Question

Question #a49bd

Answer 1

Your first reaction is actually a redox reaction (equilibrium, to be more precise) in which the silver cation, `Ag^(+)`, oxidizes the iron (II) cations, `Fe^(2+)`, to iron (III) cations, `Fe^(3+)`.

In aqueous solution, the nitrate ions will act as spectator ions, so the net ionic equation will look like this

`Fe_((aq))^(3+) + Ag_((aq))^(+) rightleftharpoons Fe_((aq))^(3+) + Ag_((s))`

The second one is a little tricky because you have two species that do not ionize in aqueous solution, phosphoric acid, `H_3PO_4`, and hydrogen sulfide, `H_2S`.

The complete ionic equation looks like this

`2H_3PO_(4(aq)) + 6Na_((aq))^(+) + 3S_((aq))^(2-) -> 3H_2S_((g)) + 6Na_((aq))^(+) + 2PO_(4(aq))^(3-)`

If you eliminate the spectator ions, you'll get

`2H_3PO_(4(aq)) + 3S_((aq))^(2-) -> 3H_2S_((aq)) + 2PO_(4(aq))^(3-)`