M¹ What is the concentration for each sample andwhat do I need to graph? thank You!Con. Standard50mg/LSampleVunknownVstandardViotalConc. Standard Absorbance Std Dev Abs(mL)(mL)(mL)(mg/L)(unitless)11.0000.000050.000.20270820.002031.0001.000050.000.22499140.0021831.0002.000050.000.51361890.003851.0003.000050.000.73972030.008141.0004.000050.000.84308160.000251.0005.000050.001.03503310.00807

A question based on quantitative analysis, which is to be accomplished.

Answered: What is the concentration for each…

Principles of Instrumental Analysis

7th Edition

ISBN:9781305577213

Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Chapter9: Atomic Absorption And Atomic Fluorescence Spectrometry

Section: Chapter Questions

Problem 9.2QAP

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The absorbance values at 250nm of 5 standard solutions, and sample solution of a drug are given below: Conc. (ug/ml) A 250 nm10 0.16820. 0.32930 0.50840. 0.66050 0.846Sample. 0.661Calculate the concentration of the sample
In the determination of Pb in a contaminated fishmeal, 5.08 g of sample was weighed. Digestion with acids was applied and brought to dryness. Then it was made up to 10 mL and the absorbance was measured, obtaining a value of 0.013. The concentrations of the calibration curve made in ug/L are: 0.011; 0.022; 0.042 and 0.084 and the absorbances are: 0.001; 0.004; 0.009 and 0.020. Calculate the concentration of Pb in the sample in ug/kg and the % of Pb in the fishmeal.
A solution with a “true” absorbance [A=-log(P0/P)] of 2.10 was placed in a spectrophotometer with a stray light percentage (Ps/P0) of 0.75. What absorbance A' would be measured? What percentage error would result?
SPECTROPHOTOMETRY 1.) Slope of regression line or Molar absorptivity (µM -1cm-1) is 0.0253 and absorbance of unknown solution is 0.131. What is the concentration of the unknown solution (µM )?
(9.29 × 105/8)-20.81 = with correct sig figs
Preparing a standard curve. 1. determine the absorbance max of [FeSCN]2+ it is 448.1 2. determine the concentration of FeSCN2+ in the stock solution. M1V1=M2V2 stock solution: ~0.200 M iron (iii) nitrate in 1M nitric acid intial volume: 0.3mL final volume: 10.3mL volume: 10mL ~0.002M potassium thiocyanate initial volume: 0.3mL final volume: 10.3mL volume: 10mL not sure if this is needed stock solutions: ~0.200M iron (iii) nitrate in 1M nitric acid: 0.207M ~0.002M iron (iii) nitrate in 1M nitric acid: 0.00209M ~0.002M potassium thiocyanate: 0.00193M
A calibration plot of absorbance vs concentration (ppm) was obatined with standard known Red 40 dye solution. - the slope of the best-fit straight line of the plot is 0.057 ppm^-1 - The absorbance of the dilute unknown sports drink was 0.88 What is the concentration of this dilute unknown sports drink?______ the answer is 15.4 ppm ( can you please show me how to calculate this problem)
1. a 50.00-mL sample containging an analyte gives a signal of 11.5(arbitrary units). A second 50-mL aliquot of teh sample, which is spiked with 1.00-mL of a 10.0-ppm standard solution of the analyte, gives a signal or 23.1. what is the concentration of analyte in the original sample?
A student completed Test Solution 1: 2.5 mL of 2.00×10−32.00×10−3 M Fe(NO3)3Fe(NO3)3 mixed with 0.5 mL of 2.00×10−32.00×10−3 M NaSCNNaSCN and topped with 2.0 mL of 0.1 M HNO3HNO3 to make a total of 5.0 mL solution. The absorbance of the solution was measured, and the calibration curve was used to calculate [FeSCN2+][FeSCN2+] at equilibrium. Concentration of [FeSCN2+][FeSCN2+] at equilibrium was 7.5×10−57.5×10−5 M. Complete the given chart and the calculation that follows. initial [Fe3+], M2= initial SCN[Fe3+], M2= M Fe3+Fe3+ + SCN−SCN− ↽−−⇀↽−−⇀ FeSCN2+FeSCN2+ Initial Change Equilibrium Calculate the equilibrium Kc for this reaction (to two significant figures
A student completed Test Solution 1: 2.5 mL of 2.00×10−32.00×10−3 M Fe(NO3)3Fe(NO3)3 mixed with 0.5 mL of 2.00×10−32.00×10−3 M NaSCNNaSCN and topped with 2.0 mL of 0.1 M HNO3HNO3 to make a total of 5.0 mL solution. The absorbance of the solution was measured, and the calibration curve was used to calculate [FeSCN2+][FeSCN2+] at equilibrium. Concentration of [FeSCN2+][FeSCN2+] at equilibrium was 7.5×10−57.5×10−5 M. Complete the given chart and the calculation that follows. initial [Fe3+], M2= initial SCN[Fe3+], M2= M Fe3+Fe3+ + SCN−SCN− ↽−−⇀↽−−⇀ FeSCN2+FeSCN2+ Initial Change Equilibrium
At 21 °C, a solution of 12 mL each of 0.00200 M Fe3+ and 0.001000 M SCN- was mixed and brought to 25.0 mL with 0.1 M HNO3. The absorbance at 450 nm was measured to be 0.350 (A450 = 0.350). This solution was then heated to 45 °C and the absorbance at 450 nm was measured to be 0.142 (A450= 0.142). Is the reaction: Fe3+(aq) + SCN -(aq) → FeSCN2+(aq) exothermic or endothermic? Explain.
Record your absorbance data for the YELLOW and RED dyes below. Calculate the dye concentration in mM for each cuvette using M1V2 = M2v2 . Remember the concentration of stock solutions (100^ % dye) is 0.020 mM(mM= millimolar =mm /L). Data for YELLOW: peak absorbance used on spectrophotometer =420nm Cuvette 1 - 100% dye = 0.680 absorption Cuvette 2 - 75% dye = 0.510 absorption Cuvette 3 - 50% dye = 0.340 absorption Cuvette 4 - 25% dye = 0.170 absorption Data for RED - peak absorption used on spectrophotometer = 500nm Cuvette 1 - 100% dye: 0.621 absorption Cuvette 2 - 75%: 0.466 absorption Cuvette 3 - 50% dye: 0.311 absorption Cuvette 4 - 25% dye: 0.1555 absorption

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