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26 Nov 2019
Calculate the moles of calcium carbonate present in a 25.00mLsample of a standard solution, assuming the standard is known tohave a hardness of 105 ppm (hardness due to CaCO3). You can assumethat the density of the sample is 1.000 g/mL and the molar mass ofcalcium carbonate is 100.0 g/mol.
If the 25.00mL sample from above was titrated with EDTA, whatvolume of a 0.00330 M EDTA solution would be needed to reach theendpoint? (Your answer should be given in milliliters.)
Calculate the moles of calcium carbonate present in a 25.00mLsample of a standard solution, assuming the standard is known tohave a hardness of 105 ppm (hardness due to CaCO3). You can assumethat the density of the sample is 1.000 g/mL and the molar mass ofcalcium carbonate is 100.0 g/mol.
If the 25.00mL sample from above was titrated with EDTA, whatvolume of a 0.00330 M EDTA solution would be needed to reach theendpoint? (Your answer should be given in milliliters.)
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