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____ forms complex with EDTA
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- 0.9350g of an impure solid containing oxalic acid was dissolved and diluted to 100.00mL. From this bulksolution 8.00mL samples were titrated with 0.01267M KMnO4, resulting in an average titration volumeof 24.55mL. The molar mass of oxalic acid is 90.0349 g/mol. determine the mass %! Thank you!6.30 g sample containing tellerium is dissolved and 47 mL of 0.03 M K2Cr2O7 is added. After the reaction is complete, excess Cr2O72- is back-titrated with 11 mL of 0.105 M Fe2+. Find the percent by mass of TeO2 in the sample.How many mL of 0.1200 M KSCN will be needed in the back titration after addition of 30 mL 0.110 M AgNO3 solution to 0.3655g KI dissolved in 100 mL water? a. 1.1951 mL b. 5.1919 mL c. 9.1519 mL d. 1.5911 mL
- A 50.00 mL sample of hard water is titrated with 0.0102 M EDTA solution (volume of blank titration= 1.5 mL) and the volume of EDTA required is 22.44mL. What is the water hardness in ppm CaCO3?The end point of a titration was reached after 22.2 mL22.2 mL of 0.050 M0.050 M disodium EDTA titrant was dispensed into a solution containing the zinc ion. Calculate the moles of disodium EDTA used. moles of disodium EDTA: = molA 0.7980-g sample of chloride was titrated using the Fajans method and required 45.32 mL of 0.1046 M AgNO3. Calculate for % Cl (MM=35.45).
- A solid sample containing chloride and with a mass equal to 6.000 g was dissolved in water and transferred to a 100.0 ml flask. A 50.0 mL aliquot of this solution was diluted to 250.0 mL. In the titration of 20.0 mL of the diluted solution, 32.0 mL of 0.2000 mol L-1 AgNO3 standard solution were used. Calculate the % of impurities in the analyzed sample. Data: Cl = 35.45Thiourea, (NH2)2CS, forms highly insoluble compounds with mercury. Therefore, the amount of thiourea in a sample can be determined by titration with mercuric ion in a reaction that can be described by: 4(NH2)2CS(aq) + Hg2+(aq) → [(NH2)2CS]4Hg2+(s) A 0.951 2-g sample containing thiourea (FM 76.12) required 14.88 mL of 4.752 mM Hg2+ to reach the end point. Calculate the mass percent of thiourea in the sample.A. What is the characteristic color of ferric ions in solution? B. Why is the titration of the oxalate in the green salt with KMnO4 performed prior to carrying out the redox titration for iron content? (Why can’t you do them the other way – iron first then oxalate?) C. In a titration using 0.02000 M KMnO4 solution, the following data were obtained: Buret readings: FINAL = 15.31 mL INITIAL = 5.02 mL How many moles of KMnO4 were used?
- Determine the % w/w chloride in the sample. A 0.3285 g sample containing chloride and inert material is titrated with 0.1012 M AgNO3, requiring 34.99 mL to reach the Ag2CrO4 end point. Titration of a blank sample consumes 0.32 mL of the AgNO3 titrant.1. A copper(II) sulfate solution of unknown concentration is placed in a colorimeter and an absorbance reading of 0.46 is recorded. Using the same solution cell, a 0.055 Μ solution of copper(II) sulfate gives an absorbance reading of 0.34. What is the concentration of the first solution? Write only the value. 2. A given 5.0g impure sample of sodium carbonate was titrated via 0.1500N HCl. The sample utilized 31.55 ml of 0.1500N HCl. What is the percentage of sodium carbonate is in the sample?Calculate the volume of 0.0407 M EDTA needed to titrate the Ca in a 0.1622 g CaCO3 (MM = 100.0869 g/mol).