In the following `[Alunderset((p))((H_2O)_6)]^(3+)+underset((q))(HCO_3^(-))hArr[Alunderset(" "(r))((H_2O)_5)OH]^(2+)+H_2underset((s))(CO_3)` species behaving as Brosnted - Lowry acids are

Options

A. (p),(s)
B. (q),(r)
C. (q),(s)
D. (p),(r)

Answer

To solve the question regarding which species behave as Brønsted-Lowry acids in the reaction given, we need to analyze the compounds involved and their roles in proton transfer.

### Step-by-Step Solution:

1. **Identify the Compounds**:
- The first compound is \([Al(H_2O)_6]^{3+}\) (denote this as P).
- The second compound is \(HCO_3^{-}\) (denote this as Q).
- The product formed is \([Al(H_2O)_5(OH)]^{2+}\) (denote this as R) and \(H_2CO_3\) (denote this as S).

2. **Understand Brønsted-Lowry Acids**:
- A Brønsted-Lowry acid is defined as a substance that donates a proton (H⁺) to another substance.

3. **Analyze Compound P**:
- \([Al(H_2O)_6]^{3+}\) can donate a proton to form \([Al(H_2O)_5(OH)]^{2+}\). Therefore, P acts as a Brønsted-Lowry acid.

4. **Analyze Compound Q**:
- \(HCO_3^{-}\) can accept a proton to form \(H_2CO_3\). Thus, Q acts as a Brønsted-Lowry base, not an acid.

5. **Analyze Compound R**:
- \([Al(H_2O)_5(OH)]^{2+}\) can accept a proton to form \([Al(H_2O)_6]^{3+}\), indicating that R acts as a Brønsted-Lowry base.

6. **Analyze Compound S**:
- \(H_2CO_3\) can donate a proton to form \(HCO_3^{-}\). Therefore, S acts as a Brønsted-Lowry acid.

7. **Conclusion**:
- The species behaving as Brønsted-Lowry acids in this reaction are P (\([Al(H_2O)_6]^{3+}\)) and S (\(H_2CO_3\)).

### Final Answer:
The species behaving as Brønsted-Lowry acids are:
- P: \([Al(H_2O)_6]^{3+}\)
- S: \(H_2CO_3\)