What is the conjugate acid-base relationship of (H2PO4)- and (HPO4)-?
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First off, the formula you gave is not quite correct. You’re missing the charge. It should be
HPO4^2-
to find the conjugate acid, Add a H+ to get
H2PO4−
Note the charge is only -1 now. This ion can lose the proton to go back to it’s conjugate base form or it can also gain a second proton to become the conjugate acid. This is an amphiprotic ion. It goes both ways
H3PO4
This final ion is phosphoric acid.
The first species mentioned in the question is also amphiprotic and could have lost its one proton to become the phosphate ion.
PO4^3-
HPO4^2-
to find the conjugate acid, Add a H+ to get
H2PO4−
Note the charge is only -1 now. This ion can lose the proton to go back to it’s conjugate base form or it can also gain a second proton to become the conjugate acid. This is an amphiprotic ion. It goes both ways
H3PO4
This final ion is phosphoric acid.
The first species mentioned in the question is also amphiprotic and could have lost its one proton to become the phosphate ion.
PO4^3-
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