A standard of solution was put through appropriate dilutions to give the concentrations of glucose (mM) shown in the accompanying table. The absorbances in the table (1.00-cm cells) were recorded at 490 m table. Use the method of least squares to find an equation relating absorbance and the concentration of glucose.

15) You measure a solution that contains two organic molecules in a 1.00 cm cuvette. The measurement is 0.2265 at 700 nm and 0.9205 and 320 nm. What are the concentrations of compound A and compound B. = 3520 M'cm';e, Compound A: Compound B: e = 620 M'cm' 700m 320nm e = 13130 M'cm" ; e = 3600 M 320nm 700m 'cm'

A liquid sample was analyzed for Fe³+. A plot of absorbance (y-axis) vs. concentration (ppm; x-axis) of the external standards produced a calibration line with an equation y = 0.2256x -0.0903 (R² = 0.9973). The absorbance of the sample was 1.25. Determine the amount of Fe³+ in the sample (in ppm).

Calculate the path length in centimetres which would give an absorbance of 0.134 of a colored dye with a molar absorptivity of 0.759 L mol-1 cm-1 at a wavelength of 645 nm if the concentration of the dye is 6.82x10-2 M. Report your answer to 3 significant figures.

The equation to calculate for molar absorptivity (ε) is ε = A/(bc) where A is absorbance (unitless), b is path length in cm, and c is concentration in M. Suppose you have a solution with concentration of 2.9 ± 0.25 M, a path length of 1 ± 0.1 cm, and an absorbance of 0.4629 ± 0.0006. What is the uncertainty or error for the molar absorptivity?

A colored ion solution has a concentration of 0.200 M with a measured absorbance A = 0.880. Another ion solution made of the same chemicals has an absorbance A = 0.172. What is the concentration of this unknown sample solution?

A compound with a molecular weight of 229.61 g/mol was dissolved in 50.0 mL of water. 1.00 mL of this solution was placed in a 10.0 mL flask and diluted to the mark. The absorbance of this diluted solution at 510 nm was 0.472 in a 1.000 cm cuvet. The molar absorptivity of the compound, at 510 nm, is 6,310 M-1 cm-1. Calculate the concentration of the compound in the initial 50.0 mL solution. A. 1.50 x 10-5 M B. 7.48 x 10-5 M C. 7.48 x 10-4 M D. 7.48 x 10-6 M

If the absorbance for the solution was 0.342, calculate the equilibrium constant, Keq, with zero places after the decimal.

Maria was tasked to determine the concentration of a Fe2(SO4)3 solution. She prepared 5 different standards of Fe2(SO4)3 using the table below as her guide. She ran the standards and the unknown solution through UV-VIS spectroscopy and recorded the absorbances of each solution.   HINT: use the dilution equation to determine the concentration of Fe2(SO4)3 in each test tube before preparing the standard curve. NOTE: No need to force the line to pass through zero. Just graph the data as is.   What is the slope of the line of the standard curve from the given data? What is the concentration of the unknown solution?

While performing absorbance measurements of standard solutions, Taranpreet used - 8 mL of solution in the cuvette for each determination. She then repeated the same measurements using - 6 mL of solution In the cuvette for each determination, For each set of measurements, she used the same spectrometer with the same cuvette, and assume that for each set of measurements the cuvette was filled high enough such that the light from the spectrometer passed through the solution. Which statement is true? O a) Using a lower volume in the cuvette will have no effect on the measured values O b) Using a lower volume in the cuvette will result in a smaller slope for the calibration curve c) Using a lower volume in the cuvette will result in a lower concentration of analyte determined in the unknown sample O d) Using a higher volume in the cuvette may result in absorbance values that are above the detection range of the spectrometer O e) Using a higher volume in the cuvette may result in a…