# Problem: Identify whether each species functions as a Bronsted-Lowry acid or a Bronsted-Lowry base in this net ionic equation.           HNO2 (aq)             +           H2PO4-         ⇌                    NO2-                     +                  H3PO4 (aq)Bronsted-Lowry _               Bronsted-Lowry _                Bronsted-Lowry _                Bronsted-Lowry _In this reaction:The formula for the conjugate _ of HNO2 is _The formula for the conjugate _ of H2PO4-  is _

###### FREE Expert Solution

Let’s define a Bronsted-Lowry Acid and a Bronsted-Lowry Base. Recall also that Bronsted-Lowry acids and bases occurs in pairs called conjugate acid/base pairs.

Bronsted-Lowry acid → proton (H+) donor

Conjugate base → one less hydrogen form of the Bronsted-Lowry acid

Bronsted-Lowry base → proton (H+) acceptor

Conjugate acid → one hydrogen greater than Bronsted-Lowry base

Given Reaction:          HNO2 (aq)  + H2PO4- ⇌  NO2-  +  H3PO4 (aq)

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###### Problem Details

Identify whether each species functions as a Bronsted-Lowry acid or a Bronsted-Lowry base in this net ionic equation.

HNO2 (aq)             +           H2PO4-         ⇌                    NO2-                     +                  H3PO4 (aq)

Bronsted-Lowry _               Bronsted-Lowry _                Bronsted-Lowry _                Bronsted-Lowry _

In this reaction:
The formula for the conjugate _ of HNO2 is _
The formula for the conjugate _ of H2PO4-  is _