Enter the net ionic equation, including phases, for the reaction og AgNO3 (aq) with Ba(OH)2 (aq).
I have Ag+ +OH- =AgOH but I don't know how to determine the phases.
Ag^+(aq), OH^-(aq), AgOH(s) but this is not stable in solution and decomposes to Ag2O(s)
To determine the phases in a chemical equation, you need to know the solubility rules for the different compounds involved. These rules indicate whether a compound is soluble (forms an aqueous solution) or insoluble (forms a solid precipitate).
In the case of the reaction between AgNO3 (silver nitrate) and Ba(OH)2 (barium hydroxide), we can use the solubility rules to determine the phases.
Solubility rules indicate that most nitrates (such as AgNO3) are soluble and hydroxides (such as Ba(OH)2) are also soluble except for a few exceptions, including barium hydroxide. Barium hydroxide is insoluble and forms a solid precipitate.
Now, let's write the overall balanced chemical equation first:
AgNO3 (aq) + Ba(OH)2 (aq) → AgOH (s) + Ba(NO3)2 (aq)
Next, to write the net ionic equation, we only consider the ions that undergo a chemical change. The soluble compounds, which completely dissociate into ions in water, are represented with (aq) and the insoluble compound is represented with (s).
The AgNO3 (aq) dissociates to give Ag+ (aq) and NO3- (aq).
The Ba(OH)2 (aq) dissociates to give Ba2+ (aq) and OH- (aq).
Since AgOH is an insoluble compound and forms a solid precipitate, we include it in the net ionic equation.
Net ionic equation:
Ag+ (aq) + OH- (aq) → AgOH (s)
So, the net ionic equation for the reaction of AgNO3 (aq) with Ba(OH)2 (aq) is Ag+ (aq) + OH- (aq) → AgOH (s).