Answer:
According to Bronsted-Lowry theory, an acid is any species that can donate H+ (proton), while a base is any species that can accept a H+ ion.
[tex]NH_{3}[/tex](aq) + [tex]H_{2}O[/tex](aq) → [tex]NH_{4}^{+}[/tex](aq)+ [tex]OH^{-}[/tex](aq)
[tex]NH_{4}^{+}[/tex] is the conjugate acid of [tex]NH_{3}[/tex]
2. [tex]ClO_{3}^{-}[/tex]
[tex]ClO_{3}^{-}[/tex](aq) + [tex]H_{2}O[/tex](aq) → [tex]HClO_{3}[/tex](aq) + [tex]OH^{-}[/tex](aq)
[tex]HClO_{3}[/tex] is the conjugate acid of [tex]ClO_{3}^{-}[/tex]
3. [tex]SO_{4}^{2-}[/tex]
[tex]SO_{4}^{2-}[/tex](aq) + [tex]H_{2}O[/tex](aq) → [tex]HSO_{4}^{-}[/tex](aq) + [tex]OH^{-}[/tex](aq)
[tex]HSO_{4}^{-}[/tex] is the conjugate acid of [tex]SO_{4}^{2-}[/tex]
4. [tex]OH^{-}[/tex]
[tex]OH^{-}[/tex](aq) + [tex]H^{+}[/tex](aq) → [tex]H_{2}O[/tex](aq)
[tex]H_{2}O[/tex] is the conjugate acid of [tex]OH^{-}[/tex]
