Mass of KxFe(C2O4)y · zH2O : 4.70 g Mass of sample : 0.175 g Mass of FeCl3 used in preparation : 1.60 g Molarity of standard NaOH used : 0.100 V1, volume of standard NaOH required for first equivalence point : 7.750 mL V2, volume of standard NaOH required for second equivalence point : 19.70 mL Calculate the percent of potassium in the sample :

Mass of KxFe(C2O4)y · zH2O : 4.70 g Mass of sample : 0.175 g Mass of FeCl3 used in preparation : 1.60 g Molarity of standard NaOH used : 0.100 V1, volume of standard NaOH required for first equivalence point : 7.750 mL V2, volume of standard NaOH required for second equivalence point : 19.70 mL Calculate the percent of potassium in the sample :

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter17: Complexation And Precipitation Reactions And Titrations

Section: Chapter Questions

Problem 17.34QAP

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Mass of KxFe(C2O4)y · zH2O : 4.70 g Mass of sample : 0.175 g Mass of FeCl3 used in preparation : 1.60 g Molarity of standard NaOH used : 0.100 V1, volume of standard NaOH required for first equivalence point : 7.750 mL V2, volume of standard NaOH required for second equivalence point : 19.70 mL Calculate the volume of standard NaOH that reacted with iron :
A pink solid has the formula CoCl3 5NH3 H2O. A solution of this salt is also pink and rapidly precipitates 3mol AgCl(s) on titration with silver nitrate solution. When the pink solid is heated, it loses 1mol H2O to give a purple solid with the same mole ratio of NH3:Cl:Co as the pink solid. The purple solid releases two of its chloride ions rapidly; then on dissolution and titration with AgNO3, release one of its chloride ions slowly. Deduce the structures, draw and name 2 octhahedral complexes
0.4545 g CaCO3 was dissolved in HCl and the resulting solution was diluted to 0.25 L. Twenty-five mL aliquot of this solution required 35.2 mL of EDTA upon performing titrimetric analysis. Determine the mass of NaH2Y·2H2O to prepare 0.5 L titrant solution. NaH2Y·2H2O is a cmpound with MW = 372.2 g/mol Note: H2Y2- = EDTA
What mass of solid Lanthanum (III) oxalate nonahydrate { La2 ( C2O4 )3 ∙ 9 H2O } can be obtained from 650 mL of 0.0170 M aqueous solution of LaCl3 by adding a stoichiometric amount of sodium oxalate ? with solution/explanation
A 5.70 g iron ore was dissolved in concentrated HCL After the dissolution, the resulting solution was made basic by adding 6.0 M NaOH slowly until the solution is slightly turbid. Urea was then added and the solution was heated for 3 hours. The precipitate was filtered using an ashless filter paper and ignited to form Fe2O3 (159.69 L /mol The mass of precipitate is 2.1g. Find the % Fe3O4 (231.54 c/mol) in the iron are sample.
Choose standard substance for standardization of titrant for argentometric titration: NaCl; Na,S½O3; Zn; H,C,O4•2H2O;
a) What mass of Fe(NH4)2(SO4)2•2H2O(s) is required to prepare a 500 mL solution containing 100 ppm (m:v) in Fe? b) Using this stock solution, what aliquot must be used to prepare calibration solutions, 100 mL volume, of the following concentrations: 0.100 ppm, 0.500 ppm, 2.00 ppm, 4.00 ppm, and 7.00 ppm.
A 2.559 g sample containing both Fe and V was dissolved under conditions that converted the elements to Fe(III) and V(V). The solution was diluted to 500.0 mL and a 50.0 mL aliquot was passed through a Walden 4+ reductor and titrated with 17.74 mL of 0.100 M Ce . A second 50.0 mL aliquot was passed through a Jones reductor and required 44.67 mL of the same Ce4+ solution to reach an endpoint. Calculate the percentage of Fe2O3 and V2O5 in the sample.
Explain why K2CrO4 is used as an indicator in Argentometric titration?
A 4.912-g sample of a petroleum product was burnedin a tube furnace, and the SO2produced was collectedin 3% H2O2.Reaction:SO2(g)+H2O2→H2SO4A 25.00-mL portion of 0.00873 M NaOH was introducedinto the solution of H2SO4, following whichthe excess base was back-titrated with 15.17 mL of0.01102 M HCl. Calculate the sulfur concentrationin the sample in parts per million.
A 0.951-g sample containing (NH4)2C2O4 and compounds was dissolved in water and made alkaline with KOH. The liberated ammonia was distilled into 50.00 mL of 0.1007 N H2SO4. The excess H2SO4 was back titrated with 11.13 mL of 0.1214 N NaOH. Calculate the percentage of nitrogen in the sample.
A 1.000-g sample containing bromide was dissolved in sufficient water to give 100.0 mL. A 50.00 mL aliquot was measured and after acidification, silver nitrate was introduced to precipitate AgBr, which was filtered, washed, and then dissolved in an ammoniacal solution of potassium tetracyanonickelate(II): Ni(CN)42- + 2AgBr(s) → 2Ag(CN)2- + Ni2+ + 2Br- The liberated nickel ion required 11.70 mL of 0.002146 M EDTA. Calculate mmol Ni in the 50.00 mL aliquot. Calculate mmol Br- in the 50.00 mL aliquot. Calculate the percentage of NaBr (102.894) in the 1.000 g sample.