pKa (source code)
= pKa
{c}
{title2=$\mathrm pK_a=-\log_{10}K_a$}
The <pKa> is the negative base-ten <logarithm> of the <dimensionless> <acid dissociation constant>. A lower <pKa> means a larger <acid dissociation constant> and a stronger tendency to donate a <proton> under the same <standard state>, <solvent>, and <temperature> conventions. The <Henderson-Hasselbalch equation> places equal <weak acid> and <conjugate base> <thermodynamic activities> at <pH> equal to <pKa>. See https://openstax.org/books/chemistry-2e/pages/14-6-buffers[Flowers et al., Chemistry 2e, the Henderson-Hasselbalch equation].
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