Using the Brønsted-Lowry concept of acids and bases, identify the Brønsted-Lowry acid and base in each of the following reactions:

HSO3 - (aq) + H2O (l) →H2SO3 (aq) + OH - (aq)

(CH3) 3N (g) + BCl3 (g) → (CH3) 3NBCl3 (s)

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1. HSO³⁻ (aq) + H₂O (l) → H₂SO₃ (aq) + OH⁻ (aq)

The Brønsted-Lowry acid is H₂O and the Brønsted-Lowry base is HSO³⁻

2. (CH₃) ₃N (g) + BCl₃ (g) → (CH₃) ₃NBCl₃ (s)

There are no Brønsted-Lowry acids and bases in this reaction.

Explanation:

According to the Brønsted-Lowry concept, when an acid (HA) and a base (B) undergoes a chemical reaction, the acid (HA) loses a proton and forms its conjugate base (A⁻), whereas the base gains (B) the proton to form its conjugate acid (HB⁺).

The chemical equation for this reaction is:

HA + B ⇌ A⁻ + HB⁺

Given reactions:

1. HSO³⁻ (aq) + H₂O (l) → H₂SO₃ (aq) + OH⁻ (aq)

The Brønsted-Lowry acid is H₂O and the Brønsted-Lowry base is HSO³⁻

Reason: In this reaction, the acid H₂O loses a proton and forms its conjugate base, OH⁻. Whereas, the base HSO³⁻ gains a proton to form its conjugate acid, H₂SO₃.

2. (CH₃) ₃N (g) + BCl₃ (g) → (CH₃) ₃NBCl₃ (s)

There are no Brønsted-Lowry acids and bases in this reaction.

Reason: In this reaction, there is no exchange of proton between the acid and the base.