1. net ionic equation for the reaction between silver nitrate and the arsenate ion
I got:
3Ag (+) + AsO4 ---> Ag3AsO4
2. net ionic equation for the precipitation of copper hexacyanoferrate (II).
I got:
2Cu (2+) + [Fe(CN)6] ---> Cu2 [Fe(CN6)]
Can someone please check and see if I did these correctly. If not, can you please example how/ what I am doing wrong.
The total electrical charge on the left side of a chemical equation must be equal to the total electrical charge on the right side. That is not the case on either chemical equation as you typed it.
The Ag3AsO4 equation is ok if we assume the ---(which looks like an arrow with the >) is actually the charge on the arsenate ion. You can write AsO4^3- and that way we don't confuse it with the arrow.
3Ag^+1 + AsO4^3- ==> Ag3AsO4(s)
Oh sorry I forgot to write the charges.
For then for the second one,
it is supposedly look like this?
2Cu (2+) + [Fe(CN)6]^(4-) ==> Cu2 [Fe(CN6)]
would that make this ionic equation correct?
That looks ok to me.
To check if your net ionic equations are correct, let's go through the steps of writing net ionic equations and compare them to your answers.
1. Net ionic equation for the reaction between silver nitrate and the arsenate ion:
First, write the balanced molecular equation:
AgNO3 + Na3AsO4 -> Ag3AsO4 + NaNO3
Next, identify the strong electrolytes that dissociate into ions in solution. In this case, AgNO3 and Na3AsO4 both dissociate:
AgNO3 -> Ag+ + NO3-
Na3AsO4 -> 3Na+ + AsO4^3-
Now, write the complete ionic equation by including all the ions:
3Ag+ + AsO4^3- + 3Na+ + NO3- -> Ag3AsO4 + 3Na+ + NO3-
Finally, simplify the equation by canceling out the spectator ions (those that appear on both sides of the equation):
3Ag+ + AsO4^3- -> Ag3AsO4
Your net ionic equation (3Ag(+) + AsO4 -> Ag3AsO4) is correct!
2. Net ionic equation for the precipitation of copper hexacyanoferrate (II):
First, write the balanced molecular equation:
CuSO4 + 2K3[Fe(CN)6] -> Cu2[Fe(CN)6] + 3K2SO4
Next, identify the strong electrolytes that dissociate into ions in solution. In this case, CuSO4 and K3[Fe(CN)6] both dissociate:
CuSO4 -> Cu2+ + SO4^2-
K3[Fe(CN)6] -> 3K+ + [Fe(CN)6]^3-
Now, write the complete ionic equation by including all the ions:
Cu2+ + SO4^2- + 2K+ + [Fe(CN)6]^3- -> Cu2[Fe(CN)6] + 2K+ + SO4^2-
Finally, simplify the equation by canceling out the spectator ions:
Cu2+ + [Fe(CN)6]^3- -> Cu2[Fe(CN)6]
Your net ionic equation (2Cu(2+) + [Fe(CN)6] -> Cu2[Fe(CN)6]) is also correct!
In both cases, your net ionic equations accurately represent the main reaction that is occurring, so well done!