nL of the unknown were pipetted into each of five 50.0-ml volumetric flasks. Various volumes of a tandard containing 12.2 ppm Cu were added to the flasks, and the solutions were then diluted to olume. Unknown (mL) L0.0 Standard (mL) Absorbance 0.0 0.201 L0.0 10.0 0.292 0.0 20.0 0.378 0.0 30.0 0.467 L0.0 40.0 0.554 A. Plot absorbance as a function of the concentration of Cu standard after final dilution and determine the equation of the line and determine the x-intercept. Calculate the copper concentration in ppm Cu in the aqueous sample.
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- The chromium in an aqueous sample was determined by pipetting 10.0 ml. of the unknown into each of five 50.0-mL volumetric flasks. Various volumes of a standard containing 12.2 ppm Cr were added to the flasks, following which the solutions were diluted to volume. Unknown,mLStandard, mLAbsorbancc 10.00.00.201 10.010.0 0.292 10.020.0 0.378 10.030.0 0.467 10.040.0 0.554 (a) Plot the data using a spreadsheet. (b) Determine an equation for the relationship between absorbance and volume of standard. (c) Calculate the statistics for the least-squares relationship in (b). (d) I)ctcrmine the conccnt ration oÍCr in ppm in the sample. (e) Find the standard deviation of the result in (d).The calcium content of a natural water sample was analyzed by flame atomic absorption spectrometry. A 5-mL sample of natural water was added to a 50-mL volumetric flask and diluted to mark with distilled water. The solution gave an absorbance of 0.457. Another 5-mL portion of the water sample was placed in a 50-mL volumetric flask and treated with 1.00 mL of a standard solution containing 0.10 mg mL-1 and diluted to mark. The mixture gave an absorbance of 0.542. Calculate the concentration (in mg mL-1) of calcium in the natural water. O 0.136 O 0.194 O 0.108 O 0.142A liquid sample was analyzed for Fe³+. A plot of absorbance (y-axis) vs. concentration (ppm; x-axis) of the external standards produced a calibration line with an equation y = 0.2256x -0.0903 (R² = 0.9973). The absorbance of the sample was 1.25. Determine the amount of Fe³+ in the sample (in ppm).
- Quinine in a 1.664 g antimalarial tablet was dissolved in sufficient 0.10 M HCl to give 500 mL of solution. A 15.00 mL aliquot was then diluted to 100.0 mL with the acid. The fluorescense intensity for the diluted sample at 347.5 nm provided a reading of 288 on an arbitrary scale. A standard 100 ppm quinine solution registered 180 when measured under conditions identical to those for the diluted sample. Calculate the mass in milligrams of quinine in the tablet.In the determination of lead content in a solid food sample, 1 g of the solid food sample was extracted with 10 mL of solvent and then diluted to a final volume of 50 mL. A calibration plot of lead standards was obtained from the standard solutions of 1 to 50 ug/mL and it gave a linear regression line of y = 0.025x + 0.004. The wavelength for lead analysis is 283.3 nm. The absorbance value for the extract was 0.302 arbitrary units. Calculate the percentage of Pb in 1 g of the solid food sample.A student weighed out 0.150 g of protein powder and dissolved it in 100 mL of water (Solution 1). The student then diluted this solution by transferring 1 mL into a 25 mL flask and diluting with water (Solution 2). Finally, 1 mL of that solution was transferred to a test tube and combined with 4 mL Bradford reagent. The absorbance of the solution in the test tube was 0.144. Assuming that the best fit linear line of the standard curve was y=0.04144x+0.01521 (μgmL), calculate the percent protein by mass in the original protein powder.
