Write equation to show the amphiprotic behavior of H2po4-
H2PO4- + H2O <=> H3O+ + HPO4-2
In this equation, H2PO4- acts as an amphiprotic species because it can both donate and accept a proton (H+). In the forward reaction, it donates a proton to water (H2O) to form hydronium (H3O+). In the reverse reaction, it can accept a proton from water to form hydrogen phosphate (HPO4-2).
The equation that shows the amphiprotic behavior of H2PO4- is:
H2PO4- + H2O ⇌ H3O+ + HPO4^2-
To understand the amphiprotic behavior of H2PO4-, we first need to know what amphiprotic means. Amphiprotic substances can act as both a proton donor (acid) and a proton acceptor (base) depending on the reaction they are involved in.
The H2PO4- ion is the conjugate base of phosphoric acid (H3PO4), which means it can accept a proton (H+) to turn back into the acid form. The equation for this proton-accepting behavior is as follows:
H2PO4- + H+ -> H3PO4
In this reaction, H2PO4- accepts a proton (H+) to form the acidic species H3PO4.
Now, let's look at the other proton-donating behavior of H2PO4-. In the presence of a strong base, it can donate a proton to form a different species. The equation for this reaction is:
H2PO4- + OH- -> HPO42- + H2O
In this reaction, H2PO4- donates a proton (H+) to the hydroxide ion (OH-) to form the species HPO42- and water (H2O).
Therefore, by understanding these two reactions, we can see how H2PO4- exhibits amphiprotic behavior.