Take the 2-minute tour ×
Chemistry Stack Exchange is a question and answer site for scientists, academics, teachers and students. It's 100% free, no registration required.

Question) Complete and balance each of the following molecular equations (in aqueous solution); include phase labels. Then, for each, write the net ionic equation.

(A) $\ce{NH_3 + HNO_3 ->}$

My Attempt: I thought that the acid $\ce{HNO3}$ would just give its hydrogen to $\ce{NH3}$ and make the resulting reaction $\ce{NH_3 + HNO_3 -> HNH_3 + NO_3}$. However the correct answer is $\ce{NH_3 + HNO_3 -> NH_4NO_3}.$

share|improve this question

1 Answer 1

Your answer is very close to the answer given, except for the following two tidbits (the first being more significant).

  1. An acid-base reaction is not the exchange of a hydrogen atom $\ce{H}$. It is the exchange of a hydrogen ion (or proton) $\ce{H+}$. Thus your answer should be: $$\ce{NH3 +HNO3 -> NH4+ + NO3-}$$
  2. The given answer combines the two ions produced into a single compound, which is reasonable given that you are not told if the reaction occurs in aqueous solution. $$\ce{NH4+ + NO3- ->NH4NO3}$$
share|improve this answer
    
+1, but I think you may have a minor oversight: the OP's question is prefaced with a specification that the reaction is taking place in aqueous solution. –  Greg E. Jul 20 at 20:19
2  
Well, then, we should show the ionic products as dissociated as in the first part of my answer. –  Ben Norris Jul 20 at 23:35

Your Answer

 
discard

By posting your answer, you agree to the privacy policy and terms of service.

Not the answer you're looking for? Browse other questions tagged or ask your own question.