Is there a net ionic equation for Ca(NO3)2 and K2CrO4?
CaCrO4 is soluble in water at room T. The solubility decreases with temperature.
http://en.wikipedia.org/wiki/Solubility_table#C
To determine if there is a net ionic equation for the reaction between Ca(NO3)2 (calcium nitrate) and K2CrO4 (potassium chromate), we first need to write out the balanced chemical equation.
The chemical formula of calcium nitrate is Ca(NO3)2, which means it dissociates into calcium ions (Ca2+) and nitrate ions (NO3-). The chemical formula of potassium chromate is K2CrO4, which dissociates into potassium ions (K+) and chromate ions (CrO4^2-).
The balanced chemical equation for the reaction can be written as:
Ca(NO3)2 + K2CrO4 → CaCrO4 + 2 KNO3
Now, let's write down the complete ionic equation by separating all the soluble ionic compounds into their respective ions:
Ca^2+ + 2 NO3^- + 2 K+ + CrO4^2- → CaCrO4 + 2 K+ + 2 NO3^-
We can notice that there are ions present on both the reactant and product sides that are the same. These are called spectator ions. In this case, the spectator ions are K+ and NO3^-.
Finally, we can write the net ionic equation by canceling out the spectator ions:
Ca^2+ + CrO4^2- → CaCrO4
Therefore, the net ionic equation for the reaction between Ca(NO3)2 and K2CrO4 is Ca^2+ + CrO4^2- → CaCrO4.
Yes, there is a net ionic equation for the reaction between calcium nitrate (Ca(NO3)2) and potassium chromate (K2CrO4).
First, let's write the balanced molecular equation for the reaction:
Ca(NO3)2 + K2CrO4 → CaCrO4 + 2 KNO3
To determine the net ionic equation, we need to break all the soluble compounds into their respective ions and remove the spectator ions (ions that appear on both sides of the equation without undergoing any changes).
The soluble compounds are:
Ca(NO3)2 → Ca^2+ + 2 NO3^-
K2CrO4 → 2 K+ + CrO4^2-
The net ionic equation is then:
Ca^2+ + CrO4^2- → CaCrO4
In this net ionic equation, the spectator ions (2 K+ and 2 NO3^-) have been removed, as they do not participate in the chemical reaction.