Enter the net ionic equation, including phases, for the reaction of AgNO3(aq) with BaO(aq).
Is it...
Ag+O2--->AgO?
yes
no. It isn't balanced, the formula for the oxide is not right, no phases are shown and there are no charges on the ions. If you wrote the molecular equation and balanced it and converted that to an ionic equation you would come closer to doing it right.
2AgNO3 + BaO ==> Ag2O + Ba(NO3)2
2Ag^+(aq) + O^2-(aq) ==> Ag2O(s)
Oh dern, okay thanks!
To determine the net ionic equation for the reaction of AgNO3(aq) with BaO(aq), we need to first write the balanced molecular equation and then identify the spectator ions.
1. Write the balanced molecular equation:
AgNO3(aq) + BaO(aq) → Ag2O(s) + Ba(NO3)2(aq)
2. Separate the soluble compounds into ions. Note the states of matter:
AgNO3(aq) --> Ag+(aq) + NO3-(aq)
BaO(aq) --> Ba2+(aq) + O2-(aq)
3. Write the complete ionic equation by representing all the ions:
Ag+(aq) + NO3-(aq) + Ba2+(aq) + O2-(aq) → Ag2O(s) + Ba2+(aq) + 2NO3-(aq)
4. Identify the spectator ions—ions that are present on both sides of the equation and do not participate in the reaction. In this case, the spectator ions are Ba2+(aq) and NO3-(aq).
5. Write the net ionic equation by removing the spectator ions:
Ag+(aq) + O2-(aq) → Ag2O(s)
So, the correct net ionic equation for the reaction of AgNO3(aq) with BaO(aq) is:
Ag+(aq) + O2-(aq) → Ag2O(s)