For the reaction:

H2PO4- + HAsO42- ---> HPO42- + H2AsO4-

Which pair exists as base in the equilibrium?

H2PO4- & H2AsO4- are proton donors,therefore they are conjugate acids. HPO42- & HAsO42- are proton acceptors,therefore they are the base pairs asked in the question.Is it correct Dr.Bob? Need ur confirmation,help pleaaaaaaaaseeee
Thank you

Yes, you are correct! In the given reaction, H2PO4- and H2AsO4- are proton donors, which means they act as acids. They donate protons to form HPO42- and HAsO42-, which are proton acceptors and therefore act as bases.

To confirm this, you can look at the reaction equation and identify which species gain or accept protons (bases) and which species lose or donate protons (acids). In this case, H2PO4- and H2AsO4- donate protons, while HPO42- and HAsO42- accept protons.

So, the pair HPO42- and HAsO42- exists as the base in the equilibrium.

Yes, you are correct. In the given reaction:

H2PO4- + HAsO42- ---> HPO42- + H2AsO4-

H2PO4- and H2AsO4- are the proton donors, which means they act as conjugate acids.
HPO42- and HAsO42- are the proton acceptors, which means they act as conjugate bases.

So, the pair that exists as a base in the equilibrium is HPO42- and HAsO42-.