Blue Blue dye stock solution Absorbance at 630 nm Calibration curve Part 1: 0.1944 M 0.00697 y=0.0682x A purple solution is prepared by mixing 5.00 mL of the blue dye solution with 6.75 mL of red dye solution. The calibration curve for each color is provided. Part 2 out of 3 (a) Determine the theoretical molar concentration of each dye in the mixture. [Blueltheoretical 8.27 x 10-2 [Red] theoretical 1.16 x 10 [Bluelexperimental " W [Redlexperimental " -1 x 10 M x 10 M (b) Using the absorbance and calibration curve for each dye, calculate the experimental molar concentration of each dye in the mixture. Red Red dye stock solution Absorbance at 500 nm Calibration curve 0.2015 M 0.00193 y=0.0170x M M

Blue Blue dye stock solution Absorbance at 630 nm Calibration curve Part 1: 0.1944 M 0.00697 y=0.0682x A purple solution is prepared by mixing 5.00 mL of the blue dye solution with 6.75 mL of red dye solution. The calibration curve for each color is provided. Part 2 out of 3 (a) Determine the theoretical molar concentration of each dye in the mixture. [Blueltheoretical 8.27 x 10-2 [Red] theoretical 1.16 x 10 [Bluelexperimental " W [Redlexperimental " -1 x 10 M x 10 M (b) Using the absorbance and calibration curve for each dye, calculate the experimental molar concentration of each dye in the mixture. Red Red dye stock solution Absorbance at 500 nm Calibration curve 0.2015 M 0.00193 y=0.0170x M M

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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(d) 3-13. Distis me Jum 4 A method of analysis yields weights for gold that are low by 0.4 mg. Calculate the caused by this uncertainty if the weight of gold in the sample is (a) 900 mg. (c) 150 mg. 1-7. The method described in Problem 3-6 is to be used for the analysis of ores that assay about 1.2% gold. What minimum sample weight should be taken if the relative error resulting from a 0.4-mg loss is not to exceed -0.2%? percent relative error (a) (b) (b) 600 mg. (d) 30 mg. 3-14. Wha stan stam 3-15. Сог mea (b) -0.5%? (a) -0.8%? (c) (d) 1.2%? 3.5 3-8. The color change of a chemical indicator requires an overtitration of 0.04 mL. Calculate the percent relative error if the total volume of titrant is (a) 50.00 mL. (c) 25.0 mL. 3-9. A loss of 0.4 mg of Zn occurs in the course of an analysis to determine that element. Calculate the per- cent relative error due to this loss if the weight of Zn in the sample is (a) 40 mg. (c) 400 mg. 3.1 3.1 (b) 10.0 mL. 3.3 2.5 (d) 40.0 mL. Fo (a (E (b) 175…
A student prepared four standard solutions of (NH4)2Fe(SO4)2 and measured their absorbance at 505 nm. She created a calibration plot with the best-fit line of y = 9372 x + 0.0539. She measured the absorbance of her diluted unknown sample solution as (4.69x10^-1) nm. If she prepared her diluted sample solution by diluting 10.00 mL of the original solution to a total volume of 50.00 mL with deionized water, what is the concentration of Fe2+ in her original solution? Answer in units of M. Note: Your answer is assumed to be reduced to the highest power possible.
Caffeine, C8H10O2N4 H2O (MW = 212.2 g/mol) has been shown to have an average absorbance of 0.644 for a concentration of 1.783 mg per 100 mL at 272 nm. A sample of 3.658 g of a soluble coffee product was mixed with water to a volume of 500 mL and a 25 mL aliquot was transferred to a flask containing 25 mL of 0.1 M H2SO4. This was subjected to the prescribed clarification treatment and made up to 500 mL. A portion of this treated solution showed an absorbance of 0.666 at 272 nm. Assumbe b = 1.0 cm. Calculate the % caffeine (w/w) in the sample.
