A solution of serum albumin was analyzed using the UV-Vis and yielded an absorbance value of 0.4531. The cuvette utilized had a length of 5.6 cm and the molar absorptivity coefficient of serum albumin is 43824 M*cm. Compute for the concentration of serum albumin a. 1.9463x10 b. 1.8563x10 c. 1.7463x10 d. 1.6463x10

A solution of serum albumin was analyzed using the UV-Vis and yielded an absorbance value of 0.4531. The cuvette utilized had a length of 5.6 cm and the molar absorptivity coefficient of serum albumin is 43824 M*cm. Compute for the concentration of serum albumin a. 1.9463x10 b. 1.8563x10 c. 1.7463x10 d. 1.6463x10

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

Chapter26: An Introduction To Chromatographic Separations

Section: Chapter Questions

Problem 26.17QAP: From the data in Problem 26-14, calculate for species C and D) (a) the resolution. (b) the length of...

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From the data in Problem 26-14, calculate for species C and D) (a) the resolution. (b) the length of column necessary to separate the two species with a resolution of 2.5.
The absorbance of an iron thiocyanate solution containing 0.00500 mg Fe/mL was reported as 0.4900 at 540nm. Calculate the specific absorptivity including units of iron thiocyanate on the assumption that a 0.100 cm cuvette was used.
Using the absorbance of [FeSCN]+2 at the wavelength of maximum absorption which you obtained in part B, and the diameter of the tube, obtained in part A,calculate the molar extinction coefficient. given info: Concentration of Fe3+ stock solution, C1 = 0.001 M Volume of stock Fe3+ solution pipetted, V1 = 25mL Concentration of diluted stock solution, C2 = 0.0004 M Volume of Fe2+ solution and KSCN (upon mixing) = 10mL Weight of KSCN = 1g The reaction taking place is given as: The reaction taking place is given as: F e 3+ (aq) + SC N − (aq) ⇔Fe [SCN] 2+ (aq) the concentration of [FeSCN]2+ after the mixing of Fe3+ and SCN- is 2.5 x 10-3 M. Moles of [FeSCN]2+ = 2.5 x 10-5 moles Diameter:1.2cm The wavelength at which maximum absorption takes place is = 480 nm
Determine the relationship between the observed/apparent value (EX) VERSUS that of the true value (ET) for the quantity being sought by writing either <, >, or = on the space provided Determination of the true concentration (ppm Fe) in a water sample using the iron-phenanthroline method. Dilution factor was not taken into account. EX _____ 1ET
(a) You measure the percent transmittance of a solution containing chromophore X at 400nm in a 1-cm path length cuvette and find it to be 50%. What is the absorbance of this solution? (b) What is the molar absorptivity of chromophore X if the concentration of X in the solution measured in question (a) is 0.5mM? (c) What is the concentration range of chromophore X that can be assayed if, when using a sample cell of path length 1, you are required to keep the aborbance between 0.2 and 0.8?
A 1.00 mL aliquot of a hydrogen peroxide (H2O2) solution was added to 2.00 mL of acidified Ti(IV) solution and the solution was transferred to a 1.00 mm cuvette. The absorbance of the solution against a matched reference cuvette containing Ti(IV) solution only was 0.250 at 410 nm. Determine the concentration of the H2O2 solution in mol dm–3 given that the molar absorptivity coefficient for the Ti(IV)–H2O2 complex is 770 dm3 mol–1 cm–1. Assuming the density of the H2O2 solution is 1.00 g mL–1, determine the concentration of the H2O2 solution as a %(w/w).
Which of the following is/are correct about Beer's law? Polychromatic wurce of radiation cause a chemical deviations. II. Real deviation ocur due to the higher concentration Mistmatched cells for sample and reference cells cause an insurumental deviation. A) I. II, and III II and III C) I and III D) Only III E) Only II
Use the data in Table 25.6 in ATKINS for the exchange current density and transfer coefficientfor the reaction:2 H+ + 2e- → H2on nickel at 25oC to determine what current density would be needed to obtain an overpotentialof 0.20 V as calculated from:(a) the Butler-Volmer equation(b) the Tafel equation.Is the validity of the Tafel approximation affected at overpotentials of 0.4 V and more?
For Indirect Iodometric Analysis of Copper... ~0.0896g KIO3 necessary to consume 350mL of 0.1 M Na2S2O3, Na2S2O3 is stored in an amber glass bottle until ready for use. Primary Standard KIO3 has 2g of KI, 50mL of DI water, and 10 mL of 1.0M HCl is added then immediately titrated with Na2S2O3 until medium yellow or straw... then 5mL of starch indicator is added and titrated again until blue black color turns clear. Unknown CuO use 1.2G of Unknown, 20mL of HNO3 heated until sample dissolved, 25 mL of DI water added and boiled until clear light blue color, after cooling 1:1 NH3 added (~34.47 mL of NH4OH reagent) until permanent deep blue color amine complex, 2g of NH4HF2 added and swirled until dissolved, 3 g of KI is added then titrated immediately with Na2S2O3 until brown color of iodide is nearly gone (brown milk color), 2 g of KSCN and 3 mL of starch indicator is then added with titration continuing until disappearance of new blue black color. 1. Na2CO3 is often added to thiosulfate…
For Indirect Iodometric Analysis of Copper... ~0.0896g KIO3 necessary to consume 350mL of 0.1 M Na2S2O3, Na2S2O3 is stored in an amber glass bottle until ready for use. Primary Standard KIO3 has 2g of KI, 50mL of DI water, and 10 mL of 1.0M HCl is added then immediately titrated with Na2S2O3 until medium yellow or straw... then 5mL of starch indicator is added and titrated again until blue black color turns clear. Unknown CuO use 1.2G of Unknown, 20mL of HNO3 heated until sample dissolved, 25 mL of DI water added and boiled until clear light blue color, after cooling 1:1 NH3 added (~34.47 mL of NH4OH reagent) until permanent deep blue color amine complex, 2g of NH4HF2 added and swirled until dissolved, 3 g of KI is added then titrated immediately with Na2S2O3 until brown color of iodide is nearly gone (brown milk color), 2 g of KSCN and 3 mL of starch indicator is then added with titration continuing until disappearance of new blue black color. 4. Why is the starch indicator solution…
What is the concentration (M) of the following compound as measured in a 1.000 cm cuvette: Molar absorptivity constant: 3525 (M*cm)-1 and Absorption: 0.5334 Hint: Use the Beer law to solve this problem Group of answer choices 1.513E-04 1.513E+04 1.513191E-04 1.513191E+04 1.5E-04
A solution of Tryptophan has an absorbance at 280 nm of 0.54 in a 0.5 cm length cuvette. Given the absorbance coefficient of trp is 6.4 x 103 Lmol-1cm-1. What is the concentration of solution?