You prepare several dilutions of an unknown compound. You measure the pance of each solution at 340 nm using a 1 cm cuvette (your results are listed in the table- -). What is the extinction coefficient (in (Mecm)') of the compound? (Hint: assume that of the individual values contains some degree of experimental error.) entration(µM) Absorbance at 340 nm 0.011 0.023 0.066 0.119 0.189

You prepare several dilutions of an unknown compound. You measure the pance of each solution at 340 nm using a 1 cm cuvette (your results are listed in the table- -). What is the extinction coefficient (in (Mecm)') of the compound? (Hint: assume that of the individual values contains some degree of experimental error.) entration(µM) Absorbance at 340 nm 0.011 0.023 0.066 0.119 0.189

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...

See similar textbooks

Similar questions

Consider the fictional transition metal 'Gc' and the complex ions formed with it: [GcI.], [Gc(NH;).]*+, and [Gc(C:O.).]>- If the A of max absorbance for one of the solutions is 450 nm, what are the possible colors for each of the solutions? (A) [GcI]³ could appear yellow, [Gc(NH;).]+ could appear purple, and [Gc(C,O.):]}- could appear blue. (B) [GcI.]- appears purple, [Gc(NH;).]+ could appear yellow, and [Gc(C.O.);]- could appear blue. (C) [GcI6]3- could appear purple, [Gc(NH3)6]3+ could appear yellow, and [Gc(C204)3]3- could appear orange. (D) [GcI6]3- could appear yellow, [Gc(NH3)6]3+ could appear purple, and [Gc(C204)3]3- could appear orange. (E) Not enough info
What is the molar extinction coefficient at 625 nm for this copper (II) acetate solution? How was it determined? Standard Solution Concentration (M) Absorbance 1 0.025 0.049 2 0.050 0.153 3 0.100 0.242 4 0.200 0.499 5 0.250 0.694
Using the concentrations found in the experiment for the iron cation and thiocyanate anion determine the Kc for iron (III) thiocyanate using 1.71mL of iron cation solution and 4.00 mL of thiocyanate anion solution. The absorbance for this mixture at 460 nm is 0.339.
In general, we want to have absorptions less than or equal to 1. Given that an ethanol solution of compound Y (150.0 g/mol) in a 1.00 cm quartz cell has an extinction coefficient (E) of 23,150 at Amax=235 nm, what is the top concentration, in uM, we should consider for compound Y? Report your answer to the correct number of significant figures.
There is a substance in a solution (8 g/liter). The length of cuvette is 2 cm and the extinction coefficient is 0.0376 M-1 cm-1, how much is the beam of light is transmitted?
A 40-mL cigarette smoke sample was collected and made to react with 10 mL of the NOx indicator mixture solution. The color was allowed to develop and the absorbance reading a UV-Vis spectrophotometer at 550 nm. The absorbance reading of the sample was 0.570. Calculate: a. Concentration of NO₂ (in µg NO₂/mL) if the equation of the line from a standard calibration curve is: y = 1.259x + 0.0222 b. Concentration of NO₂ gas (in µg NO₂/L) in the gaseous sample
Please give me correct solution.
6. The UV-Vis absorption spectrum was measured for three different concentrations (10 mM, 20 mM, and 30 mM) of an analyte that we will call orangium as shown in the figure below. A 1.000 cm cuvette is used for all of the experiments. 1.00 0.90 0.80 0.70 0.60 a 0.50
2. One of the common methods used to determine phosphorus in urine isto treat urine with molybdenum(VI) resulting in a complex compoundof 12- molybdophosphate and then reduced using ascorbic acid produces a blue-colored compound called molybdenum blue (max = 650 nm). A patient's urine sample collected over 24 hours produced 1122 mL of urine. A total of 1 mL of the sample was treated with Mo(VI) and ascorbic acid and diluted until it reached a volume of 50 mL. A calibration curve is also prepared by treating 1 mL of standard phosphate solution in the same way. The absorbance of the standard solution and the sample was then measured at a wavelength of 650 nm and produced the following data: Solution Absorbance at λ 650 nm Phosphate 1 ppm Phosphate 2 ppm Phosphate 3 ppm Phosphate 4 ppm Urine sample 0,230 0.436 0,638 0,848 0.518 a. Create a calibration curve for the data and determine the slope, intercept, and R values of 2! Determine the concentration of phosphates found in urine samples…
If the absorbance for the solution was 0.342, calculate the equilibrium constant, Keq, with zero places after the decimal.
deriving equation from equation 2 and 3
2. One of the common methods used to determine phosphorus in urine isto treat urine with molybdenum(VI) resulting in a complex compoundof 12- molybdophosphate and then reduced using ascorbic acid produces a blue-colored compound called molybdenum blue (max = 650 nm). A patient's urine sample collected over 24 hours produced 1122 mL of urine. A total of 1 mL of the sample was treated with Mo(VI) and ascorbic acid and diluted until it reached a volume of 50 mL. A calibration curve is also prepared by treating 1 mL of standard phosphate solution in the same way. The absorbance of the standard solution and the sample was then measured at a wavelength of 650 nm and produced the following data: Solution Absorbance at λ 650 nm Phosphate 1 ppm Phosphate 2 ppm Phosphate 3 ppm Phosphate 4 ppm Urine sample 0,230 0.436 0,638 0,848 0.518 a. Create a calibration curve for the data and determine the slope, intercept, and R values of 2! Determine the concentration of phosphates found in urine samples…