Identify Bronsted Lowry acids in the reaction given below ?
`[AIH_(2)O)_(6)]^(3+)+HCO_(3) rarr [A] (H_(2)O)(OH)]^(2+) +H_(2)CO_(3)`

Options

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

Answer

To identify the Bronsted-Lowry acids in the given reaction:

**Reaction:**
\[ [Al(H_2O)_6]^{3+} + HCO_3^{-} \rightarrow [Al(H_2O)_5(OH)]^{2+} + H_2CO_3 \]

### Step-by-Step Solution:

1. **Understand the Bronsted-Lowry Theory:**
- According to the Bronsted-Lowry theory, an acid is defined as a substance that donates a proton (H⁺), while a base is a substance that accepts a proton.

2. **Identify the Species in the Reaction:**
- The reactants are \([Al(H_2O)_6]^{3+}\) and \(HCO_3^{-}\).
- The products are \([Al(H_2O)_5(OH)]^{2+}\) and \(H_2CO_3\).

3. **Analyze the First Reactant:**
- The species \([Al(H_2O)_6]^{3+}\) can donate a proton to form \([Al(H_2O)_5(OH)]^{2+}\).
- Since it donates a proton, \([Al(H_2O)_6]^{3+}\) is a Bronsted-Lowry acid.

4. **Analyze the Second Reactant:**
- The bicarbonate ion \(HCO_3^{-}\) can accept a proton to form \(H_2CO_3\).
- Since it accepts a proton, \(HCO_3^{-}\) is a Bronsted-Lowry base.

5. **Analyze the Products:**
- The product \(H_2CO_3\) can donate a proton to revert back to \(HCO_3^{-}\).
- Since it can donate a proton, \(H_2CO_3\) is also a Bronsted-Lowry acid.

6. **Conclusion:**
- The Bronsted-Lowry acids in the reaction are \([Al(H_2O)_6]^{3+}\) and \(H_2CO_3\).

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

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