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

Principles of Instrumental Analysis

7th Edition

ISBN:9781305577213

Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Chapter15: Molecular Luminescence Spectrometry

Section: Chapter Questions

Problem 15.10QAP

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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 __________ %?
A 5.00 mL tap water sample was measured out with a volumetric pipette, and added to a 25 mL Erlenmeyer flask. It was then titrated with a 0.0100 M Na2EDTA.2H2O solution, and found to take 0.635 mL of the EDTA solution to reach the blue endpoint. How many moles of the 0.0100 M Na2EDTA.2H2O were added in the titration reaction? Show calculation. How many moles of calcium ions were reacted? Show calculation.
Five white, 500-mg uncoated ascorbic acid (AA) tablets with an average weight of 0.6100-g were pulverized in a mortar. A sample of the powdered ascorbic acid weighing 0.4610-g was placed in an iodine flask and was dissolved in 50-mL H2SO4 then 5-g of KBr was added to the resulting solution. The solution was titrated with 46.73-mL of 0.0152 M STD. KBrO3 to reach a faint yellow endpoint then 3-g KI and 5-mL Starch TS. The blue color solution is then titrated with 2.78-mL of 0.1047 M STD. Na2S2O3 to reach the disappearance of the blue iodostarch complex. MW: KBrO3 = 167.0 ; KIO3 = 214.0 ; Na2S2O3 = 158.11 ; C6H8O6 = 176.12 Compute the milligrams of pure AA per tablet from the assay. None of the choices 349.7 mg 264.3 mg 462.7 mg
A CaCO3 solution that will be used to standardize EDTA was prepared by dissolving 3.1251 g of solid CaCO3 in 100 mL dilute HCl. 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
A 47.6 mL aliquot from a 0.5 L solution that contains 0.45g of MnSO4 (MW is 151 g/mol) required 41.9 mL of an EDTA solution to reach the titration endpoint. What mass of CaCO3 (MW is 100.09 g/mol) will react with 1.58 mL of the EDTA solution?
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
Traces of aniline can be determined by reaction with an excess of electrolytically generated Br2: C6H5NH2 + 3Br2 =====è C6H2Br3NH2 + 3H+ + 3Br- The polarity of the working electrode is then reversed, and the excess bromine is determined by a coulometric titration involving the generation of Cu(I): Br2 + 2Cu+ ===è 2Br- + 2Cu2+ Suitbale quantities of KBr and copper (II) sulfate were added to a 25.0 ml sample containing aniline (C6H5NH2). Calculate the mass in micrograms of C6H5NH2 in the sample from the accompanying data. Working electrode Functioning as Generation Time (min) with a constant current of 1.00 mA Anode 3.76 cathode 0.270
A 2.00 mL sample of commercial bleach was diluted with water to a 100.00 mL volumetric flask. A 20.00 mL aliquot of the diluted sample was treated with excess KI. The liberated iodine was titrated with 0.1050 M Na2S2O3, requiring 12.5 mL to reach the starch indicator end point. Calculate the % w/v NaOCl in the sample.
A 5.00 mL tap water sample was measured out with a volumetric pipette, and added to a 25 mL Erlenmeyer flask. It was then titrated with a 0.0100 M Na2EDTA.2H2O solution, and found to take 0.635 mL of the EDTA solution to reach the blue endpoint. a.) How many moles of the 0.0100 M Na2EDTA.2H2O were added in the titration reaction? Show calculation. b.) How many moles of calcium ions were reacted?
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
1. How much volume (mL) is needed to standardize 0.05M of EDTA using 180mg of magnesium ribbon? MW: 24g/mol2. How many grams of EDTA is required to prepare 250mL of a 0.05M solution? MW: 292g/mol3. What is the Molarity of the EDTA solution if 35mL of the titrant was added to 0.2g of calcium carbonate? Round off to four decimal places
The buret was filled with 0.100 M HCl solution. Then was transferred in a 25.0 mL of saturated calcium hydroxide solution (2g of calcium hydroxide per 100 ml of water) in two separate E-flasks. Then 2 drops of phenolphthalein was added to each flask Titration data for the determination of solubility and Ksp of calcium hydroxide: Trial 2: Final Buret reading (ml)-26.10; Initial Buret reading (ml)- 19.80; Temperature (Celcius)- 25 Voume of HCl used: Trial 2- 6.30mL 1. Compute for the moles of H+ used and the moles of OH- present. moles of H+ used = (concentration of HCl) × (volume of HCl used)moles of OH- = moles of H+ used 2. Construct an ICE table for the reaction.3. Calculate the molar solubility (in mol/L) of OH- and Ca2+.4. Determine the solubility of Ca(OH)2 in g/L. (MM of Ca(OH)2 = 74.096 g/mol). 5. Calculate the Ksp of Ca(OH)26. Compute for the percent error of the experimental value for Ksp of Ca(OH)2 with the literature…