A student measures k for a certain blue dye to be 400.4 M-1 at 560 nm. What is the molarity of the dye in a solution with an absorbance of 0.118 at this wavelength?
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A student measures k for a certain blue dye to be 400.4 M-1 at 560 nm. What is the molarity of the dye in a solution with an absorbance of 0.118 at this wavelength?
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- 1.) Beer's Law can be used to find the concentration of a solution by measuring its absorbance. The law is given by ?=???A=ϵbC Where A is the absorbance, ?ϵ is the molar absorptivity, b is the pathlength of the light (the width of the sample cell), and C is the concentration of the solution. A student is analyzing a solution of a metal, and finds that the absorbance of the solution is 0.532. If ?=187 L⋅g−1⋅cm−1ϵ=187 L⋅g−1⋅cm−1 and ?=1 cmb=1 cm , what is the concentration of the metal in solution (in g/L)? * 352 * 2.84×10−32.84×10−3 * 2.84×10−22.84×10−2 * 96.8 2.) How many significant figures does the number 0.00358 have? Group of answer choices a.1 b.2 c.3 d.5 3.) A 10.00 mL solution of a certain food dye has a concentration of 1.47 g /L. What is the total mass of food dye in the solution? Report your answer with the correct number of significant figures.You have two solutions of the same compound that are blue. one is very pale and the other is very intense. Absorbance of each solution was measured with a spectrophotometer at the same wave length at which the solution absorbs. (A) Which solution has the higher absorbance? (B) Which is the more concentrated solution?The concentration of a dilute aspirin solution is 0.000530 M 0.000530 M . Standard solutions of this compound were used to prepare a Beer's law plot which gives a slope of 1550.1 M −1 1550.1 M − 1 . What is the expected absorbance value for the aspirin solution?
- A sample containing an unknown concentration of FeCl3 is measured to have an absorbance of 0.43 at 334 nm in a 1.0 cm cuvet. What is the molar concentration of the solution e = 1925.93The molar absorptivity constant of a particular chemical is 2.31 M/cm. Determine the concentration of a solution made from this chemical that has an absorbance of 0.408 with a cell path length of 1.12 cm.What is the concentration of a tyrosine solution when the absorbance at 280 nm is 1.5 using a 1 cm cuvette and the molar extinction coefficient is 1405 L/mol·cm?
- 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.In an analytical laboratory a chemical compound namely Paracetamol (151.163 g/mol) is determined in a sample. A sample weighing 0.0295 g was dissolved in a solvent and diluted the solution to 1 L. The solution has λ max at 243 nm (ε=2.6×104 cm-1 mol-1 L). The solution exhibits an absorbance of 0.638 in a 2 cm cell. Calculate the percentage paracetamol in the sample.A solution has a %T value of 48.2% at 600 nm. What is the absorbance of this solution at this wavelength?
- A student measures k for a certain blue dye to be 600.4 M-¹ at 560 nm. What is the molarity of the dye in a solution with an absorbance of 0.204 at this wavelength? Ens notator 50 Tot 00.01 Pardet id abiem abw & neuloa siipi toimulo: Hobia nroy, at le doua insonas silt el tráveni 00 001 et gauzulibCalculate the molar absorptivity and absorbance of a 1.00 x 104 M solution, which has atransmittance of 32.1% , when the path length is 2.5 cm at 650 nm. (The molar absorptivity for the FD&C dye “Red No. 3” (Erythrosine) 8.25104 M‒1·cm‒1 at 526 nm. Calculate the expected absorbance of solution of Red No. 3 with a concentration of 4.00×10–6M when measured at 629 nm in a 2.00 cm cell.