What will be the the net ionic equations for the following ones: - a) agno3 + kcl b) ni(no3)2 + na2s c) cacl2 + na2co3. 2) write out the total ionic equation and cancel anything that is common on both sides ca+2(aq) + 2cl-(aq) + 2na+(aq) + co3-2(aq) --> caco3(s) + 2na+(aq) + 2cl-(aq)

The molecular equation is

AgNO3(aq]+HCl(aq]→AgCl(s]+HNO3(aq]

How did I get this equation? Consider each reactant or product separately:

1 mole of AgNO3 contains 1 mole of Ag+ and 1 mole of NO−3 ions.

Ag+(aq]+NO−3(aq]+H+(aq]+Cl−(aq]→AgCl(s]⏐⏐↓+H+(aq]+NO−3(aq]

The net ionic equation is

Ag+(aq]+Cl−(aq]→AgCl(s]⏐⏐↓

Now try some of the others on your own

2fe + 3h2so4 -> fe2(so4)3 + 3h2

it is necessary to balance equations in order to get the proper amount of reactants as well as products in order not to make a miscalculation.

you cannot change the subscripts as that would change the substance itself. for instance, diatomic elements such as h2 only have the subscript two when a gas. another example would be so4, if you were to change the subscript, the element would no longer be sulfate.

we change the coefficients instead as that only changes the number of molecules rather than the substance itself.

hope this !

if you mean hydrogen and oxygen then water is the product