Solutions of cobalt (II) ions have a magenta color with a molar absorptivity constant (e) value at 511 nm of 5.87 M-1cm-1. A 0.500 mL sample is transferred from a 50.0 mL stock solution of Co(NO3)2 and diluted with water to a final volume of 7.50 mL. The dilution had an absorbance value at 511 nm in a standard c

Solutions of cobalt (II) ions have a magenta color with a molar absorptivity constant (e) value at 511 nm of 5.87 M-1cm-1. A 0.500 mL sample is transferred from a 50.0 mL stock solution of Co(NO3)2 and diluted with water to a final volume of 7.50 mL. The dilution had an absorbance value at 511 nm in a standard c

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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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.
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 3650-mg sample containing bromate and bromide was dissolved in sufficient water to give 250.0 mL. After acidification, silver nitrate was added to a 25.00 mL aliquot where the resulting precipitate was filtered, washed and then redissolved in an ammoniacal solution of potassium tetracyanonickelate(II) according to the reaction: Ni(CN), + 2 AgBr) → 2 Ag(CN), + Ni? + 2 Br The liberated nickel ion required 26.73 mL of 0.02089 M EDTA. The bromate ion in a 10.00 mL aliquot was reduced to bromide with As* prior to the addition of silver nitrate. The same procedure was followed and the released nickel ion was titrated with 21.94 mL of the EDTA solution. Calculate the percentage of impurity in the sample. Br (79.904) a. 24.45% b.34.38% c. 41.17% d. 65.62%
Gold can be determined in solutions containing high concentrations of diverse ions by ICP. Aliquots of 50.0 mL of the sample solution were transferred to each of four 100.0 mL volumetric flasks. A solution was prepared containing 10.0 mg/L Au in 20% H2SO4, and quantities of this solutions were added to the sample solution to give 0, 2.5, 5 and 10 mg/L added Au in each of the flask. The solutions were made up to a total volume of 100.0 mL, mixed and analyzed by ICP. The resulting data are presented in the following table: Added Au (mg/L) Emission Intensity (Counts) 0.0 12568 2.5 19324 5.0 26622 10.0 40021 a) Attach an excel graph for the determination showing the X intercept. b) Calculate the concentration of gold in the sample, report with its uncertainty. c) The known concentration of gold in the sample is 8.51 mg/L. Test the hypothesis that your result is equal to this value at the 95% confidence level. l
A cyanide solution with a volume of 13.72 mL was treated with 25.00 mL of Ni2+ solution(which contained an excess of Ni(II) ions) to convert the cyanide to the complex ion tetracyanonickelate(II): 4CN- + Ni2+ → 6 Ni(CN)2- The excess Ni 2+ was then titrated with 10.15 mL of 0.01307 M EDTA. One mole of this reagent reacts with one mole of Ni(II) as follows: Ni(CN)42- does not react with EDTA. If 39.35 mL of EDTA was required to react with 30.10 mL of the original Ni 2+ solution, calculate the molarity of CN- in the 13.72 mL cyanide sample.
The phosphate in a 3.000 g sample of industrial detergent was precipitated by the addition of 1.000 g of AgNO3. The solution was filtered and the filtrate required 18.23 mL of 0.1377 M KSCN for titration to the FeSCN2+ end point. Calculate the percentage of phosphate in the detergent.
A solution was prepared by dissolving 1210 mg of K3Fe(CN)6 (329.2 g/mol) in sufficient water to give 775 mL. Calculate(a) the molar analytical concentration of K3Fe(CN)6.(b) the molar concentration of K+.(c) the molar concentration of Fe(CN)63-.(d) the weight/volume percentage of K3Fe(CN)6.(e) the number of millimoles of K+ in 50.0 mL of this solution.(f) ppm Fe(CN)63- .(g) pK for the solution.(h) pFe(CN)6 for the solution.
0.1745 g of primary standard Na2C2O4 is used to set a freshly prepared KMnO4 solution and 30.24 mL of KMnO4 solution is spent at the turning point. Since 36.92 mL of this KMnO4 solution is consumed for the determination of iron in 0.5618 g ore sample, calculate the amount of iron in the ore in terms of % iron (III) oxide and % iron (III) chloride. (Fe: 56, K: 39, Mn: 55, O: 16, Na:23, C: 12, Cl: 35.5 g/mol) (Please type answer)
A 1.000-g sample containing KHC204, H2C204, and impurities required 38.22 mL of 0.1000 M NaOH for acid-base titration. Another 1.000-g sample required 27.02 mLof 0.04000 M KMNO, for redox titration in acid solution, according to the following reaction: Mno, + 5C,0,2- + 16H* 2 2MN2* + 10co, + 8H,0 How many mmols of KHC,0, are there in the sample? 1.351 mmols KHC204 1.582 mmols KHC204 O 1.120 mmols KHC204 1.911 mmols KHC204
A 0.4140-g sample of impure Na2CO3 (FW 105.99) was analyzed by the Volhard method. After adding 50.00 mL of 0.06911 M AgNO3, the sample was back titrated with 0.05781 M KSCN, requiring 21.33 mL to reach the end point. What is the % purity of the Na2CO3sample?
Gold can be determined in solutions containing high concentrations of diverse ions by ICP-AES. Aliquots of 50.0 mL of the sample solution were transferred to each of four 100.0 mL volumetric flasks. A solution was prepared containing 10.0 mg/L Au in 20% H2SO4 and quantities of this solution were added to the sample solutions to give 0, 2.5, 5, and 10 mg/L added Au in each of the flasks. The solutions were made up to a total volume of 100.0 mL, mixed, and analysed by ICP-AES. The resulting data are presented in the following table. Added Au, mg/L Emission Intensity Count 12,568 19,324 26,622 40,021 0.0 2.5 5.0 10.0 Calculate the concentration of gold in the original sample.
The Fe content in a water sample from a well was determined by subjecting an aliquot of 25.00ml of sample to treatment with HNO3, excess SCN- and finally a dilution of the treated solution to 50.00mL with distilled water. A 10.00ml aliquot of a 5.97 x 10-4M Fe3 + solution was treated in the same way. It was observed that the color of both solutions was the same when the optical path of the standard solution was 3.04cm and that of the well water sample was 2.61cm. Determine the ppm of Fe in the well water sample.