Question #7f381
2 Answers
Explanation:
Nitric acid and sodium hydroxide will neutralize each other in a
The balanced chemical equation that describes this neutralization reaction looks like this
#"HNO"_ (3(aq)) + "NaOH"_ ((aq)) -> "H"_ 2"O"_ ((l)) + "NaNO"_ (3(aq))#
The interesting thing to notice here is that you can write a net ionic equation for this reaction by taking into account the fact that nitric acid is a strong acid and sodium hydroxide is a strong base.
You will have
#"HNO"_ (3(aq)) -> "H"_ ((aq))^(+) + "NO"_ (3(aq))^(-)#
#"NaOH"_ ((aq)) -> "Na"_ ((aq))^(+) + "OH"_ ((aq))^(-)#
Sodium nitrate is soluble in water, which implies that it exists as ions in aqueous solution.
This means that you can write a complete ionic equation for this reaction
#"H"_ ((aq))^(+) + "NO"_ (3(aq))^(-) + "Na"_ ((aq))^(+) + "OH"_ ((aq))^(-) -> "H"_ 2"O" _ ((l)) + "Na"_ ((aq))^(+) + "NO"_ (3(aq))^(-)#
Notice that some ions are present on both sides of the chemical equation--these ions are called spectator ions.
To get the net ionic equation, remove the spectator ions
#"H"_ ((aq))^(+) + color(red)(cancel(color(black)("NO"_ (3(aq))^(-)))) + color(red)(cancel(color(black)("Na"_ ((aq))^(+)))) + "OH"_ ((aq))^(-) -> "H"_ 2"O" _ ((l)) + color(red)(cancel(color(black)("Na"_ ((aq))^(+)))) + color(red)(cancel(color(black)("NO"_ (3(aq))^(-))))#
You will end up with
#"H"_ ((aq))^(+) + "OH"_ ((aq))^(-) -> "H"_ 2"O"_ ((l))#
Explanation:
In a neutralization reaction like this one, a (Brønsted-Lowry) acid and a (Brønsted-Lowry) base are mixed to yield a salt and water (most often in the liquid phase, so we put an
The reaction we have so far is
The acid and base are most generally present as ions dissolved in solution, so we write an
To find out if the salt is soluble, we refer to a solubility guidelines:
Compounds containing
This is the molecular equation for this reaction. Would you know how to make the ionic equations for this reaction?