A 5.455-g sample of impure CaCl2 is dissolved and treated with excess potassium carbonate solution. The dried CaCO3 (calcium carbonate) precipitate weighs 4.010-g. Calculate the percent by mass of CaCl2 in the original mixture.
I just need help because I do get the balanced equation and all. But I think I am wrong. For my mass of CaCl2, I got 4.446 grams but then wouldnt that make the fraction for percent yeild too big?
No of mol of CaCO3 precipitated = w/M
w = weight of CaCo3 = 4.010 g
M = molarmass of CaCO3 = 100 g/mol
= 4.010/100 = 0.0401 mol
1 mol CaCO3 = 1 mol CaCl2
No of mol of CaCl2 present in sample = 0.0401 mol
amount of CaCl2 present in sample = 0.0401*111 = 4.45 g
percent by mass of CaCl2 = wt of cacl2/wt of sample*100
= 4.45/5.455*100
= 81.6 %
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