[Boxxxed]

We mixed 30 ml of 0.1667m/L CuSO4*5H20 with 40 mL 0.33 mol/L Na2CO3

We yielded 0.603g precipitate so I just need to calculate theoretical yield. It says Na2CO3 was in excess. How to I get a balanced formula so I can calculate yield?

[Borek]

Don't you know what you were preparing?

[Boxxxed]

That's all the info I have

[Boxxxed]

I know there is CuCO3 and Na2SO4 produced but what happens to the water?

[Boxxxed]

Formula must be something like

CuSO4+Na2CO3------>CuCO3+Na2SO4

with CuCO3 being the precipitate.

If the ratio is 1:1 then I have calculated the mass of CuCO3 to be 0.50 g.

%yield = 0.50/0.603 = 83%

Can someone tell me if I am right? I just guessed the 1:1 ratio as I don't know how to get the balanced formula.

[Borek]

Ah, so when you write "formula", you mean "reaction equation". You are asked to calculate reaction stoichiometry using a balanced reaction equation, but you were not earlier taught how to balance reactions? Hard to believe.

You can safely write the reaction ignoring water, you started with already dissolved copper sulfate, so the fact that solid is hydrated is no longer important.

Yield is actual/theoretical, not the other way around. 0.50g of copper carbonate is wrong, no idea how you got it (even if - accidentally - 1:1 is a correct molar ratio).

[Boxxxed]

I redid the calculations and got 0.6176 g CuCO3. Which is a 97.6 % yield. I was noodling around and got the answer in the previous post, not sure where the sheet of paper went.

[Borek]

That looks much better.