2. A water sample from a local cave system was tested for total water hardness. An EDTA titer was prepared by titrating 30.00 mL aliquot from 1750.00 pm CaCO: standard. For the standardization, it took 50.10 mL EDTA. A 30.00 mL water sample aliquot was then tested for total hardness, and it used 44.30 mL EDTA. Summary of results: Standardization 1750 ppm Volume of sample EDTA (mL) used Sample analysis 30.00 mL CACO3 standard Standard aliquot EDTA (mL) used Determine the following: a. Titer (mg CaCO3/mL EDTA) b. Total hardness (ppm CaCO3) 30.00 mL 44.30 mL 50.10 mL

2. A water sample from a local cave system was tested for total water hardness. An EDTA titer was prepared by titrating 30.00 mL aliquot from 1750.00 pm CaCO: standard. For the standardization, it took 50.10 mL EDTA. A 30.00 mL water sample aliquot was then tested for total hardness, and it used 44.30 mL EDTA. Summary of results: Standardization 1750 ppm Volume of sample EDTA (mL) used Sample analysis 30.00 mL CACO3 standard Standard aliquot EDTA (mL) used Determine the following: a. Titer (mg CaCO3/mL EDTA) b. Total hardness (ppm CaCO3) 30.00 mL 44.30 mL 50.10 mL

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter20: Molecular Spectroscopy And Photochemistry

Section: Chapter Questions

Problem 67CP

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An EDTA solution prepared from its disodium salt was standardized using 0.250-g primary standard CaCO3 (MW=100.087) and consumed 28.50 mL of the solution. The standard solution was used to determine the hardness of a 2.0 L sample of mineral water, which required 35.57 mL EDTA solution. Express the analysis in terms of ppm CaCO3
Complexometric titrations are generally conducted to determine divalent cations. The most important applications are the titration of calcium and magnesium with EDTA. (a) A supplement tablet containing about 300.00 mg of calcium ion was dissolved, filtered, and diluted to 100.00 ml volume. Several 2.00 ml samples of the total solution were titrated with 0.0100 M EDTA solution. The mean corrected titration volume was 13.65 mL. Calculate the calcium content of the supplement tablet in mg units. (b) A sample of Epsom Salt of mass 0.7567 g was dissolved uniformly in distilled water in a 250.00 mL volumetric flask. Portions of the magnesium ion solution of volume 10.00 mL were titrated using a 0.01000 M solution of EDTA. The mean corrected titration volume was 12.25 ml. Calculate the percentage by mass (% w / w) of the magnesium in the Epsom Salt sample. (c) A 100.00 mL sample of tap water was titrated with 0.0100 M EDTA solution. The mean corrected titration volume was 14.80 mL. Determine…
A CaCO3 solution that will be used to standardize EDTA was prepared by dissolving 3.1251 g of solid CaCO3 in 100 mL dilute HCI. A 20.00 mL aliquot was taken for titration with EDTA consuming 32.00 mL of the titrant to reach the endpoint. Express the concentration of EDTA in molarity and in CaCO3 titer. MM Na2H2Y2•2H2O = 372.24 g/mole; MM CACO3 = 100.09 g/mole %3D
A sample of water from a river was analyzed by titrating a 125 mL aliquot with 0.0210 M EDTA, consuming 22.52 mL. Express the hardness of the water in ppm of CaCO3.
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In a Complexometric Titration Experiment, the preparation of the EDTA solution is as follows: In a 250 mL beaker, weigh 0.10 g MgCl2*6H2O and 1.0 g NaOH. Add approximately 200 mL distilled water and stir to dissolve. Add about 2.0 g of EDTA and transfer the solution quantitatively to a 1-L volumetric flask. Dilute to the mark with distilled water. What is the purpose of adding MgCl2*6H2O? Please show COMPLETE solution.
Titration of Ca²+ and Mg²+ in a 50.00-mL hard water sample required 23.65 mL of 0.01205 M EDTA. A second 50.00-mL aliquot was made strongly basic with NaOH to precipitate Mg²+ as Mg(OH)2(s). The supernatant liquid was titrated with 14.53 mL of the EDTA solution. Calculate the total hardness of the water sample, expressed as ppm CaCO3.
A freshwater sample containing Ca2+ and Mg2+ will be analyzed using EDTA titration. The EDTA titrant was standardized by dissolving 0.5005g of CaCO3 (99.00% purity) in 100.0mL. A 10.00-mL aliquot was then titrated using 24.93 mL of EDTA titrant to the Eriochrome Black T endpoint. A sample with a volume of 250.00 mL is titrated with 20.32 mL of the EDTA titrant in an ammonia buffer at pH 10.00. Another 250.00 mL sample was then treated with NaOH to precipitate Mg(OH)2 and was then titrated at pH 13.00 with 10.43 mL using the same EDTA solution. FW: CaCO3 (100.09 g/mol) & MgCO3 (84.314 g/mol) Questions: Find concentration of EDTA titrant in M. Calculate the Amount of CaCO3 and MgCO3 in the sample. Express your answers in moles and ppm of each compound.
A freshwater sample containing Ca2+ and Mg2+ will be analyzed using EDTA titration. The EDTA titrant was standardized by dissolving 0.5005g of CaCO3 (99.00% purity) in 100.0mL. A 10.00-mL aliquot was then titrated using 24.93 mL of EDTA titrant to the Eriochrome Black T endpoint. A sample with a volume of 250.00 mL is titrated with 20.32 mL of the EDTA titrant in an ammonia buffer at pH 10.00. Another 250.00 mL sample was then treated with NaOH to precipitate Mg(OH)2 and was then titrated at pH 13.00 with 10.43 mL using the same EDTA solution. FW: CaCO3 (100.09 g/mol) & MgCO3 (84.314 g/mol) c. What is the total hardness of the water sample expressed as ppm CaCO3. Total hardness = ____ ppm CaCO3
A freshwater sample containing Ca2+ and Mg2+ will be analyzed using EDTA titration. The EDTA titrant was standardized by dissolving 0.5005g of CaCO3 (99.00% purity) in 100.0mL. A 10.00-mL aliquot was then titrated using 24.93 mL of EDTA titrant to the Eriochrome Black T endpoint. A sample with a volume of 250.00 mL is titrated with 20.32 mL of the EDTA titrant in an ammonia buffer at pH 10.00. Another 250.00 mL sample was then treated with NaOH to precipitate Mg(OH)2 and was then titrated at pH 13.00 with 10.43 mL using the same EDTA solution. FW: CaCO3 (100.09 g/mol) & MgCO3 (84.314 g/mol) a. What is the concentration of the EDTA titrant? b. Calculate the Amount of CaCO3 and MgCO3 in the sample. Express your answers in ppm of each compound. mol Ca2+ = _____ mol mol Mg2+ = _____ mol [Ca2+] = ______ ppm CaCO3 [Mg2+] = ______ ppm CaCO3
A freshwater sample containing Ca2+ and Mg2+ will be analyzed using EDTA titration. The EDTA titrant was standardized by dissolving 0.5005g of CaCO3 (99.00% purity) in 100.0mL. A 10.00-mL aliquot was then titrated using 24.93 mL of EDTA titrant to the Eriochrome Black T endpoint. A sample with a volume of 250.00 mL is titrated with 20.32 mL of the EDTA titrant in an ammonia buffer at pH 10.00. Another 250.00 mL sample was then treated with NaOH to precipitate Mg(OH)2 and was then titrated at pH 13.00 with 10.43 mL using the same EDTA solution. FW: CaCO3 (100.09 g/mol) & MgCO3 (84.314 g/mol) Question: What is the concentration of EDTA titrant in M?