Question

For the following reaction, k < 1, classify each of the reactants and products based on their strength as Bronsted-Lowry acids or bases. HCOO⁻, C₆H₅NH₃, HCOOH, C₆H₅NH₂?

Answer 1

To classify the reactants and products as Bronsted-Lowry acids or bases, HCOO⁻ and HCOOH can act as acids, while C₆H₅NH₃ and C₆H₅NH₂ can act as bases. At equilibrium, there will be a greater concentration of reactants present.

Step-by-step explanation:

To classify the reactants and products in terms of their strengths as Bronsted-Lowry acids or bases, we need to consider their ability to donate or accept a proton. A Bronsted-Lowry acid is a species that donates a proton, while a Bronsted-Lowry base is a species that accepts a proton.

In the given reaction, HCOO⁻ and HCOOH can act as Bronsted-Lowry acids because they can donate a proton. C₆H₅NH₃ and C₆H₅NH₂ can act as Bronsted-Lowry bases because they can accept a proton.

At equilibrium, the concentration of reactants and products will depend on the specific reaction conditions and the value of the equilibrium constant (k). However, since k is less than 1, it indicates that the reaction favors the reactants, meaning that there will be a greater concentration of reactants present at equilibrium.