Question

Carbonate ion, perchloric acid, phosphate ion, h2c2O4, if they are acid what is the conjugate base if they are base what is the conjugate acid???

Answer 1

First, let us define Bronsted Lowry acid/base:

Bronsted Lowry acid: any species that will donate H+ (protons) in solution, and makes pH lower (i.e HCl)

Bronsted Lowry base: any species that will accept H+ (protons) in solution, and makes pH higher (NH3 will accept H+ to form NH4+)

Typically, acid/bases are shown in the left (reactants)

when we write the products:

Bronsted Lowery conjugate base = the base formed when the B.L. acid donates its H+ proton ( i.e. HCl -> Cl-

Bronsted Lowery conjugate acid = the acid formed when the B.L. base accept its H+ proton ( i.e. NH4+ has accept H+ proton)

Note that, typically conjugate bases/acids are shown in the right (product) side

So, from your reaction:

Carbonate ion = CO3-2 --> weak base, its conjugate acid is HCO3-

perchloric acid HClO4 --> strong acid, then conjguate base --> ClO4-

phosphate ion = PO4-3 --> weak base, its conjugate acid is HPO4-2

H2C2O4 = weak acid, its conjugate base is HC2O4-