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.

FREE Expert Solution

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: 

99% (424 ratings)
View Complete Written Solution
Problem Details
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.

Frequently Asked Questions

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 Complete Ionic Equations concept. You can view video lessons to learn Complete Ionic Equations. Or if you need more Complete Ionic Equations practice, you can also practice Complete Ionic Equations practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Davis' class at OLE MISS.