A student prepared a series of starch standards using the iodine method and measured the absorbance at 590 nm. She obtained the following data.
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- A standard curve was performed using an Absorbance spectrophotometer, and the equation of that line was determined to be y = .1563x + .025. The absorbance of an unknown was measured at .35. Calculate the concentration of the unknown according to the standard curve.Given that the percent transmittance of light through a sample was 27.6% what is the absorbance of the solution? Rounded to two sig figs.In determining the amount of copper and the identity of the copper compound in the unknown sample, a 100-mL solution containing 120.8 mg of the sample was initially prepared. Then, 5.00 mL of this solution was pipetted and diluted with deionized water in another 100-mL volumetric flask. The absorbance of this diluted solution was determined three times at the analytical wavelength. The concentration of Cu is 12.678 mg/L, what is the mass of Cu in the analyzed solution and the mass of Cu in the unknown sample?
- A 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.Please complete Table 2 and show the calculations for protein concentration and the concentration of the undiluted sample. a). Using Excel software, enter data from Table 1 to plot a standard curve (corrected average absorbance on Y-axis and protein concentrations on X-axis). The standard curve must contain correct labels on both axes. b). From the standard curve, obtain a best fit line and equation. c). Use the best fit equation and data from Table 2 to find the concentrations of proteins in sample A2-D2 and E1. [onto your plotted standard curve, indicate where A595 of A2-D2 and E1 are located] d). Calculate the concentrations of proteins in undiluted samples A to E. Thank you very much.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.
- An unknown concentration of [FeSal]+ gave an absorbance reading of 0.301. Calculate the concentration of the solution, given that the slope of the standard curve was 1280 and the y intercept was -0.00821.A 131.7 mg sample of powdered Carbamazepine tablets was boiled with ethanol, filtered and then made up to 100 mL with ethanol. 5 mL of this solution was then diluted to 250 mL with ethanol and the absorbance at 285 nm found to be 0.486 in a 1cm path length cell.Calculate the content (% m/m) of Carbamazepine in the powder, taking A(1%, 1 cm) as 490.(State your answer to 1 decimal place and include the units)Five standard chromium (VI) solutions were prepared through serial dilution technique with corresponding absorbance readings at 540 nm wavelength (as follows: Absorbance Concentration A1 = 0.650 C1 = 1.9 ppm A2 = 0.712 C2 = 4.0 ppm A3 = 1.370 C3 = 6.0 ppm A4 = 2.050 C4 = 8.0 ppm A5 = 3.423 C5 = 10.0 ppm The sample solution gives an average absorbance reading of 0.713. What is then the concentration of chromium (VI) ion in the sample?
- Five standard chromium (VI) solutions were prepared through serial dilution technique with corresponding absorbance readings at 540 nm wavelength as follows: Absorbance Concentration A1 = 0.650 C1 = 1.9 ppm A2 = 0.712 C2 = 4.0 ppm A3 = 1.370 C3 = 6.0 ppm A4 = 2.050 C4 = 8.0 ppm A5 = 3.423 C5 = 10.0 ppm The sample solution gives an average absorbance reading of 0.713. What is then the concentration of chromium (VI) ion in the sample? (Note: please provide necessary solutions)The nickel level in a soil sample was determined using AAS. A 3.0 g sample was dissolved in acid and then diluted to a total volume of 100.0 mL. The absorbance of this solution determined at a wavelength of 232 nm, was found to be0.3. Several standard solutions were tested under the same conditions and a calibration curve shown below was obtained. Calculate the mass of nickel in mg.You are measuring the concentration of an unknown protein sample, and the absorbance at 595 nm (or A595) of your unknown is greater than that of the highest-concentration standard solution. It is not advisable to simply extrapolate the line of the standard curve to calculate the concentration of the unknown In this scenario, what would be the best strategy to measure the concentration of your unknown (instead of extrapolating from the standard curve)?