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

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\$~ceNH_3 + HNO_3 -> ?\$

I thought that the acid \$ceHNO3\$ would just give its hydrogen to \$ceNH3\$ and make the resulting reaction:

\$\$ceNH_3 + HNO_3 -> HNH_3 + NO_3\$\$

However the correct answer is \$ceNH_3 + HNO_3 -> NH_4NO_3\$. Why is this?  Your answer is very close to the answer given, except for the following two tidbits (the first being more significant).

An acid-base reaction is not the exchange of a hydrogen atom \$ceH\$. It is the exchange of a hydrogen ion (or proton) \$ceH+\$. Thus your answer should be: \$\$ceNH3(aq) +HNO3(aq) -> NH4+(aq) + NO3-(aq)\$\$

The given answer combines the two ions produced into a single compound. \$\$ceNH4+(aq) + NO3-(aq) ->NH4NO3(aq)\$\$

The result of #2 would be reasonable if you had not been told that the reaction was occurring in aqueous solution. In aqueous solution, the products should have been those of #1, since ammonium nitrate is freely soluble in water.

See more: At&Amp;T Mailbox Number Specified By System Manager, At&T Official Site  Molecular equation:

\$\$ceNH3(aq) + HNO3(aq) -> NH4NO3(aq)\$\$

Net ionic equation:

\$\$ceNH3(aq) + H^+(aq)-> NH4^+(aq)\$\$

Note: \$ceNH4NO3\$ is not solid in aqueous solution. It is quite soluble. Highly active question. Earn 10 reputation (not counting the association bonus) in order to answer this question. The reputation requirement helps protect this question from spam and non-answer activity.

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