A sample of iron ore weighing 800 mg was treated with HNO3 , boiled to dryness and redissolved in dilute HCl. After filtration and removal of undissolved silica, the liquid was passed through a Walden reductor. The collected sample was titrated with 0.0210 M KMnO4 , requiring 12.0 mL to reach the end point. Calc %Fe (55.845) in the ore.
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A sample of iron ore weighing 800 mg was treated with HNO3 , boiled to dryness and redissolved in dilute HCl. After filtration and removal of undissolved silica, the liquid was passed through a Walden reductor. The collected sample was titrated with 0.0210 M KMnO4 , requiring 12.0 mL to reach the end point. Calc %Fe (55.845) in the ore.
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- 1. A sample of feldspar weighing 1.500g is decomposed, and eventually there is obtained a mixture of KCI and NaCi weighing 0.1801 g. These chlorides are dissolved in H20, a 50-mL pipetful of 0.08333 N AGNO3 is added, and the precipitate is filtered off. The filtrate requires 16.47 mL of 0.100ON KCNS, with ferric alum as indicator. Calculate the percentage of K20 in the silicate.Calcium in a 5.00 mL urine sample was precipitated, redissolved and required 16.15 mL of 0.1157 N KMnO4. Calculate the % (w/v) of calcium in the urine.Percentage purity of a sample of 0.1350 g of As2O3 assayed iodometrically using 23.5 mL of 0.1055N iodine solution
- A sample of feldspar weighing 1.500g is decomposed, and eventually there is obtained a mixture of KCl and NaCl weighing 0.1801 g. These chlorides are dissolved in H2O, a 50-mL pipetful of 0.08333 N AGNO3 is added, and the precipitate is filtered off. The filtrate requires 16.47 mL of 0.1000N KCNS, with ferric alum as indicator. Calculate the percentage of K2O in the silicate.5. 0.1500 g sample of chromium ore was dissolved and the chromium oxidized to chromate ion. The solution was treated with 25.00 mL of 0.3500 M AGNO3. The resulting precipitate, from the reaction of the excess and analyte in 1: 1 mole relationship, Ag2CrO4 was removed and discarded. The excess AGNO3 required 30.50 mL of 0.200 M KSCN for titration in a 1:1 mole relationship. Calculate the % Cr2O3 in the ore if the mole relationship between Cr2O3 and CrO42- is 1:2 respectively.A spectrophotometric method for the analysis of iron has a linear calibration curve for standards of 0.00, 5.00, 10.00, 15.00, and 20.00 ppm. An iron ore sample with an expected iron content of 40–60% w/w is to be analyzed by this method. An approximately 0.5-g sample is taken, dissolved in a minimum of concentrated HCl, and diluted to 1 L in a volumetric flask using distilled water. A 5.00-mL aliquot is removed with a pipet. To what volume (10, 25, 50, 100, 250, 500, or 1000 mL) should it be diluted to minimize the uncertainty in the analysis? Explain.
- 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.Six iron tablets containing FeSO4.7H2O were dissolved in 100-ml of 0.1M HNO3 with gentle heating. All of the Fe2+ is converted to Fe3+ by the strong oxidizing conditions. After the solution had cooled to room temperature , 2.5-ml of 35wt% NH4OH was added. The precipitate Fe2O3-xH2O that was filtered weighed 0.345g. Thermogravimetric analysis of the crude product showed a 10.5% weight loss . A. How many waters of hydration were in the precipitate B. How much iron is present in each tabletGold 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
- 100 kg of roasted zinc ore with composition: 66% ZnO, 3% ZnS, 10% PbO, 14% Fe;0, 1% Al;O, 6% SiO; is reduced in a horizontal retort furnace with 45 kg coke having 90% C and 10% SiO,. In the furnace 91% of Zno is reduced to Zn 100% of Pbo is reduced to Pb 75 % of Fes0, is reduced to Fe, 25 % of Fe,O, is reduced to Feo Neglect the vaporization of Pb and Fe and accept that they will not reoxidize. 1. Determine the weight of zinc and the percentage of zinc gained from the ore. 2. Determine the theoretical weight of C required for the reduction of Zno and the percentage of the excess C. 3. Determine the weight and the percentage of the residual material in the retort furnace after the removal of zinc vapor.what volume of decinormal k2cr2o7 solution would be needed to convert 1.19 g of tin to stannic chloride in acidic medium?(a) What is the percentage of MnO2 in a pyrolusite ore if a sample weighing 0.4000 g is treated with a 0.6000 g of pure H2C2O4.2H20 and dilute H2SO4 and after reduction has taken place (MnO2 + H2C2O4 + 2H+ Mn2+ + 2CO2 + 2H2O), the excess oxalic acid requires 26.26 mL of 0.1000 N KMNO4 for titration? (b) If pure As2O3 were used instead of oxalic acid, how many grams would be required in order for the other numerical data to remain the same?