A 5.00 (10.01) 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
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- 3-3 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) 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]
- 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/molA 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?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.
- Suppose that you used smaller volumetric apparatus to prepare 0.250 M NH3 solution by diluting 84.6 (±0.8) µL of 28.0 (±0.5) wt% NH3 up to 5.00 (±0.02) mL. Find the uncertainty in 0.250 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 doEstimate the absolute deviation and the coefficient of variation for the results of the following calculations. Round each result so that it contains only significant digits. The numbers in parentheses are absolute standard deviations. (1.203 (+0.004) × 103 + 1.625 (±0.005) × 102 – 34.012(±0.001) y = - %3D 3.9201 (±0.0006) × 10-3
- The operations involved in preparing a diluted solution from a more concentrated solution are shown. What is the absolute uncertainty in the concentration of the diluted solution? 0.363 (±0.004) M×15.00 (±0.03) mL 100.00 (±0.08) mL None of those ±0.09 M ±0.000 6 M ±0.00 4 M ±0.01 M ±0.000 01 M = 0.054 45M (unrounded)Rewrite the number 3.123 56 (+0.167 89%) in the forms (a) number (6absolute uncertainty) and (b) number (+percent relative uncertainty) with an appropriate number of digits.Attem 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 hulu