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

Sep 18, 2016

${H}^{+} + H {O}^{-} \rightarrow {H}_{2} O$.

$0.85 \cdot m o l$ $H {O}^{-}$ are required.

#### Explanation:

The balanced equation clearly specifies a 1:1 equivalence.

Alternatively, we could write:

$H {O}^{-} + {H}_{3} {O}^{+} \rightarrow 2 {H}_{2} O$

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 $\left[{H}_{3} {O}^{+}\right] \left[H {O}^{-}\right] = {10}^{- 14}$. And if there are $0.85 \cdot m o l$ $H {O}^{-}$, there must be a corresponding molar quantity of ${H}^{+}$.