Classify the following as acid or base according to Bronsted - Lowry concept.
(i) `CH_(3)COO^(-)`
(ii) `H_(3)O^(+)`
(iii) `SO_(4)^(2-)`
(iv) `HCl`

Options

A. `{:((i),(ii),(iii),(iv),),("Bronsted acid","Bronsted base","Bronsted base","Bronsted acid",):}`
B. `{:((i),(ii),(iii),(iv),),("Bronsted acid","Bronsted acid","Bronsted acid","Bronsted base",):}`
C. `{:((i),(ii),(iii),(iv),),("Bronsted base","Bronsted acid","Bronsted base","Bronsted acid",):}`
D. `{:((i),(ii),(iii),(iv),),("Bronsted acid","Bronsted acid","Bronsted base","Bronsted base",):}`

Explanation

To classify the given species according to the Bronsted-Lowry concept, we need to determine whether each species acts as an acid (donates a proton, H⁺) or as a base (accepts a proton, H⁺).

### Step-by-Step Solution:

1. **Identify the first species: `CH₃COO⁻` (acetate ion)**
- The acetate ion can accept a proton (H⁺) to form acetic acid (CH₃COOH).
- Since it accepts a proton, it is classified as a **Bronsted base**.

2. **Identify the second species: `H₃O⁺` (hydronium ion)**
- The hydronium ion can donate a proton (H⁺) to form water (H₂O).
- Since it donates a proton, it is classified as a **Bronsted acid**.

3. **Identify the third species: `SO₄²⁻` (sulfate ion)**
- The sulfate ion can accept a proton (H⁺) to form hydrogen sulfate (HSO₄⁻).
- Since it accepts a proton, it is classified as a **Bronsted base**.

4. **Identify the fourth species: `HCl` (hydrochloric acid)**
- HCl can donate a proton (H⁺) to form chloride ion (Cl⁻).
- Since it donates a proton, it is classified as a **Bronsted acid**.

### Summary of Classifications:
- (i) `CH₃COO⁻` - Bronsted base
- (ii) `H₃O⁺` - Bronsted acid
- (iii) `SO₄²⁻` - Bronsted base
- (iv) `HCl` - Bronsted acid