A solution containing 0.584 mole/L of CUSO4 and had a 0.510 absorbance reading in a 1.0cm cell at 520nm. Calculate the molar absorptivity of CuSO4 at 520nm. 0.873 L mole cm 0.853 L mole" mm" 0.923 L mole" cm O 0 773 L mole cm
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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 10.0-mL aliquot of a standard manganese solution containing 62.5 mg/L of Mn is oxidized to MnO4- and diluted to 50.0 mL in a volumetric flask. The absorbance is measured in a 1.00-cm cell at 525 nm is 0.343. Next, a 850-mg steel sample containing manganese in dissolved in acid and diluted to 250 mL. A 50.0-mL aliquot is treated with KIO4 to oxidize Mn to MnO4- and diluted to 100.0 mL. If the absorbance at 525 nm is 0.468 in a 1.00-cm cell, calculate the weight percent of Mn in the steel.A10.00 solution 0.050M of AgNO3 was titrated with 0.0250 M of NaBR using an calomel electrode. ( E= 0.241) Find the voltage of the cell when: 0.1ml, 10.00ml, 20.00ml and 30.00 ml of titrant is added. Ag+ + Br- --> AgBr (s) Ag+ + e- ---> Ag(s) ( E= 0.799) Use this reaction for Nerst equation Ksp= 5.0x10^-13
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- An unknown sample of Librium was analyzed using polarography. A 50 mL sample containing the sample gave a limiting current of 0.40 uA. 5.00 mL of 5.00 mM standard Librium solution was added to the 50 mL sample and diluted to 100 ml. The wave height of the standard containing the sample gave a limiting current of 0.95 UA. What is the concentration of Librium in the unknown sample?a. 0.11 mmb. 0.21 mMc. 0.55 mmd. 2.0 mme. none of theseplease help with 1 and 2, all information given Calculate the number of moles of Zn2+ in the 20 mL aliquot (show workings) 1.050/65.38= 0.016mol (0.016x20)/250= 0.00128mol Calculate the number of moles of EDTA in the average titre (show workings) Mol EDTA= 0.00122 Volume of EDTA consumed= 0.02106L 0.00122mol/0.02106L=0.0579mol 1. Calculate the concentration of the EDTA solution (show workings) 2. 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 21.60Calculate the expected absorbance value of a 0.12 M aqueous solution of a solution if the extinction coefficient is € = 2.95 dm^3 mol^-1 cm^-1.The path length of the solution cell used for the measurement is 1.00 cm.
- A 20 ml aliquot of drinking water containing Fe(II) and Fe (III) is treated with hydroquinone to reduce all dissolved iron to Fe(II),0- phenanthroline is added and the aliquot is diluted to 50 ml and the absorbance in a 2.00 cm cell is 0.085 at 510 nm. Calculate the iron content of the water as ppm? ε = 1.11 x 104 L/mol cmThe concentration of yeast RNA in an aqueous solution is 12.0 mg/L. The absorbance is found to be 0.208 when this solution is placed in a 1.00 cm cell at 265 nm. Its molecular weight is 5.7 x 103 g/mol. a) Calculate the molar absorptivity of the yeast RNA. b) What will be the absorbance if the solution is 6.0 mg/L and the path length is 1.00 cm? c) What will be the absorbance if the solution is 12 mg/L and the path length is 2.00 cm? (Show your work)Analysis of ammonia via Nesslerization is based on measuring the absorbance at 420 nm of a yellowish complex formed between HgI42- and ammonia following the reaction below: 2[???4]2− + ??3 + 3??− → ??2???2? + 7?− + 2?2O Using a 1.00 cm cell, the absorbance of a reagent blank is 0.099, the absorbance of a 0.060 mM standard is 0.223. A 5.00 mL aliquote from a 1.00 L sample was reacted with Nessler reagent and diluted to 10.0 mL. The resulting solution had an absorbance of 0.685.