HSO4 + HCO3 -> SO4 + H2CO3

How would I know which are Bronsted-Lowry acids?

B-L acids donate protons. Which one donated a proton. It appears to me that HSO4^- donates a proton (because it is SO4^-2 on the right) so HSO4^- must be an acid. HCO3^- accepts a proton (it is H2CO3 on the right) so it must be a base.

Hco4- + Hco3- = so42- + co3

To determine which species are Bronsted-Lowry acids in the given equation, you need to understand the definition of a Bronsted-Lowry acid. According to the Bronsted-Lowry theory, an acid is a substance that donates a proton (H+ ion) in a chemical reaction.

In the given equation: HSO4 + HCO3 -> SO4 + H2CO3

The species that donate protons in this equation are the Bronsted-Lowry acids. Let's analyze each species:

1. HSO4: This species can donate a proton (H+) because it has a hydrogen atom that can be easily transferred.

2. HCO3: This species also has a hydrogen atom that can donate a proton (H+).

On the other hand, SO4 and H2CO3 are not capable of donating protons in this reaction. Therefore, HSO4 and HCO3 are the two Bronsted-Lowry acids in this equation.

To determine which compounds are Bronsted-Lowry acids in the given reaction HSO4 + HCO3 -> SO4 + H2CO3, we need to understand the concept of acids and bases according to the Bronsted-Lowry definition.

According to the Bronsted-Lowry theory, an acid is a substance that donates a proton (H+ ion), while a base is a substance that accepts a proton. In the given reaction, we can identify the acids and bases by examining which compounds donate or accept protons.

In the reaction HSO4 + HCO3 -> SO4 + H2CO3, HSO4 and HCO3 are both compounds containing hydrogen atoms. When these compounds react, it is likely that proton transfer occurs.

HSO4 contains a hydrogen atom that can potentially be donated as a proton, so it can be considered as a Bronsted-Lowry acid. HCO3, on the other hand, can accept a proton and is therefore a Bronsted-Lowry base in this reaction.

After the reaction takes place, SO4 and H2CO3 are formed. SO4 does not contain any hydrogen atoms, so it does not act as an acid or a base in this reaction. H2CO3, however, contains two hydrogen atoms that were accepted as protons, suggesting that it acts as a Bronsted-Lowry base in this reaction.

Therefore, in the given reaction, HSO4 and H2CO3 are the Bronsted-Lowry acids, while HCO3 is the Bronsted-Lowry base.