Show complete solution. Round-off your answers to four decimal places The amount of copper in a wire was determined by a redox titration using KMnO4 as the titrant. A 0.4185-g sample was dissolved in acid and the liberated Cu2+ quantitatively reduced to Cu+, using a reductor column. Titrating with 0.0250 M KMnO4 requires 41.27 mL to reach the endpoint. Determine the % w/w CuO in the sample of meteorite. Answer: % CuO = ______
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Show complete solution. Round-off your answers to four decimal places
The amount of copper in a wire was determined by a redox titration using KMnO4 as the titrant. A 0.4185-g sample was dissolved in acid and the liberated Cu2+ quantitatively reduced to Cu+, using a reductor column. Titrating with 0.0250 M KMnO4 requires 41.27 mL to reach the endpoint. Determine the % w/w CuO in the sample of meteorite.
Answer:
% CuO = ______
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- A 0.2653 g of pure potassium dichromate was dissolved in 15 mL of 1.5 M sulfuric acid and transferred to a 250.0 mL volumetric flask and diluted to the mark with distilled water. A 25.0 mL aliquot of this solution was transferred to another 250.0 mL volumetric flask and diluted to the mark with distilled water and this solution has an absorbance 0f 0.387 in a 2.00 cm cell. Calculate the molar absorptivity of potassium dichromate.A community in a mountainous area of Bohol uses water collected from a nearby natural spring. A sample was submitted to a laboratory for the analysis of its total hardness. Describe the preparation of the following reagents: 100 mL of 1.0M stock EDTA solution. 0 L of 0.010 M EDTA solution from the stock EDT solution. 0 mL of 500.0 ppm of CaCO3 solution from a primary standard (assume solvent is distilled water only).A 0.5000 g primary standard sodium oxalate (Na2C204, FW=134.00 g/mol) was dissolved in 50 mL of 1 M H2SO4 and required 21.00 mL of the titrant, potassium permanganate (KMnO4, FW=58.03 g/mol) to reach the end point. Calculate the molarity of the titrant *Identify which served as the reducing agent in the titration. * Identify which served as the oxidizing agent in the titration. * Identify the specific name of the redox ti trimetric method used. * Identify the (a) appropriate indicator in t he titration and (b) its type.
- Please help me out with making flowchart with thes steps. Write the result. Procedure 1. Place 20 drops of each of the following aqueous solutions to separate centrifuge tubes: 0.1M Cr (NO3)3, 0.1M Al (NO3)3, 0.1M Co (NO3)2, 0.1M Zn (NO3)2, 0.1M Mn (OH)2, 0.1M Ni (NO3)2, 0.1 M Fe (NO3)3. Make each solution basic by adding few drops of 6M NH4OH. Confirm using a litmus paper. 2. Add 5 drops of freshly prepared 6M (NH4)2S to each centrifuge tube. Place the samples in the centrifuge machine for 3 mins. After centrifuge record results. Decant the supernatant liquid of all the samples. 3. Add one drop of NH4OH in each centrifuge tubes. Add 20 drops of distilled water in each centrifuge tubes. Then add a few drops of 6M HCl in each solution. Place the samples in the water bath for 10 mins. After water bath, centrifuge the samples for 3 mins. 4. After centrifuge, add a few drops of 6M NH4Cl in each sample. Decant the supernatant liquid in each sample. 5. To the centrifuge containing…A piece of Gold weighing 12,359 Kg is suspected of being contaminated with Iron. To perform an instrumental analysis and To confirm whether or not it contains Fe, a portion of the sample (0.954 g) is taken from the piece and dissolved with 25 mL of aqua regia. Heats up For its complete dissolution, it is cooled and made up to 100 mL. A 10 mL aliquot is taken from this solution and made up to 50 mL. From This last solution is given the appropriate treatment to visualize Fe+2, for which the 1,10-phenanthroline reagent is added. (it forms a complex that is red in color) and is taken to a visible spectrophotometer and with a 12 mm cell a absorbance of 0.45. Previously, a calibration curve of Fe+2 was obtained under the same instrumental conditions obtaining the following data: (view table) Calculate the purity of the gold piece, assuming impurities only due to Fe.please answer what you can. thank you so much in advance. :) Standardisation of EDTA using zinc metal Mass of zinc = 1.050 g. Calculate the number of moles of zinc in the 250 mL flask (show workings) Calculate the concentration zinc in the 250 mL flask (show workings) Calculate the number of moles of Zn2+ in the 20 mL aliquot (show workings) Calculate the number of moles of EDTA in the average titre (show workings) Calculate the concentration of the DILUTED EDTA solution (show workings) Sample No. 1 2 3 4 Final Burette reading (mL) 20.25 42.75 22.90 44.50 Initial Burette reading (mL) 0.05 20.25 1.50 22.90 Final-Initial Titre (mL) 20.20 22.50 21.40 21.60
- An sample of eggshell that weighs 1.0014g and is 51μm thick is titrated with disodium EDTA. A solution of the 1.0014g sample and 30 mL of HCl is vacuum filtered after being mixed. The product of the filtration is added to a 250mL volumetric flask and is diluted by being filled to the 250 mL mark with deionized water. 10 mL of this diluted mixture is mixed with EBT indicator and titrated with 0.05 M disodium EDTA. It takes 12.3 mL of disodium EDTA to notice a change in color. What percent mass of calcium is in the eggshell?A 3.25 g sample of an iron-containing mineral was dissolved in an acid medium and calibrated to 500 mL. A 25.00 mL aliquot was titrated with 0.0025 M KMnO4 spending a volume of 9.32 mL. Subsequently, a 25.00 mL aliquot was passed through a Walden reducer to later titrate it with the same permanganate solution, using a volume of 14.15 mL for the titration. Determine the percentage of Fe(III) in the sample and report it as % Fe2O3A 0.1093-g sample of impure Na2CO3 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 27.36 mL to reach the end point. Report the purity of Na2CO3 sample.
- A 20.0 mL sample of commercial bleach was diluted with water to a 250.0 mL volumetric flask. A 50.0 mL aliquot of the diluted sample was treated with excess KI and starch. The liberated iodine was titrated with 0.399 M Na2S2O3, requiring 13.9 mL to reach the end point. (a) Identify the type of redox titration method used. (b) Identify the indicator and endpoint color. (c) Calculate the % w/v NaOCl in the sample.Prepare 100.00 mL of a solution with ALL the following chemicals into together; CHEMICALS PROVIDED solid FeCl3 6H2O, iron(II) chloride hexahydrate (source of FeCl3) dilute hydrochloric acid in the rack – 3.0 M solid sodium salicylate – 99.7% assay Concentrations needed in the 100mL solution FeCl3: 0.020 M HCl: 0.050 M Salicylate (mg/L): 40.25 PLEASE SHOW HOW TO CALUATE AND WORK. The only equations you will need to use are the equations for molarity and dilutions.Use the data provided for stock concentration and mass to calculate the concentrations of each solution. Solution A) A stock solution of 0.0100 M solution of K3[Fe(CN)6] is provided. Calculate the volume of the stock solution needed to prepare 100.0 ml of .00200 M K3[Fe(CN)6]. Deionized water should be used to dilute the solution. Solution B) Calculate the volume of solution A needed to prepare 50.0 ml of .0010 M K3[Fe(CN)6]. Deionized water should be used to dilute this solution.