Answered: your understanding of today's…

your understanding of today's experiment, how would you explain to the student how she could determine the concentration of Blue #1 in her sample? Use your own Beer's

Living by Chemistry

2nd Edition

ISBN:9781464142314

Author:Angelica M. Stacy

Publisher:Angelica M. Stacy

ChapterU5: Fire: Energy , Thermodynamics, And Oxidation-reduction

SectionU5.116: How Absorbing: Spectroscopy

Problem 6E

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In determining the concentration of a sample X, it was found that it has maximum absorbance at 275 nm. Compound X, has molar absorptivity at 275 nm of 8400 L / mol.cm. Using a spectrophotometer with a 1 cm cuvette, an absorbance of 0.70 was found. What is the concentration of compound X in the sample?
2. You have two solutions of the same compound that are blue. One is very pale and the other is very intense. Absorbance of each solution was measured with a spectrophotometer at the same wavelength at which the solution absorbs. a) Which solution has the higher absorbance? b) Which is the more concentrated solution?
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In spectophotometry, what should be done if there is a greater absorbance reading than the most concentrated solution?
Two samples were analyzed using a colormeter on a cellphone: one containing only distilled water, and another containing an unknown solution. The distilled water sample had a Red value of 206, while the unknown solution had a Red value of 118. Calculate the absorbance of the unknown solution. -log (4) A = -log a) -0.242 b) 0.573 c) 0.242 d) 0.000 CASAT
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2. ] You make 150.0 mL of a copper(II) sulfate solution but forget to cover it before leaving for the day. The next class, you measure the volume and find that you only have 132.0 mL remaining. You didn’t record the initial concentration, but you measure the absorbance of the remaining solution at 620 nm and find that it is 0.386. You also construct the following calibration curve for CuSO4: Standard solution Abs620 0.50 M 0.424 0.40 M 0.336 0.30 M 0.247 0.20 M 0.159 (refer to image) a. What is the value for k (in Beer’s Law)? Provide a calculation or graph to support your answer. b. What is the concentration of the (remaining) solution? c. What was the concentration of the original solution from the first class? d. If you removed 7.5 mL from the 132.0 mL solution in the process of measuring the absorbance, how much water should you add to obtain the original concentration that you solved for in part (c)?
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I have 4 Questuion Q1: find the A , T , T% of a 2.4X10-3 mol L-1 solution of a substance whose molar absorptivity is 313 L M-1 cm -1 at 520 nm when measured in a cell of 2.00 cm pathlength ؟ Q2: A sample in a 1 cm cuvette transmits 79% of light at 280 nm , what is the absorbance ? if the molar extinction coefficient is 2.0 M-1 cm-1 , what is the concentration of the sample ? Q3 : the aspirin an analgesic form complex with metal ion which has a molar absorpitvity of 8000 L M-1 cm-1 at ( lenada max 435 nm ) . calculate the absorbance of 6.77 X 10-5 M solution of the complex measured in a 1.00 cm cell at 435 nm ? Q4 :Find the A and T% of a 6.5X10-4 Mol L-1 solution of a drug ( molecular weigth 200 ) whose absorpitvity is 0.026 L cm-1 g-1 at 520 nm when measured in a cell of 2.00 cm pathlength ?
A blue product absorbs light at 590 nm (ε590nm = 7,600 M-1 cm-1). Its concentration was too concentrated to determine an accurate absorbance reading. Therefore, the solution was diluted in the following manner before reading it's absorbance. 0.500 mL was added to 1.000 mL of water to make "Dilution 1". Then 0.700 mL of "Dilution 1" was added to 3.000 mL of water to make "Dilution 2". The absorbance reading of "Dilution 2" was determined to be 0.220 when using a 1 cm pathlength. Determine the millimolar (mM) concentration of the blue product in the enzyme reaction. Indicate the concentration to the precision of 3 decimal places. ANS: 0.078 nM. Would like some steps on how to get this answer. Thanks.