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What is the total ionic equation for the following reaction?

[tex]\[ H_2CrO_4 + Ba(OH)_2 \][/tex]

A. [tex]\[ H_2CrO_4^{-} + 2OH^{-} \rightarrow CrO_4^{-} + 2H_2O \][/tex]

B. [tex]\[ 2H^{+} + CrO_4^{-} + 2OH^{-} \rightarrow CrO_4^{-} + 2H_2O \][/tex]

C. [tex]\[ 2H^{+} + CrO_4^{-} + Ba^{2+} + 2OH^{-} \rightarrow Ba^{2+} + CrO_4^{-} + 2H_2O \][/tex]

Sagot :

GinnyAnswer
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.
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