Buffer solutions are typically prepared by dissolving an appropriate salt in water and then adjusting the $\mathrm{pH}$ to the desired position by addition of the conjugate acid or base.
For example, to prepare a $\pu{100 mM}$ ammonium acetate solution at $\mathrm{pH}~9,$ you’d first prepare a $\pu{100 mM}$ ammonium acetate, and then add ammonium hydroxide dropwise until the desired $\mathrm{pH}$ was achieved (a titration, using a pH meter to determine endpoint).
I’d like to work out (roughly—I understand that what I’m about to describe is nothing more than an approximation, but it’s a reproducible approximation at least which is good enough for our needs) directly how much ammonium hydroxide and acetic acid I would need to make up the same solution.
I understand the fundamental Henderson–Hasselbalch equation:
$$\mathrm{pH} = \mathrm{p}K_\mathrm{a} + \log\frac{[\ce{A}]}{[\ce{HA}]}$$
But as I see $\ce{A}$ is ammonium and $\ce{HA}$ is ammonium acetate. Thus, in my example I don’t really simplify things that much.
Additionally the majority of examples I’ve found look at acidic buffers rather than alkali ones. Does my equation therefore need to be rearranged further to take account of this?