What was done to ensure that there are no morechloride ions present in the precipitate?Addition of A&NO, to the precipitateA washings and checking if the washingsbecome cloudyEvaporation of the chloride ions byBheating the precipitate in a crucibleFiltration using an ashless filter paper totrap the chloride ions on the paperAddition of more HCl and testing if theDsolution becomes acidic

Here we have to choose the correct method to ensure that there are no more chloride ions present in…

What was done to ensure that there are no more chloride ions present in the precipitate? Addition of AgNO, to the precipitate A washings and checking if the washings become cloudy Evaporation of the chloride ions by В heating the precipitate in a crucible Filtration using an ashless filter paper to trap the chloride ions on the paper Addition of more HCl and testing if the D solution becomes acidic

What was done to ensure that there are no more chloride ions present in the precipitate? Addition of AgNO, to the precipitate A washings and checking if the washings become cloudy Evaporation of the chloride ions by В heating the precipitate in a crucible Filtration using an ashless filter paper to trap the chloride ions on the paper Addition of more HCl and testing if the D solution becomes acidic

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter20: Applications Of Oxidation/reduction Titrations

Section: Chapter Questions

Problem 20.26QAP

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While working in a metal processing facility, Letlen had accidentally mixed two metal vatstogether creating an alloy. One vat was labeled for cadmium, while the other was not. It canbe assumed that these are of pure metal composition. To identify this metal, Letlen took 1.000 g of the homogenous alloy sample composed ofcadmium and the unknown metal, dissolved, and diluted it to exactly 100.0 mL in avolumetric flask. A 20.00-mL aliquot was taken and titrated this using 22.82 mL of 0.05000M EDTA. In a second 20.00-mL aliquot, the Cd was masked through the addition of HCN/NaCN buffer.The titration of the unknown metal in the aliquot required 15.13 mL of EDTA.MW: Cd (112.411 g/mol) a. Calculate the moles of Cd and the moles of unknown metal in the 20.00-mL aliquot.b. Calculate the moles of Cd and the moles of unknown metal in the sample.
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Which characteristic of a precipitate doesn’t do well for gravimetric analysis. a Readily filtered and washed free of contaminants b Of sufficiently high solubility (Ksp) c Unreactive with constituents of the atmosphere and high purity d Of known composition after it is dried or, if necessary, ignited. e None of the above
The sulfur content of insoluble sulfides that do not readilydissolve in acid can be measured by oxidation with Br2to SO42.25Metal ions are then replaced with Hby an ion-exchange column,and sulfate is precipitated as BaSO4with a known excess ofBaCl2. The excess Ba2is then titrated with EDTA to determinehow much was present. (To make the indicator end point clearer,a small, known quantity of Zn2also is added. The EDTA titratesboth the Ba2and the Zn2.) Knowing the excess Ba2, we cancalculate how much sulfur was in the original material. To analyzethe mineral sphalerite (ZnS, FM 97.46), 5.89 mg of powderedsolid were suspended in a mixture of CCl4and H2O containing1.5 mmol Br2. After 1 h at 20 C and 2 h at 50 C, the powder dis-solved and the solvent and excess Br2were removed by heating.The residue was dissolved in 3 mL of water and passed throughan ion-exchange column to replace Zn2with H. Then 5.000 mLof 0.014 63 M BaCl2were added to precipitate all sulfate as BaSO4.After the addition of…
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