Problem: Consider the following acid-neutralization reactions involving the strong base NaOH(aq):HNO3(aq) + NaOH(aq) → NaNO3(aq) + H2O(l)HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)NH4+(aq) + NaOH(aq) → NH3(aq) + Na+(aq) + H2O(l)As we saw in Section 4.3, nitric acid and hydrochloric acid are strong acids. Write net ionic equations for the neutralization of the nitric acid.

We are asked to write the net ionic equation for the neutralization of nitric acid.

HNO₃(aq) + NaOH(aq) → NaNO₃(aq) + H₂O(l)

Dissociate the aqueous species to ions:

H⁺(aq) + NO₃^-(aq) + Na⁺(aq) + OH^-(aq) →Na⁺(aq) + NO₃^-(aq) + H₂O(l)

Cancel spectators ions:

Consider the following acid-neutralization reactions involving the strong base NaOH(aq):

HNO₃(aq) + NaOH(aq) → NaNO₃(aq) + H₂O(l)
HCl(aq) + NaOH(aq) → NaCl(aq) + H₂O(l)
NH₄⁺(aq) + NaOH(aq) → NH₃(aq) + Na⁺(aq) + H₂O(l)

As we saw in Section 4.3, nitric acid and hydrochloric acid are strong acids. Write net ionic equations for the neutralization of the nitric acid.

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Net Ionic Equations concept. You can view video lessons to learn Net Ionic Equations. Or if you need more Net Ionic Equations practice, you can also practice Net Ionic Equations practice problems.