Consider the equilibrium Which are the Bronsted-Lowry bases? A)PO₄³^- and HPO₄²^- B)PO₄³^- and OH^- C)PO₄³^- and H₂O D)H₂O and OH^- E)H₂O and HPO₄²^-

Question

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Bronsted-Lowry bases are the species that can accept a proton (H+). In the given equilibrium, only OHS1U1P1-S1S1P0 and POS1U1B14S1U1B0S1U1P13S1S1P0S1U1P1-S1S1P0 have lone pairs of electrons to accept a proton, and hence they are the Bronsted-Lowry bases. Option A and C also have S1U1P1 which can donate a proton and hence cannot be bases. Option D has only OH- which is a strong base and dissociates completely in water, so it cannot exist in equilibrium with other species. Option E has HPOS1U1B14S1U1B0S1U1P12S1S1P0S1U1P1-S1S1P0 which can donate a proton and hence cannot be a base.

Consider the Equilibrium Which Are the Bronsted-Lowry