determine the acid, base, conjugate acid, and conjugate base in the following reaction.\nhno₃ + h₂o ⇌ h₃o⁺ +…

Explanation:

Step1: Recall Bronsted - Lowry acid - base theory

In Bronsted - Lowry theory, an acid donates a proton ((H^{+})), and a base accepts a proton.

Step2: Analyze (HNO_{3})

(HNO_{3}) donates a proton ((H^{+})) to (H_{2}O). So, (HNO_{3}) is the acid.

Step3: Analyze (H_{2}O)

(H_{2}O) accepts a proton ((H^{+})) from (HNO_{3}). So, (H_{2}O) is the base.

Step4: Determine conjugate acid

When (H_{2}O) accepts a proton ((H^{+})), it forms (H_{3}O^{+}). So, (H_{3}O^{+}) is the conjugate acid.

Step5: Determine conjugate base

When (HNO_{3}) donates a proton ((H^{+})), it forms (NO_{3}^{-}). So, (NO_{3}^{-}) is the conjugate base.

Answer:

Acid: (HNO_{3}) Conjugate Acid: (H_{3}O^{+}) Base: (H_{2}O) Conjugate Base: (NO_{3}^{-})