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- At 21 °C, a solution of 12 mL each of 0.00200 M Fe3+ and 0.001000 M SCN- was mixed and brought to 25.0 mL with 0.1 M HNO3. The absorbance at 450 nm was measured to be 0.350 (A450 = 0.350). This solution was then heated to 45 °C and the absorbance at 450 nm was measured to be 0.142 (A450= 0.142). Is the reaction: Fe3+(aq) + SCN -(aq) → FeSCN2+(aq) exothermic or endothermic? Explain.Suppose that you are trying to measure the concentration of SO2 in air. To do that, you followed the para-rosaniline method. The SO2 was collected in a 10-ml solution of HgCl4 2- then diluted to 25 ml after the addition of the appropriate reagents. The absorbance owas measured at 650 nm in a 2.0-cm cell, yielding a value of 0.535. A standard sample was prepared by substituting a 1.00 mL sample of a standard solution containing the equivalent of 15.00 ppm SO2 for the airsample. The absorbance of the standard is found out to be 0.191. Report the concentration of SO2 in the air in parts per million. The density of air is 1.19 g/LA 2.78 ✕ 10−4 M solution of a compound has an absorbance of 0.417 at 520 nm in a 1.00 cm cell. The solvent's absorbance under the same conditions is 0.020. (a) What is the molar absorptivity of the unknown compound? M -1cm-1(b) What is the concentration of the compound in a solution, if the absorbance of the solution in a 1.00 cm cell at 520 nm is 0.391? M
- To determine the concentration of these analyte ions in a mixture, the mixture absorbance is analyzed in a cell with a pathlength of 1.00 cm at 396 nm and at 550 nm, yielding values of 0.109 and 0.0.183, respectively. What is the molar concentrations of X3+ in the sample? What are the molar concentrations of Y2+ in the sample?The measures absorbance of a solution with a pathlength of 1.00 cm is 0.544. If the concentration is 1.40 x 10^-3 M, what is the molar absorptivity for this analyte?3+ The sodium salt of 2-quinizarinsulfonic acid (NaQ) forms a complex with Al* that absorbs strongly at 560 nm. Use the data from this paper to find the formula of the complex. In all solutions, cAl 3.7 x 10° M, and all measurements were made in 1.00-cm cells. b. Find the molar absorptivity of the complex and its uncertainty. а. cQ, M 1.00 x 105 2.00 x 105 3.00 x 105 4.00 x 105 5.00 x 105 6.00 x 105 8.00 x 105 1.00 x 104 A560 0.131 0.265 0.396 0.468 0.487 0.498 0.499 0.500
- Give a clear handwritten answer with explanationThe measured absorbance of a solution with a pathlength of 1.00 cm is 0.544. If the concentration is 1.4010-3 M, what is the molar absorptivity for this analyte?An unknown chemical has an absorbance of 0.265 in a 1.0cm cuvette at a concentration of 0.703 M. What is the chemical's absorptivity constant in M cm? Report your answer to three decimals.
- The molar absorptivities of compounds X and Y were measured with pure samples of each: ε (M-1 cm-1) λ (nm) X Y 272 16,440 3,870 327 3,990 6,420 A mixture of compounds X and Y in a 1.00-cm cell had an absorbance of 0.957 at 272 nm and 0.559 at 327 nm. Find the concentrations of Y in the mixture. 4.43 x 10-5 M 3.03 x 10-6 M 5.95 x 10-5 M 3.56 x 10-4 M4. Calculate the expected absorbance of solution of a 5.50x10-6 M solution of Blue # measured at 629 nm in a 1.50cm cell. The molar absorptivity for Blue #1 is 1.30x105 M-1.cm-1 at 629 nm.When 8.0 ml of 0.00200M KSCN is mixed with 2.0 ml of 0.00200M Fe(NO3)3, the measured absorbance (A) at 450 nm is 0.285. The cell’s pathlength (b) is 1.0 cm; the absorptivity (ε) constant is 4700M-1cm-1. Calculate Kf for Fe(SCN) +2.
