Enter the Net Ionic Equation including phases, for the reaction of AgNO3 and Ba(OH)2.
I would for this, assume the silver nitrate and barium hydroxide were initially in aqueous solution, the problem did not state that.
To determine the net ionic equation for the reaction between AgNO3 (silver nitrate) and Ba(OH)2 (barium hydroxide), we need to first write the balanced chemical equation for the reaction. Then, we can identify the spectator ions and remove them to obtain the net ionic equation.
Step 1: Write the balanced chemical equation:
AgNO3 (aq) + Ba(OH)2 (aq) → AgOH (s) + Ba(NO3)2 (aq)
The equation above represents the reaction between AgNO3 and Ba(OH)2, where they combine to form AgOH (silver hydroxide) as a precipitate and Ba(NO3)2 (barium nitrate) as the soluble product.
Step 2: Identify the spectator ions:
Spectator ions are the ions that remain unchanged throughout the reaction and do not participate in the formation of the precipitate. In this case, the spectator ions are the NO3- (nitrate) ions from AgNO3 and the Ba2+ (barium) ions from Ba(OH)2.
Step 3: Write the net ionic equation:
To obtain the net ionic equation, we need to remove the spectator ions from the balanced equation. They cancel each other out, leaving only the ions involved in the formation of AgOH (s):
Ag+ (aq) + OH- (aq) → AgOH (s)
This is the net ionic equation for the reaction of AgNO3 and Ba(OH)2. It represents the formation of silver hydroxide (AgOH) from the combination of silver ions (Ag+) and hydroxide ions (OH-).
Note: It is important to include the phases (s, aq) to indicate whether the substance is a solid (s) or in aqueous solution (aq). In this case, AgOH is a solid precipitate, while Ag+ and OH- are in aqueous solution.