Question

Neutralisation ionic equation help please?

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

Answer 1

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^-`

Answer 2

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.