Based on your experience in this experiment, briefly discuss the relative precision permitted by a graduated cylinder, a pipet and a buret. Give several circumstances under which you would use each instrument over the other two.
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- 1. Research on the limitation of accuracy of the following instruments: • analytical balance • top-loading balance • serological pipette • graduated cylinder • burette • volumetric flask • Erlenmeyer flask • beaker 2. Define the term, "measurement uncertainty". Among the instruments listed above, which ones have the highest uncertainty? Which ones have the lowest? 3. Based on the measurement uncertainty of the above instruments, which instruments would yield the lowest percent error?The pharmacist attempts to weigh 80mg of sodium carbonate on a balance having a sensitivity requirement of 4mg. Calculate the maximum potential error in terms of percentage.How many of the following should be included in a good hypothesis? (i) A prediction of the results of the experiment (ii) A step-by-step walkthrough of how to do the experiment with specific references to amounts of reactants, glassware used, and other experimental details (iii) A summation of the data collected after doing the experiment, with comments on accuracy and precision if possible. (iv) A detailed list of chemicals that will be used (v) Waste disposal procedures (vi) A brief scientific explanation of the predicted results. Said another way, the hypothesis should include a scientific explanation of why the predicted results are expected. 1 2 3 4 5
- In analytical chemistry, what is a standard method? Include any sources you used to answer this question. Give an example of a standard method, and the reference for it. 2.In the Analytical Chemistry laboratory, one of the B.Sc student Ms. Fatma wanted to analyze the presence of Iron(II) ion in the water samples collected from Sohar Industrial Area in the Sultanate of Oman and analyzed by Spectrophotometric method. (1) 250.00 mL of this water sample (Solution A) known to contain unknown amount of FeSO4. She has diluted Solution A by a dilution factor 10 to make 250.00 mL solution, which she labeled Solution B. Using Spectrophotometer, she has measured the absorbance value (0.642) for Solution B at 508 nm using 1.00 cm cell (cuvet). The molar absorptivity value for Fe2* ion at 508 nm is ɛ508 = 30.8 M-1cm1. (i) What volume of the solution A did she require to make the 250.00 mL of Solution В? (ii) in (i)? What instrument should she use to transfer the volume of the Solution A calculated (ii) Concentration of FeSO4 in Solution B. (iv) Concentration of FeSO4 in Solution A. Mass of FeSO4 in Solution A (Show your calculation) (v)Provide a concise explanation of Mass spectrometry (MS) in regard to food samples. include the specific application name (e.g., Identification andQuantification of Mercury in Salmon), outline a brief description of samplepreparation procedures, and provide a summary of the obtained results from the analytical process
- Categorize each as a determinate or an indeterminate error and further classify determinate errors as instrumental, method or personal. a) An unknown sample being weighed is hygroscopic. b) One component of a mixture being analyzed quantitatively by GC reacts with the column packing. c) A radioactive sample being counted repeatedly without any change in condition yields a slightly different count at each trial. d) The tip of the pipet used in the analysis is broken. e) In measuring the same peak heights of a chromatogram, two technician each report different heights.What impact would using a much smaller sample have on the accuracy of your resultsA quality-control laboratory analyzes a product mixture us-ing gas-liquid chromatography. The separation of components ismore than adequate, but the process takes too long. Suggest twoways, other than changing the stationary phase, to shorten theanalysis time
- When measuring iron in river water by spectrophotometry using the ferrozine reaction that is described in the class notes, a student finds that they cannot distinguish their samples from noise (i.e. they are below the limit of detection) when they use a 1-cm cuvette. The student makes the decision to use a 5-cm cuvette in their method instead. a) By how much should the student expect their sample measurements to increase by? Why? b) Will their reagent blank also increase by the same amount? Why or why not? 3.(Concentration) You are tasked to prepare 50.000 ppm of a caffeine standard for an analysis. If you need to prepare 500.00 (±0.08) mL of this solution, how much (in grams) solid, pure caffeine are you supposed to dissolve? What absolute uncertainty is associated with your mass measurement if the prepared solution has a 0.12% percent relative uncertainty? Write your answer using the appropriate number of digits. Note that the formula mass of caffeine is 194.194 g/mol with negligible error. (absolute error) How many significant figures does your reported mass have? --- (number of sig. figs.)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?