0.4545 g CaCO3 was dissolved in HCl and the resulting solution was diluted to 0.25 L. Twenty-five mL aliquot of this solution required 35.2 mL of EDTA upon performing titrimetric analysis. Determine the molarity of EDTA
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0.4545 g CaCO3 was dissolved in HCl and the resulting solution was diluted to 0.25 L. Twenty-five mL aliquot of this solution required 35.2 mL of EDTA upon performing titrimetric analysis. Determine the molarity of EDTA
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- An EDTA solution was prepared by dissolving approximately 3 grams of Na2H2Y•H2O in sufficient water to give 1 liter of solution. This solution was then standardized against 50.00 mL aliquots of 0.004517 molar Mg2+. An average titration volume of 32.22 mL was required. Determine the molar concentration of EDTA.A 0.7352g sample of ore containing Fe3+, Al3+ and Sr2+ was dissolved and made up to 500.00 mL. The analysis of metals was performed by a chemistry using complexation volumetry. Initially, an aliquot of 50.00 mL had its pH adjusted to 1.0 and titrated with a standard solution of EDTA 0.02145 mol/L, requiring 6.95 mL to reach the end point. Subsequently, another 25.00 mL aliquot was buffered at pH=5 and titrated with the same EDTA solution, requiring 6.24 mL to reach the end point. Finally, a third aliquot of 25.00 mL was titrated at pH=11, requiring 11.10 mL of the same EDTA solution to complete the titration. Determine the percentage of each of the metals in the sample Given the molar masses: Fe=55.845 g/mol; Al=26.982 g/mol and Sr=87.620 g/mol.The Zn in a 0.7556-g sample of foot powder was titrated with 21.27 mL of 0.01645 M EDTA. Calculate the percentage of Zn in this sample. A silver nitrate solution contains 14.77 g of primary-standard grade AgNO3 in 1.00 L. What volume of this solution will be needed to react with 0.2631 g of NaCl.
- An EDTA solution was allowed to react with Pb²⁺ to produce 0.25 M PbY²⁻, 2.67×10⁻⁸ M Pb²⁺ and an excess of 0.10 M at equilibrium (K = 1.1×10⁸). What will be the hydronium ion concentration of the resulting solution?As part of a geological team that studied a local cave, you brought with you a bunch of 1.00 g rock samples to be studied. Each rock was prepared and titrated against 0.050 M EDTA. a. Calculate the percent calcite (CaCO3) content of rock A if it was titrated with 48.0 mL EDTAChromel is an alloy composed of nickel, iron and chromium.A 0.6472 g sample was dissolved and diluted to 250 mL. When a50 mL aliquot of 0.05182 M EDTA was mixed with an equal volumeof the diluted sample and all the three ions were chelated, a 5.11 mLback titration with 0.06241 M copper (II) was required.The chromium in a second 50 mL aliquot was masked through theaddition of hexamethylenetetramine, titration of the Fe and Nirequired 36.28 mL of 0.05182 M EDTA.Iron and chromium were masked with pyrophosphate in a third50 mL aliquot and the nickel was titrated with 25.91 mL of theEDTA solution.Calculate the percentage of nickel, chromium and iron in thealloy.
- 0.28g 0f MBr is dissolved in distilled water and made up to 250mL mark in a volumetric flask. 25 mL of this solution is titrated against 0.019 M silver nitrate solution using eosin as indicator. The end point was obtained at 12.4 mL of AgNO3 solution . Calculate the molar mass of the metal bromide.A solution was prepared by dissolving about 30.00m g of EDTA in approximately 1 L of water and standardizing against 50.00-mL aliquots of 0.004356 M Mg2+. An average titration of 32.65 mL was required. Calculate the molar concentration of the EDTA.Calamine, which is used for relief of skin irritations, is a mixture of zinc and iron oxides. A 1.022-g sample of dried calamine was dissolved in acid and diluted to 250.0 mL. A 50.00 mL aliquot was suitably buffered and titrated with 2.40 mL of 0.002727 M ZnY-2 (Zn-EDTA) solution to allow the following reaction: Fe+3 + ZnY-2 → FeY- + Zn+2. Molecular mass: Fe2O3 = 165.74 a. The weight of sample in the aliquot portion is _________g ? b. the percentage composition of Fe2O3 in the sample is ______ % ?
- A 0.2431 g sample of CaCO3 is dissolved in 6 M HCl and the resulting solution is diluted to 250.0 mL in a volumetric flask. Titration of a 25.00 mL sample of the solution requires 28.55 mL of EDTA to reach the Eriochrome Black T endpoint. A blank containing the same amount of Mg2+ requires 2.60 mL of EDTA. What is the molarity of the EDTA solution?A 0.5745 g sample of an alloy containing principally bismuth and lead is dissolved in nitric acid and diluted to 250.0 mL in a volumetric flask. A 50.00 mL aliquot is withdrawn, the pH adjusted to 1.5, and the bismuth titrated with 30.26 mL of 0.01024 M EDTA. The pH of the solution is then increased to 5.0 and the lead titrated with 20.42 mL of the same EDTA solution. Calculate the percentages of lead and bismuth in the alloy.Chromel is an alloy composed of nickel, iron and chromium. A 0.6553-g sample was dissolved and diluted to 250.0 mL. When a 50.00-mL aliquot of 0.05173 M EDTA was mixed with an equal volume of the diluted sample, all three ions were chelated, and a 5.34-mL back titration with 0.06139 M copper (II) was required.The chromium in a second 50.0-mL aliquot was masked through the addition of hexamethylenetetramine; titration of the Fe and Ni required 36.98 mL of 0.05173M EDTA. Iron and chromium were masked with pyrophosphate in a third 50.00-mL aliquot, and the nickel was titrated with 24.53 mL of the EDTA solution. Calculate the percentage of Cr in the alloy. Express your answer in 2 decimal places.