An excess of sodium carbonate, Na2CO3, in solution is added to a solution containing 16.49 g CaCl2. After performing the experiment, 13.43 g of calcium carbonate, CaCO3, is produced.

Question

Calculate the percent yield of this reaction.

Answer 1

So Seth S.,

Write the balanced equation for the precipitation reaction.

Convert the given reactant masses, etc. into moles. Compare the ratio of moles of the supplied reactants, to what the reaction requires. Determine which reactant is limiting (use ratios in the balanced reaction as a guide). From the limiting reactant, step across to product (CaCO3) as moles. Convert that to mass, using the molar mass of CaCo3= theoretical yield. Experimental/theoretical = %yield .

If you wanted to take it a bit further, you could look up the solubility product of CaCO3, since not all the CaCO3 necessarily precipitates, and adjust the theoretical for that. Even further, you could adjust for the ionic strength of the dissolved byproduct ions,and for any "common ion effects". But that's gilding the lily a bit, for a high school course?