Groundwater Hardness -EDTA titration
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Hardness in groundwater is due to the presence of metal ions, primarily Mg2+ and Ca2+. Hardness is generally reported as ppm CaCO3 or mmol/L Ca2+. To measure the water hardness, a sample of groundwater is titrated with EDTA, a chelating agent; in the presence of the indicator eriochrome black T, symbolized as In. Eriochrome black T, a weaker chelating agent than EDTA, is red in the presence of Ca2+ and turns blue when Ca2+ is removed.
..............red.................................blue
Ca(In)2+ + EDTA --> Ca(EDTA)2+ + In
A 50.00 mL sample of ground water is titrated with 0.0850 M EDTA. Assume that Ca2+ accounts for all of the hardness in groundwater. If 11.10 mL of EDTA is required to titrate the 50.00 mL sample, what is the hardness of the groundwater in molarity and in parts per million of CaCO3 by mass?
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Solution Summary
The hardness of groundwater is determined from an EDTA titration.
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Moles of EDTA used = 0.0850 M x 0.01110 L = 9.435 x 10-4 mol
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