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.

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

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