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- You have a solution with a concentration of 0.80 mM, and you put it in a cuvette with a 1.0cm pathlength. You read an absorbance of 0.400. What is the extinction coefficient of your analyte? Question 4 options: 0.50 mmole/L/cm 0.50 mmol/L (cm)-1 0.50 L/mmole/cm 0.50 mM cmHere is the protocol for a UV-Vis spectrophotometer to detect water and chlorine-carbon. 1.Dissolve the water and chlorine-carbon compounds in a solvent, such as water. 2.Prepare a standard solution of known concentration that is similar to the sample being measured. 3.Calibrate the spectrophotometer using the standard solution. 4.Measure the absorbance of the sample using the spectrophotometer. 5.Calculate the concentration of the compounds in the sample using the calibration curve obtained from the standard solution. How is the spectrophotometer calibrated with standard solutions? When is the blank solution placed in the spectrophotmeter?A 0.1 g amine-containing compound is dissolved in water then diluted to 100 mL. You subject it to spectroscopic analysis, in order to get the concentration of amine in this compound. Next, you get 1 mL of the previously diluted sample then dilute it again to 250 mL for measurement. Then, you fill 3/4 of a 1-cm cuvette with this diluted sample, and you run an analysis using an AAS. The recorded absorbance is 0.545 at 410 nm. What is the molecular weight of the compound? (The molar absorptivity is 1.23 x 104 cm-1 mol-1 L.)
- A. Copper sulfate pentahydrate is often used to teach students about Beer’s Law by making a standard curve (linear regression). The bright blue color of the solution has a peak absorbance in the red range of the electromagnetic spectrum. The absorbance value is proportional to concentration. How many grams of CuSO4 5H2O to make up 250 mL of a 0.2 M stock of this solution? B. Using M1V1 = M2V2 how many mL would a student need to measure out in graduated cylinder to make up a 50 mL (V2) solution of 0.1M, 0.05 M, 0.025M 0.0125M solutions for a standard curve at the peak wavelenth for this compound?A. Copper sulfate pentahydrate is often used to teach students about Beer’s Law by making a standard curve (linear regression). The bright blue color of the solution has a peak absorbance in the red range of the electromagnetic spectrum. The absorbance value is proportional to concentration. How many grams of CuSO4 5H2O to make up 250 mL of a 0.2 M stock of this solution? B. Using M1V1 = M2V2 how many mL would a student need to measure out in graduated cylinder to make up a 50 mL (V2) solution of 0.1M, 0.05 M, 0.025M 0.0125M solutions for a standard curve at the peak wavelenth for this compound? I need help with part B of this question.A 0.1 g amine-containing compound is dissolved in water then diluted to 100 mL. To get the concentration of amine in this compound, you subject it to spectroscopic analysis. So, you get 1 mL of the previously diluted sample then dilute it again to 250 mL for measurement. Then, you fill 3/4 of a 1-cm cuvette with this diluted sample then you run an analysis using an AAS. The recorded absorbance is 0.545 at 410 nm. Solve for the molecular weight of the compound. The molar absorptivity is 1.23 x 104 cm-1 mol-1 L.
- After creating her standard curve for absorption versus the concentration (M) of FD&C Red 40, a student found that her best fit linear line for FD&C Red 40 was y = 2,962x + 0.005. Her Kool-Aid sample had an absorbance of 0.685. If 0.543 grams of Kool-Aid powder was used to prepare an 8-fl oz cup of her assigned flavor, what is the percent by mass of FD&C Red 40 in her 8-fl oz cup?A calibration plot of absorbance vs concentration (ppm) was obatined with standard known Red 40 dye solution. - the slope of the best-fit straight line of the plot is 0.057 ppm^-1 - The absorbance of the dilute unknown sports drink was 0.88 What is the concentration of this dilute unknown sports drink?______ the answer is 15.4 ppm ( can you please show me how to calculate this problem)Which statement is true? Statement 1: In Thin Layer Chromatography (TLC), the polar compounds will have a greater Rf value compared to that of non-polar compounds.Statement 2: The stationary phase in TLC is polar.
- Using the calibration curve y=0.146x+-0.368 find the the quantity of unknown protein that gives a measured absorbance of 0.918 when a blank has an absorbance of 0.138.2. In UV and visible spectrophotometry, the specimen is generally dissolved in a solvent, and determinations are made at room temperature using a path length of 1 cm. Give the most common solvents suitable for UV or visible spectrophotometry.Can you TYPE the definitions of the all of words please Chromatography TLC Stationary phase Mobile phase Elute Eluent Rf Value Elution chamber TLC “spotter”