Identify the Brønsted-Lowry acid, the Brønsted-Lowry base, the conjugate acid, and the conjugate base in each reaction: (a) (CH3) 3N (aq) + H2O (l) ⇌ (CH3) 3NH + (aq) + OH - (aq) (b) HNO3 (aq) + H2O (l) ⇌H3O + (aq) + NO3 - (aq) Drag the appropriate items to their respective bins.

Writing the equation properly:

(CH₃) ₃N + H₂O ⇄ (CH₃) ₃NH⁺ + OH⁻

HNO₃ + H₂O ⇄ H₂O + NO₃⁻

The bronsted-lowry theory defines an acid as a proton donor and a base as a proton acceptor.

In a bronsted-lowry acid-base reaction, the original acid gives up its proton and becomes a conjugate base. Also, the original base accepts a proton and becomes a conjugate acid. For every acid, there is a conjugate base and for every base there is a conjugate acid.

What differentiates an acid from its conjugate base is a proton. The difference between a base and its conjugate acid is a proton.

(CH₃) ₃N + H₂O ⇄ (CH₃) ₃NH⁺ + OH⁻

Bronsted-lowry base acid conjugate acid conjugate base

HNO₃ + H₂O ⇄ H₃O⁺ + NO₃⁻

Bronsted-lowry acid base conjugate acid conjugate base