If solution contains 0.85 mol of OH, how many moles of H+ would be required to reach the equivalence point in a titration?

1 Answer
Sep 18, 2016

H^+ + HO^(-) rarr H_2O.

0.85*mol HO^- are required.

Explanation:

The balanced equation clearly specifies a 1:1 equivalence.

Alternatively, we could write:

HO^(-) + H_3O^(+) rarr 2H_2O

And the fashion seems to favour this representation.

The given equations are equivalent they represent the acid/base equilibrium that occurs in water, which at 298 K, can be written as [H_3O^+][HO^-]=10^(-14). And if there are 0.85*mol HO^-, there must be a corresponding molar quantity of H^+.