Answer to Question #85177 in General Chemistry for Victor
A piece of chalk (mainly calcium carbonate) is placed in 250. mL of 0.348 M HCl.
All the CaCO3 reacts, releasing carbon dioxide gas, and leaving a clear solution.
35.00 mL of the solution is pipetted into another flask.
28.8 mL of 0.0509 M NaOH is required to titrate the HCl remaining in this 35.00-mL portion.
What was the original mass of CaCO3 in the piece of chalk?
Cm=n/V and n=Cm x V = 0.348 x 0.25 =0.087 mol HCl
n=0.0509 x 0.0288 = 0.0015 mol NaOH
ntotal= n1-n2=0.087 – 0.0015 =0.0855 mol HCl
CaCO3 + 2HCl = CaCl2 + CO2 + H2O
n=0.0855:2= 0.04275 mol CaCO3 m= n x Mr= 0.04275 x 100= 4.275