Question

 

Label each reactant and product in this reaction as a Bronsted acid or base.

H₂Y^- + H₂Z^-  <==> H₃Y + HZ^2- acid base

Answer 1

According to Bronsted-Lowry acid base definition:

An acid is a proton donor, any species that donates an \(\mathrm{H}^{+}\) ion. An acid must contain \(\mathrm{H}\) in its formula. An acid donates a proton to water.

A base is a proton acceptor, any species that accepts an \(\mathrm{H}^{+}\) ion.

A base must contain a lone pair of electrons to bind the \(\mathrm{H}^{+}\) ion.

The base accepts a proton from water.

Provided reaction is \(\mathrm{H}_{2} \mathrm{Y}^{-}+\mathrm{H}_{2} \mathrm{Z}^{-} \longleftrightarrow \mathrm{H}_{3} \mathrm{Y}+\mathrm{HZ}^{2-}\)

\(\mathrm{H}_{2} \mathrm{Y}^{-}\) receives one proton, so this is by definition actsas Bronstedbase.

\(\mathrm{H}_{2} \mathrm{Z}^{-}\) donates oneproton,so this is by definition acts as Bronsted acid.