Midterm 1 question

[006033476]

The pyridine ring occurs in many compounds, including pharmaceuticals and vitamins.
In 2016 approximately 20,000 tons of pyridine was produced worldwide.
If the value of Kb for pyridine (C5H5N) is 1.8 × 10-9, calculate the equilibrium constant for:
C5H5NH+(aq) + H2O(I) = CsH5N(aq) + H3O*(aq)


By any chance does anyone know the answer to this question for midterm 1?

[Madison Yang 1L]

The given reaction is the dissociation of a weak acid, C5N5NH (aq). So we're looking for Ka. We are given Kb, and can use the relation Kw = Ka*Kb to solve for Ka.

[Cristina Subratie 1C]

so here we are essentially finding the equilibrium constant for the conjugate base of the acid in the equation provided. you can solve for Ka and then use the formula provided in the previous reply in order to solve for Kb since we know Kw and Ka.