For the following reactions, name the Bronsted-Lowry acids and bases. Then name the conjugate acid and bases.

H3O+(aq) + CN-(aq) <==> HCN(aq) + H2O

I'm really confused on this whole concept even thought it's not really difficult. I said:
acids: H3O+
bases: CN-
conjugate acid: HCN
conjugate base: H2O
However, it seems to me that since this is an equilibrium reaction, there would have to be a conjugate acid/base, etc, on both sides on the equation. Could someone explain this a little better?

I don't know much about chemistry, but I think that your acid and conjugate base are correct. check out Keith's question a little further down on this page, maybe he can help you out

You may be trying to make it too hard OR you may not have the definitions down. Your answers are right.
Just remember the definitions: An acid is a proton donor; a base is a proton acceptor. An acid (the H3O^+) is donating a proton to the CN^- so the base it produces on the other side of the equation(H2O) is its conjugate base. That is, the H3O^+/H2O is the acid/conjugate base pair. Similarly, CN^- is the base because it accepts a proton to become HCN. That makes CN^-/HCN a base/conjugate acid pair. And you are correct, also, that this should exist on both sides of the equation but that is so whether the reaction is at equilibrium or not. We could look at the right side going to the left (the reaction in reverse), in which case, H2O is the base on the right side going to H3O^+, its conjugate acid on the left side. Similarly, HCN is the acid on the right side going on the left to CN^- which is its conjugate base. I think you just need a little practice and confidence and you will do fine. I hope this helps.

You are on the right track with identifying the acids and bases in the reaction. Let's break it down step by step:

H3O+(aq) + CN-(aq) <==> HCN(aq) + H2O

The reactants are H3O+ and CN-. H3O+ is the acid in this reaction because it donates a proton (H+) to the CN- ion. Therefore, H3O+ is the Bronsted-Lowry acid.

CN-, on the other hand, accepts the proton from H3O+ and acts as a proton acceptor. Therefore, CN- is the base in this reaction.

Now, let's look at the products. H2O is formed when H3O+ donates its proton to CN-. Since H2O has accepted the proton, it is acting as a base. Therefore, H2O is the conjugate base of the H3O+ acid.

HCN is formed when CN- accepts the proton from H3O+. Since HCN has gained a proton, it is acting as an acid. Therefore, HCN is the conjugate acid of the CN- base.

To summarize:

Acids:
- H3O+

Bases:
- CN-

Conjugate Acids:
- HCN

Conjugate Bases:
- H2O

It is important to note that in an equilibrium reaction like this one, the acid-base pairs will exist on both sides of the equation. In this case, the acid/base pair is H3O+/H2O on one side and CN-/HCN on the other side of the equation. The reaction can go in either direction, and the acid/base pairs will still be present. This is consistent with the concept of equilibrium, where both forward and reverse reactions occur simultaneously.