The pharmacist attempts to weigh 120 mg of codeine sulfate on a balance with a sensitivity requirement of 6 mg. Calculate the maximum potential error in terms of percentage.
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The pharmacist attempts to weigh 120 mg of codeine sulfate on a balance with a sensitivity requirement of 6 mg. Calculate the maximum potential error in terms of percentage.
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- 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.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)Norepinephrine can be analyzed in human urine. A fixed amount of DHBA was added to each sample and standard in a fixed concentration. Please explain the analytical function of adding DHBA. To the 1 mL of urine sample, small amounts of 1 µg/mL norepinephrine standard is added and the following results were obtained. What is the concentration of the norepinephrine in the urine sample with uncertainty?
- You are preparing a 100.0 mL standard solution needed for titration analysis. The NaOH (40 g/mol) pellets are measured to be 0.5341 g in a balance with acceptable uncertainty of +0.001 g. Mass of the pellets is recorded after taring the container. The pellets are put in a beaker and added with 50 ml distilled water measured by a graduated cylinder. The solution is then quantitatively transferred to a 100-mL volumetric flask with uncertainty of ±0.08 mL and diluted to a 100-mL mark. What is the concentration (M) of the solution and estimate its uncertainty by propagation? Assumption: There is no uncertainty in molar mass. Express your answer as C+/- u M.What are the advantages and disadvantages of volumetric and gravimetric analysis?The analysis shows different concentrations based on replicate determinations of Zn in a water sample: 0.754 mg, 0.721 mg, 0.734 mg, 0.731 mg and 0.742 mg. What is the absolute error if the standard solution has 0.750 mg of Zn?
- 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-1The protein concentration of a protein isolate was determined using the Bradford assay. Five dilution of bovine serum albumin (BSA) were prepared from a 5.00 mg/mL BSA stock solution. To these dilutions, 100 µl of Bradford reagent were added. After 5 minutes, the absorbance was taken at 595 nm. Standard # BSA, in mg/mL Volume of Bradford reagent, A595 in mL 1 5.0 0.000 1.00 5.0 0.134 3 2.00 5.0 0.265 4 3.00 5.0 0.388 4.00 5.0 0.497 The supernatant dilution was prepared by mixing 49 µL of the protein isolate with 16 µL water. The absorbance was taken 5 minutes after addition of 100 mL Bradford reagent. Calculate the protein concentration (in mg/mL) of the original isolate if the absorbance at 595 nm was 0.413. Note: Final answer format must be x.xxx (three decimal places). Round off only in the final answer. Do not round off in the middle of calculation.1. (a) A solution of NaCl is prepared by dissolving 0.0056 g NaCl with enough H2O in a volumetric flask to yield a final volume of 10 mL. Assuming a standard (0.1 mg) analytical balance and class A glassware is employed, calculate the concentration of the solution (M) and its corresponding error. The atomic weights of Na and Cl are 22.98976928(2) and 34.45(1), respectively (the number in parentheses indicating the error in the last digit). (b) What would the error be if a 1mL transfer pipet was employed (10x) rather than the 10 mL volumetric flask?
- A volumetric calcium analysis on triplicate samples of the blood serum of a patient believed to be suffering from a hyperparathyroid condition produced the following data: mmol Ca/L = 3.15, 3.25, 3.26. What is the 95% confidence interval for the mean of the data, assuming no prior information about the precision of the analysis?2. The analytical ability of two lab technicians was compared by having each perform analyses for arsenic using the same method on samples having the same origin. For analyst A, s.d. = 0.12%, N=6; and for analyst B, s.d. = 0.06%, N-5. Do these results suggest a difference in the precision of the two chemists?After determining the absorbance of several standards of known concentration, the trend line for a calibration curve plotting absorbance (y-axis) against concentration (uM, x-axis) is determined to be y=4.244x+0.0000. The absorbance of a solution of unknown concentration is determined to be 0.604. Calculate the concentration of the unknown solution in microM. Give answer to 3 decimal places
