Neutralisation ionic equation help please?

How come the H^+ is not balanced in the ionic equation of neutralisation, H^+ +OH^- = H_2

2 Answers
May 18, 2018

Because the equation does not represent reality....

Explanation:

We should have....

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

...equivalently....

H_3O^+ +HO^(-)rarr2H_2O(l)

The hydride ion, H^-, does not exist in aqueous solution....and addition of hydride salts (which do exist) to water would give dihydrogen gas...

H^(-) + H_2O(l) rarr 1/2H_2(g) + HO^-

May 19, 2018

The answer is that "H"^"+" does not have to be balanced.

Explanation:

I believe you meant to write the equation

"H"^"+" + "OH"^"-" → "H"_2"O"

When balancing equations, we do not balance "H"^"+".

We balance "H" atoms, and then we balance charge.

Your equation has two "H" atoms on the left and two on the right, so "H" atoms are balanced.

Your equation has "+1 - 1 = 0" charge on the left and zero charge on the right, so charge is balanced.