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The pH of a liquid is 8.2 + 0.1. Find [H1] and its absolute and relative uncertainty.
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- (a) The pH of a solution is 5.42 + 0.05. Find [H1] and its uncertainty. (b) What is the relative uncertainty in [H1]? (c) Show that the relative uncertainty depends on the uncertainty in pH, but not on the value of pH.The pH of a solution is 6.70 ± 0.02. What is the concentration of H+ in the solution and its absolute uncertainty? (H*] = M ± M(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?
- What is a 99% confidence interval uncertainty of the slope when we are given a trendline with a slope of 42.211 and an R² value of 0.9991 for a set of 145 data points?Perform the calculations and determine the absolute and percent relative uncertainty. Express each answer with the correct number of significant figures. To avoid rounding errors, do not round your answers until the very end of your calculations. [9.8 (+0.3) - 2.31 (+0.01)] 8.5 (+0.6) absolute uncertainty: + percent relative uncertainty: + 8 9.2 (+0.4) × ([5.4 (±0.3) × 10−³] + [5.6 (±0.1) × 10−³]) = absolute uncertainty: ± 0.005 percent relative uncertainty: + % %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 10-13
- If the pH of a solution is 2.78 with an absolute uncertainty of ±0.05, what is the [H+] and its uncertainty? O [H+] = 1.66 x 10-3 M uncertainty in the concentration O [H+] = 1.66 x 10-3 M uncertainty in the concentration O [H+] = 1.34 x 10-4 M uncertainty in the concentration 1.78 x 10-5 M O [H+] 1.33 x 10 M -4 uncertainty in the concentration= 1.91 x 10-4 M -1.25 x 10-5 M 1.65 x 10-5 MSuppose 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.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.
- 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?Determine the volume of a sample of copper in (m³) with a mass of 2.2 x 105 tons and a density of 8.96 g/cm. (1 ton = 2205 lbs, 1 lb = 16 ounces, 1 kg = 2.20 lbs,1 kg = 1000g. 100 cm = 1m) %3D %3! %3D1) Report the results of this calculation along with both the percent relative and absolute uncertainties. 417.3 ± 0.4 × 71.8 ± 0.7(647.21 ± 0.2 − 182.3 ± 0.4) Absolute uncertainty:Percent uncertainty: