Arrhenius, Bronsted-Lowry, and Lewis Acids and Bases Assignment

Consider this reaction: NH4+ + HPO42− → NH3 + H2PO4− Which is the Bronsted-Lowry acid ? NH4+ HPO42- HPO42- H2PO4-

A

According to the Arrhenius definitions of acids and bases, choose the bases from the list of acids and bases. Check all that apply. Ba(OH)2 HIO3 H2CO3 CsOH

A and D

Consider this reaction: HCO3− + H2S → H2CO3 + HS− Which is the Bronsted-Lowry base? H2S HCO3- HS- H2CO3

B

Consider this reaction: NH4+ + HPO42− → NH3 + H2PO4− Which is the conjugate base? NH4+ NH3 HPO42- H2PO4-

B

Identify the Lewis acid in this balanced equation: N(CH3)3 BH3 (CH3)3N:BH3

B

Identify the Lewis base in this balanced equation: Fe3+ H2O Fe(H2O)63+

B

Consider this reaction: HCO3− + H2S → H2CO3 + HS− Which is the conjugate acid? H2S HCO3- HS- H2CO3

D

Explain how water behaves in this reaction. Which definition of acids and bases would you apply?

Water behaves as a base in this reaction. The Bronsted-Lowry definition is applied, because the reaction involves the transfer of H+ from one reactant to the other. A Bronsted-Lowry base is defined as a substance that accepts a proton. Because water gains a proton to form H3O+ in this particular reaction, it acts as a base.