0.9583 g of sample was dissolved in 80 mL of xylene and extracted with three 15 mL quantities of water. The combined aqueous extracts were diluted to 50.0 mL and then shaken with 10 mL toluene. The toluene was then discarded. The absorbance of the aqueous solution when measured in a 1cm path length cell was 0.134 at 278 nm.Calculate the free chlorampenicol content of the sample in ppm, given A(1%, 1cm) = 298 at 278 nm.
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0.9583 g of sample was dissolved in 80 mL of xylene and extracted with three 15 mL quantities of water. The combined aqueous extracts were diluted to 50.0 mL and then shaken with 10 mL toluene. The toluene was then discarded. The absorbance of the aqueous solution when measured in a 1cm path length cell was 0.134 at 278 nm.
Calculate the free chlorampenicol content of the sample in ppm, given A(1%, 1cm) = 298 at 278 nm.
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- The DPD colorimetric method is used to determine the amount of residual chlorine in the sample. In this method, the free chlorine in the sample oxidizes the colorless amine N,N-diethyl-p-phenylenediamine to a colored compound that absorbs strongly at 520 nm. The analysis of a set of calibration standards gave the following results:ppm Cl2 Absorbance0.00 0.00310.50 0.12321.00 0.32411.50 0.54382.00 0.76422.50 0.95513.00 1.1565A 10.00 mL water sample from a public water supply was diluted to 250 mL and analyzed for free chlorine residual, giving an absorbance of 0.3210.A. Find the equation of the line.B. What is the molar absorptivity of Cl2 (FW = 70.9) at 250 nm?C. Calculate the free chlorine residual of the sample as ppm Cl2.D. Calculate ppm BaCl2 (FW = 208.2)?Please answer the following with complete solution. Thank you. A mixture placed in an Erlenmeyer flask comprises 6mL of silica gel and 40mL of a solvent containing, in solution, 100mg of a non-volatile compound. After stirring, the mixture was left to stand before a 10mL aliquot of the solution was extracted and evaporated to dryness. The residue weighed 12mg. Calculate the adsorption coefficient, K=CS/CM, of the compound in this experiment.A 10.00 mL of natural water sample containing Ni2+ was pipetted into a volumetric flask and diluted to 50.00 mL with pure water. In the second 10.00 mL of natural water sample transferred into a volumetric flask, exactly 4.00 mL of a Ni2+ solution with a concentration of 5.99 mg/L was added and then diluted to 50.00 mL with pure water. The measured absorbance is A1= 0.436 and A2 = 0.663. What is the Ni2+ concentration in unit of mg/L in the natural water sample?
- Exactly 6.00 ml of acetic acid (density = 1.05 g/mL), MW =60.05) was added to a 1 –liter volumetric flask, and the flask was filled to the mark with distilled water. A portion of the resulting solution was added to a conductance cell (k = 1.25 cm-1), and the conductance was found to be 416 μS. Calculate the dissociation constant Ka of acetic acid. ΛoH+= 349.8 Scm2/mole and ΛoCH3COO- = 41 Scm2/moleOne common way to determine phosphorous in urine is to treat the sample after removing the protein with molybdenum (VI) and then reducing the resulting 12-molybdophosphate complex with ascorbic acid to give an intense blue-coloured species called molybdenum blue. The absorbance of molybdenum blue can be measured at 650 nm. A 24-hour urine sample was collected, and the patient produced 1122 mL in 24 hours. A 1.00 mL aliquot of the sample was treated with Mo (VI) and ascorbic acid and diluted to a volume of 50.00 mL A calibration curve was prepared by treating 1.00 mL aliquot of phosphate standard solution in the same manner as the urine sample. The absorbances of the standards and the urine sample were obtained at 650 nm and the following results were obtained. ppm, P aBSORBANCE (A) 1.003.00 0.230 2.00 0.436 3.00 0.638 4.00 0.848 Urine sample 0.518 ffind the slope and intercept, then graph it.A 50.0 mL juice extract is colorimetrically assayed using Nelson’s test. One milliliter (1.00 mL) of the solution and the standard glucose solution (concentration: 1mg/mL) were treated with freshly prepared Nelson’s reagent and arsenomolybdate reagent and then diluted to 10.0 mL separately in properly labeled test tubes. Absorbance at 480 nm for the standard is 1.702 and for the sample, 0.926. A. What is the principle behind the assay? B. Calculate the concentration of the reducing sugar in the 50.0 mL sample in mg/mL. Apply Beer-Lambert’s law.
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- The ethyl acetate concentration in an alcoholic solution was determined by diluting a 10.00-mL sample to 100.00 mL. A 20.00-mL portion of the diluted solution was refluxed with 40.00 mL of 0.04672 M KOH:CH3COOC2H5 + OH- → CH3COO- + C2H5OHAfter cooling, the excess OH2 was back-titrated with 3.41 mL of 0.05042 M H2SO4. Calculate theamount of ethyl acetate (88.11 g/mol) in the original sample in grams0.56 g 1,4‐dimethoxybenzene, 0.9 mL 2‐chloro‐2‐methylpropane, 5 mL nitrobenzene and 0.52 g graphite were combined, and the mixture was refluxed for 1.5 hours. It was then cooled to room temperature and filtered. The filtered graphite was washed with 15 mL hexane. The filtrate was distilled under vacuum to remove any remaining 1,4‐dimethoxybenzene, 2‐chloro‐2‐ methylpropane and nitrobenzene (6.3 g), yielding 0.44 g 1,4‐di‐tert‐butyl‐2,5‐dimethoxybenzene (43.4% yield). What is the Atom economy, E factor, and effective mass yield?A 50.0 mL juice extract is colorimetrically assayed using Nelson’s test. One milliliter (1.00 mL) of the solution and the standard glucose solution (concentration: 1mg/mL) were treated with freshly prepared Nelson’s reagent and arsenomolybdate reagent and then diluted to 10.0 mL separately in properly labeled test tubes. Absorbance at 480 nm for the standard is 1.702 and for the sample, 0.926. Calculate the concentration of the reducing sugar in the 50.0 mL sample in mg/mL. Apply Beer-Lambert’s law: A=bc.