + CrO_4^{2-} + 2H_2O
\][/tex]
This final equation represents the total ionic equation of the given reactions involving chromic acid and barium hydroxide in aqueous solution.
