net ionic equation for silver sulfate
The net ionic equation for silver sulfate (Ag2SO4) can be written as:
2Ag+ + SO42- -> Ag2SO4
This equation shows that two silver ions (Ag+) react with one sulfate ion (SO42-) to form silver sulfate (Ag2SO4).
To write the net ionic equation for silver sulfate, we need to first write the balanced chemical equation for the reaction that takes place when silver sulfate dissolves in water.
The chemical formula for silver sulfate is Ag2SO4. When it dissolves in water, it dissociates into its ions:
Ag2SO4(s) → 2Ag+(aq) + SO4^2-(aq)
The 2Ag+ ions and SO4^2- ions are the ions that are responsible for the overall reaction. However, in a net ionic equation, we only include the ions that take part in the chemical reaction.
Since both Ag+ and SO4^2- ions are present as reactants and products, they are not involved in a chemical reaction. Therefore, the net ionic equation for silver sulfate would simply be:
No reaction occurs, hence there is no net ionic equation.
To determine the net ionic equation for silver sulfate, we need to start with the balanced molecular equation.
The molecular equation for the reaction between silver sulfate (Ag2SO4) and water (H2O) is:
Ag2SO4 (aq) + H2O (l) → Ag+ (aq) + SO4^2- (aq) + H2O (l)
In this equation, Ag2SO4 dissociates into Ag+ ions and SO4^2- ions when dissolved in water. However, water (H2O) remains unchanged throughout the reaction.
Next, we need to identify the spectator ions—ions that don't undergo a chemical change and remain as they are in the reaction. In this case, the spectator ions are the H2O molecules.
By eliminating the spectator ions, we obtain the net ionic equation:
Ag2SO4 (aq) → Ag+ (aq) + SO4^2- (aq)
This net ionic equation represents only the species that are actually involved in the chemical change, which in this case is the dissociation of silver sulfate into Ag+ and SO4^2- ions.