I understand that when $\mathrm{pH}= \mathrm{p}K_\mathrm{a}$, the buffer solution will be at its maximum capacity, and there will be equal concentrations of the acid/conjugate acid and the base/conjugate base.
However, when $\mathrm{pH} > \mathrm{p}K_\mathrm{a}$, why is it that $\ce{[A^-] > [HA]}$? Shouldn't it be the other what around since the Henderson-Hasselbalch equation is:
$$\mathrm{pH}= \mathrm{p}K_\mathrm{a} + \log \frac{\ce{[A^-]}}{\ce{[HA]}}$$
So $\frac{\ce{[A^-]}}{\ce{[HA]}}$ should be less than $0$, so $\ce{[HA]}$ must be greater.
Why is it that when $\mathrm{pH} > \mathrm{p}K_\mathrm{a}$, the concentration of the conjugate base ($\ce{[A-]}$) is greater than the concentration of the acid ($\ce{[HA]}$)?