Solutions of silver nitrate and sodium chromate are mixed. What is the net ionic equation?
I got: 2Ag(aq) + CrO4-2(aq) -> Ag2CrO4(s)
is that right?
see above.
Yes, your net ionic equation is correct. When solutions of silver nitrate (AgNO3) and sodium chromate (Na2CrO4) are mixed, a precipitation reaction occurs, forming silver chromate (Ag2CrO4) as a solid precipitate. The net ionic equation can be written as:
2Ag+(aq) + CrO4^2-(aq) → Ag2CrO4(s)
This equation shows the species that are directly involved in the reaction, while spectator ions (ions that do not take part in the reaction) are omitted.
To determine the net ionic equation for the reaction between silver nitrate (AgNO3) and sodium chromate (Na2CrO4), we first need to write the balanced complete ionic equation.
The balanced complete ionic equation is as follows:
2Ag+(aq) + 2NO3-(aq) + 2Na+(aq) + CrO4^2-(aq) -> Ag2CrO4(s) + 2Na+(aq) + 2NO3-(aq)
In this equation, the ions that appear on both sides of the equation and don't participate in the reaction are called spectator ions. In this case, the sodium ions (Na+) and nitrate ions (NO3-) are spectator ions.
Now, we can remove the spectator ions from the equation to obtain the net ionic equation:
2Ag+(aq) + CrO4^2-(aq) -> Ag2CrO4(s)
So yes, your net ionic equation is correct:
2Ag(aq) + CrO4^2-(aq) -> Ag2CrO4(s)