Write the conjugate acid and base of NH3 .

To determine the conjugate acid and base of $NH X_{3}$ , we use the Brønsted–Lowry theory, where:

NH₄⁺NH₃+H⁺

NH₄⁺ donates a proton (H⁺) to form NH₃ (conjugate base of NH₄⁺) and H⁺ (not NH₂⁻). **Correction:** NH₃ is the base, NH₂⁻ is its conjugate base (not shown here).

NH₃+H⁺ProtonationNH₄⁺

Formation of NH₄⁺ (conjugate acid) from NH₃

NH₃ (Base)NH₃ (Base)NH₄⁺NH₂⁻

Brønsted–Lowry acid-base relationships of NH₃: NH₃ gains H⁺ → NH₄⁺ (acid); NH₃ loses H⁺ → NH₂⁻ (base).

A conjugate acid is formed when a base accepts a proton ( $H X^{+}$ ).
A conjugate base is formed when an acid donates a proton.

For $NH X_{3}$ (ammonia):

Conjugate acid of $NH X_{3}$ : When $NH X_{3}$ accepts a proton ( $H X^{+}$ ), it forms $NH X_{4} X^{+}$ (ammonium ion). $NH X_{3} + H X^{+} NH X_{4} X^{+}$ Thus, the conjugate acid is $NH X_{4} X^{+}$ .
Conjugate base of $NH X_{3}$ : $NH X_{3}$ itself acts as a base when it accepts a proton. Its conjugate base is formed by removing a proton from its conjugate acid ( $NH X_{4} X^{+}$ ), which is $NH X_{2} X^{-}$ (amide ion). $NH X_{4} X^{+} NH X_{3} + H X^{+}$ Thus, the conjugate base is $NH X_{2} X^{-}$ .

In summary:

Conjugate acid of $NH X_{3}$ : $NH X_{4} X^{+}$
Conjugate base of $NH X_{3}$ : $NH X_{2} X^{-}$

Discussion

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