Write the net ionic equation including the phases?

Based off of this reaction - ${\text{HClO"_4(aq) + "NaOH" (aq) -> "H"_2"O"(l) + "NaClO}}_{4} \left(a q\right)$

Nov 28, 2017

${\text{H"_ 3"O"_ ((aq))^(+) + "OH"_ ((aq))^(-) -> 2"H"_ 2"O}}_{\left(l\right)}$

Explanation:

Perchloric acid is a strong acid and sodium hydroxide is a strong base, so right from the start, you should be able to say that the net ionic equation that describes this neutralization reaction is

${\text{H"_ 3"O"_ ((aq))^(+) + "OH"_ ((aq))^(-) -> 2"H"_ 2"O}}_{\left(l\right)}$

Perchloric acid will ionize completely in aqueous solution to produce hydronium cations and perchlorate anions.

${\text{HClO"_ (4(aq)) + color(blue)("H"_ 2"O"_ ((l)))-> "H"_ 3"O"_ ((aq))^(+) + "ClO}}_{4 \left(a q\right)}^{-}$

Sodium hydroxide will also ionize completely in aqueous solution to produce sodium cations and hydroxide anions

${\text{NaOH"_ ((aq)) -> "Na"_ ((aq))^(+) + "OH}}_{\left(a q\right)}^{-}$

When you mix these two solutions, you will end up with

"HClO"_ (4(aq)) + color(blue)("H"_ 2"O"_ ((l))) + "NaOH"_ ((aq)) -> "H"_ 2"O"_ ((l)) + "NaClO"_ (4(aq)) + color(blue)("H"_ 2"O"_ ((l)))

The complete ionic equation looks like this--keep in mind that sodium perchlorate is soluble in aqueous solution!

${\text{H"_ 3"O"_ ((aq))^(+) + "ClO"_ (4(aq))^(-) + "Na"_ ((aq))^(+) + "OH"_ ((aq))^(-) -> 2"H"_ 2"O"_ ((l)) + "Na"_ ((aq))^(+) + "ClO}}_{4 \left(a q\right)}^{-}$

Eliminate the spectator ions

"H"_ 3"O"_ ((aq))^(+) + color(red)(cancel(color(black)("ClO"_ (4(aq))^(-)))) + color(red)(cancel(color(black)("Na"_ ((aq))^(+)))) + "OH"_ ((aq))^(-) -> 2"H"_ 2"O"_ ((l)) + color(red)(cancel(color(black)("Na"_ ((aq))^(+)))) + color(red)(cancel(color(black)("ClO"_ (4(aq))^(-))))

to get the net ionic equation

${\text{H"_ 3"O"_ ((aq))^(+) + "OH"_ ((aq))^(-) -> 2"H"_ 2"O}}_{\left(l\right)}$