How do you use the Henderson-Hasselbalch to calculate the pH of a buffer solution that is .50 M in #NH_3# and . 20 M in #NH_4Cl#?
Before I introduce Henderson-Hasselbalch's equation, we should identify the acid and base. Ammonia
Now, we can use this equation:
As you can see, we are given a pKb instead of a pKa. But, no worries we can use the following equation that relates both constants to each other:
We can solve for the pKa by subtracting the given pKb from 14:
Thus, your pKa is 9.25
Next, we can obtain the [base] and [acid] from the question.
We're not really concerned with the chloride anion that attached to the ammonium ion because it's a spectator ion and it has no effect on the buffer system.
Now, we have all of the information to determine the pH. Let's plug our values into the equation: