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- A sample containing calcium was analyzed by gravimetry, converting all calcium to calcium oxalate monohydrate (CaC2O4 • H2O). The sample weighing 0.2654 g was dissolved by adding 6M HCl, and then ammonium oxalate solution was added to precipitate all the calcium. The precipitate was suction filtered and dried in an oven at 95 °C for one hour. The solid obtained weighed 0.3216 grams.Calculate:A) The percentage of CaCO3B) The percentage of Ca C) The percentage of CaOAn ore containing Fe3O4 was analyzed by dissolving a 1.5419-g sample in concentrated HCl. HNO3 was then added to oxidize any Fe2+ to Fe3+. The Fe3+ was precipitated as Fe(OH)3 by adding NH3. The precipitate was collected by filtration and was finally heated yielding 0.8525 g of Fe2O3. Report the concentration of Fe3O4 in the sample as %(w/w). (Note: the final answer is said to be 53.4%)400 g sample containing chloride ions (MW=35.45 g/mol) was dissolved in 50.0mL of distilled water. A 15.0 mL aliquot was taken, and was further diluted to 50.0 mL using distilled water. The diluted solution was then titrated using a 0.0989 M AgNO3 solution, and it consumed a total of 31.9 mL of the titrant in order to reach the end point. What is the concentration of the undiluted chloride solution? Round off to three (3) significant figures. What is the % (w/v) concentration of the undiluted chloride solution? Round off to two (2) decimal points. What is the % (w/w) of Cl- composition of the sample? Round off to two (2) decimal points.
- 1,5419 g of magnetite (Fe3O4) ore; Fe+2 and Fe + 3 in concentrated HCL to form a mixtureit's unraveling. Adding HNO3 to all Fe +2s Fe +3 e and Fe+3 s NH, addingwith Fe(OH)3, precipitating into. Sediment in the form of Fe3O4 after necessary operationsand 0.8525 g. Calculate the percentage of Fe3O4 in the sample.A 0.6560 g mixture of KCN (MW=65.116 g/mol) and NaCN (MW=49.005 g/mol) was dissolved in water. AgNO3 was added to the solution, precipitating all of the CN− in solution as AgCN (MW=133.886 g/mol). The dried precipitate weighed 1.505 g. Calculate the weight percent of KCN and NaCN in the original sample. KCN wt% = ~ 66.01 NaCN wt% = ?Toxic Cr(VI) can be precipitated from an aqueous solution by bubbling SO2 through the solution. How much SO2 is required to treat 3.00x10^8L of 4.00x10^-2 mM Cr(VI)? 2CrO4^-2 + 3SO2 + 4H^+ —> Cr2(SO4)3 + 2H2O ___kg
- What weight of sample in gram containing 8.00 % Fe3O4 (MW= 231.53 g/mole) must be taken to obtain a precipitate of Fe (OH)3 (MW= 106.867 g/mol) that, when ignited to Fe2O3 (MW = 159.69 g/mole), weighs 150.0 mg0.1724g of a mineral containing MnO₂ was dissolved and then treated with excess iodide according to the following unbalanced reaction: MnO2(s) + H+ → Mn²+ + I2 + H₂O The I₂ released was titrated with a solution of Na₂S2O3 0.07320 mol/L, requiring 14.65 mL to reach the point end of degree a) Determine the percentage of MnO₂ in the ore. b) When iodine solutions are used as titrants these are prepared by dissolving 1₂ in concentrated KI. Explain the reason for the need for KI in the preparation of these solutions?A 1.9300 g impure sample of Fe(NH4)2(SO4)2 (FW = 392.14) was dissolved in 75 mL 0.75 M H2SO4 and was titrated with the standard KMnO4 in problem 1. Titration of the sample required 24.00mL while the blank containing 75mL 0.75 M H2SO4 required 0.75 mL of the KMnO4 titrant. Calculate the concentration of Fe(NH4)2(SO4)2 in %w/w in the impure 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.3 L contaminated air 50 mL 0.0116 M in an air pollution analysisCarbon dioxide (CO2) BaCO3 is passed through Ba (OH) 2 solution.is precipitated as. Excess of base, next to phenol phthalate (f.f.) indicatorIt is titrated with 23.6 mL of 0.0108 M HCl. CO2 in this air sampleCalculate its concentration in ppm. (Density of CO2Take it as 1.98 g / L. C = 12, O = 16 g / mol).1. A newly discovered iron ore was weighted (5.408 g) and worked up to produced 0.3785 g of ignited Fe2O3 precipitate. What is the percent purity of the iron in the sample? 2. Distinguish between equivalence point and end point.