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? a) Using a lower volume in the cuvette will have no effect on the measured values b) Using a lower volume in the cuvette will result in a smaller slope for the calibration curve O 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 calibration curve that is

0.1120 g of a solid sample containing copper was dissolved by acid and transferred to a 250.00 mL volumetric flask and volume was made up with distilled water.  The solution was then diluted by a factor of 25.  The final solution was analyzed by atomic absorption spectrophotometry and the concentration was found be 2.982 ppm, What is the weight percentage of copper in the original solid sample?  Keep four significant figures in your final answer.

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.

Sarah wasn't sure about Ben's results, so she repeated the experiment and found the best-fit line listed below for her standard calibration curve of absorbance vs concentration in M. y=34232 +0.0064 She then prepared a solution that had 5.00 ml 0.002 Miron(1) nitrate in 1 M nitric acid, 3.00 ml. 0.002 M potassium thiocyanate, and 2.00 mL DI water. If the absorbance for the solution was 0.603, calculate the equilibrium constant. Ke with zero places after the decimal Type your answer...

A 10.00 g sample containing an analyte was transferred to a 250 mL volumetric flask and diluted to volume. When a 10.00 mL aliquot of the resulting solution was diluted to 25.00 mL it was found to give a signal of 0.235 (arbitrary units). A second 10.00 mL aliquot was spiked with 10.00 mL of a 1.00 ppm standard solution of the analyte and diluted to 25.00 mL. The signal for the spiked sample was found to be 0.502. Calculate the weight percent of analyte in the original sample.

0.1040 g of a solid sample containing copper was dissolved by acid and transferred to a 250.00 mL volumetric flask and volume was made up with distilled water. The solution was then diluted by a factor of 20. The final solution was analyzed by atomic absorption spectrophotometry and the concentration was found be 3.109 ppm, What is the weight percentage of copper in the original solid sample? Keep four significant figures in your final answer. Do not try to include the "%" in your answer. e.g. if your final answer is 10.01%, only write 10.01 in the box.

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The determination of iron in wines was carried out by atomic absorption spectrophotometry, using the standard addition method. To do this, 10 mL of wine were placed in five 50 mL volumetric flasks; then 0, 5, 10, 15 and 20 mL of a 10 ppm iron standard solution were added to each of them. Next, they were gauged with distilled water and the absorbance was measured, obtaining the values ​​of 0.040, 0.062, 0.081, 0.102 and 0.125 respectively. Calculate the regression parameters and obtain the iron concentration in the wine, in µg / mL.

An unknown amount of a compound with a molecular mass of 270.57 g/mol is dissolved in a 10 mL volumetric flask. A 1.00 mL aliquot of this solution is transferred to a 25 mL volumetric flask, and enough water is added to dilute to the mark. The absorbance of this diluted solution at 355 nm is 0.495 in a 1.000 cm cuvette. The molar absorptivity for this compound at 355 nm is €355 = 6149 M-¹cm-¹. What is the concentration of the compound in the cuvette? concentration: What is the concentration of the compound in the 10 ml flask? concentration: How many milligrams of compound were used to make the 10 mL solution? mass: M M mg

A sample solution containing quinine was analysed by fluorescence spectroscopy. 5 mL of the sample solution was diluted with 0.1 M HCl to a final volume of 100 mL. The fluorescence of the solution was measured and gave a value of 54. A reference solution containing 0.086 mg/mL of quinine gave a fluorescence reading of 38. A blank solution gave a fluorescence reading of 21. Calculate the quinine content of the sample solution in mg/mL.