A 100.0 mL sample containing Zn2+ was treated with 50.0 mL of 0.0500 M EDTA to complex all the Zn2+ and leave excess EDTA in solution. The excess EDTA was then back titrated, requiring 10.00 mL of 0.0500 M Mg2+. What was the concentration of Zn2+ in the original solution?
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- A 25.00 mL sample containing Fe3+ was treated with 10.00 mL of 0.03676 M EDTA to complex all the Fe3+ and leave excess EDTA in solution. The excess EDTA was then back-titrated, requiring 2.37 mL of 0.04615 M Mg2+. What was the concentration of Fe3+ in the original solution in ppm Fe3+?Chromel is an alloy composed of nickel, iron, and chromium. A 0.6418-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 5.27-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 35.81 mL of 0.05173 M EDTA. Iron and chromium were masked with pyrophosphate in a third 50.0-mL aliquot, and the nickel was titrated with 25.77 mL of the EDTA solution. Calculate the percentages of nickel, chromium, and iron in the alloy. Percentage of nickel = % Percentage of iron = Percentage of chromium = % %A 50.00 mL solution containing Ni2+ and Fe2+ was treated EDTA to bind all the metal ions. After back titration, the amount of EDTA used is 2.500 mmol. In another 50.00 mL solution was added pyrophosphate to mask the Fe2+ ions, and the solution required 25.00 mL of 0.04500 M EDTA. Calculate the ppm Fe (55.85 g/mol) in the solution.
- The Cr metal was dissolved in HCl. The pH was suitably adjusted by adding ammnoniaammonium buffer solution and 15.00 mL of 0.01768 M EDTA were introduced. The excess reagent required a 4.30-mL back-titration with 0.008120 M Cu2+. Calculate mass of Cr metal.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.3. A 50.00 mL solution containing Ni2+ and Fe2+ was treated EDTA to bind all the metal ions. After back-titration, the amount of EDTA used is 2.500 mmol. In another 50.00 mL solution was added pyrophosphate to mask the Fe2+ ions, and the solution required 25.00 mL of 0.04500 M EDTA. Calculate the ppm Fe (55.85 g/mol) in the solution.
- 25.0 mL of an unknown Ni2+ solution was treated with 25.00 mL of 0.05283 M Na2EDTA. The pH of the solution was buffered to 5.5 and then back-titrated with 17.61 mL of 0.02299 M Zn2+. What was the unknown Ni2+ M?EXAMPLE: Chromium(III) is slow to react with EDTA (H4Y) and is therefore determined by back-titration. A pharmaceutical preparation containing chromium(III) is analyzed by treating a 2.63g sample with 5mL of (0.0103M) EDTA. Following reaction, the unreacted EDTA is back-titrated with 1.32mL of (0.0112M) zinc solution. What is the percent chromium chloride in the pharmaceutical preparation?Determine the concentration of [Zn²+] in the complexometric titration of Zn2+ with EDTA, where 15.00 mL of 0.0525 M EDTA was used in the 25.00 mL of sample solution. 1.58 x 10-2 M 0.7875 M 0.0315 M 0.0630 M
- The cadmium and lead ions in a 50.00 mL sample required 40.09 mL of a 0.005000 M EDTA for titration. A 75.00 mL portion of the same sample was made basic and treated with excess KCN masking the cadmium as Cd(CN)42-. This solution required 21.42 mL of the EDTA for titration. Calculate the concentration of Cd2+ and Pb2+ in the sample ppm and in M.Calculate the pZn of a solution prepared by mixing 25.0 mL of 0.0100 M EDTA with 50.0 mL of 0.00500 M Zn2+. Assume that both the Zn2+ and EDTA solutions are buffered with 0.100 M NH3 and 0.176 M NH4Cl.Calculate PCa of the solution that results when 50.0 mL of 0.0050 M Ca2+ is titrated with 25.00 mL of 0.0100 M EDTA in a solution buffered to a conastant pH of 10.00.