How To Write The Net Ionic Equation For Na3PO4 + NiCl2 = Ni3(PO4)2 + NaCl

In this video we'll write the balanced net, ionic equation for Na, Three for plus nicl2. This is sodium phosphate and nickel ii chloride. First thing we need to do is balance the molecular equation. I can see I need to put a 3 in front of the nickel ii chloride.

So that'll balance those. Now I have six of these chlorine atoms, I'll put a 6 here. I can put a 2 here, and I think, yep, this equation is balanced. So we have the balanced molecular equation. Now we can write the state's sodium compounds. They are. Aqueous or soluble, they dissolve in water split apart into their ions and the same with compounds with chlorine, almost always soluble or aqueous.

They will split apart into their ions compounds with phosphate tend to be insoluble. The exceptions are elements in group 1 and ammonium phosphate. So in this case, this should be in the soluble, which means it'll be a solid when this reaction takes place it'll form. This solid it'll be a precipitate it'll fall to the bottom of the test tube. So we write. Soluble, we won't split this apart and then sodium chloride that is aqueous.

So we have our states now we can split the strong electrolytes into their ions that'll. Give us the complete ionic equation. Sometimes called the total ionic equation. So sodium is in Group 1 on the periodic table 1, plus and the phosphate it's, always three minus. So we have two times three, six, sodium ions and all right aqueous at the end I won't write that.

Now, plus two of the phosphate ions, the chloride ion is always a one. Minus and we have two of them. So the nickel is two-plus that's.

Why we were calling it nickel 2. So we'll, add three times the one nickel ion three nickel, two, plus ions, plus three times two is six chloride ions. So these are the reactants in the products we said, we don't split solids apart when we do net ionic equations.

So we have n Three for 2, plus 6 times the 1. And we said, plus and minus there. So 6, sodium ions, plus 6 chloride ions. So this is the total or complete ionic equation. Now we can cross. Out spectator ions, these are ions that appear on both sides of the chemical equation.

They haven't changed, so we're, not interested in them in the reactants. We have 6 sodium ions in the products we have 6, sodium ions cross them out. We have 6 chloride ions in the reactants 6 and the products cross them out, but everything else is unique. So this is going to be the net ionic equation for Na, Three, 4, plus nicl2.

Let me clean this up, and I'll write the states in, and then we'll have our net ionic. Equation so this is the balanced net ionic equation for sodium phosphate, plus nickel 2 chloride. Our charge is conserved in the number of atoms, they're conserved as well. This is a balanced net ionic equation. And this is Dr. B. Thanks for watching.