A 4.51 g sample of chalk is mixed with 23.8 mL of 3.0 M hydrochloric acid. It is filtered to obtain 3.64 g of calcium carbonate. What is the percent of calcium carbonate in the chalk?
No.of moles of HCl reacted = (23.8 x 10-3 L) x (3.0 M) = 0.0714 mol
Calcium carbonate reacts with HCl as shown below:
CaCO3 + 2 HCl ------------> CaCl2 + CO2 + H2O
From this balanced reaction, we have:
1 mole of CaCO3 reacts with 2 moles of HCl
Hence, 1 mole of HCl reacts with 1/2 mole of CaCO3
Therefore, 0.0714 mol of HCl reacts with (1/2) x 0.0714 mol mole of CaCO3 = 0.0357 mol mole of CaCO3
Molar mass of CaCO3= 100.0869 g/mol
Hence, Mass of CaCO3 in chalk = (0.0357 mol) x ( 100.0869 g/mol) = 3.573 g
Mass of chalk = 4.51 g
Hence, percent of calcium carbonate in the chalk will be:
percentage = (3.573 g) / (4.51 g) x 100 %
percentage = 0.7923 x 100 %
percentage = 79.23 %
A 4.51 g sample of chalk is mixed with 23.8 mL of 3.0 M hydrochloric acid....
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