Question

question
a buffer solution in which the ( k_{mathrm{a}} ) of the acid is greater than the ( k_{mathrm{b}} ) of the conjugate base will be
select the correct answer below:
acidic
basic
neutral
not a buffer

Explanation:

When \(K_{a}\) (acid dissociation constant) of the acid is greater than \(K_{b}\) (base dissociation constant) of the conjugate base, the acid - base pair in the buffer solution will produce more \(H^{+}\) ions. According to the relationship \(K_{a}\times K_{b}=K_{w}\) (\(K_{w} = 10^{- 14}\) at \(25^{\circ}C\)), a larger \(K_{a}\) means a smaller \(K_{b}\). The dominant species in terms of proton - donating ability (due to higher \(K_{a}\)) will make the buffer solution have a higher concentration of \(H^{+}\) ions compared to \(OH^{-}\) ions, resulting in an acidic buffer.

Answer:

acidic