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Mobile App Chapter 1: Q6E (page 9)
Question: Show by suitable net ionic equations that each of the following species can act as a Bronsted-Lowry base:
\({\rm{a) H}}{{\rm{S}}^ - }\)
\({\rm{b)\;PO}}_4^{3 - }\)
\({\rm{c) NH}}_2^ - \)
\({\rm{d)}}{{\rm{C}}_2}{{\rm{H}}_5}{\rm{OH}}\)
\({\rm{e)}}{{\rm{O}}^{2 - }}\)
\({\rm{f) }}{{\rm{H}}_2}{\rm{PO}}_4^ - \)
Short Answer
The net ionic equations are as follows
Step by step solution
Bronsted-Lowry's Concept
The Bronsted-Lowry's acid is proton \(\left( {{H^ + }} \right)\) donor and its base is proton acceptor.
Suitable net ionic equations
If a base is added to water, protons moved from water molecules to base molecules which is known as a base ionization reaction. As per the nature of solute dissolved in it, water can act as either an acid or a base.
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