The Tl in a 9.76-g sample of rodenticide was oxidized to the trivalent state and treated with an unmeasured excess of Mg/EDTA solution. The reaction is Tl+3 + MgY-2 → TlY- + Mg+2 Titration of the liberated Mg2+ required 15.34-mL of 0.08560 N EDTA. The type of titration involved in the assay is ___ (direct/indirect/residual) and the percentage of Tl2SO4 in the sample is ____%. Molecular mass: Tl2SO4 = 504.8

The Tl in a 9.76-g sample of rodenticide was oxidized to the trivalent state and treated with an unmeasured excess of Mg/EDTA solution. The reaction is Tl+3 + MgY-2 → TlY- + Mg+2 Titration of the liberated Mg2+ required 15.34-mL of 0.08560 N EDTA. The type of titration involved in the assay is _ (direct/indirect/residual) and the percentage of Tl2SO4 in the sample is __%. Molecular mass: Tl2SO4 = 504.8

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter10: Potentiometry And Redox Titrations

Section: Chapter Questions

Problem 8P

See similar textbooks

Similar questions

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
The ethyl acetate concentration in an alcoholic solution was determined by diluting a 10.00-mL sample to 100.00 mL. A 20.00-mL portion of the diluted solution was refluxed with 40.00 mL of 0.04672 M KOH:CH3COOC2H5 + OH- → CH3COO- + C2H5OHAfter cooling, the excess OH2 was back-titrated with 3.41 mL of 0.05042 M H2SO4. Calculate theamount of ethyl acetate (88.11 g/mol) in the original sample in grams
A sample of pure CaCO3 (FW= 100.1 g/mol) weighing 0.350g was dissolved in concentrated HCI (MW= 36.45 g/mol) and diluted to 250mL in a volumetric flask. A 50.0mL aliquot required 35.00mL of an EDTA solution for titration. A 5.0-mL water sample to be analysed for its hardness was diluted to 250mL. A 10.00mL aliquot required 24.50mL of the EDTA solution to reach the EBT endpoint. 1. Calculate the molarity of the EDTA solution. 2. Calculate the water hardness in pm CaCO3.
The Kjedahl procedure was used to analyze 256 µL of a solution containing 37.9 mg protein/mL. The liberated NH3 was collected in 5.00 mL of 0.033 6 M HCl, and the remaining acid required 6.34 mL of 0.010 M NaOH for complete titration. What is the weight percent of nitrogen in the protein? wt%
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
25.00 mL aliquots of the solution in problem 1 are titrated with EDTA to the calmagite end point. A blank containing a small measured amount of Mg^2+ requires 2.12 mL of the EDTA to reach the end point. An aliquot to which the same amount of Mg^2+ is added requires 25.88 mL of the EDTA to reach the end point.
Titration of Ca2+ and Mg2+ in a 50.00 mL sample of hard water 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 , filtered, and titrated with 14.53 mL of same EDTA solution. Calculate the ff: a.)The total hardness of water sample. b.)Concentration in ppm CaCO3 in the sample. c.)Concentration in ppm MgCO3 in the sample
A 10.0 mL sample containing Fe³⁺ and Cu²⁺ was diluted to 100.0 mL solution. A 20.0 ml aliquot required 25.0 ml of 0.0500 M EDTA for complete titration. A separate 20.0 ml aliquot of the diluted sample was treated with NH₄F to protect the Fe³⁺. Then the Cu²⁺ was treated with thiourea. Upon addition of 25.0 mL of 0.0500 M EDTA, the Fe³⁺ was liberated from its fluoride complex and formed an EDTA complex. The excess EDTA required 21.5 mL of 0.0180 M Pb²⁺ to reach an end point, using xylenol orange. (a) Identify the masking agent. (b) Identify the auxiliary complexing agent. (c) Calculate the molar concentration of the Fe³⁺ in the original sample. (d) Calculate the molar concentration of the Cu²⁺ in the original sample
What is the mass of pure dry CaCO3 (MW: 100.0869 g/mol) standard used in the standardization of EDTA solution? Assume that 1.758 M EDTA solution was computed based on the titration of CaCO3 standard. The volume of titrant needed to reach the endpoint was 35.00 mL. Ca2+ + Y4- → CaY2- 0.1500 g 5.630 g 6.158 g 0.6158 g
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 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.
The Tl in a 9.76-g sample of rodenticide was oxidized to the trivalent state and treated with an unmeasured excess of Mg/EDTA solution. The reaction is Tl+3 + MgY-2 → TlY- + Mg+2 . Molecular mass: Tl2SO4 = 504.8 a. Titration of the liberated Mg2+ required 13.34-mL of 0.03560 N EDTA. The type of titration involved in the assay is (direct/indirect/residual) __________ ? b. percentage of Tl2SO4 in the sample is ______________% ?