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+ solution with an unknown concentration and an absorbance value of 0.392. The slope-intercept form of the equation of the line is y = 4538.1x +0.0077. The unknown was analyzed on the same instrument as the standard curve solutions at the same temperature. What is the Fe³+ concentration of the unknown solution? [Fe³+] = mol/L Absorbance Iron(III) thiocynate standard curve 1.0 V 0.5 0.0001 Fe³+ concentration (M) 0 0.0002
The table below describes a procedure in preparing standard solutions of a protein sample with different concentrations. (A) Determine the concentrations of each tube if the starting concentration of the protein is 500 mg mL (B) Determine the equation of the line if the concentration (x-axis) was plotted vs the absorbance (y-axis). (C) What is the concentration, in mg mL, of the diluted unknown protein sample if the absorbance at 595 nm is 0.333? L-1. Tube Volume of protein, Volume of water, Final concentration, Absorbance #3 mL mL (at 595 nm) mg mL-1 0.00 5.00 0.113 12 0.70 4.30 0.184 3 1.40 3.60 0.251 14 2.10 2.90 0.329 15 2.80 2.20 0.385 3.50 1.50 0.454 17 4.20 0.80 0.503 8 5.00 0.00 0.577 Suppose that the unknown protein (diluted) sample in 4.C was diluted from a protein stock solution. Determine the concentration of the original unknown protein stock solution if 2.00 mL of the protein solution was mixed with 8.00 mL of water to create the unknown protein (diluted) sample in 4.C.
Treatment of ammonia with phenol in the presence of hypochlorite yields indophenol, a blue product that absrobs light at 625 nm, which çan be used for the spectrophotometric determination of ammonia. gan OCF OH + NH3 indophenol anion To determinè the ammonia concentration in a sample of lake water, three samples are prepared. In sample A, 10.0 mL of lake water is mixed with 5 mL of phenol solution and 2 mL of sodium hypochlorite solution, and diluted to 25.0 mL in a volumetric flask. In sample B, 10.0 mL of lake water is mixed with 5 mL of phenol solution, 2 mL of sodium hypochlorite solution, and 2.50 mL of a 5.50 x 10-4 M ammonia solution, and diluted to 25.0 mL. Sample C is a reagent blank. It contains 10.0 mL of distilled water, 5 mL of phenol solution, and 2 mL of sodium hypochlorite solution, diluted to 25.0 mL. The absorbance of the three samples is then measured at 625 nm in a 1.00 cm cuvette. The results are shown in the table. Sample Absorbance (625 nm) A 0.361 B 0.608 C…
(5) A sample of sodium phosphate is dissolved in water to give 100.00 mL of solution (Solution A). Then this solution is diluted 5 times to give the final solution (Solution B). Solution B is Known to contain 3.920 x 1022 number of PO43- ions, which has an absorption peak at 460 nm and absorbance value of 0.355 in a 1.000 cm cuvette. (i) Calculate the molar absorptivity of Solution B. (ii) What mass of sodium phosphate (MM 163.94 g/mol) dissolved in Solution A.
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.
The following data are obtained from three standard soltions using UV-Vis spectroscopy: What is the colar concentration (M) of an unknown solution with an absorbance of 0.180 at 255 nm? The unknown solution contains the same analyte as the standard solution does. The molar mass of the analyte is 188.65 g/mol a) 4.82x10-5b)1.9x10-3c)3.60x10-4d)1.9x10-5e)1.8x 10-4
4. The molar absorptivities of the indicator weak acid HIn (K₁ = 1.42 x 105) and its conjugate base In at 570 were determined as ε(HIn) = 7120 and ɛ(In) = 961. The optical length b = 1.00 cm. (a) What is the absorbance of an unbuffered indicator solution having total indicator concentration 8.0 × 10%. (b) What is the absorbance of a buffered indicator solution having total indicator concentration 8.0 x 105 and pH = 6.5.
The absorbance of an unknown dye solution is measured to be 1.06 by a spectrometer. The calibration plot of the spectrometer is provided below. What is the molar concentration of the unknown sample (in mole L)? Absorbance vs. Molarity 18 y3 67024x-0.0343 16 14 12 1 0.8 0.6 0.4 0.2 01 0.2 0.000005 00001 0000015 Concentration of solutions, mol/L 0.00002 0.000025 000003 0 163e-5 O 2.35e-6 0 163 0 235 Absorbance
Differentiate between qualitative analysis and quantitive analysis?