Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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- Spectroscopy and a Calibration Curve Prepare a series of standard solutions of the colored compound with known concentrations by diluting the stock solution with distilled water. Use volumetric flasks to ensure accurate dilutions. Let's assume we have a stock solution of potassium permanganate (KMnO4) with a concentration of 0.100 M (molar). We will prepare five standard solutions with the following concentrations by diluting the stock solution with distilled water: 0.020 M 0.040 M 0.060 M 0.080 M 0.100 M Measure the absorbance of each standard solution at the wavelength of maximum absorbance (λmax) using the UV-Vis spectrophotometer. Record the absorbance values. For 0.020 M: Absorbance = 0.150 For 0.040 M: Absorbance = 0.290 For 0.060 M: Absorbance = 0.440 For 0.080 M: Absorbance = 0.580 For 0.100 M: Absorbance = 0.730 Plot a calibration curve by graphing the absorbance values (y-axis) against the corresponding concentrations (x-axis) of the standard solutions. Use a linear…arrow_forwarda) If an unknown sample containing FeSCN2+ has an absorbance of 0.542, what is the concentration of FeSCN2+ in the unknown sample? b) What are the units of concentration? c) If the path length of light is 13.5 mm (millimeters), what is the absorptivity coefficient, ?ε, for FeSCN2+? d) What are the units of the absorptivity coefficient, ?ε?arrow_forwardAn ethanol solution of 3.5 mg/100 ml of compound Y (150.0 g/mol) in a 1.00 cm quartz cell has an absorbance (A) of 0.972 at λmax=235 nm. What is its molar extinction coefficient? Report your answer to the correct number of significant figures. Do not include units in your answer.arrow_forward
- 2) In a laboratory study, a calibration was performed using NH4C1 to analyze ammonium spectrophotometrically. The results of the study are given below. According to this, when the 5.0 mL sample containing ammonium is completed to 50 mL with pure water, find the amount of NH4 in the sample whose absorbance was found as 0.12 according to the table. (N: 14 g / mol, H: 1 g / mol, Cl: 35.5 g / mol). Concentration (mg/L) Absorbance 0.01 5 0.05 7.5 0.1 10 0.15 12 0.18arrow_forwardA colored ion solution has a concentration of 0.200 M with a measured absorbance A = 0.880. Another ion solution made of the same chemicals has an absorbance A = 0.172. What is the concentration of this unknown sample solution?arrow_forwardIam stuck on how to start this problem. Youo are presented with a sample of freshly squeezed carrot juice and are asked to determine how much beta-carotene is presented in the juice. A beer's Law plots is constructed from the absorbances at 451 nm for six standard solutions of beta-carotene, with concentrations ranging from 0.75-7.5 µM. Linear regressions data: y=0.1431x-0.0078(R2=0.9998) a)The carrot juice is diluted by one-fourth, and the absorbance at 451 nm of this solutions is measured to be 0.676. Based on this information, what is molor concentration of beta-corotene in the original(undilited) sample of carrot juice? b) If the original sample of carrot juice was 312 mL, calculated the mass(g) of beta-carotene presentedarrow_forward
- A compound with a molecular weight of 229.61 g/mol was dissolved in 50.0 mL of water. 1.00 mL of this solution was placed in a 10.0 mL flask and diluted to the mark. The absorbance of this diluted solution at 510 nm was 0.472 in a 1.000 cm cuvet. The molar absorptivity of the compound, at 510 nm, is 6,310 M-1 cm-1. Calculate the concentration of the compound in the initial 50.0 mL solution. A. 1.50 x 10-5 M B. 7.48 x 10-5 M C. 7.48 x 10-4 M D. 7.48 x 10-6 Marrow_forward(d) The Beer-Lambert law states that the absorbance (A) of light by a solution in a cuvette is given by. A = ID==ecL In=-= where lo is the incident light intensity, / is the transmitted light intensity, e is the molar absorptivity, c is the concentration of the solution, and Lis the path length of the cuvette. (1) Light with a wavelength of 800 nm is passed through a cuvette containing a solution of Coumarin dye. After passing through the cuvette, the light intensity was reduced to 10% of its initial value. What is the absorbance of the solution of Coumarin dye? (1) The concentration of the Coumarin dye is 0.004 mol dm3, and the cuvette has a path length of 1 cm. What is the molar absorptivity of Coumarin dye at 800 nm, in units of m² mot¹?arrow_forwardCan you help me on questions 2 AND 3arrow_forward
- Hh.130.arrow_forward2. ] You make 150.0 mL of a copper(II) sulfate solution but forget to cover it before leaving for the day. The next class, you measure the volume and find that you only have 132.0 mL remaining. You didn’t record the initial concentration, but you measure the absorbance of the remaining solution at 620 nm and find that it is 0.386. You also construct the following calibration curve for CuSO4: Standard solution Abs620 0.50 M 0.424 0.40 M 0.336 0.30 M 0.247 0.20 M 0.159 (refer to image) a. What is the value for k (in Beer’s Law)? Provide a calculation or graph to support your answer. b. What is the concentration of the (remaining) solution? c. What was the concentration of the original solution from the first class? d. If you removed 7.5 mL from the 132.0 mL solution in the process of measuring the absorbance, how much water should you add to obtain the original concentration that you solved for in part (c)?arrow_forwardConclusion 5: You are tasked with analyzing a suspiciously pink sample of drinking water to establish if it has unsavory levels of MnO4-contamination. It has an absorbance of 0.83 at 544 nm when measured in a cuvette that is 1 cm across. Using the equation of your trend line from Plot 4, determine the concentration of KMnO4 in moles/liter. Convert this concentration to grams of manganese/liter and compare it to the EPA guideline above. Trandline is Absorbtion = 2000(Concentration KMnO4) (Y=Mx)arrow_forward
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