To determine which are the base-conjugate acid pairs in the given reaction, let's first recall the concept of conjugate acid-base pairs. A conjugate acid-base pair consists of two species that differ by a single proton ([tex]\( H^+ \)[/tex]) transfer. The acid donates a proton to become its conjugate base, while the base accepts a proton to become its conjugate acid.
The reaction provided is:
[tex]\[ HClO_3 + NH_3 \rightarrow NH_4^+ + ClO_3^- \][/tex]
1. Identify the acids and bases:
- [tex]\( NH_3 \)[/tex] (ammonia) is acting as a base.
- [tex]\( HClO_3 \)[/tex] (chloric acid) is acting as an acid.
2. Analyze what happens to the reactants:
- [tex]\( NH_3 \)[/tex] (ammonia) accepts a proton ([tex]\( H^+ \)[/tex]) to form [tex]\( NH_4^+ \)[/tex] (ammonium ion), which is its conjugate acid.
- [tex]\( HClO_3 \)[/tex] (chloric acid) donates a proton ([tex]\( H^+ \)[/tex]) to form [tex]\( ClO_3^- \)[/tex] (chlorate ion), which is its conjugate base.
3. Determine the base-conjugate acid pair:
- [tex]\( NH_3 \)[/tex] (the base) becomes [tex]\( NH_4^+ \)[/tex] (its conjugate acid).
Therefore, the base-conjugate acid pair in this reaction is [tex]\( NH_3 \)[/tex] and [tex]\( NH_4^+ \)[/tex].
So, the correct option is:
[tex]\[ \boxed{NH_3 \text{ and } NH_4^+} \][/tex]
