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

Answer:

#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^+#.