A solution of a weak acid will consist of the acid and its conjugate base.
True or False
false
Yes, of course: Take acetic acid
acetic acid + H2O<-->H3O+ + acetateion-
The system is in equilibrium.
true
To determine whether the statement is true or false, we need to understand the concept of weak acids and their conjugate bases.
A weak acid is an acid that doesn't fully ionize in water, meaning it only partially dissociates into its ions. The conjugate base of an acid is the species that remains after the acid loses a proton.
In the case of a weak acid, when it is dissolved in water, it will exist in a state of equilibrium between the acid and its conjugate base. The reaction can be represented as follows:
HA + H2O ↔ H3O+ + A-
Where HA represents the weak acid and A- represents the conjugate base.
Based on this understanding, we can see that the statement is false. A solution of a weak acid does not just consist of the acid and its conjugate base. It includes both the acid and its conjugate base, as well as other species such as the hydronium ion (H3O+) formed from the ionization of water.
Therefore, the correct answer is false.