Answer to Question #153706 in General Chemistry for KELSEA

Question

In a laboratory test of the metal activity series, a student places a strip of lead metal into aqueous silver nitrate.  Write the net ionic equation for this reaction.

Answer 1

The balanced molecular equation would be;

$Pb_{(s)} + 2AgNO_{3(aq)} \to Pb(NO_3)_{2(aq)} + 2Ag_{(s)}$

And the balanced complete ionic equation would be;

$Pb_{(s)} + 2Ag^+_{(aq)} + 2NO_{3(aq)}^- \longrightarrow Pb^{2+}_{(aq)} + 2NO_{3(aq)}^- + 2Ag_{(s)}$

Removing the spectator ions (which is NO₃^- in this case), the net ionic reaction becomes;

$Pb + 2Ag^+ + \longrightarrow Pb^{2+} +2Ag$

And the balanced net ionic equation is therefore;

$Pb_{(s)} + 2Ag^+_{(aq)} \longrightarrow Pb^{2+}_{(aq)} + 2Ag_{(s)}$