Question

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

Answer 1

`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^+`.