Identify Bronsted -Lowry acids in the reactions given .
`[Al(H_(2)O)_(6)]^(+3) + HCO_(3)^(-) hArr`
`underset(C)([Al(H_(2)O)_(5)(OH^(-))]^(2+)) + underset(D)(H_(2)CO_(3))`
The correct Answer

Options

A. `A,C`
B. `B,D`
C. `A,D`
D. `B,C`

Explanation

To identify the Bronsted-Lowry acids in the given reaction, we will follow these steps:

### Step 1: Understand the Reaction
The reaction provided is:
\[ [Al(H_2O)_6]^{3+} + HCO_3^{-} \rightleftharpoons [Al(H_2O)_5(OH)^{2+}] + H_2CO_3 \]

### Step 2: Identify the Bronsted-Lowry Acid
According to the Bronsted-Lowry theory, an acid is defined as a species that can donate a proton (H⁺ ion).

### Step 3: Analyze the Reactants
1. **Reactant A**: \([Al(H_2O)_6]^{3+}\)
- This species has six water molecules (H₂O) coordinated to aluminum.
- When it reacts, it donates one proton (H⁺) to form \([Al(H_2O)_5(OH)^{2+}]\).
- Since it donates a proton, it is classified as a Bronsted-Lowry acid.

2. **Reactant B**: \(HCO_3^{-}\)
- This species does not donate a proton in this reaction; instead, it accepts a proton to form \(H_2CO_3\). Therefore, it is not a Bronsted-Lowry acid.

### Step 4: Analyze the Products
1. **Product C**: \([Al(H_2O)_5(OH)^{2+}]\)
- This species has one hydroxide ion (OH⁻) and five water molecules. It does not donate a proton in this reaction; it is a base because it has accepted a proton from \([Al(H_2O)_6]^{3+}\).

2. **Product D**: \(H_2CO_3\)
- This species can donate a proton to form \(HCO_3^{-}\). Thus, it is also classified as a Bronsted-Lowry acid.

### Conclusion
The Bronsted-Lowry acids in the reaction are:
- **Reactant A**: \([Al(H_2O)_6]^{3+}\)
- **Product D**: \(H_2CO_3\)

### Final Answer
The Bronsted-Lowry acids are \([Al(H_2O)_6]^{3+}\) and \(H_2CO_3\).

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