# Can all neutralization reactions between a strong acid and a strong base be described by the net ionic equation of H+ (aq) + OH- (aq) --> H2O (l)? Please explain. If the above net ionic equation is incorrect, then what could be the correct net ionic equation? Can this example work? EX: 2H+ (aq) + 2A- (aq) + B+ (aq) + OH- (aq) --> H3O+ (aq) + BA (aq)

The above net ionic equation is correct.

H+(aq) + OH- (aq) --> H2O (l)

We only have to elaborate this for confirmation. Let me give you a similar example for this.

The reaction of Sodium Hydroxide (NaOH) and Hydrochloric acid (HCl) forming NaCl and water can be written as...

## See This Answer Now

Start your 48-hour free trial to unlock this answer and thousands more. Enjoy eNotes ad-free and cancel anytime.

The above net ionic equation is correct.

H+(aq) + OH- (aq) --> H2O (l)

We only have to elaborate this for confirmation. Let me give you a similar example for this.

The reaction of Sodium Hydroxide (NaOH) and Hydrochloric acid (HCl) forming NaCl and water can be written as follows:

NaOH + HCl ---> NaCl + H2O

**we put the proper notation to each of them.

NaOH (aq) + HCl (aq) ---> NaCl(aq) + H2O (l)

**next, we rewrite aqueous solution (aq) showing their ionic components.

Na+(aq)+OH-(aq)+H+(aq)+Cl-(aq) -> Na+(aq)+Cl-(aq)+H2O(l)

**then by removing the spectator ions, we will have the final net ionic equation.

H+(aq) + OH- (aq) --> H2O (l)