# Why doesn't barium nitrate react with sulfuric acid?

Mar 6, 2016

It does react with sulfuric acid!

#### Explanation:

Barium nitrate, "Ba"("NO"_3)_2, will react with sulfuric acid, ${\text{H"_2"SO}}_{4}$, to produce barium sulfate, ${\text{BaSO}}_{4}$, and aqueous nitric acid, ${\text{HNO}}_{3}$.

Barium sulfate is insoluble in water and will precipitate out of solution.

The balanced chemical equation for this double replacement reaction looks like this

${\text{Ba"("NO"_3)_text(2(aq]) + "H"_2"SO"_text(4(aq]) -> "BaSO"_text(4(s]) darr + 2"HNO}}_{\textrm{3 \left(a q\right]}}$

The complete ionic equation for this reaction looks like this

${\text{Ba"_text((aq])^(2+) + 2"NO"_text(3(aq])^(-) + 2"H"_text((aq])^(+) + "SO"_text(4(aq])^(2-) -> "BaSO"_text(4(s]) darr + 2"H"_text((aq])^(+) + 2"NO}}_{\textrm{3 \left(a q\right]}}^{-}$

To get the net ionic equation, eliminate spectator ions, i.e. the ions that are present on both sides of the equation

"Ba"_text((aq])^(2+) + color(red)(cancel(color(black)(2"NO"_text(3(aq])^(-)))) + color(red)(cancel(color(black)(2"H"_text((aq])^(+)))) + "SO"_text(4(aq])^(2-) -> "BaSO"_text(4(s]) darr + color(red)(cancel(color(black)(2"H"_text((aq])^(+)))) + color(red)(cancel(color(black)(2"NO"_text(3(aq])^(-))))

This will give you

${\text{Ba"_text((aq])^(2+) + "SO"_text(4(aq])^(2-) -> "BaSO}}_{\textrm{4 \left(s\right]}} \downarrow$

Barium sulftate is a white insoluble solid that precipitates out of solution. 