Question #e80d3

1 Answer
Stefan V.
Oct 22, 2017

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"#.

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