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Chemistry
What is the formula to calculate the concentration of BSA in the sample. The absorption coefficient at 280nm: k1^mg/ml = 0.7 [mL/mg.cm].
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- Absorbance at 453 nm 8393939 7 fl. oz./20 ml Beer-Lambert's Law (Spectrophotometry) #1 Fe (aq) + KSCN(s) FESCN "(aq) + K" (aq) 3+ To determine the moles of Fe (aq) in a 100. mL sample of an unknown solution, excess KSCN(s) is added to convert all the Fe (aq) into the dark red species FeSCN"(aq), as represented by the equation above. The absorbance of FESCN"(aq) at different concentrations is shown in the graph below. 2+ 0.50 目0.40 0.30 0.20 01 0. 0. 5 x 10-5 10 x 10-5 Concentration of FESCN2+ (M) If the absorbance of the mixture is 0.20 at 453 nm, haw many moles of Fe (aq) were present in the 100. mL sample? (Assume that any volume change due to adding the KSCN(s) Iis negligible.) 3+, 4x10-4 mol 3 x 104 mol (B) 4x 10-6 mol 3x 10-6 mol(5) A sample of sodium phosphate is dissolved in water to give 100.00 mL of solution (Solution A). Then this solution is diluted 5 times to give the final solution (Solution B). Solution B is Known to contain 3.920 x 1022 number of PO43- ions, which has an absorption peak at 460 nm and absorbance value of 0.355 in a 1.000 cm cuvette. (i) Calculate the molar absorptivity of Solution B. (ii) What mass of sodium phosphate (MM 163.94 g/mol) dissolved in Solution A.A student wanted to determine the level of lead in amoxicillin powder, so he transferred 148 mg of the powder to 200 ml volumetric flask and completed the volume volumetrically, then he transferred 5 ml of the obtained solution to 50 ml volumetric flask and completed the volume properly, and read the absorbance of the obtained solution on AAS. The reading was 0.48. and the calibration equation was: "Y =12.25 x- 0.05" (concentration microg./mL). ?"Calculate the content of lead in amoxicillin as "ppm 326.5.a O 605.0 .b O 60.5.c O 17.5.d O 584.7.e O أخل اختياري
- A student wanted to determine the level of lead in amoxicillin powder, so he transferred 148 mg of the powder to 200 ml volumetric flask and completed the volume volumetrically, then he transferred 5 ml of the obtained solution to 50 ml volumetric flask and completed the volume properly, and read the absorbance of the obtained solution on AAS. The reading was 0.48. and the calibration equation was: "Y =12.25 x- 0.05" (concentration microg./mL). Calculate the content of lead in amoxicillin as "ppm"? O a. 326.5 O b. 605.0The molar absorptivity (ε) of the FeSCN2+ complex ion is 4700 M-1 · cm-1 at a wavelength of 450 nm. Using a 1-cm sample tube, you measure the absorbance as (2.0x10-1). What is the concentration of FeSCN2+?2. Two substances, A and B, have the same molar extinction coefficient at 260 nm: 1.80 x 10 dm³mol'cm'. At 340 nm A no longer absorbs, and for B EB = 6.22 x 103 dm³mol'cm'. A solution of the two has an absorbance of 0.215 at 340 nm and 0.850 at 260 nm in a 1 cm thick cell. Calculate the concentrations of A and B.
- 6. Blue Blue dye stock solution 0.293 M Absorbance at 630 nm 0.00265 Calibration curve y = 0.0833x A solution is prepared by diluting 2.79 mL of the blue dye stock solution to 25.00 mL. The measured absorbance for the prepared solution is listed in the data table. (a) What is the theoretical molar concentration? [Blue]theoretical x 10 |M (b) What is the experimental molar concentration? [Blue]experimental x 10 M (c) What is the percent error? Percent error (blue) = %A standard solution was put through appropriate dilutions to give the concentrations of iron shown in the table that follows. The iron(II)-1,10-phenanthroline complex was then formed in 25.0-mL aliquots of these solutions, following which each was diluted to 50.0 mL. The following absorbances (1.00-cm cells) were recorded at 510 nm: Calculate the concentration, in ppm, of a sample with an abosrbance of 0.829. Fe(II) concentration (ppm) A510 4.00 0.160 10.0 0.390 16.0 0.630 24.0 0.950 32.0 1.260 40.0 1.580A mixture is prepared by combining 10.72 mL of 2.52 x 10-3 M Fe(NO3)3 with 10.00 mL of 1.76 x 10-3 M KSCN. The solution turns red due to the formation of FeSCN2+. The absorbance is measured and, using a calibration plot, the [FeSCN2+] at equilibrium is found to be 2.25 x 10-4 M.Complete the following ICE table Fe3+ + SCN- ⇌ FeSCN2+ initial (M) (A) (B) (C) change (M) (D) (E) (F) equilibrium (M) (G) (H) (I) What is the value of Kc?
- 3.) The accuracy of a spectrophotometer is evaluated by preparing a solution of 60.06 ppm K2Cr2O7 and measuring its absorbance at a wavelength of 350 nm in a cell with a pathlength of 1.00 cm. The expected absorbance is 0.640. What is the expected molar absorptivity of K2Cr2O7 at this wavelength?The standard curve was made by spectrophotographic analysis of equilibrated iron(III) thiocyanate solutions of known concentration. You are asked to analyze a Fe(SCN)2+ solution with an unknown concentration and an absorbance value of 0.392. The slope-intercept form of the equation of the line is y = 4538.1x +0.0077. The unknown was analyzed on the same instrument as the standard curve solutions at the same temperature. What is the Fe³+ concentration of the unknown solution? [Fe³+] = mol/L Absorbance Iron(III) thiocynate standard curve 1.0 V 0.5 0.0001 Fe³+ concentration (M) 0 0.0002Calculate 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. (
