cheer wine lab

can you explain how I can get 1.596 mg/L of concentration of Fe3+ in dilutes sample and can you also make the calibration curve.

Using the lab instructions and data table with data, please help me complete part 1 and 2 of my lab worksheet

A solution of a dye was analyzed by spectrophotometry, and the following calibration data were collected using a 1 cm cuvette. *graph in attachemnt*   Using the calibration data above for the dye solution, what is the dye concentration in a solution with an absorbance (A) = 0.52 if it was measured in a 1 cm cuvette?   Group of answer choices 3.0 x 10-6 M 6.0 x 104 M 2.0 x 10-6 M Not enough information is provided.

I need help finding the %Composition for %cychohexane and %toluene. The formula (area of peak/total area) * 100%

Determine the standard concentration of A through E and then the absorbance. I just need clarification on if I add together the two ml values given.

The ppm concentration of Pb2+ in a blood sample were measured with Spectrophotometry. 5.00 mL of a blood sample were taken and this sample gave a signal of 0.301 a.u.. Another 5.00 mL of a blood sample were mixed with 0.50 mL og 1.75 ppm Pb2+. Then, this mixture was diluted to 25.00 mL and this diluted mixture gave a signal of 0.406 a.u.. What is the ppm concentration of a blood sample?

NAME: LAB SECTION: EXPERIMENT 21: Spectroscopy of Dyes POSTLAB EXERCISE 1. AUV/V is a spectrometer used to measure the absorbance of a solution of hemoglobin bound to oxy- gen at 590 nm. The molar absorptivity was determined to be 8.57 × 104 M-'cm-. The cuvette used had a 1.00-cm sample pathlength. The measured absorbance was ), 140. What was the concentra- tion of hemoglobin in the solution? 2. What would be the absorbance of the solution in question 1 if the pathlength were 2.00 cm? nohntooote 196

The maximum number of spectra that can be recorded per second by ToF-MS is limited by the time taken by the slowest ions to go from the source to the detector. If the slowest ion took 45.6 microsecond to travel, at what frequency could you record spectra if a new extraction cycle were begun each time this heaviest ion reached the detector? 30000 spectra/s 10000 spectra/s 11000 spectra/s 500 spectra/s 22000 spectra/s

= 1 5 Absorbance vs. Concentration y = 0.2755x 0.2- 0.1- 1.400 2.000 1.800 1.600 1.000 0.200 1.200 0.400 0.600 Concentration (M) Using the calibration curve, calculate the molar concentration for a solution with a measured absorbance of 0.374. Round your answer to 3 significant digits Concentration = M X Sub Absorbance 0.7- 0.6- 0.5 0.4- 0.800

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.

3. The lead in a swab sample, lead standards, together with a blank were made up in 5.00 mL volumetric flasks using 0.2 % HNO3. 20 μL aliquots of these solutions were injected into the spectrophotometer and the absorbance measured at 217 nm. The following results were obtained. lead / ppb Absorbance 0 0.0591 10.00 0.0858 50.00 0.1926 100.0 0.3260 150.0 0.4594 200.0 0.5929 Swab sample 0.3700 (a) Determine the amount of lead in the swab sample in μg.

In the HQS-Mg fluorescence part of Lab 6, a calibration curve is made of fluorescence intensity vs. MgCl2 concentration (M). The standard solutions for the calibration curve were made by mixing a small amount of 0.01 M MgCl2 with some HQS solution. Calculate the concentration of MgCl2 (M) in each of the following standards. Report your concentrations to 3 sig figs. Fluorescence Volume of 0.01 M Volume of 1 mM Concentration of MgCl2 (M) Intensity MgCl2 (mL) HQS (mL) 0.031250902 0.8 100 0.049490754 0.8 50 0.059803507 2 100 0.085834029 3.6 100 Hint: The total volume of each solution is volume of 0.01 M MgCl2 + volume of 1 mM HQS.

To determine 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 data is in the table below.    Unknown sample Trial 1 Trial 2 Trial 3 Absorbance (AU) 0.378 0.379 0.377 What is the corrected absorbance?