Question

Question #e80d3

Answer 1

Acetic acid.

Explanation:

To find the conjugate acid of a Bronsted - Lowry base, you add a proton, `"H"^(+)`, to the chemical formula of the base.

Keep in mind that because you're adding a proton and not a hydrogen atom, `"H"`, you need to keep track of the charge of the conjugate acid as well.

In this case, your Bronsted - Lowry base is the acetate anion, `"CH"_3"COO"^(-)`. Notice that this anion carries a `1-` charge, so right from the start, you know that after you add the proton, the resulting compound will be electrically neutral.

`overbrace((1-))^(color(blue)("starting charge")) + overbrace((1+))^(color(blue)("charge of H"^(+))) = 0`

You can thus say that you have

`"CH"_ 3"COO"^(-) + "H"^(+) -> "CH"_ 3"COOH"`

The conjugate acid of the acetate anion is acetic acid, `"CH"_3"COOH"`.