Question

Identify Bronsted - Lowry acids in the given reaction.

${\left[Al{\left(H_{2}O\right)}_6\right]}^{3+}+HC{O}_3^{-}\rightleftharpoons {\left[Al{\left(H_{2}O\right)}_5\left(O{H}^{-}\right)\right]}^{2+}+H_{2}C{O}_3$
A B C D

• A. A and C
• B. B and D
• C. A and D
• D. B and C

Answer 1

The correct option is C A and D

$H^{+}$ donor is an acid.

$\therefore \left[Al\right(H_{2}O{)}_6{]}^{3+}-H^{+}\to \left[Al\right(H_{2}O{)}_{5}O{H}^{-}{]}^{2+}$
Acid Base

$HC{O}_3^{-}+H^{+}\to H_{2}C{O}_3$
Base Acid

Proton donors are Bronsted - Lowry acids. $[Al{\left(H_{2}O\right)}_6{]}^{3+}$ is an acid because it donates a proton.

$H_{2}C{O}_3$ is the conjugate acid of $HC{O}_3^{-}$.