At 580 nm, which is the wavelength Fe(SCN) has a molar absorptivity of 7.00 x 10' 1. cm' mot. Calculate of its maximum absorption, the complex (a) the absorbance of a 4.47 x 10' M solution of the complex at 580 nm in a 1.00-cm cell (b) the percent transmittance of the solutions described in (a) (c) the absorbance of a solution that has half the transmittar of that described in (a)
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- At 580 nm, the wavelength of its maximum absorption, the complex Fe(SCN)2+ has a molar absorptivity of 7.00x 103 L cm-1 mol-1. Calculate (a) the absorbance of a 3.40 x 10–5 M solution of the complex at 580 nm in a 1.00-cm cell. (b) the absorbance of a solution in which the concentration of the complex is twice that in (a). (c) the transmittance of the solutions described in (a) and (b). (d) the absorbance of a solution that has half the transmittance of that described in (a).At 580 nm, the wavelength of its maximum absorption, the complex Fe(SCN)2+ has a molar absorptivity of 7.00 X 103 L mol-1 cm-1. Calculate (a) the absorbance of a 2.50 X 10-5 M solution of the complex at 580 nm in a 1.00-cm cell. (b) the absorbance of the solution in which the concentration of the complex is twice that in part (a) (c) the transmittance of the solutions described in parts (a) and (b) (d) the absorbance of a solution that has half the transmittance of that described in part (a) answer letter d pleaseAt 580 nm, the wavelength of its maximum absorption, the complex Fe(SCN)2+ has a molar absorptivity of 7.00 X 103 L mol-1 cm-1. Calculate (a) the absorbance of a 2.50 X 10-5 M solution of the complex at 580 nm in a 1.00-cm cell. (b) the absorbance of the solution in which the concentration of the complex is twice that in part (a) (c) the transmittance of the solutions described in parts (a) and (b) (d) the absorbance of a solution that has half the transmittance of that described in part (a)
- At 580 nm, the wavelength of its maximum absorption, the complex Fe(SCN)2+ has a molar absorptivity of 7.00x103 L mol-1 cm-1. Calculate a.) the absorbance of 2.50x10-5 M solution of the complex at 580 nm in 1.00-cm cell. b.) the absorbance of a solution in which the concentration of the complex is twice that in part (a). c.) the transmittance of the solutions described in parts (a) and (b). d.) the absorbance of a solution that has half the transmittance of that described in part (a).. A solution containing the complex formed between two substances has a molar absorptivity of 9.32 X 103 L mol-1 cm-1 at 470 nm. a)What is the absorbance of a 6.24x10-5 M solution of the complex at 470 nm in a 1.00 cm cell? b)What is the percent transmittance of the solution described in (a)? c)What is the molar concentration of the complex in a solution that has the absorbance described in (a) when measured at 470 nm in a 5.00 cm cell . A solution containing the complex formed between two substances has a molar absorptivity of 9.32 X 103 L mol-1 cm-1 at 470 nm. a)What is the absorbance of a 6.24x10-5 M solution of the complex at 470 nm in a 1.00 cm cell? b)What is the percent transmittance of the solution described in (a)? c)What is the molar concentration of the complex in a solution that has the absorbance described in (a) when measured at 470 nm in a 5.00 cm cellBeryllium(II) forms a complex with acetylacetone (166.2 g/mol). Calculate the molar absorptivity of the complex, given that a 2.25 ppm solution has a transmittance of 37.5% when measured in a 1.00-cm cell at 295 nm, the wavelength of maximum absorption.
- Titanium and vanadium form colored complexes when treated with hydrogen peroxide in 1 M sulfuric acid. The titanium complex has an absorption maximum at 415 nm, and the vanadium complex has an absorption maximum at 455 nm. A 1.00 × 10−3 M solution of the titanium complex exhibits an absorbance of 0.816 at 415 nm and of 0.485 at 455 nm, while a 2.00 × 10−3 M solution of the vanadium complex exhibits absorbances of 0.425 and 0.608 at 415 and 455 nm, respectively. A 1.000-g sample of an alloy containing titanium and vanadium was dissolved, treated with excess hydrogen peroxide, and diluted to a final volume of 1000 mL. The absorbance of the solution was 0.697 at 415 nm and 0.533 at 455 nm. Calculate: a) The concentration of titanium and vanadium in the sample. b) The percentages of titanium and vanadium in theCalculate ∆ in kJ/mol if a d1 complex has an absorption maximum at 545 nm.At 580 nm, the wavelength of its maximum absorption, the complex Fe(SCN)2+ has a molar absorptivity of 7.00x103 L mol-1 cm-1. Calculate letter D ONLY a.) the absorbance of 2.50x10-5 M solution of the complex at 580 nm in 1.00-cm cell. = 0.175 b.) the absorbance of a solution in which the concentration of the complex is twice that in part (a). c.) the transmittance of the solutions described in parts (a) and (b). d.) the absorbance of a solution that has half the transmittance of that described in part (a).
- At 580nm, the wavelength of its maximum absorption, a 3.75 x10^-5 M solution of the complex FeSCN2+ has an absorbance of 0.2734 in a 1.00cm cell. what will be the absorbance of a solution in a 2.0 cm cell with concentraion 1.25* 10-5 concentrationThe absorption coefficient of a glycogen-iodine complex is 0.20 at light of 450 nm. What is the concentration when the transmission is 40 % in a cuvette of 2 cm?You are working with metal thiocyanate complex, M(SCN)+, with a molar absorptivity constant, ε, of 2700 cm−1M−1 at 500 nm. If you are is using a 1.00 cm cuvette for absorbance measurements at 500 nm, what concentration of M(SCN)+ will give an absorbance value of 0.280?