net ionic equations of nitric acid with CO3 2- and with PO4 3-.
H^+(aq) + CO3^-2(aq) ==> H2O(l) + CO2(g)
The remainder of the question is not clear.
I didn't balance the equation. Place a coefficient of 2 for H^+ on the left.
To determine the net ionic equations of nitric acid with CO3 2- and PO4 3-, we need to first write out the balanced molecular equations and then identify the spectator ions.
1. Nitric acid (HNO3) with CO3 2-:
The balanced molecular equation is:
2 HNO3 + CO3 2- → 2 HCO3- + H2O + NO3-
Next, we need to break down the soluble compounds into their respective ions:
HNO3 → H+ + NO3-
CO3 2- → CO3 2-
The complete ionic equation is:
2 H+ + 2 NO3- + CO3 2- → 2 HCO3- + H2O + NO3-
To obtain the net ionic equation, we need to identify the spectator ions. In this reaction, H+ and NO3- ions appear on both sides of the equation and do not participate in the reaction. Therefore, they are considered spectator ions.
The net ionic equation is:
CO3 2- → HCO3-
2. Nitric acid (HNO3) with PO4 3-:
The balanced molecular equation is:
HNO3 + PO4 3- → HPO4 2- + NO3-
Breaking down the soluble compounds into ions:
HNO3 → H+ + NO3-
PO4 3- → PO4 3-
The complete ionic equation is:
H+ + NO3- + PO4 3- → HPO4 2- + NO3-
Once again, we identify the spectator ions, and in this case, H+ and NO3- are spectator ions.
The net ionic equation is:
PO4 3- → HPO4 2-
These are the net ionic equations for nitric acid with CO3 2- and PO4 3-, respectively.