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- The absorbance values at 250nm of 5 standard solutions, and sample solution of a drug are given below: Conc. (ug/ml) A 250 nm10 0.16820. 0.32930 0.50840. 0.66050 0.846Sample. 0.661Calculate the concentration of the sampleIn the determination of Pb in a contaminated fishmeal, 5.08 g of sample was weighed. Digestion with acids was applied and brought to dryness. Then it was made up to 10 mL and the absorbance was measured, obtaining a value of 0.013. The concentrations of the calibration curve made in ug/L are: 0.011; 0.022; 0.042 and 0.084 and the absorbances are: 0.001; 0.004; 0.009 and 0.020. Calculate the concentration of Pb in the sample in ug/kg and the % of Pb in the fishmeal.A solution with a “true” absorbance [A=-log(P0/P)] of 2.10 was placed in a spectrophotometer with a stray light percentage (Ps/P0) of 0.75. What absorbance A' would be measured? What percentage error would result?
- In the development o f an analytical method for the quantitative analysis o f iron using Atomic Absorption spectrophotometry (AAS), a linear calibration curve for standards o f 0.00, 5.00, 10.00, 15.00 and 20.00 ppm was prepared. An iron ore sample with an expected iron content o f 40-60% w/w is to be analysed by this method. An approximately 0.5-g sample is taken, dissolved in a minimum amount o f concentrated HC1 and diluted to 1 L in a volumetric flask using distilled water. A 5.00-mL aliquot is removed with a pipette. With explanation, to what volume (10, 25, 50, 100, 250 500 or 1000 mL) should the 5.00 mL aliquot be diluted, to minimize the uncertainty in the analysis?.Q1. To determine the concentrations (mol/L) of Co(NO3)2 (A) and Cr(NO3)3(B) in an unknown sample, the following representative absorbance data wereobtained.A (mol/L) B (mol/L) 510nm 575nm5×10−1 0 0.714 0.0970 6×10−2 0.298 0.757Unknown Unknown 0.671 0.330Measurements were made in 1.0 cm glass cells.i. Calculate the four molar absorptivities: ∈A(510), ∈A(575), ∈B(510) and ∈B(575).ii. Calculate the molarities of the two salts A and B in the unknown.Prepare a calibration curve to determine the Pb content in a well water sample using atomic absorption spectrophotometry; the following data were recorded: % T 100 75.2 56.6 42.5 31.9 24.6 13.8 ppm Pb 0 0.2 0.4 0.6 0.8 1.0 1.4 A 50 mL aliquot of well water is taken and diluted twice, the% T reading is taken and a value of 40.6% is recorded. Calculate the ppm of Pb in the well water.
- 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 acid-base indicator HIn undergoes the following reaction in dilute aqueous solution: HIncolor1H++Incolor2 The following absorbance data were obtained for a 5.00 I0-4 M solution of HIn in 0.1 M NaOH and 0.1 M HC1. Measurements were made at wavelengths of 485 nm and 625 nm with 1.00-cm cells. 0.1 M NaOH A485 = 0.075 A625 = 0.904 0.1 M HC1 A485 = 0.487 A625 = 0.181 In the NaOH solution, essentially all of the indicator is present as In-; in the acidic solution, it is essentially all in the form of HIn. (a) Calculate molar absorptivities for In- and HIn at 485 and 625 nm. (b) Calculate the acid dissociation constant for the indicator ¡fa pH 5.00 buffer containing a small amount of the indicator exhibits an absorbance of 0.567 at 485 nm and 0.395 at 625 nm (1.00-cm cells). (c) What is the pH of a solution containing a small amount of the indicator that exhibits an absorbance of0.492 at 485 nm and 0.245 at 635 nm (1.00-cm cells)? (d) A 25.00-mL aliquot of a solution of purified weak organic acid HX required exactly 24.20 mL of a standard solution of a strong base to reach a phenolphthalein end point. When exactly 12.10 mL of the base was added to a second 25.00-mL aliquot of the acid, which contained a small amount of the Indicator under consideration, the absorbance was found to be 0.333 at 485 nm and 0.655 at 625 nm (1.00-cmcells). Calculate the pH of the solution and Ka for the weak acid. (e) What would be the absorbance of a solution at 485 and 625 nm (1.50-cm cells) that was 2.00 10-4 M in the indicator and was buffered to a pH of 6.000?