To write the total ionic equation for the reaction between [tex]\( H_2CrO_4 \)[/tex] (chromic acid) and [tex]\( Ba(OH)_2 \)[/tex] (barium hydroxide), we need to follow a few steps.
### Step-by-Step Solution:
1. Identify the reactants and their states:
- Chromic acid ([tex]\( H_2CrO_4 \)[/tex]) will dissociate into [tex]\( 2H^+ \)[/tex] and [tex]\( CrO_4^{2-} \)[/tex] in an aqueous solution.
- Barium hydroxide ([tex]\( Ba(OH)_2 \)[/tex]) will dissociate into [tex]\( Ba^{2+} \)[/tex] and [tex]\( 2OH^- \)[/tex] in an aqueous solution.
Therefore, the dissociation in water is:
[tex]\[
H_2CrO_4 (aq) \rightarrow 2H^+ (aq) + CrO_4^{2-} (aq)
\][/tex]
[tex]\[
Ba(OH)_2 (aq) \rightarrow Ba^{2+} (aq) + 2OH^- (aq)
\][/tex]
2. Write the molecular equation:
[tex]\[
H_2CrO_4 (aq) + Ba(OH)_2 (aq) \rightarrow BaCrO_4 (s) + 2H_2O (l)
\][/tex]
3. Separate the compounds into their ions (total ionic equation):
[tex]\[
2H^+ (aq) + CrO_4^{2-} (aq) + Ba^{2+} (aq) + 2OH^- (aq) \rightarrow BaCrO_4 (s) + 2H_2O (l)
\][/tex]
4. Check for spectator ions:
In this reaction, [tex]\( Ba^{2+} \)[/tex] and [tex]\( CrO_4^{2-} \)[/tex] combine to form an insoluble precipitate [tex]\( BaCrO_4 \)[/tex], and the [tex]\( 2H^+ \)[/tex] and [tex]\( 2OH^- \)[/tex] combine to form water.
5. Confirm the balanced total ionic equation:
[tex]\[
2H^+ (aq) + CrO_4^{2-} (aq) + Ba^{2+} (aq) + 2OH^- (aq) \rightarrow 2H_2O (l) + BaCrO_4 (s)
\][/tex]
This is the balanced total ionic equation for the reaction between chromic acid and barium hydroxide.
