Editing Weak base (section)

==Percentage protonated==
As seen above, the strength of a base depends primarily on pH. To help describe the strengths of weak bases, it is helpful to know the percentage protonated-the percentage of base molecules that have been protonated. A lower percentage will correspond with a lower pH because both numbers result from the amount of protonation. A weak base is less protonated, leading to a lower pH and a lower percentage protonated.<ref name="Maskill1985">{{cite book|author=Howard Maskill|title=The physical basis of organic chemistry|url=https://books.google.com/books?id=4AXwAAAAMAAJ|year=1985|publisher=Oxford University Press, Incorporated|isbn=978-0-19-855192-8}}</ref>

The typical proton transfer equilibrium appears as such:

:<math>B(aq) + H_2O(l) \leftrightarrow HB^+(aq) + OH^-(aq)</math>

B represents the base.

:<math>Percentage\ protonated = {molarity\ of\ HB^+ \over\ initial\ molarity\ of\ B} \times 100\% = {[{HB}^+]\over [B]_{initial}} {\times 100\%}</math>

In this formula, [B]<sub>initial</sub> is the initial molar concentration of the base, assuming that no protonation has occurred.