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- Many ions form colored solutions when dissolved in water. For example, aqueous Cu2+ solutions are light blue and aqueous Ni2+ solutions look light green. These metals in particularare often found in stainless steel. Would you expect their presence in your samples to interfere in the spectrophotometric analysis of permanganate at 525 nm? Why or why not? I think the answer is that I would expect the Cu2+ in my samples to interfere but not Ni2+ because the Ni2+ is green, signifying a higher wave length that the spectrometer wouldn't be able to pick up on because it was only set to 525 (blue-ish) where as the green is 530-ish. I just want to make sure thanks!In the process of performing a spectrophotometric determination of Fe, an analyst prepares a calibration curve using a single-beam spectrometer, such as a Spec-20. After preparing the calibration curve, the analyst drops the cuvette used for the method blank and the standards. The analyst acquires a new cuvette, measures the absorbance of the sample, and determines the %w/w Fe in the sample. Will the change in cuvette lead to a determinate error in the analysis? Explain.Quantitative Analysis by External Standard Method Calcium in a juice sample is determined by atomic absorption spectrophotometry. A stock solution of calcium is prepared by dissolving 1.834 g of CaCl, 2H20 in water and diluting to 1000.0 mL. A substock calcium solution was prepared by transferring 10.00 mL of the stock to a 100.00 mL volumetric flask and diluting to the mark. Three standard solutions of calcium were prepared by transferring 2.500 mL. 5.00 mL and 10.00 mL of substock to 50.00 mL volumetric flasks and diluting to the mark. The sample is prepared by transferring 1.000 mL of fruit juice from the original bottle to a 25.00 mL flask and diluting to the mark. Strontium chloride is added to all solutions before dilution to avoid phosphate interference. Instrumental response of the standards is measured against the blank, and the following readings are recorded: 9.10, 18.6 and 37.0. The sampie reading is 28.1. Using the multipoint method, find the concentration of calcium in…
- What is the purpose of a calibration curve in analytical chemistry?What are the differences between systematic and random errors and how do they effect accuracy and precision? In what circumstances would you use standard addition (versus a normal calibration curve) to determine the amount of an analyte in a sample? A urine sample, containing analyte Z is analysed by the standard addition method where 5 mL of the original sample was mixed with increasing amounts of a Z standard and each solution diluted to a volume of 50 mL prior to analysis. A plot of the final concentration of the standard in each of the 50 mL samples (x axis) versus The measured signal from the analysis of each 50 mL sample (on y axis) produced a straight line with the general equation: y = 44.72x + 4.06 what was the final concentration of Z in the 50 mL standard addition sample? what was the initial concentration of Z in the original urine sample?Example: You wish to prepare a calibration curve for the spectrophotometric determination of permanganate. You have a stock 0.100 M solution of KMnO4 and a series of 100 mL volumetric flasks. What volumes of the stock solution will you have to pipet into the flasks to prepare standards of 1.00 x10³, 2.00 x10-³, 5.00 x103, and 10.0 x103 M KMnO4 solutions? Solution: for 1.00 x10-³ 0.1 (M1X V1)conc. = (M2 X V2) dil mmol |x V1 = 1.0 × 10-3 -) x 100 (ml) mL mmoly mL V₁= 1.0 mL stock solution. Take home work for the 2.00 x10-3, 5.00 x10³, and 10.0 x10-³ M.
- To determine the molar concentration of a metal ion in a solution of unknown concentration, a student fırst made five standard solutions that contain the metal ion of interest and measured the absorbance of each solution in a spectrophotometer at its Amax- A calibration curve was obtained that had an equation of y = 5.747 x + 0.013 Next, the student pipetted 15.0 mL of the initial solution of unknown concentration into a 100.0 mL volumetric flask, and filled the flask with deionized water to the line. The absorbance of this final diluted solution was found to be A = 0.226 at Amax. The color of the original and diluted solution was blue. What is the molarity of the original solution, as well as an approximate Amax for this metal ion? 2max = 599 nm and concentration is 0.247 M Amax 457 nm and concentration is 0.247 M %3D 2 max = 457 nm and concentration is 0.0371 M 1 max 599 nm and concentration is 0.0371 M Amax = 599 nm and concentration is 0.00557 MThe pH of a liquid is 8.2 + 0.1. Find [H1] and its absolute and relative uncertainty.The spectroscopic data in the table is generated with five solutions of known concentration. Concentration (M) 0.0133 m= 0.0266 0.0532 0.106 0.213 Absorbance 0.1271 What is the intercept of the linear regression line? 0.08531 0.5388 1.069 Use a spreadsheet program, such as Microsoft Excel, to graph the data points and determine the equation of the best-fit line. 1.954 What is the slope of the linear regression line formed by these points? M-1
- The validation process comprises four main steps that are : hardware validation, software validation, method validation and system suitability. To evaluate a spectrophotometer’s accuracy by measuring absorbance, a solution of 60.06 mg/L K2Cr2O7 in 0.0050M H2SO4 was carefully prepared together with a 0.0050 M H2SO4 as a reagent blank. If the spectrometer’s signal is properly calibrated, it has been reported that this solution should provide an absorbance of 0.640 +- 0.010 at wavelength 350 nm. Which one of the validations mentioned above had been involved in this process? Explain your choiceFor the determination of Fe3 +, 25 mL of sample taken from sea water is diluted to 100 mL and a quantity of the obtained solution is taken and Fe3 + is determined by atomic absorption spectrophotometer. The absorbance values of the standard and sample solutions are below, and calculate the Fe3 + concentration in sea water in mg / L by drawing the relevant graph.Solution Absorbance1 mg / L Fe3 + 0.04095 mg / L Fe3 + 0.205110 mg / L Fe3 + 0.411615 mg / L Fe3 + 0.620820 mg / L Fe3 + 0.8222Sample Solution 0.5155A 5.3 × 10-2 M solution is to be used to prepare a series of five 100 mL solutions of varying concentration for use in creating a calibration curve for a spectrophotometric experiment. Determine the concentrations of each of the five dilutions if 10 mL aliquots of the current solution is used for V1.