Question #a49bd

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Question #a49bd

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Answer 1 · 2015-05-21T01:26:57

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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