\underset{\text{formula equation}}{2 AgNO_3(aq) + BaCl_2(aq)} →2 AgCl(s) + Ba(NO_3)_2(aq)
Question 15.8: 2 AgNO3(aq) + BaCl2(aq)→2 AgCl(s) + Ba(NO3)2(aq) formula eq...
\underset{\text{total ionic equation}}{(2 Ag^+ + 2 NO^-_3) + (Ba^{2+} + 2 Cl^-)}→2 AgCl(s) + Ba^{2+} + 2 NO^-_3
\underset{\text{net ionic equation}}{Ag^+ + Cl^-→AgCl(s)}
Although AgCl is an ionic compound, it is written in the un-ionized form on the right side of the ionic equations because most of the Ag^+ and Cl^- ions are no longer in solution but have formed a precipitate of AgCl The Ba^{2+} and NO^-_3 ions are spectator ions.
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