Question #a49bd

1 Answer
Stefan V.
May 21, 2015

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-)#

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