Complete the Bronsted- Lowry reaction, placing each product by its appropriate label.

HCO3^-+HNO2 (double arrows) need a spot for acid and for base.

To complete the Bronsted-Lowry reaction of HCO3^- + HNO2, we need to identify the acid and base species involved.

Let's start by understanding the Bronsted-Lowry definition of acids and bases. According to Bronsted-Lowry, an acid is a species that donates a proton (H+), while a base is a species that accepts a proton (H+).

In the given reaction, HCO3^- is a base because it can accept a proton (H+), and HNO2 is an acid because it can donate a proton (H+).

Now, to complete the reaction, we need to write down the products by their appropriate labels (acid or base).

HCO3^- + HNO2 (double arrows)

The base (HCO3^-) will react with the acid (HNO2). When a base reacts with an acid, it forms a conjugate acid-base pair.

So, in this reaction, HCO3^- (base) will accept a proton from HNO2 (acid) to form its conjugate acid, which is formed by adding an additional H+ to the base.

HCO3^- (base) + HNO2 (acid) <--> __________ (acid) + __________ (base)

After the reaction, we have:

HCO3^- (base) + HNO2 (acid) <--> H2CO3 (acid) + NO2^- (base)

Therefore, the reaction is completed, and the products are labeled as follows:

HCO3^- (base) + HNO2 (acid) <--> H2CO3 (acid) + NO2^- (base)

To summarize, in the Bronsted-Lowry reaction of HCO3^- + HNO2, HCO3^- acts as a base and HNO2 acts as an acid. The reaction yields H2CO3 as the conjugate acid of HCO3^- and NO2^- as the conjugate base of HNO2.