What is the net ionic equation for the reaction of AgNO3 with Ba(OH)2?

I think the answer you want is

Ag+ + OH^- ==> AgOH but it isn't that simple.

To determine the net ionic equation for the reaction between AgNO3 (silver nitrate) and Ba(OH)2 (barium hydroxide), we first need to write the balanced molecular equation.

The balanced molecular equation for the reaction can be written as follows:

AgNO3 + Ba(OH)2 -> AgOH + Ba(NO3)2

Next, we can split the soluble compounds (compounds that dissociate in water) into their respective ions. In this case, AgNO3 and Ba(NO3)2 are soluble, while AgOH and Ba(OH)2 are insoluble.

The dissociation of the soluble compounds is as follows:

AgNO3 -> Ag+ + NO3-
Ba(OH)2 -> Ba2+ + 2OH-

Since AgOH is insoluble, it will remain in its molecular form and not dissociate.

Now, we can write the complete ionic equation by including the individual ions involved in the reaction:

Ag+ + NO3- + Ba2+ + 2OH- -> AgOH + Ba2+ + 2NO3-

Finally, to determine the net ionic equation, we eliminate the spectator ions (ions that appear on both sides of the equation and do not participate in the reaction). In this case, Ba2+ and NO3- are spectator ions because they appear on both the reactant and product side of the equation. Thus, we remove them from the equation:

Ag+ + OH- -> AgOH

Therefore, the net ionic equation for the reaction between AgNO3 and Ba(OH)2 is Ag+ + OH- -> AgOH.