Using the data below, please create a calibration graph and determine the concentration of the unknown sample.| | Standard #1 | Standard #2 | Standard #3 | Unknown sample ||-----------------|--------------|--------------|--------------|----------------|| Concentration | 1.5 x 10^-3 M | 2.0 x 10^-3 M | 2.5 x 10^-3 M | ? || Absorbance | 0.61 | 0.80 | 0.98 | 0.72 |a) 1.6 x 10^-3 M b) 1.8 x 10^-3 M c) 2.1 x 10^-3 M d) 2.2 x 10^-3 M To determine the concentration of the unknown sample, plot the concentration values of the standards on the x-axis and the absorbance values on the y-axis. Use these points to draw a calibration line. Then, locate the absorbance value of the unknown sample (0.72) on the y-axis and find the corresponding x-axis value to estimate its concentration.

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Answered: Using the data below, please create a…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A 10.0-mL aliquot of a standard manganese solution containing 62.5 mg/L of Mn is oxidized to MnO4- and diluted to 50.0 mL in a volumetric flask. The absorbance is measured in a 1.00-cm cell at 525 nm is 0.343. Next, a 850-mg steel sample containing manganese in dissolved in acid and diluted to 250 mL. A 50.0-mL aliquot is treated with KIO4 to oxidize Mn to MnO4- and diluted to 100.0 mL. If the absorbance at 525 nm is 0.468 in a 1.00-cm cell, calculate the weight percent of Mn in the steel.
You have prepared several dilutions of a standard compound. You measure the absorbance of each solution at 340 nm using a 1 cm cuvette and your results are listed in the table below. Determine the concentration of an unknown sample with an absorbance of 0.085 at 340 nm. Concentration (uM) Absorbance at 340 nm 2. 0.009 4. 0.020 0.061 16 0.111 32 0.189
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The molar absorptivity constant of a particular chemical is 2.31 M/cm. Determine the concentration of a solution made from this chemical that has an absorbance of 0.521 with a cell path length of 1.04 cm.
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.
A solution with %T = 75.9% has an absorbance equal to: A = log (1 T) T= (% T 100)
Please find standard de
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Calculate the concentration of unknown red dye solution
Concentration Fe(SCN)2+ (M) Absorbance 0.0001 0.386 0.0002 0.774 0.0003 1.154 0.0004 1.527 0.0005 1.931 Question 2 Analysis Section 1 1. Open a spreadsheet program, like Excel or Desmos, and plot your data points, with Absorbance on the y-axis and Concentration on the x-axis. 2. Fit a linear trendline and make sure the equation is labeled on your graph, including the R² value. 3. Fill in your equation below. Absorbance = -Concentration + The slope of your equation gives you the s-1 in the Beer's law equation: A = scl. Since I = 1 cm, the slope is equal to the ɛ of Fe(SCN)2+. The units of & are 1/(M*cm).
solve question i & ii

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