The balanced net ionic equation for the neutralization reaction involving equal molar amounts of hno3 and koh is

 The  net ionic  equation for  the neutralization  reaction involving  equal molar amount amount of  HNo3  and KoH  is 

H^+   +  OH^-  =  H2O (l)

    explanation
write  the   chemical equation
HNO3 (aq) + KOH(aq) =  KNO3(aq) +H2O  (l)

ionic   eequation

H^+(aq)  +  NO3^- (aq) +  K^+9aq)   OH^-(aq) = K^+ (aq) + NO3^-(aq)  + H2O(l)

cancel the  spectator  ions( ions which  does  not  take  place in  equation ) for this case    is  NO3^-  and  No3^-

thus the  net ionic  is

H^+(aq)  + OH^- (aq)  =  H2O(l)

H⁺(aq) + OH⁻(aq) --> H₂O(l)

Explanation:

1) Write the molecular chemical equation:


HNO₃(aq) + KOH(aq) ---> H₂O(l) + KNO₃(aq)


2) Identify the kind of reaction:


It is a acid base neutralization, which is a double replacement equation.


3) Set the ionization (dissociation) of the acid and the base compounds:


i) HNO₃(aq) ---> H⁺ (aq) + NO₃⁻ (aq)

ii) KOH (aq) --> K⁺ (aq) + OH⁻ (aq)


4) Identify whether the products are soluble ionic compounds and they dissociate in water or remain solids (phases).


i) KNO₃ is soluble, so it will dissociate: KNO₃(aq) --> K⁺(aq) + NO₃⁻(aq)


ii) H₂O slightly dissociates, so it will remain liquid: H2O (l)


5) Write the total ionic equation:


H⁺ (aq) + NO₃⁻(aq) + K⁺(aq) + OH⁻ (aq) --> K⁺ (aq) + NO₃⁻(aq) + H₂O(l)


6) Eliminate the spectator ions (those that are repeated in reactant and product sides, K⁺(aq) y NO₃⁻(aq):


H⁺(aq) + OH⁻(aq) --> H₂O(l)


That is the net ionic equation.