During a mass spectrometry experiment, the spectrum of vascular endothelial growth factor A (VEGF-A) was acquired. The absolute error of VEGF-A, having a mass of 1024.5210 Da was 0.06 Da. Calculate the relative error (ppm).

During a mass spectrometry experiment, the spectrum of vascular endothelial growth factor A (VEGF-A) was acquired. The absolute error of VEGF-A, having a mass of 1024.5210 Da was 0.06 Da. Calculate the relative error (ppm).

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

How are you supposed to answer this question if no values are given besides the Kb of the possible analytes?
3.25 mL of Biomarker A (4.21 x 10-7 mol L-1) was brought up to volume with deionized water in a 50 mL volumetric flask. What is the final concentration after this dilution (in mol/ L)
The absorbance of a cationic iron(II) sample solution was measured in a spectrophotometer, but the instrument returned an error because the absorbance was too high. The sample was then diluted by using a pipette to take 100.0 μLμL of the sample and injecting it into a cuvette already containing 2.00 mLmL of water (total volume is 2.00 mLmL + 100.0 μLμL). The absorbance value of the diluted solution corresponded to a concentration of 7.71×10−6 M M . What was the concentration of the original solution? Express the concentration to three significant figures with the appropriate units.
A student weighed out 0.150 g of protein powder and dissolved it in 100 mL of water (Solution 1). The student then diluted this solution by transferring 1 mL into a 25 mL flask and diluting with water (Solution 2). Finally, 1 mL of that solution was transferred to a test tube and combined with 4 mL Bradford reagent. The absorbance of the solution in the test tube was 0.187. Assuming that the best fit linear line of the standard curve was y = 0.04144 x + 0.01521 (μ g mL), calculate the percent protein by mass in the original protein powder.
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?
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.
Chemistry 0.1237 (±0.0001) g of sodium carbonate (Na2CO3) required 22.46 (±0.02) cm3 of aqueous HCl for complete neutralisation. Determine the concentration of the HCl in mol dm–3 together with its uncertainty in mol dm–3 to an appropriate number of digits. You may assume the error in the molar mass of Na2CO3 is negligible.
The data in the table are used to create a calibration curve for the determination of RNA from its absorbance at 260 nm. Use a spreadsheet and the least-squares method to determine the slope and y-intercept of the best straight line fit to the calibration curve. Do not subtract the blank reading when creating the calibration curve. m= RNA (µg) 0.00 10.29 20.58 30.87 41.16 mass= Absorbance at 260 nm 0.227 0.452 0.786 1.078 1.296 Hg-1 Using the slope and intercept of the calibration curve, determine the quantity of RNA in a sample that gives an absorbance of 0.523. µg
A student weighed out 0.150 g of protein powder and dissolved it in 100 mL of water (Solution 1). The student then diluted this solution by transferring 1 mL into a 25 mL flask and diluting with water (Solution 2). Finally, 1 mL of that solution was transferred to a test tube and combined with 4 mL Bradford reagent. The absorbance of the solution in the test tube was 0.11. Assuming that the best fit linear line of the standard curve was y = 0.04144 x + 0.01521 (μ g mL), calculate the percent protein by mass in the original protein powder.
Mass spectrometric measurements of zinc near the detection limit gave the following counts: 75.1, 68.2, 64.1, 93.5, 55.6, 70.8, 80.7, 72.3, 59.2, and 76.8. A blank solution was measured 10 times and gave a mean signal of 18 counts. A sample containing 1.20 µM Zn2+ gave a signal of 1 159 counts. What is the concentration detection limit for zinc?
As part of an analytical chemistry laboratory course, a student measured the Ca2+ content in two water samples, city-supplied drinking water and well-supplied drinking water, using two different analytical methods, flame atomic absorption spectrometry (FAAS) and EDTA complexometric titration. The results of this experiment are given in the table as the mean Ca2+concentration (?¯) and standard deviation (?) in parts per million (ppm). Each sample was measured five times (n=5) by each method. Method City-Supplied Drinking Water (?¯±?x¯±s) Well-Supplied Drinking Water (?¯±?x¯±s) FAAS 57.57±0.68 ppm 64.77±0.70 ppm EDTA titration 58.32±0.96 ppm 65.62±0.97 ppm Method Comparison: For each drinking water sample (city and well), compare the Ca2+ content measured by FAAS and EDTA titration. Calculate the ? value for each sample. Do the methods produce statistically different results at the 95% confidence level when measuring the Ca2+content of the city-supplied drinking water? Do the…
Calculate the standard deviation of the following results: 20,19,18,10,15,14