Question

In the following reaction acts as Bronsted-Lowry acid and acts as Bronsted-Lowrybase:
${\mathrm{NH}}_3\left(\mathrm{aq}\right)+H_{2}O\left(l\right)\to {{\mathrm{NH}}_4}^{+}\left(\mathrm{aq}\right)+{\mathrm{OH}}^{-}\left(\mathrm{aq}\right)$

• A. ${\mathrm{NH}}_3$
• B. $H_{2}O$
• C. ${{\mathrm{NH}}_4}^{+}$
• D. ${\mathrm{OH}}^{-}$

Answer 1

Answer: (A), (B)

The correct options are
A ${\mathrm{NH}}_3$
B $H_{2}O$

According to Bronsted-Lowry an acid is a substance that donates ${\text{H}}^{+}$ ion, while a base is a substance that accepts a ${\text{H}}^{+}$ ion in a solution.

In the given reaction, ${\text{NH}}_3$ is acting as a Bronsted-Lowry base as it accepts ${\text{H}}^{+}$ ion to form ${\text{NH}}_4^{+}$ while ${\text{H}}_2\text{O}$ acts as a Bronsted-Lowry acid as it donates ${\text{H}}^{+}$ ion to form ${\text{OH}}^{-}$.