In the concentration range of 1 to 100 µg/mL P , phosphate suppresses the atomic absorption of Ca in a linear manner. The absorbance levels off, however, between 100 and 300 µg/mL P. Explain. How can this effect be reduced?
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In the concentration range of 1 to 100 µg/mL P , phosphate suppresses the atomic absorption of Ca in a linear manner. The absorbance levels off, however, between 100 and 300 µg/mL P. Explain. How can this effect be reduced?
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- DoA solution of copper(II) sulfate is observed to be blue in color. The maximum absorbance is expected to occur in what wavelength range? 500-560 nm (green) 380-435 nm (violet) 610-750 nm (red) 580-595 nm (yellow) 435-480 nm (blue). A solution containing the complex formed between two substances has a molar absorptivity of 9.32 X 103 L mol-1 cm-1 at 470 nm. a)What is the absorbance of a 6.24x10-5 M solution of the complex at 470 nm in a 1.00 cm cell? b)What is the percent transmittance of the solution described in (a)? c)What is the molar concentration of the complex in a solution that has the absorbance described in (a) when measured at 470 nm in a 5.00 cm cell . A solution containing the complex formed between two substances has a molar absorptivity of 9.32 X 103 L mol-1 cm-1 at 470 nm. a)What is the absorbance of a 6.24x10-5 M solution of the complex at 470 nm in a 1.00 cm cell? b)What is the percent transmittance of the solution described in (a)? c)What is the molar concentration of the complex in a solution that has the absorbance described in (a) when measured at 470 nm in a 5.00 cm cell
- please help with this textbook activity. I need parts A,B,C pleaseA mixture is prepared by combining 10.72 mL of 2.52 x 10-3 M Fe(NO3)3 with 10.00 mL of 1.76 x 10-3 M KSCN. The solution turns red due to the formation of FeSCN2+. The absorbance is measured and, using a calibration plot, the [FeSCN2+] at equilibrium is found to be 2.25 x 10-4 M.Complete the following ICE table Fe3+ + SCN- ⇌ FeSCN2+ initial (M) (A) (B) (C) change (M) (D) (E) (F) equilibrium (M) (G) (H) (I) What is the value of Kc?4. To analyze the Cu(NO3)2 unknown solution in Part 3, your group constructed a plot of absorbance vs. concentration, commonly called a calibration curve or standard curve. The absorbance at the top of the peak (i.e., at the wavelength of maximum absorbance) was chosen for these measurements. What is the potential advantage of using the wavelength of maximum absorbance, rather than some other wavelength? Can you think of a situation in which you might want to choose a different wavelength? (Hint: Scientists often do not have the luxurý of analyzing pure substances dissolved in distilled water!)
- A solution in part C initially contains (4.06x10^-4) molar SCN¯ and (2.960x10^-3) molar Fe3+. This solution was then measured using the colorimeter, and an absorbance of (4.9800x10^-1) was recorded.The constant determined in part A of the experiment was found to be (3.8200x10^3). Using the data provided above, determine the equilibrium concentration of SCN", [SCN]E in this solution. Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: x10 Answer unitsA 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 solution containing a complex formed between thiourea and Bi (III) has a molar absorptivity of 9.32 × 103 L / cm.mol at 470 nm. Questions: A) What is the absorbance of a 5.67 × 10-5 M solution of the complex at 470 nm in a 1.00 cm cell? B) What is the transmittance of the solution? C) What would the concentration be if we have the same absorbance obtained in (a) at 470 nm in a 2.50 cm cell?
- The iron content of a municipal water supply was determined by an atomic absorption procedure. The absorbance of the water, after a ten-fold dilution was 0.500 at 248.3 nm. A standard solution prepared by dissolving 0.1500 g of pure iron wire in acid, diluting to 1.00 L and then making a 25-fold dilution, had an absorbance of 0.750. Calculate the ppm Fe in the water sample.Ligand X forms a complex with both cobalt and copper, each of which has a maximum absorbance at 510 nm and 645 nm, respectively. A 0.256 g sample containing cobalt and copper was dissolved and diluted to a volume of 100.0 mL. A solution containing ligand X was added to a 50.0 mL aliquot of the sample solution and diluted to a final volume of 100.0 mL. The measured absorbance of the unknown solution was 0.484 at 510 nm and 0.354 at 645 nm, when measured with a 1.00 cm cell. The molar absorptivities of the cobalt and copper complexes at each wavelength are shown in the table. Molar Absorptivity (e, M-¹cm-¹) Wavelength λ, nm 510 645 [Co²+] = What is the concentration of cobalt and copper in the final diluted solution? [Cu²+] = Co 36437 1241 wt% Co²+ = Cu 5526 17520 What is the weight percent of cobalt (FM = 58.933 g/mol) and copper (FM = 63.546 g/mol) in the 0.256 g sample? wt% Cu²+ == M M %3a) What is the unit of absorbance? b)When he exponential trend line of iron concentration vs time is y=4.2 exp(-0.24x) x is time in min and y is concentraion of phen iron complex solution. c)Explain the relationshipp between temperature vs decay constant and temperature vs half life. d) The concentration of iron in solution a is 5 mg/l. A total volume of solution a is 10 mL in beaker. If 20ml of phenanthroline solution is added into the solution A beaker. Wha is the final concentration of ionafter two solutions are mixed. e)Why do we need to blank or zero the specrometer??
