Question
In: Chemistry
An EDTA standard was made at 22.5 °C by dissolving 0.6206 g (uncorrected mass) of Na2H2EDTA·2H2O...
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.]
[EDTA standard (corrected to 20 °C): 3.34072 mM]
Solutions
queen_honey_blossom answered 1 year agoRelated Solutions
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A standard iodate solution is prepared at 22.0 °C by dissolving 0.9123 g (uncorrected mass) of...
A standard iodate solution is prepared at 22.0 °C by dissolving
0.9123 g (uncorrected mass) of KIO3 with deionized water in a
499.92 mL volumetric flask. To standardize the Na2S2O3 solution, a
10.005 mL aliquot of the KIO3 solution is acidified, treated with
excess KI, and titrated with Na2S2O3, requiring 22.05 mL to reach
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1)
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