In the reaction, HClO3 + N2H4 ⇌ ClO3– + N2H5+, which one of the sets below lists both of the acid species involved in the equilibrium?

Question

In the reaction, HClO3 + N2H4 ⇌ ClO3– + N2H5+, which one of the sets below lists both of the acid species involved in the equilibrium?

BlackTom AI · Accepted Answer

When identifying acid species in a chemical equilibrium, focus on species that donate protons (Bronsted acids) in the given reaction.
Option a: HClO3 and N2H5+. HClO3 is a strong acid (donates H+ to form ClO3−). N2H5+ is the conjugate acid of N2H4 (hydrazine); it can donate a proton in acid-base contexts, so it is indeed an acid species in this equilibrium. This option correctly lists both acid participants.
Option b: N2H4, ClO3−. Here, N2H4 is a base (it accepts protons) rather than an acid in this context, and ClO3− is the conjugate base, not an acid. Therefore, this set does not list the acid species involved.
Option c: HClO3, N2H4. While HClO3 is an acid, N2H4 is primarily a base in this reaction (it accepts a proton to form N2H5+). This combination omits one of the acid species (N2H5+), so it’s incomplete.
Option d: N2H4, N2H5+. N2H4 is a base, and N2H5+ is an acid (its conjugate pair with N2H4), but this pair does not reflect both acid species present in the equilibrium, since HClO3 is the other acid involved. This option misrepresents the set of acids by focusing on the hydrazine/hydrazinium pair only.

CHM1051 MUM S2 2025 CHM1051 Practice Exam 2

In the reaction, HClO3 + N2H4 ⇌ ClO3– + N2H5+, which one of the sets below lists both of the acid species involved in the equilibrium?

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