2. Use the trendline equation from the calibration plot (that you wrote down in Table 2) to calculate the concentration of the unknown solution. Hint: the trendline equation is in the format of y = mx + b, where y is the absorbance (from Table 2) and x is the unknown concentration (that you will solve for). Try to show your work by typing into the group discussion, or you have the option to hand-write and submit a picture of your hand- written work.

2. Use the trendline equation from the calibration plot (that you wrote down in Table 2) to calculate the concentration of the unknown solution. Hint: the trendline equation is in the format of y = mx + b, where y is the absorbance (from Table 2) and x is the unknown concentration (that you will solve for). Try to show your work by typing into the group discussion, or you have the option to hand-write and submit a picture of your hand- written work.

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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Absorbance = 2.000 - log(%T) If %T = 12.6% what is the absorbance of the solution?
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After determining the absorbance of several standards of known concentration, the trendline for a calibration curve (AKA a standard curve) plotting absorbance (y-axis) against concentration (M, x-axis) is determined to be y = 4.586x + -0.0010 %3D The absorbance of a solution of unknown concentration is determined to be 0.68. Calculate the concentration of the unknown solution in M. Give your answer to thrėe decimal places.
How would I do 2? the concentration iron is 1.85mg/vitamin tablet, and the absorbance at 508nm is 0.37
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The best fit curve line to an absorbance vs. concentration plot for standard solutions of a dye has a slope of 0.1815 mL/mg and intercept of 0.0477. A sample solution prepared of the same dye has an absorbance of 0.464 at the wavelength used to establish the Beer's law plot. What is the concentration of dye in the prepared solution? Select one: O a. 0.132 mg/mL b. 2.29 mg/mL O c. 0.464 mg/mL O d. 2.82 mg/mL e. 0.0365 mg/mL Next page Law Tutorial Part 2 Jump to... Exp #9 - Laboratory Practical► Worksheet étv A
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After determining the absorbance of several standards of known concentration, the trendline for a calibration curve (AKA a standard curve) plotting absorbance (y-axis) against concentration (M, x-axis) is determined to be y = 4.943x + -0.0001 The absorbance of a solution of unknown concentration is determined to be 0.48. Calculate the concentration of the unknown solution in M. Give your answer to three decimal places.
Determine the concentration of your prepared Iron (III) Salicylate Dianion solution (pure ASA) in the 10.0 mL of 1.0 M NaOH in mg/mL (Part D) using Beer's Law plot. Hint:You need to use the measured absorbance reading of your prepared Iron (III) dianion (absorbance reading: 0.83). Information from the plot: Standard: Concentration ofASA in Standards (mg/mL) A: 0.18 B: 0.14 C: 0.10 D: 0.070 E: 0.040 Mass of salicylic acid (g) 0.17g Volume of acetic anhydride (mL) 0.34mL Mass of filter paper (g) 0.35gMass of "impure" ASA and filter paper (g) 0.49g Mass of prepared "impure" ASA (g) 0.14g Melting point range of prepared ASA (°C) 20.9 °C Melting point range of standardASA (°C) 18.5°C Percent purity: 28.57% Percentage yield: 66.7% Chemical equation: C7H6O3 + C4H6O3pure ASA knowing that two consecutive dilutions were done to prepare the solution. Show all of your work.C9H8O4 + C2H4O2 b) Then, calculate the mass (in mg) of