A 4.00 (+0.01) mL Class A transfer pipet is used to transfer 4,00 mL of a 0.294 (40.005) M Cu stock solution to a 100.00 (+0.08) Class A volumetric flask. Deionized water is used to bring the flask to volume, Calculate the concentration of the diluted soluion in the volumetric flask and report its absolute uncertainty. Significant figures are graded for this problem. To avoid rounding errors, do not round your answers until the very end of your calculations. [Cu*] = %3D M M
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- The standard solution is prepared by dissolving a known mass of zinc pellets with conc. HCl. The solution is then neutralized, transferred into a 250 mL volumetric flask and filled to the calibration mark. If 0.9809 g of Zn was weighed using an electronic balance with a relative uncertainty of ± 0.01 % and the 250 mL volumetric flask has a known relative uncertainty of ± 0.06 %, what would be the absolute uncertainty of the concentration of the solution? The molecular weight of the zinc pellets is 65.39 g/mol3-3 Types of Error; 3-4 Propagation of Uncertainty from Random Error (30 min) If A = 3.475 (+0.002), B = 87.336 (±0.001), C = 10.004 5 (±0.000 5), D = 11.8 (+0.2), and E = 5.10 (±0.03), report the answers of the following calculations with both the absolute uncertainty and the percent relative uncertainty. a) (A - B) XE c) b) (C+D)/(AXE) d) [(A+B+C) x (B-C-E)] / [DXE] (10-D)/(E/1000) Answer w/ absolute uncertainty: -428 (13) or -427.7 (±2.5) Answer w/% relative uncertainty: -428 (±0.6%) or -427.7 (±0.5⁹%) b) Answer w/ absolute uncertainty: 1.23 (±0.01) or 1.230 (+0.013) Answer w/ % relative uncertainty: 1.23 (±1%) or 1.230 (+1.1%) Answer w/ absolute uncertainty: 3 (±1) x 10-10 or 3.1 (±1.4) × 10-10 Answer w/ % relative uncertainty: 3 (±50%) x 10-10 or 3.1 (±46%) × 10-10 Answer w/ absolute uncertainty: 121 (±2) or 121.0 (+1.4) Answer w/ % relative uncertainty: 121 (±2%) or 121.0 (±1.8%)A 5.00 (+0.01) mL Class A transfer pipet is used to transfer 5.00 mL of a 0.259 (+0.003) M Cu²+ stock solution to a 100.00 (+0.08) Class A volumetric flask. Deionized water is used to bring the flask to volume. Calculate the concentration of the diluted soluion in the volumetric flask and report its absolute uncertainty. Significant figures are graded for this problem. To avoid rounding errors, do not round your answers until the very end of your calculations. [Cu²+] = M H M
- A stock solution of 0.225 +/- 0.003 M NaNO2 was transferred to a 100 mL volumetric flask (class A) and diluted to the mark. If 7 mL of the stock solution was transferred using one 5-mL and two 1-mL volumetric pipettes, what is the new concentration of the solution and the uncertainty? Please show how to calculate the uncertainty, that is the one part I don't understand how to do(a) For use in an iodine titration, you prepare a solution from 0.222 2 (+0.000 2) g of KIO3 [FM 214.001 0 (+0.000 9)] in 50.00 (+0.05) mL. Find the molarity and its uncertainty with an appropriate number of significant figures. (b) Would your answer be affected significantly if the reagent were only 99.9% pure?3-3 Types of Error; 3-4 Propagation of Uncertainty from Random Error ¹. If A = 3.475 (±0.002), B = 87.336 (±0.001), C = 10.004 5 (±0.000 5), D = 11.8 (±0.2), and E = 5.10 (±0.03), report the answers of the following calculations with both the absolute uncertainty and the percent relative uncertainty. a) (A - B) X E c) (10-) / (E/1000) b) (C+D)/(A X E) d) [ (A + B + C) x (B - C - E)] / [DXE]
- For a concentration technique, Stotal is given as 19.31 ± 0.035, Smb is 0.22 ± 0.008, and kA is 0.154 1 0.007 ppm, where Stotal is the signal, kA is the method's sensitivity for the analyte and Smb is the signal from the method blank. If we want the absolute percent uncertainty of the concentration CA to be 2.6%, which statement is false below? (Hint: refer to sections 4B.1 and example 4.7 in your textbook) We must improve the uncertainty in KA to 10.004 ppm-¹. O Uncertainty in the method's sensitivity dominates the absolute uncertainty. O Improving the signal's uncertainty will improve the absolute uncertainty.EXAMPLE Significant Figures in Laboratory Work You prepared a 0.250 M NH, solution by diluting 8.46 (0.04) mL of 28.0 (10.5) wt% NH, [density=0.899 (+0.003) g/mL] up to 500.0 (+0.2) mL. Find the uncertainty in 0.250 M. The molecular mass of NH3, 17.031 g/mol, has negligible uncertainty relative to other uncertainties in this problem.A calibrated pipet delivers a mean volume of 24.991 mL with a standard uncertainty of ± 0.006 mL. What is the uncertainty if you deliver four aliquots to reach 100 mL?
- a) To prepare 250mL of 0.100 M H2SO4, a student uses graduated pipette and a 250mL volumetric flask having uncertainty of ±0.02mL and ±0.1mL respectively. Calculate the volume of concentrated sulfuric acid 96% (±3) used and the uncertainty in 0.100M. dH2SO4 96 % = 1.84 (±0.05) g/mL FMH2SO4 = 98.079 g/mol b) If you want to prepare 1.00 L of buffer at pH 7.54 with a total phosphate concentration of 0.500 M, how many grams of each selected compounds below would you mix? Given that: H3PO4 (FM 98.00), NaH2PO4 (FM 119.98), Na2HPO4 (FM 141.96), and Na3PO4 (FM 163.94)? Ka1 = 7.1 x 10-3; Ka2 = 6.3 x 10-8; Ka3 = 4.5 x 10-13Attem A 4.00 (+0.01) mL Class A transfer pipet is used to transfer 4.00 mL of a 0.328 (+0.005) M Cu2+ stock solution to a 100.00 (+0.08) Class A volumetric flask. Deionized water is used to bring the flask to volume. Calculate the concentration of the diluted soluion in the volumetric flask and report its absolute uncertainty. Significant figures are graded for this problem. To avoid rounding errors, do not round your answers until the very end of your calculations. [Cu²*] = 0.0117 M 土 0.095 M 山T四 étv huluYour instructor has asked you to prepare 2.00 L of 0.169 M NaOH from a stock solution of 53.4 (60.4) wt% NaOH with a density of 1.52 (60.01) g/mL. (a) How many milliliters of stock solution will you need? (b) If the uncertainty in delivering the NaOH is 60.10 mL, calculate the absolute uncertainty in the molarity (0.169 M). Assume negligible uncertainty in the formula mass of NaOH and in the final volume, 2.00 L.