- In a Bradford assay, 11 µl of a protein isolate sample was diluted by adding 21 µl of water prior to the addition 2.0 mL Bradford reagent. Calculate the protein concentration (in mg/mL) of the original protein isolate sample whose absorbance reading at 595 nm is 0.304 after dilution. The protein standard solutions used for the calibration curve of the Bradford assay was constructed using bovine serum albumin (BSA) stock solution whose concentration is 200 µg/mL. The concentration and the corresponding absorbance reading at 595 nm of the protein standard solutions are summarized in the table below: Standard soln # 1 2 13 4 6 conc of BSA 12.00 24.00 36.00 48.00 60.00 (pg/mL) Absorbance at 595 nm 0.000 0.156 0.249 0.328 0.411 0.528 zNote: Final answer format must be x.xxx (three decimal places). Round off only in the final answer. Do not round off in the middle of the calculation.In a Bradford assay, 17 pl of a protein isolate sample was diluted by adding 24 pl of water prior to the addition 2.0 mL Bradford reagent, Calculate the protein concentration (in mg/ml) of the original protein isolate sample whose absorbance reading at 595 nm is 0,384 after dilution The protein standard solutions used for the calibration curve of the Bradford assay was constructed using bovine serum albumin (BSA) stock solution whose concentration is 200 ug/mL The concentration and the corresponding absorbance reading at 595 nm of the protein standard solutions are summarized in the table below: Standard soln # 3 6 conc of BSA Kug/mL) 12.00 24.00 36.00 48.00 60.00 Absorbance lat 595 nm 0.000 0.156 0.249 0.328 0.411 0.528 zNote: Final answer format must be x.xox (three decimal places) Round off only in the final answer. Do not round off in the middle of the calculationThe Na* concentration in a blood serum sample was determined using the method of standard addition and atomic spectroscopy. 25.00 mL aliquots of serum were pipetted into five 50.00 mL volumetric flasks into which 2.640 M NaCl standard was added as shown in the table below. After dilution to volume, the emission of each solution was measured and used to plot a calibration graph. Flask 1 23 4 5 Vol. of standard (mL) 0 1.00 2.00 3.00 4.00 Emission signal 3.13 5.40 7.89 10.30 12.48 Analytical signal (emission) 14 42 10 12 4 2 0 0 0.05 y = 44.697x + 3.12 R² = 0.9995 0.1 0.15 Concentration of added analyte (M) 0.2 a) Using the plotted calibration graph, calculate the Na* concentration in the blood serum sample. b) Provide a possible reason why the serum sample might have been analysed using this analytical procedure. 0.25
- 0.1120 g of a solid sample containing copper was dissolved by acid and transferred to a 250.00 mL volumetric flask and volume was made up with distilled water. The solution was then diluted by a factor of 25. The final solution was analyzed by atomic absorption spectrophotometry and the concentration was found be 2.982 ppm, What is the weight percentage of copper in the original solid sample? Keep four significant figures in your final answer.Exactly 5.00 mL aliquots of a solution containing analyte X were transferred into 50.00-mL volumetric flasks and the pH of the solution is adjusted to 9.0. The following volumes of a standard solution containing 2.00 µg/mL of X were then added into each flask and the mixture was diluted to volume: 0.000, 0.500, 1.00, 1.50 and 2.00 mL. The fluorescence of each of these solutions was measured with a fluorometer, and the following values were obtained: 3.26, 4.80, 6.42, 8.02 and 9.56, respectively. ii. Using relevant functions in Excel, derive a least-squares equation for the data, and use the parameters of this equation to find the concentration of the phenobarbital in the unknown solution.in a standard addition calibration method, 50.0 ml volumetric flasks were used. A 5.0 ml aliquot of a solution containing penobarbital was put in each. The solutions were made basic with KOH and mixed with different increments of 2.0 ppm standard penobarbital. The volumes were adjusted to 50,0 ml and absorbances were measured as follows 0.00 0.50 1.00 Volume added (ml) 1.50 2.00 0.33 0.48 0.64 0.80 0.96 Absorbance Calculate the concentration of phenobarbital in the unknown (Use graphical or numerical solutions) Selected Answer: 2.000 ppm 0.410 ppm Answers: 2.000 ppm 5.000 ppm 0.315 ppm