[Punde]

hey this is a punde and i have an lab to do for chem. I have two solids, and one of them is impure with NaCl. I have to react the two solids (but the teacher didn't give us a procedure). I'm not even copmletely sure if two solids can react together. The teacher gave us two possiblities for what the solids are:

1. (Na3PO4-12H2O (solid crystal)) + (CuCl2 + NaCl (the impure solid))

or

2. (CuSO4-5H2O (solid Crystal)) +  (Na2CO3 + NaCl (the impure solid))

I have to figure out a procedure (which is supposed to be the same, no matter which option i get). For the lab, we can also burn/dehydrate the chemicals. We just can't add any more chemicals. I think that the procedure has something to do with how the other chemical in the equation (not the impure one) is a hydrate. This is an COMMON ION EFFECT. So can you guys help me figure out the procedure and the products for the above o-ptions? Any help would be appreciated.THANKS!!

[Albert]

What property do copper(II) phosphate and copper(II) carbonate share?

[Punde]

Is it that they're both insoluble in water? Because if it is, then when I mix either of the two combinations of chemicals, would H2O form (from the hydrate) with either Cu3PO4 or CuCO3 forming as a precipitate? Then I think I could dehydrate the the H2O out, but then the Cu3PO4/CuCO3 would still be left with sodium chloride/sodium sulfate (I think). I know that NaCl is soluble, which probably means that NaSO4 is to. That means that they would dissolve in the water, and if the water is dehydrated out, then the only thing left would be the Cu3PO4/CuCO3. Is what I just said what would actually happen?

[Albert]

Now, you obviously can't use the water of crystallization to dissolve your salts. I believe you're alowed to use pure water to do this, aren't you?

Before doing it, however, you must weight both salts: the pure and the impure.

You, then, dissolve them (all the salts you start from are lovely soluble) and, finally, you'll get a solid precipitate, depending on the experiment either a phosphate or a carbonate.

Weight that too and do your calculations (I don't think you need help with them, do you?).

It's easier to do than to describe. 

[Punde]

Thanks a lot, this really helped me.   

[Punde]

Okay, I think I have it now. I'm just not sure on how the balanced equations would look. Would I include the NaCl from the impure chemical in the balanced equation?

[Albert]

Okay, I think I have it now. I'm just not sure on how the balanced equations would look. Would I include the NaCl from the impure chemical in the balanced equation?

No, because sodium salts are completely dissociated in solution.

[Punde]

One last question about balancing the equation. If I'm adding pure water to dissolve everything in, I have to include the pure H2O as a reactant separate from the hydrate, right?

[Borek]

No. It doesn't react, it is just a solvent.

[Punde]

hey this is punde again can u tell me one last thing if my balanced chemical equations are right or not...and one more thing can you check the states of the reactants and products and if i m missing the reactants or products(nacl or h20 etc..) These are the following balanced chemical reactions...

2 Na3PO4 • 12 H2O(s) + 3 CuCl2(aq) >> Cu3(PO4)2(s) + 6 NaCl(aq) + 12 H2O(l)

CuSO4 • 5 H2O(s) + Na2CO3(aq) >> CuCO3(s) + Na2SO4(aq) + 5 H2O( l)

SORRY TO DISTURB YOU!! and thanx for the information

[Borek]

2 Na3PO4 • 12 H2O(s) + 3 CuCl2(aq) >> Cu3(PO4)2(s) + 6 NaCl(aq) + 12 H2O(l)

Check H₂O.