Show with proper examples that both `HPO_4^(2-)` ion and `H_2O` can act as Bronsted acid as well as Bronsted base.

Which can act as an acid as well as a base-

The species that can act both as Bronsted acid and as Bronsted base in water are-

Conjugate base of HPO_4^(-2) is :

Each of HCO_(3)^(-) and HPO_(4)^(2-) can act both as Bronsted acid and base-why? Write the formula of conjugate base and conjugate acid in each case.

Each of HS^(-) and NH_(3) can act as both Bronsted acid and Bronsted base-why? Write the formula of conjugate base and conjugate acid in each case.

The species: H_(2)O,HCO_(3)^(-),HSO_(4)^(-) and NH_(3) can act both as Bronsted acids and bases. For each case give the corresponding conjugate acid and base.

The species : H_2O, HCO_3-, HSO_4- , and NH_3 can act both as bronsted acids and bases. For each case give the corresponding conjugate acid and conjugate base

SF_(4) acts as both Lewis acid Lewis base. Explain.

(1) HPO_(4)^(2-) can act both as a Bronsted base and as a Bronsted acid. Write the equation of equilibrium established by HPO_(4)^(2-) as an acid and a base in aqueous solution. Also write the expressions of K_(a) & K_(b) in two cases. (2) What are the conjugate acid and base of HS^(-) ?

Give example of a reaction in which H_(2)O acts oxidising agent.