At pH 4.5, which of the following acids would be most...

At $\mathrm{pH} 4.5$, which of the following acids would be most dissociated?
(a) Hexanoic acid $(\mathrm{pKa}=4.88)$
(b) $\mathrm{p}$ -Nitrobenzoic acid $(\mathrm{pKa}=3.4 \mathrm{I})$
(c) Octanoic acid $(\mathrm{pKa}=4.89)$
(d) Acetic acid (ethanoic acid) $(\mathrm{pKa}=4.74)$

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Key Concepts

Henderson-Hasselbalch Equation

The Henderson-Hasselbalch equation is a mathematical relationship that links the pH of a solution, the pKa of an acid, and the ratio of the concentrations of its conjugate base to the undissociated acid. This equation is useful for estimating the degree of dissociation of an acid in a solution and understanding how changes in pH affect the acid-base equilibrium.

pKa

pKa is a measure of the strength of an acid in solution. It represents the pH at which half of the acid molecules have donated their protons and become dissociated. A lower pKa value indicates a stronger acid because it means the acid is more willing to lose a proton at a given pH, leading to a higher degree of dissociation.

Acid Dissociation Equilibrium

Acid dissociation equilibrium refers to the balance established between an acid and its conjugate base when it donates a proton in solution. The degree to which an acid dissociates depends on the relative values of the solution pH and the acid's pKa, with the equilibrium shifting toward the dissociated form when the pH exceeds the pKa.

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