Question

An EDTA standard was made at 22.5 °C by dissolving 0.6206 g (uncorrected mass) of Na2H2EDTA·2H2O in a 499.859 mL volumetric flask. Several 9.9873 mL aliquots of unknown were titrated for total divalent metal ions, and required an average of 23.197 mL of EDTA solution to reach the end point. After precipitation of Mg2+ from several additional 9.9873 mL aliquots of unknown, an average of 15.660 mL of titrant was required to reach the end point. All blanks were zero. Determine the total hardness in mg/L as CaCO3, given that the molar mass of CaCO3 = 100.0868 g/mol. Finally, calculate the concentrations of Ca2+ and Mg2+ individually, in mM. Be sure to explicitly show the mole ratio in your sample stoichiometry calculations— do not treat this like a dilution problem. [Note: you do not have to show how to calculate the density of water at 22.5 °C, the buoyancy correction factor for EDTA, or the molar mass of CaCO3, but you do have to show how to use each of these quantities in the sample problems.]

Answers are below I just need help with how to get them:

[EDTA standard (corrected to 20 °C): 3.34072 mM]

[Intermediate answer: [Ca2+] + [Mg2+] = 7.75933 mM]

[Total hardness: 776.606 mg/L as CaCO3]

[Individual ions: 5.23822 mM Ca2+; 2.52110 mM Mg2+]

Answer 1

m = true mass; m’ = measured mass; da = density of air (0.0012 g/ml); dw = density of calibration weights (8.0 g/ml); d = density of weighed object

for the ion Ca and Mg is the same