With your knowledge on analytical separation and analyses, outline a suitable analytical separation protocol that can be employed to recover polluted river bodies and make them wholesome for drinking. [
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With your knowledge on analytical separation and analyses, outline a suitable analytical separation protocol that can be employed to recover polluted river bodies and make them wholesome for drinking. [
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- Treatment of ammonia with phenol in the presence of hypochlorite yields indophenol, a blue product that absrobs light at 625 nm, which can be used for the spectrophotometric determination of ammonia. ocr -OH • NH, indophenol anion To determine the ammonia concentration in a sample of lake water, three samples are prepared. In sample A, 10.0 mL of lake water is mixed with 5 mL of phenol solution and 2 mL of sodium hypochlorite solution, and diluted to 25.0 mL in a volumetric flask. In sample B, 10.0 mL of lake water is mixed with 5 mL. of phenol solution, 2 mL of sodium hypochlorite solution, and 2.50 mL of a 5.50 x 10-4 M ammonia solution, and diluted to 25.0 mL. Sample C is a reagent blank. It contains 10.0 mL of distilled water, 5 mL of phenol solution, and 2 ml. of sodium hypochlorite solution, diluted to 25.0 mL. The absorbance of the three samples is then measured at 625 nm in a 1.00 cm cuvette. The results are shown in the table. Sample Absorbance (625 nm) A 0.374 В 0.621 0.045…A mixture containing only KCl and NaBr is analyzed by the Mohr method. A 0.2125-g sample is dissolved in 25 mL of water and titrated to the Ag2CrO4 endpoint, requiring 25.63 mL of 0.1110 M AgNO3. A blank titration requires 1.15 mL of titrant to reach the same end point. Report the %w/w KCl and NaBr in the sample. KCl = 74.551 NaBr = 102.89A sample (50 mL) of a bottled water was added to a 100 mL volumetric flask and then diluted to the mark. From this stock solution, 50 mL was taken, added to a 100 mL volumetric flask and diluted to the mark. Final concentration of the serial dilution: 587.7161ppm. 1. what is the concentration in the original bottle (ppm)
- A forensic chemist is given a white powder by the investigator of a crime scene. The investigator wants to know if the powder is a pure substance or a mixture. The chemist dissolves some of the powder in deionized water making a clear solution. She finds that a precipitate forms when she adds an excess aqueous solution of sodium chloride. She filters the precipitate and washes it several times with deionized water. To this filtrate she then adds an aqueous solution of sodium carbonate. A precipitate forms. Question: Draw two pictures representing a molecular / atomic / ionic view of what occurred when a precipitate formed with the addition of sodium chloride solution. Choose the type of particle that is the most appropriate for this reaction. Place charges on any ions indicating charge values (+1, -2, etc.) when they are known. If charges are unknown indicate whether the ion is positive or negative. Clearly indicate which picture represents before the reaction occurs. Should…1. A sample of pure sodium oxalate, Na2C2O4 , weighing 0.2856 g is dissolved in water, sulfuric acid is added, and the solution titrated at 70°C , requiring 45.12 mL of a KMNO4 solution. The end point is overrun and back-titration is carried out with 1.74 mL of a 0.1032 N solution of oxalic acid. Calculate the normality of the KMNO4 solution. Hint: A redox reaction is involed between oxalate and permanganate. Look at the changes in oxidation state by determining the balanced redox reaction: 5C20,2 + + 2MN2+ 2 Mn04 + 10H* → 10CO2 + 8H20A 12.63 g sample of calcium ore was dissolved in HCl and gravimetrically analyzed, through the precipitation of calcium into CaC2O4 · H2O. The precipitate was filtered, washed, dried, and ignited at 500 oC until the weight was constant, giving a final mass of 2.35 grams pure CaCO3 (100.087 g/mol). Calculate the % Calcium (40.078 g/mol) in the sample.
- A sample containing chlorophenol, C6H4ClOH, was analysed by gravimetric analysis. A 0.783-g of this sample goes through a chemical process allowing the chlorine in the chlorophenol to precipitate as silver chloride, weighing 0.271 g. Calculate the % (wt/wt) of the chlorophenol in the sample, assuming that chlorophenol is the only source of chlorine in the sample. Provide your answer to two decimal places and without units. Avoid using scientific notation.A mixture containing only KCl and NaBr is analyzed by the Mohr method. A 0.2125- g sample is dissolved in 25 mL of water and titrated to the Ag2CrO4 end point, requiring 25.63 mL of 0.1110 M AgNO3. A blank titration requires 1.15 mL of titrant to reach the same end point. Report the %w/w KCl and NaBr in the sample.KCl = 74.551 NaBr = 102.89Any shipment of peanuts that contains more than 25 ppb of this dangerous fungus is rejected. A company receives 18 t of peanuts to make peanut butter. What is the maximum mass, in g, of fungus that is allowed? Hint 1 t = 1000 kg.In many areas, the drinking water standard for nitrate ions is 5.00 ppb. Calculate the mass, in μg, of nitrate ions allowed in one glass 251 mL of tap water. A ground water analyst found that the concentration of lead (Pb) in the well near a village was 60 ppb. If 0.375 mg of lead were found in a sample, what would be the volume of the sample of well water in litres (L)?
- A student performed a titration to determine the exact concentration of NaOH(aq). The titration was performed against a standard 0.1000 M HCl(aq) solution. Phenolphthalein indicator was used. The following end-point volumes were recorded by the student in units mL: Trial Number Volume 1 25.06 2 25.15 3 25.02 4 25.17 5 25.07 Calculate the 95% confidence limit. Assume that there is no outlier. Provide your answer to the correct number of decimal places, without units, and without the ± sign. Use the T-table shown below.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?148. Addition of 50.00 mL of 2.238 m H2SO4 (solution density = 1.1243 g/mL) to 50.00 mL of 2.238 M BaCl2 gives a white precipitate. (a) What is the mass of the precipitate in grams? (b) If you filter the mixture and add more H2SO4 solution to the filtrate, would you obtain more precipitate? Explain.
