Question

For the following reaction, the reactants are favored at equilibrium. Classify each of the reactants and products based on their strength as Bronsted-Lowry acids or bases. (CH3)2NH2 HCOO-(CH3)2NH HCOOH

Answer 1

In the given reaction, (CH3)2NH2 is a base, HCOO-(CH3)2NH is also a base, and HCOOH is an acid. The concentration of reactants is greater than the concentration of products at equilibrium.

Step-by-step explanation:

In order to classify each species as a Bronsted-Lowry acid or base, we need to understand that a Bronsted-Lowry acid donates a proton (H+) and a Bronsted-Lowry base accepts a proton. In the given reaction, (CH3)2NH2 is a base because it can accept a proton, HCOO-(CH3)2NH is also a base because it has the ability to accept a proton, and HCOOH is an acid because it can donate a proton.

At equilibrium, the concentration of reactants and products will depend on the reaction's equilibrium constant (K). Since the reactants are favored at equilibrium, this suggests that the concentration of reactants is greater than that of the products.