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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.

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Answer:

Explanation:

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