Ionic equation:
[tex]\text{H}_2\text{PO}_4^{-} + \text{HAsO}_4^{2-} \to \text{HPO}_4^{2-} + \text{H}_2\text{AsO}_4^{-}[/tex]
The acid and base in a conjugate pair differ by only one proton [tex]\text{H}^{+}[/tex]. The acid loses one proton to produce a conjugate base, whereas the base gains a proton to produce its conjugate acid.
[tex]\text{H}_2\text{PO}_4^{-}[/tex] loses one proton to produce [tex]\text{HPO}_4^{2-}[/tex] in this reaction.
[tex]\text{H}_2\text{PO}_4^{-} \to \text{H}^{+} + \text{HPO}_4^{2-}[/tex]
Meanwhile, [tex]\text{HAsO}_4^{2-}[/tex] gains one proton to form [tex]\text{H}_2\text{AsO}_4^{-}[/tex].
[tex]\text{HAsO}_4^{2-} + \text{H}^{+} \to \text{H}_2\text{AsO}_4^{-}[/tex]
Therefore
Ionic equation:
The acid and base in a conjugate pair differ by only one proton . The acid loses one proton to produce a conjugate base, whereas the base gains a proton to produce its conjugate acid.
loses one proton to produce in this reaction.
Meanwhile, gains one proton to form .
Therefore
