To determine the base-conjugate acid pair in the reaction:
[tex]\[ \text{HClO}_3 + \text{NH}_3 \rightarrow \text{NH}_4^+ + \text{ClO}_3^- \][/tex]
we need to analyze the nature of each species involved according to the Bronsted-Lowry theory.
Step-by-step analysis:
1. Identify the base and the acid in the reactants:
- HClO[tex]\(_3\)[/tex] is a Bronsted-Lowry acid as it donates a proton (H[tex]\(^+\)[/tex]).
- NH[tex]\(_3\)[/tex] is a Bronsted-Lowry base since it accepts a proton (H[tex]\(^+\)[/tex]).
2. Determine the products formed:
- When NH[tex]\(_3\)[/tex] accepts a proton, it becomes NH[tex]\(_4^+\)[/tex].
- The remaining part of HClO[tex]\(_3\)[/tex] after donating a proton is ClO[tex]\(_3^-\)[/tex].
3. Identify the conjugate acid of the base:
- A conjugate acid is formed when a base gains a proton. Hence, NH[tex]\(_4^+\)[/tex] is the conjugate acid of NH[tex]\(_3\)[/tex].
4. Pairing the base and its conjugate acid:
- NH[tex]\(_3\)[/tex] (base) and NH[tex]\(_4^+\)[/tex] (conjugate acid) is a pair since NH[tex]\(_3\)[/tex] can accept a proton to become NH[tex]\(_4^+\)[/tex].
Therefore, the correct base-conjugate acid pair is:
[tex]\[ \text{NH}_3 \text{ and } \text{NH}_4^+ \][/tex]
This corresponds to the second option:
[tex]\[ \text{NH}_3 \text{ and } \text{NH}_4^+ \][/tex]
