Suppose that a solution has an absorbance of 0.226 at a wavelength of 450 nm. If the concentration of the solution is 24 μM, what is the value of the molar absorptivity? The data were taken with a standard 1-cm cuvette.
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Suppose that a solution has an absorbance of 0.226 at a wavelength of 450 nm. If the concentration of the solution is 24 μM, what is the value of the molar absorptivity? The data were taken with a standard 1-cm cuvette.
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- Suppose that a solution has an absorbance of 0.250 at a wavelength of 450 nm. If the concentration of the solution is 22 μM, what is the value of the molar absorptivity? The data were taken with a standard 1-cm cuvette. molar absorptivity in (L cm^−1 mol^-1):Calculate the molar absorptivity of a solute when its measured absorbance is 1.050 with a concentration of 1.45 x 10-3 M. Assume the path length of the cell is 1.0 cm.A 5.00×10−4 M solution of analyte is placed in a sample cell that has a pathlength of 1.00 cm. At a wavelength of 490 nm, the solution’s absorbance is 0.338. What is the analyte’s molar absorptivity at this wavelength?
- A group of students made 5 standard solutions and measured their corresponding absorbance values at a wavelength of 525.0 nm to generate the graph below. Absorbance of Standard Solutions to Find Concentration of Unknown X Solution 0.50 y = 75.9x + 0.0045 R? = 0.9946 0.40 %3D 0.30 0.20 0.10 0.00 0.001 0.002 0.003 0.004 0.005 0.006 Concentration of X (mole/L) The colorless reactants V and W form unknown X from the reaction: 2V + W 5 X A solution is prepared by mixing together the following: Volume 0.0150 M V (mL) Volume 0.0150 M W (mL) 6.00 4.00 This solution reaches equilibrium, and then is placed in a 1.00 cm wide cuvet and inserted into the spectrometer, producing an absorbance reading of 0.275 at a wavelength of 525.0 nm. Calculate Keg for the above reaction, including units. AbsorbanceThe nitrite in a series of standard solutions (mg/L, n = 5) are converted to azo dye and the slope of the calibration curve is 2.0 ppm. A 10.00-mL mineral water sample is treated in the same way as standards and diluted to a final volume of 100.00-mL It gives an absorbance of 0.80. The absorbance of blank solution under the same conditions is 0.10. Calculate ppm (mg/L) of NO2 (46 g/mol) and the molarity of NaNO2 (69 g/mol) in the original sampleA student prepared four standard solutions of (NH4)2Fe(SO4)2 and measured their absorbance at 505 nm. She created a calibration plot with the best-fit line of y = 9372 x + 0.0539. She measured the absorbance of her diluted unknown sample solution as (4.69x10^-1) nm. If she prepared her diluted sample solution by diluting 10.00 mL of the original solution to a total volume of 50.00 mL with deionized water, what is the concentration of Fe2+ in her original solution? Answer in units of M. Note: Your answer is assumed to be reduced to the highest power possible.
- From experimental data, a plot of absorbance (in arbitrary units, a.u.) at a wavelength of 630 nm (on the y-axis) was plotted against the concentration (in mg/L) of Cu2+ (on the x-axis) in known solutions and a linear relationship was found with an equation of y = 7.22x+0.05. If an unknown solution had an absorbance of 1.20 a.u. at a wavelength of 630 nm, what is its concentration of Cu2+?The concentration of a dilute aspirin solution is 0.000530 M 0.000530 M . Standard solutions of this compound were used to prepare a Beer's law plot which gives a slope of 1550.1 M −1 1550.1 M − 1 . What is the expected absorbance value for the aspirin solution?In an analytical laboratory a chemical compound namely Paracetamol (151.163 g/mol) is determined in a sample. A sample weighing 0.0295 g was dissolved in a solvent and diluted the solution to 1 L. The solution has λ max at 243 nm (ε=2.6×104 cm-1 mol-1 L). The solution exhibits an absorbance of 0.638 in a 2 cm cell. Calculate the percentage paracetamol in the sample.
- A standard curve of absorbance vs. concentration has a linear trendline of y = 0.56x + 0.987. Use this trendline to calculate the concentration of an unknown sample that has an absorbance of 1.245.Calculate the concentration of a colored solution if the molar absorptivity is 39.80 M-1•cm-1 and the absorbance is 0.777. The path length of the sample is 1.00 cm.Calculate the molar absorptivity of benzene (FW = 78.11 g/mol) at 256 nm if a 25.80 mg of benzene per 250.0 mL solution using hexane (FW = 86.18 g/mol) as the solvent exhibited an absorbance of 0.2660 in a 10.00 cm cuvette. Pure hexane has negligible absorbance at this wavelength.