Write the molecular equation and the net ionic equation for each of the following aqueous reactions.

Ca(NO3)2 + K2CO3

FeSO4 + NaCl

NiCl2 + NaBr

Ca(NO3)2 + K2CO3

I assume Ca(NO3)2 is (aq) and K2CO3 is (aq); technically the dry materials won't react.

Write the molecular equation.
Ca(NO3)2 + K2CO3 ==> CaCO3(s) + 2KNO3

The reaction takes place because CaCO3 is insoluble. To change to an ionic equation, convert everything into ions EXCEPT
a. gases
b. insoluble materials.
c. weak electrolytes.

Ca^+2 + 2NO3^- + 2K^+ + CO3^-2 ==> CaCO3 + 2K^+ + 2NO3^-

Now cancel common ions that appear on both sides; i.e., 2NO3^- and 2K^+ and the NET ionic equation is
Ca^+2(aq) + CO3^-2(aq) ==> CaCO3(s)

The others are done the same way IF they react.

2K+Pb2+2NO3+2K+cap

Pressures

Ca(NO3)2 + K2CO3

Molecular equation: Ca(NO3)2 + K2CO3 → 2KNO3 + CaCO3

Net ionic equation: Ca2+ + CO3^2- → CaCO3

And now, brace yourself, for the thrilling adventures of FeSO4 and NaCl!

FeSO4 + NaCl

Molecular equation: FeSO4 + 2NaCl → FeCl2 + Na2SO4

Net ionic equation: Fe2+ + 2Cl^- → FeCl2

And we're back with another thrilling episode of NiCl2 vs. NaBr!

NiCl2 + NaBr

Molecular equation: NiCl2 + 2NaBr → NiBr2 + 2NaCl

Net ionic equation: Ni2+ + 2Br^- → NiBr2

Hope you enjoyed these "aqueous reactions" starring our lovely cast of chemical compounds!

To write the molecular equation and the net ionic equation for each of the given aqueous reactions, we need to first determine the products by swapping the positive ions (cations) of the reactants.

1. Ca(NO3)2 + K2CO3:
The cation Ca2+ from Ca(NO3)2 will combine with the anion CO32- from K2CO3, yielding CaCO3 as one of the products. The remaining ions, K+ and NO3-, will remain unreacted.

The molecular equation is:
Ca(NO3)2 + K2CO3 → CaCO3 + 2KNO3

To obtain the net ionic equation, we need to identify the soluble compounds and the ions that are not spectator ions. In this case, all the compounds are soluble, so we need to break them down into their constituent ions. The balanced ionic form of the equation is:

Ca2+ (aq) + 2NO3- (aq) + 2K+ (aq) + CO32- (aq) → CaCO3 (s) + 2K+ (aq) + 2NO3- (aq)

The net ionic equation is:
Ca2+ (aq) + CO32- (aq) → CaCO3 (s)

2. FeSO4 + NaCl:
The cation Fe2+ from FeSO4 will combine with the anion Cl- from NaCl, yielding FeCl2 as one of the products. The remaining ions, Na+ and SO42-, will remain unreacted.

The molecular equation is:
FeSO4 + 2NaCl → FeCl2 + Na2SO4

To obtain the net ionic equation, we again need to determine the soluble compounds and the relevant ions. In this case, FeSO4 and NaCl are both soluble, so we break them down into their constituent ions. The balanced ionic form of the equation is:

Fe2+ (aq) + SO42- (aq) + 2Na+ (aq) + 2Cl- (aq) → FeCl2 (s) + Na2SO4 (aq)

The net ionic equation is:
Fe2+ (aq) + 2Cl- (aq) → FeCl2 (s)

3. NiCl2 + NaBr:
The cation Ni2+ from NiCl2 will combine with the anion Br- from NaBr, yielding NiBr2 as one of the products. The remaining ions, Na+ and Cl-, will remain unreacted.

The molecular equation is:
NiCl2 + 2NaBr → NiBr2 + 2NaCl

To obtain the net ionic equation, we determine the soluble compounds and the relevant ions. Both NiCl2 and NaBr are soluble, so we break them down into their constituent ions. The balanced ionic form of the equation is:

Ni2+ (aq) + 2Cl- (aq) + 2Na+ (aq) + 2Br- (aq) → NiBr2 (s) + 2Na+ (aq) + 2Cl- (aq)

The net ionic equation is:
Ni2+ (aq) + 2Br- (aq) → NiBr2 (s)

Remember, the net ionic equation excludes spectator ions, which are the ions that appear on both sides of the equation and do not participate in the reaction.