Question

In: Chemistry

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

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???

Solutions

Expert Solution

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-


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