Determination of the concentration of Zn(II) in a sample of river water was carried out by the standardaddition method. A standard solution of 20 ppm Zn(II) was prepared and added to the filtered river watersample. The prepared series of solutions were then measured for absorbance with AAS and the resultswere as follows:1.Fe(lII) 20 ppm (ml) Sample (ml)H2O (ml)A0,010.1110,2180.1670,470.2230,616.0.2860,810.3471,010.401a. Draw a calibration curve for the volume of Zn(II) vs. absorbance and concentration Zn(II) vs.absorbanceb. Based on the available data, what is the concentration of Zn(II) in the sample

Answered: Image /qna-images/answer/8b7e67b8-e910-42d2-adc7-e12220cb37ee.jpg

Answered: Determination of the concentration of…

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 9.7QAP

See similar textbooks

Similar questions

The amount of iron in a meteorite was determined by a redox titration using KMnO4 as the titrant. A 0.4185 -g sample was dissolved in acid and the liberated Fe3+ quantitatively reduced to Fe2+, using a reductor column. Titrating with 0.0044 M KMnO4 requires 28.76 mL to reach the end point. Determine the %w/w Fe2O3 in the sample of meteorite. (Fe = 55.845 amu, Fe2O3 = 159.69 g/mol
The iron content of a municipal water supply was determined by an atomicabsorption procedure. The absorbance of the water, after a five-fold dilution, was0.755 at 248.3 nm. A standard solution, prepared by dissolving 0.2018 g of pureiron wire in acid, diluting to 250.0 mL, and then making a 100-fold dilution, hadan absorbance of 1.015. Calculate the ppm Fe in the water sample
The absorbance of a solution containing 5.0 x 10^-3 g/L of a solute in a 1.00 m cell is 1.00. Calculate the absorptivity and the molar absorptivity if the molecular mass of the solute is 1.25.
The absorbance value for the Standard was 0.625 and [FeSCN^ 2+ ] std is 2.00E 4M Calculate the [FeSCN^ 2+ ] in the equilibrium mixture, report the answer to the correct significant figures. The absorbance of the equilibrium solution was 0.451
The molar absorptivity of a compound at 500 nm wavelength is 252 M-1cm-1. Suppose one prepares a solution by dissolving 0.00140 moles of a solute in enough water to make a 500.0 mL solution. What would be the absorbance in a 3 .00 mm pathlength cell?
Commercial Vanadyl Sulfate (VOSO4) is contaminated with H2SO4 and H2O. A solution was prepared dissolving 0.2447 g of impure VOSO4 in 50.00 mL of water. A spectrophotometric analysis indicated that the The concentration of vanadyl ions, VO2+ (blue) was 0.0243 M. A 5.00 mL sample was passed through a column filled with a cation exchange resin in H+ form, to retain the vanadyl ion and the eluent necessary for its titration 13.03 mL of NaOH 0.02274 M. Calculate the percentage by weight of each component (VOSO4, H2SO4, and H2O) in commercial vanadyl sulfate. (Pm VOSO4, 162.96; H2SO4, 97.94)
You want to determine the amount of iron(III) in acomplex salt. You make a 100.0 mL solution of the complex salt by dissolving 0.0670 g of complex salt with water to the mark on a 100.0 mL volumetric flask. You get an absorbance reading for the iron from the spectrometer of 0.334. The molar absorptivity is determined to be 17605 L/mole∙cm and the pathlength is 1.00 cm. Determine the molarity of iron(III) in solution. Determine the mass percentage of iron(III) in the complex salt.
A standard solution was put through appropriate dilutions to give the concentrations of iron shown in the table that follows. The iron(II)-1,10-phenanthroline complex was then formed in 25.0-mL aliquots of these solutions, following which each was diluted to 50.0 mL. The following absorbances (1.00-cm cells) were recorded at 510 nm: Calculate the concentration, in ppm, of a sample with an abosrbance of 0.829. Fe(II) concentration (ppm) A510 4.00 0.160 10.0 0.390 16.0 0.630 24.0 0.950 32.0 1.260 40.0 1.580
4. determine the amount in mg of the amount of Ag present from ICP mass digested: 1.0821g/L dilution of 10ml stock solution to 100ml volumetric flask X=0.98 (intensity)
A Dubosq colorimeter consists of a cell of fixed path length and a cell of variable path length. By adjusting the length of the latter until the transmission through the two cells is the same. the concentration of the second solution can be inferred from that of the former. Suppose that a plantdye of concentration 25 μg dm-3 is added to the fixed cell. the length of which is 1.55 em. Then a solution of the same dye. but of unknown concentration. is added to the second cel l. It is found that the same t ransmittance is obtained when the length of the second cel l is adjusted to 1.18 em. What is the concentration of the second solution?
A solution containing 5.54 ppm KMnO4 exhibits72.5 %T in a 1.50-cm cell at 520 nm. A. Calculate the absorbance of the solution. B. Calculate the molarity of potassium permanganate. C.
The standard curve was made by spectrophotographic analysis of equilibrated iron(III) thiocyanate solutions of known concentration. You are asked to analyze a Fe(SCN)2+Fe(SCN)2+ solution with an unknown concentration and an absorbance value of 0.4150.415 . The slope-intercept form of the equation of the line is ?=4558.4?+0.0147y=4558.4⁢x+0.0147 . The unknown was analyzed on the same instrument as the standard curve solutions at the same temperature. What is the Fe3+Fe3+ concentration of the unknown solution?

SEE MORE QUESTIONS

Recommended textbooks for you

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

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

Publisher:

Cengage Learning

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

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

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS