In the Bronsted-Lowry theory of acids, an acid will lose a proton (H+) and leave behind the conjugate base of the acid. The conjugate base of a strong acid is?
The conjugate base of a strong acid is always a weak base. Strong acids completely dissociate in water, meaning they readily lose a proton (H+) and form their conjugate base. Since strong acids have a tendency to donate protons, their conjugate bases have a weak affinity for accepting protons and therefore act as weak bases. It is important to note that the strength of an acid is not related to the strength of its conjugate base.
To determine the conjugate base of a strong acid in the Bronsted-Lowry theory, we need to first understand what a strong acid is. A strong acid is an acid that completely donates its protons (H+) when dissolved in water. Therefore, a strong acid essentially loses all of its protons, leaving only the conjugate base.
To find the conjugate base, we need to identify the acid first. In the case of a strong acid, the acid itself is the molecule that donates the protons. For example, let's consider hydrochloric acid (HCl), which is a common example of a strong acid. In water, HCl dissociates into H+ and Cl-. Here, HCl is the acid, donating the H+ ion, and Cl- is the conjugate base.
Therefore, for a strong acid, the conjugate base is the remaining anion or the negative ion after the acid donates its protons. In the case of hydrochloric acid (HCl), the conjugate base is chloride (Cl-).