Final answer:
In the equilibrium reaction with k < 1, NO₂⁻ acts as a strong conjugate base of the weak acid HNO₂, whereas (C₂H₅)₃NH is the weak conjugate acid of the weak base (C₂H₅)₃N.
Step-by-step explanation:
In the given reaction, since k < 1, we can deduce that the forward reaction is not favored, and thus the reactants are stronger than the products in terms of their roles as Brønsted-Lowry acids and bases. Specifically, NO₂⁻ is the conjugate base of HNO₂, which implies that nitrous acid (HNO₂) is a weak acid. On the other hand, (C₂H₅)₃NH is the conjugate acid of (C₂H₅)₃N, indicating that triethylamine ((C₂H₅)₃N) is a weak base. The product HNO₂ is also a weak acid, yet because the reaction favors the left side, it is stronger than its conjugate base NO₂⁻. The (C₂H₅)₃NH is a weak base as well, but in the context of this equilibrium, it acts as an acid weaker than its conjugate base.
Classification of Reactants and Products as Bronsted-Lowry Acids or Bases
For the given reaction, NO₂⁻ is a Bronsted-Lowry base because it can accept a proton (H⁺) to form HNO₂. (C₂H₅)3NH is also a Bronsted-Lowry base because it can accept a proton to form (C₂H₅)3NH₂. HNO₂ is a Bronsted-Lowry acid because it can donate a proton to form NO₂⁻.
Summary of Classification
NO₂⁻ - Bronsted-Lowry Base
(C₂H₅)3NH - Bronsted-Lowry Base
HNO₂ - Bronsted-Lowry Acid