I know that when you have aqueous solutions, then the pKa and the pKb are linked to each other (pKa + pKb = 14). Is there an equivalent relationship between pKa and pKb in non aqueous environments? I'm currently looking at a paper where they have measured pKb values in glacial acetic acid (https://pubs.acs.org/doi/epdf/10.1021/ic50084a055), but I'm interested in finding the pKa values for a different set of compounds in glacial acetic acid. Thank you.
Bruckenstein and Kolthoff give some values in the abstract, which is available in the free preview. Notable among acids: perchloric acid, $pK_a=4.87$; hydrogen chloride, $pK_a=8.55$.
Also given is an autodissociation constant, whose base-10 logarithm is $-14.45$. Thus whereas we render $pK_a+pK_b=14$ in water under ambient conditions, the corresponding constant in glacial acetic acid would be $14.45$. As an example, citing the hydrogen chloride acid dissociation constant given above, we can compute the $pK_b$ of the conjugate base chloride ion as $14.45-8.55=5.90$ (significant zero).
- S. Bruckenstein and I. M. Kolthoff (1956). "Acid-Base Equilibria in Glacial Acetic Acid. III. Acidity Scale. Potentiometric Determination of Dissociation Constants of Acids, Bases and Salts". J. Am. Chem. Soc. 78, 13, 2974–2979. https://doi.org/10.1021/ja01594a014