Identify the conjugate base in the following reaction.

H2O (l) + HCO31- (aq) �¨ H3O+ (aq) + CO32- (aq)?

Identify the Bronsted-Lowry acid in the following reaction.

H2O (l) + HCO31- (aq) �¨ H3O+ (aq) + CO32- (aq)

Well, well, well! Looks like we've got some chemistry going on here! Let me juggle with these terms for you.

The conjugate base in the reaction is CO32- (aq), because it is formed when the acid, HCO31- (aq), donates a proton to water.

Now, let's find the Bronsted-Lowry acid. Drum roll, please! The Bronsted-Lowry acid is HCO31- (aq), because it donates a proton to water, forming H3O+ (aq).

Remember, chemistry can be tricky, but with a little humor, we can brighten up even the most acidic situations!

The conjugate base in the given reaction is CO32- (aq).

The Bronsted-Lowry acid in the reaction is H2O (l).

To identify the conjugate base in a reaction, you need to first identify the acid. In this case, the acid is represented by the species that donates a proton (H+) in the reaction. The species that accepts the proton is known as the conjugate base.

Looking at the reaction:
H2O (l) + HCO3^1- (aq) → H3O+ (aq) + CO3^2- (aq)

In this reaction, H2O (water) donates a proton to HCO3^- (bicarbonate ion). So, water (H2O) is the acid, and HCO3^- is the species that accepts the proton. Therefore, the conjugate base in this reaction is CO3^2- (carbonate ion).

Now, let's move on to identifying the Bronsted-Lowry acid in the same reaction. The Bronsted-Lowry definition of an acid is a species that donates a proton. In this reaction, H2O donates a proton to HCO3^- (bicarbonate ion). Therefore, the Bronsted-Lowry acid in this reaction is H2O (water).

Just remember the definition.

An acid is a proton donor; a base is a proton acceptor. What does all of that mean? Look for the one on the left with more H than the one on the right with fewer H. More H means acid; fewer H means conjugate base. Crazy talk. The acid is HCO3^- and the conjugate base is CO3^2-. It should be obvious to you that the pair is HCO3^-/CO3^2-. So the one with more H is HCO3^- and that is the acid of the pair; CO3^2- is the one with fewer H so it is the conjugate base.

The other pair obviously is H2O/H3O^+. Same thing. H2O must be the base (fewer H) and H3O^+ must be the conjugate acid (more H).