How do you calculate the percentage of C5H5N that forms C5H5NH^+ in .10M solution of C5H5N. Kb= 1.7 × 10^-8
Multiply the concentration by the Kb then square root the product.
So you’re calculating percent dissociation of the conjugate acid after adding 0.1 M of the base to water. I use an ICE table to solve this problem then calculate the percent dissociation: amount dissociated/[initial] and multiply by 100%. I’m letting A- be the pyridine and HA be the conjugate acid of pyridine:
A- + H2O—> HA+ OH-
I 0.1M ------- 0 0
C -x +x +x
E 0.1-x x x
solve for x:
then find percent dissociation: (amount dissociated/initial concentration)*100%=
(4.12e-5/0.1)*100%=0.0412% conjugate acid dissociated after adding 0.1M base to water.