Question

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

Answer 1

Answer: H⁺(aq) + OH⁻(aq) --> H₂O(l)


Step-by-step 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.

Answer 2

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)