In the Spectrophotometric determination of Iron experiment, the calibration curve is plotted as absorbance vs. concentration (unit: mol/L). The curve is a straight line written as y=(1.0000x10^0)x-0.0235. The path length of the cuvette used in the lab is 1.0 cm. What is the molar extinction coefficient of the tris(phenanthroline) iron(II) in L/(mol*cm)?
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- The standard curve was made by spectrophotographic analysis of equilibrated iron(III) thiocyanate solutions of known concentration. You are asked to analyze a Fe(SCN)2+Fe(SCN)2+ solution with an unknown concentration and an absorbance value of 0.4150.415 . The slope-intercept form of the equation of the line is ?=4558.4?+0.0147y=4558.4x+0.0147 . The unknown was analyzed on the same instrument as the standard curve solutions at the same temperature. What is the Fe3+Fe3+ concentration of the unknown solution?The following results were obtained when each of a series of standard silver solutions was analyzed by flame atomic spectrometry. Concentration, ng ml1 5 10 15 20 25 30 Absorbance 0.003 0.127 0.251 0.390 0.498 0.625 0.763 1. Using a graphing paper, plot the calibration curveThe determination of iron in wines was carried out by atomic absorption spectrophotometry, using the standard addition method. To do this, 10 mL of wine were placed in five 50 mL volumetric flasks; then 0, 5, 10, 15 and 20 mL of a 10 ppm iron standard solution were added to each of them. Next, they were gauged with distilled water and the absorbance was measured, obtaining the values of 0.040, 0.062, 0.081, 0.102 and 0.125 respectively. Calculate the regression parameters and obtain the iron concentration in the wine, in µg / mL.
- A green solution containing Ni+2 ions absorbs 580 nm light. Undiluted, a sample of this solution sampled in a 1.00 cm diameter cuvette has an absorbance of 0.9765 a.u.. If the molar absorptivity coefficient for Ni+2 is 6.3 x 104 M -1 cm -1 at 580 nm, how much of the original stock Ni+2 solution (in mL) needs to be added to water to create a total dilute solution volume of 10.00 mL that measures an absorbance of 0.146 a.u. at 580 nm? Report your answer to 3 significant figures. Do not include the "mL' unit label in your responseA chemist received a report from an analysis involving the iron-phenanthroline method, containing the calibration curve for Fe standards (20 ppm, 30 ppm, 40 ppm, 50 ppm, and 60 ppm) and their corrected absorbances. The report stated that the equation of the line and r2 were as follows: y = 0.015066 x – 0.154424 r2 = 0.9997 The sample they tested gave a corrected reading of 0.417. How much Fe is present in ppm? 2.80 17.43 2.60 37.93The nitrate in water was analyzed using a spectrophotometric method. The absorbances of the standards and the unknown sample were obtained at 550 nm.Solution Absorbance 2.00 µM 0.0656.00 µM 0.20510.00 µM 0.33814.00 µM 0.47418.00 µM 0.598Unknown 0.402 Write the equation of the lineWhat is the standard deviation of the calibration curve?
- A standard solution was put through appropriate dilutions to give the concentrations of iron shown in the table that follows. The iron(II)-1,10-phenanthroline complex was then formed in 25.0-mL aliquots of these solutions, following which each was diluted to 50.0 mL. The following absorbances (1.00-cm cells) were recorded at 510 nm: Calculate the concentration, in ppm, of a sample with an abosrbance of 0.829. Fe(II) concentration (ppm) A510 4.00 0.160 10.0 0.390 16.0 0.630 24.0 0.950 32.0 1.260 40.0 1.580A student made a calibration curve for iron (III) using the above procedure with a slope of 70 M-1cm-1 and intercept is 0. An unknown sample of Fe+3 has absorbance of 0.35. What is its concentration?An ethanol solution of 3.5 mg/100 ml of compound Y (150.0 g/mol) in a 1.00 cm quartz cell has an absorbance (A) of 0.972 at λmax=235 nm. What is its molar extinction coefficient? Report your answer to the correct number of significant figures. Do not include units in your answer.
- Calculate the extinction coefficient of each peak if the measurements were made for a sample concentration of 12.8 µM in a cuvette with a path length of 1 cm. State any assumptions you need to make for the calculations and show your calculations clearly λ (nm) Absorbance 260 3.086 280 1.967 420 0.601Mary performed an experiment with industrial wastewater samples for determination of iron content. α-phenanthroline was added in order to obtain a strong coloured complex. A calibration graph was constructed as follow. Deduce the analytical technique used and calculate the concentration of wastewater analysed which demonstrated absorbance reading of 0.269 (sample 1), 0.532 (sample 2) and 0.478 (sample 3).Nitrite ion, NO2-, is a preservative for bacon and other foods, but it is potentially carcinogenic. A spectrophotometric determination of NO2- makes use of the following reactions: A 5.00 cm cell was used to measure absorbance. Here is an abbreviated procedure for the determination. 1. To 50.0 mL of unknown solution containing nitrite is added 1.00 mL of sulfanilic acid solution. 2. After 10 min, 2.00 mL of 1-aminonapthalene solution and 1.00 mL of buffer are added. 3. After 15 min, the absorbance is read at 520 nm in a 5.00-cm cell. The following solutions were annaylzed: A. 50.0 mL of food extract known to contain no nitrite(that is a neglible amount); final absorbance =0.153 B. 50.0 mL of food extract suspected of containg nitrite ; final absorbance= 0.622 C. Same as B, but with 10 microliters of 7.50x10^-3 M NaNO2 added to the 50.0 mL sample; final absorbance= 0.967 a) Calculate the molar absorptivity of the colored product. Remember that a 5.00 cm cell was used b) How many…