What is the conjugate acid and base of #HSO_4^-#?
Here's what I got.
The thing to remember about conjugate acids is that they are the chemical species that is formed when a Bronsted-Lowry base accepts one proton,
This means that in order to find the conjugate acid of a substance that can act as a Bronsted-Lowry base, all you have to do is add a proton to it.
But keep in mind that a proton carries a
In your case, the hydrogen sulfate anion,
#overbrace("HSO"_ (4(aq))^(-))^(color(blue)("base")) + "H"_ ((aq))^(+) -> overbrace("H"_ 2"SO" _(4(aq)))^(color(darkgreen)("conjugate acid"))#
Notice that because you're adding a
Similarly, conjugate bases are chemical species that are formed when a Bronsted-Lowry acid donates one proton.
This means that you can find the conjugate base of a Bronsted-Lowry acid by removing a proton from it.
In your case, the hydrogen sulfate anion can act as a Bronsted-Lowry acid and donate a proton to form the sulfate anion,
#overbrace("HSO"_ (4(aq))^(-))^(color(darkgreen)("acid")) -> "H"_ ((aq))^(+) + overbrace("SO"_ (4(aq))^(2-))^(color(blue)("conjugate base"))#
Once again, notice that the charge is balanced because removing a