You have a solution with a concentration of 0.50 mM, and you put it in a cuvette with a 1.0cm pathlength. You read an absorbance of 0.600. What is the extinction coefficient of your analyte? Question 4 options: 1.2 mM cm 1.2 mmole/L/cm 1.2 L/mmole/cm 1.2 mmol/L (cm)-1
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- You have a solution with a concentration of 0.80 mM, and you put it in a cuvette with a 1.0cm pathlength. You read an absorbance of 0.400. What is the extinction coefficient of your analyte? Question 4 options: 0.50 mmole/L/cm 0.50 mmol/L (cm)-1 0.50 L/mmole/cm 0.50 mM cm45.0 mL of an unknown FeCl3 solution is diluted to a total volume of 230.0 mL. The diluted FeCl3 solution measured an absorbance of 0.223. Calculate the molarity of the undiluted unknown FeCl3 solution if the molar extinction coefficient is 230.0 M-1⋅cm-1 and a path length of 1.00 cm. Group of answer choices 0.000190 M 0.00496 M 0.00593 M 10.0 M 0.00399 M3. An indicator is a dye whose spectrum changes with pH. Consider the following data for the absorption spectrum of an indicator (pK = 4) in its ionized and nonionized form. InH+ → In + H* Molar absorptivity, ɛ (M1.cm1) InH+ (nm) In 400 10,000 420 15,000 2,000 440 8,000 8,000 460 12,000 480 3,000 The absorbance of the indicator solution is increased in a 1-cm cell and found to be 400 420 440 460 480 (nm) A 0.250 0.425 0.400 0.300 0.075 a. Calculate the pH of the solution. [4.0] b. Calculate the absorbance of the solution at 440 nm and pH 6.37 for the same total indicator concentration. [0.400] c. If you want to measure the quantum yield of fluorescence of In and H* independently, what wavelength would you choose for exciting In H+? For exciting In? Why?
- A solution containing a mixture of the compounds X and Y had an absorbance of 0.814 at 443 nm and an absorbance of 0.699 at 520 nm when measured with a 1.00 cm cell. The molar absorptivities (e) of X and Y at each wavelength are shown in the table. [X] = Wavelength (2, nm) [Y] = 443 Incorrect 520 2.13 x10-5 1.23 x10-4 Incorrect Molar Absorptivity (c. M-¹cm-¹) X What are the concentrations of X and Y in this mixture? 16180 3936 Y 3817 6333 4 M M1) Titrant 5 mg H2O/ mL Resolution 2.5 µg H2O/step Detection limit is 125 µg H2O for a 5 g sample (= 25 ppm) 2) Titrant 2 mg H2O/ mL Resolution 1 µg H2O/step Detection limit is 50 µg H2O for a 5 g sample (= 10 ppm) You have a 10 g sample which is expected to contain 200 µg H2O. True or false? 1. Titrant 5mg/mL is the preferred system over 2. Titrant 2mg/mL for this sample. True FalseQ1
- So Please don't provide the handwriting solutionThe absorbance values at 250nm of 5 standard solutions, and sample solution of a drug are given below: Conc. (ug/ml) A 250 nm10 0.16820. 0.32930 0.50840. 0.66050 0.846Sample. 0.661Calculate the concentration of the sampleA solution of a specific vitamin has a 4max of 271 nm and a concentration of 2.73 x 10-"M. The absorbance of the solution at 271 nm is A = 0.155. What is the molar absorptivity of the vitamin at 271 nm? A sample path length is 1.00 cm. molar absorptivity: L mol-'cm-!
- 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.Concentration Fe(SCN)2+ (M) Absorbance 0.0001 0.386 0.0002 0.774 0.0003 1.154 0.0004 1.527 0.0005 1.931 Question 2 Analysis Section 1 1. Open a spreadsheet program, like Excel or Desmos, and plot your data points, with Absorbance on the y-axis and Concentration on the x-axis. 2. Fit a linear trendline and make sure the equation is labeled on your graph, including the R² value. 3. Fill in your equation below. Absorbance = -Concentration + The slope of your equation gives you the s-1 in the Beer's law equation: A = scl. Since I = 1 cm, the slope is equal to the ɛ of Fe(SCN)2+. The units of & are 1/(M*cm).Chemistry