Question: Show by suitable net ionic equations that each of the following species can act as a Bronsted-Lowry base: (a) \({H_2}O\) (b) \(O{H^ - }\)(c) \(N{H_3}\)(d) \(C{N^ - }\)(e) \({S^{2 - }}\)(f) \({H_2}PO_4^ - \)

Bronsted-Lowry base is a species that can accept a proton from another molecule. In short, Bronsted-Lowry base is a proton acceptor.

\(\begin{array}{l}Conjugate\,\,Base + \Pr oton \to \,Acid\\\,\,\,\,\,\,\,\,\,\,{H_2}O\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\, + \,\,\,\,\,\,\,\,\,{H^ + }\,\,\,\, \to {H_3}{O^ + }\end{array}\)

\(\begin{array}{l}Conjugate\,\,Base + \Pr oton \to \,Acid\\\,\,\,\,\,\,\,\,\,\,\,\,\,\,O{H^ - }\,\,\,\,\,\,\,\,\,\,\,\,\,\, + \,\,\,\,\,\,\,{H^ + }\,\,\,\,\,\, \to {H_2}O\end{array}\)

\(\begin{array}{l}Conjugate\,\,Base + \Pr oton \to \,Acid\\\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,N{H_3}\,\,\,\,\,\,\, + \,\,\,\,\,\,\,\,\,\,{H^ + }\,\,\,\, \to N{H_4}\end{array}\)

\(\begin{array}{l}Conjugate\,\,Base + \Pr oton \to \,Acid\\\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,C{N^ - }\,\,\,\,\,\,\,\,\,\, + \,\,\,\,\,\,\,\,{H^ + }\,\,\,\,\, \to HCN\end{array}\)