In: Chemistry
Pay attention to the ratio. An acid of pKa = 8.0 is present in a solution with a pH of 6.0. What is the ratio of protonated to the deprotonated form of the acid? Show your work
According to Henderson-Hasselbalch equation,
pH = pKa + log [A-]/[HA]
Given values are pH = 6, pKa = 8
By substituting the values we get,
6 = 8 + log [A-]/[HA]
log [A-]/[HA] = -2
[A-]/[HA] = antilog (-2)
= 0.01
But according to question we need protonated to deprotonated ratio [HA]/[A-]
[HA]/[A-] = 1/0.01
[HA]/[A-] = 100