Net ionic equations for:
Br- + AgNO3
CO3 + AgNO3
Cl-+ AgNO3
I + AgNO3
PO4^-3 + AgNO3
SO4^-2 + AgNO3
S^-2 + AgNO3
They all formed ppt,but I don't know where to go from here. Even a couple to get me started would be greatly appreciated!
If you know they all form ppts you have most of the problem done.
Br^-(aq) + Ag^+(aq) ==> AgBr(s)
S^2-(aq) + 2Ag^+(aq) ==> Ag2S(s)
To write net ionic equations, we need to first determine the reactants and products involved in the reaction. From the provided information, it is given that all of the reactions formed precipitates (ppt). We can use this information to predict the products and then write the balanced net ionic equations.
Let's go through a couple of examples to get started:
1. Br- + AgNO3
In this reaction, we have bromide ion (Br-) reacting with silver nitrate (AgNO3). To determine the products, we can use the solubility rules. According to the rules, silver bromide (AgBr) is insoluble and forms a precipitate. The balanced equation for this reaction is:
Br- + AgNO3 → AgBr↓ + NO3-
Here, the solid (↓) symbol indicates the formation of a precipitate.
2. CO3 + AgNO3
In this case, carbonate ion (CO3) reacts with silver nitrate (AgNO3). Again, we use the solubility rules to determine the products. According to the rules, silver carbonate (Ag2CO3) is insoluble and forms a precipitate. The balanced equation is:
CO3 + 2AgNO3 → Ag2CO3↓ + 2NO3-
Here, a coefficient of 2 is added to balance the equation.
You can use a similar approach for the remaining reactions:
3. Cl- + AgNO3
According to the solubility rules, silver chloride (AgCl) is insoluble and forms a precipitate. Write the balanced net ionic equation.
4. I + AgNO3
According to the solubility rules, silver iodide (AgI) is insoluble and forms a precipitate. Write the balanced net ionic equation.
Continue with the remaining reactions using the solubility rules to determine the products and then balance the equations. Remember, the insoluble products will form a precipitate.