Calculate the concentration of silver in each sample. Are there any problems? How will you address each of the identified problems? Standards Absorbance Ag (ppb) 0.00 0.000 2.00 0.013 10.0 0.076 20.0 0.162 30.0 0.245 50.0 0.405 75.0 0.598 100.0 0.748 Samples Absorbance 08002 0.079 08003 0.058 08004 0.129 08005 0.082 08006 0.797 08007 0.063 08008 0.009 08009 0.028 08010 0.136
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- Calculate the amount of manganese (54.94 g/mol) from a processed ore using the following data. Standardization data: 2.000 mL KMnO4 = 0.02015 g Na2C2O4 (134 g/mol) Sample analysis data: Weight of sample = 0.1012 g Na2C2O4 used(in excess)= 0.3200 g KMnO4 used for back-titration = 9.93 mL Rxn: 2MnO4- + 5C2O42- + 16H+ → 2Mn2+ + 10CO2 + 8H2OTo calculate the unknown concentration of a chemical in a solid sample, 4 different calibrationcurves were plot using 4 different methods. Which of the following method is considered asacceptable? a. Method 4, R? = 0.998b. Method 1, R2 = 0.650c. Method 2. R' = 0.890d. Method 3, R' = 0.169Detailed calculations on how to prepare the solutions listed below Solution: 50 mL 1 M oxalic acid Oxalic acid Mw = 90.03 g mol-1 Oxalic acid purity = 98% Solution: 10 mL 3 M sulfuric acid Sulfuric acid Mw = 98.079 g mol-1 Sulfuric acid density = 1.84 g mL-1 Sulfuric acid purity = 98% Solution: 10 mL saturated potassium oxalate potassium oxalate (monohydrate used) Mw = 184.23 g mol-1 Solubility of potassium oxalate in water at 25°C = 360 mg mL-1 Solution :20 mL 3% hydrogen peroxide Hydrogen peroxide is commercially available as a 32% solution.
- Determine the percentage Fe in a sample of limonite from the following data:Sample : 0.5000g ; KMnO4 used = 50.00 ml ; 1.000ml of KMnO4 is equivalent 0.005317 g Fe,FeSO4 used = 6.00 ml; 1.000ml FeSO4 is equivalent 0.009200 g FeO ( ans 44.59 %)5.00 mL of stock solution is diluted to 25.00 mL, producing solution ALPHA. 10.00 mL of solution ALPHA is diluted to 25.00 mL, resulting in solution BETA. 10.00 mL of solution BETA is then diluted to 25.00 mL, producing solution GAMMA. dilution factor for ALPHA from stock solution = 0.167 dilution factor for BETA from ALPHA solution = 0.0476 part c and d?What weight of sample must be taken so that each 50 mg BaCl2 obtained in a gravimetric silver determination shall correspond to 10% of the Cl in the original sample? BaCl2 (208.23) Cl (35.45)
- 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 student determined the concentration of total reducible iodine in the aqueous phase based on the average of their 'best two' determinations in Part 1 to be 0.0185 M. They also determined the concentration of 12 in the CH2Cl2 phase based on the average of their 'best two' determinations in Part 2 to be 0.0200 M. Determine what the concentration of 13 in water would be based on this student's previous work. Report your final answer, in mol/L, to 4 decimal places and only include the numerical value (no units). Do not use scientific notation for this question. Do not give handwriting solution.How to prepare these solutions? 250.0 mL 0.125 M stock Na2S2O3 solution from Na2S2O3·5H2O crystals 250 mL 0.10 M NaOHNOTE: Use the 1.0 M NaOH prepared250.0 mL standard 2500 ppm Cu(II) stock solutiona. Weigh and dissolve appropriate amount of Cu(NO3)2·5H2O crystals in enough distilled water.
- 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.Dilute the stock solution: Using the solutions in the burets, carefully measure the following quantities of Co(NO3)2 solution and water into 5 large test tubes, to a total of 5.00 mL in each test tube. Yes, the optional video says to make 10.00 mL total, but 5.00 mL is sufficient at this time and generates less waste. Use the buret to measure the cobalt solution and the water. Test tube No. 1 2 3 4 5 mL Co2+ Soln 1.00 2.00 3.00 4.00 5.00 mL H2O 4.00 3.00 2.00 1.00 0.00 Total mL 5.00 5.00 5.00 5.00 5.00 Mix each test tube thoroughly: hold the top of the tube and mix the bottom well. Transfer a portion of each diluted sample into a clean, dry sample cuvette. fill the concentration table and do calculations please1. The standard solutions of iron(III) thiocyanate (solutions of known concentration) were prepared for you by mixing the solutions as shown in Table 1.a. Because of the very high concentration of KSCN used in each test tube, you can assume essentially all of the Fe(NO3)3 that has been added has reacted to form FeSCN2+ (by Equation 2, in the Background). Calculate the molar concentration of Fe(NO3)3 in each standard after it is diluted with the other solutions, which equals the concentration of FeSCN2+ formed in each sample (show your work for at least one of these calculations).These are the concentrations that were used in the standard curve. I have the table and the equation 2 on the top attached