Complete and also balance the following molecular equation (in aqueous solution); encompass phase labels. Then, create the network ionic equation.

You are watching: Enter the molecular equation representing aqueous nitric acid and aqueous ammonia reacting.

$~\ceNH_3 + HNO_3 -> ?$

I assumed that the acid $\ceHNO3$ would certainly just offer its hydrogen come $\ceNH3$ 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 really close to the prize given, other than for the complying with two tidbits (the first being an ext significant).

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

The provided answer combine the two ions developed into a solitary compound. $$\ceNH4+(aq) + NO3-(aq) ->NH4NO3(aq)$$

The an outcome of #2 would certainly be reasonable if you had not been told that the reaction was arising in aqueous solution. In aqueous solution, the assets should have been those of #1, due to the fact that ammonium nitrate is easily soluble in water.

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Molecular equation:

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

Net ionic equation:

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

Note: $\ceNH4NO3$ is no solid in aqueous solution. It is quite soluble.


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