In the titration of 25.00 mL of a water sample, it took 19.990 mL of 3.480x 10−3 M EDTA solution to reach the endpoint. Calculate the number of moles of EDTA required to titrate the water sample. (enter your answer with 3 significant figures) The total hardness is due to one or a combination of Ca2+, Mg2+, and Fe2+ in your sample. It is convenient to express this hardness as though it was entirely due to Ca2+. Making this assumption, determine the number of moles of Ca2+ present in the bottled water sample titrated. (enter your answer with 3 significant figures) The total hardness is always listed in parts-per-million (ppm) of CaCO3 (or mg CaCO3 / Kg H2O). Since the density of water is 1.0 g/mL, one ppm would be the same as the number of mg of CaCO3 per liter of water. Determine the number of moles of CaCO3 present in the titrated sample of water, assuming that all the Ca2+ combines with CO32−. (enter your answer with 3 significant figures) Calculate the number of grams of CaCO3 present and convert to mg. (enter your answer with 3 significant figures) Convert the number of mL of bottled water used in each sample titration to Liters. (enter your answer with 3 significant figures) Calculate the ppm of CaCO3 = mg CaCO3 / Liters H2O used. (enter your answer with 3 significant figure
In the titration of 25.00 mL of a water sample, it took 19.990 mL of 3.480x 10−3 M EDTA solution to reach the endpoint.
Calculate the number of moles of EDTA required to titrate the water sample. (enter your answer with 3 significant figures)
The total hardness is due to one or a combination of Ca2+, Mg2+, and Fe2+ in your sample. It is convenient to express this hardness as though it was entirely due to Ca2+. Making this assumption, determine the number of moles of Ca2+ present in the bottled water sample titrated. (enter your answer with 3 significant figures)
The total hardness is always listed in parts-per-million (ppm) of CaCO3 (or mg CaCO3 / Kg H2O). Since the density of water is 1.0 g/mL, one ppm would be the same as the number of mg of CaCO3 per liter of water. Determine the number of moles of CaCO3 present in the titrated sample of water, assuming that all the Ca2+ combines with CO32−. (enter your answer with 3 significant figures)
Calculate the number of grams of CaCO3 present and convert to mg. (enter your answer with 3 significant figures)
Convert the number of mL of bottled water used in each sample titration to Liters. (enter your answer with 3 significant figures)
Calculate the ppm of CaCO3 = mg CaCO3 / Liters H2O used. (enter your answer with 3 significant figures)
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