Question

Using the Br?nsted-Lowry concept of acids and bases, identify the Br?nsted-Lowry acid and base in each of the following reactions:
H2PO3?(aq)+H2O(l)?H3PO3(aq)+OH?(aq)

(CH3)2NH(g)+BF3(g)?(CH3)2NHBF3(s)

Drag the appropriate items to their respective bins.

H2PO3- H2O BF3 (CH3)2NH

Bronsted Lowry Acid Bronsted Lowry Base Neither

Answer 1

Answer:

$H_2PO_3^-$ is Bronsted Lowry base.

$H_2O$ is Bronsted Lowry acid.

Explanation:

According to the Bronsted Lowry conjugate acid-base theory:

• An acid is defined as a substance which donates protons and form conjugate base
• A base is defined as a substance which accepts protons and forms conjugate acid.

$H_2PO_3^-(aq)+H2O(l)\rightarrow H_3PO_3(aq)+OH^-(aq)$

$H_2PO_3^-$ is Bronsted Lowry base.It accepts protons and forms conjugate acid $H_3PO_3$

$H_2O$ is Bronsted Lowry acid.It donates protons and forms conjugate base $OH^-$

$(CH_3)_2NH(g)+BF_3(g)\rightarrow (CH_3)_2NHBF_3(s)$

There in no exchange of proton in an above reaction.Neither of the reactants and products are Bronsted Lowry acid or Bronsted Lowry base