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.
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- (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?Your 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.-3 A 0.3202 (±0.0001) g sample of a pure monoprotic acid required 20.04 (±0.02) cm° of 0.1005 (±0.0005) mol dm neutralisation. Find the molar mass of the acid in g mol together with its uncertainty also in g mol, with an appropriate number of digits. NaOH for -1 Select one: a. 1.59 x 102+ 0.2 g mol b. 1.60 x 10 + 0.03 g mol C. 1.590 x 102 + 0.03 g mol d. 1.590 x 10- + 0.2 g mol 1.60 x 10-+0.2 g mol е. Clear my choice
- Example 2: You prepared a 0.250 M NH3 solution by diluting 8.45 (±0.04) mL of 28.0 (±0.5) wt% NH3 [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, 17.0306 g/mol, has negligible uncertainty relative to other uncertainties in this problem. %3DThe pH of a solution is 6.70 ± 0.02. What is the concentration of H+ in the solution and its absolute uncertainty? (H*] = M ± MEXAMPLE 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.
- 1. How many milliliters of 53.40(±0.06) (w/w) % NaOH with a density of 1.52(±0.01)g/mL will you need to prepare 1.000 L of 0.200 M NaOH? Keep 1 extra sig fig in your answer (4). 2. If the uncertainty in delivering NaOH is ±0.01 mL, calculate the absolute uncertainty in molarity (0.200 M). Assume there is negligible uncertainty in the formula mass of NaOH and in the final volume (1.000 L) Hint: You will need to calculate the molarity of the 53.40% NaOH. One way to solve this is to assume that you have 100.00 grams of the initial NaOH solution. Determine how many grams are NaOH. Convert that value to moles NaOH. Using the density, determine the volume of your 100.00 grams of solution.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?(2) In the Analytical Chemistry Laboratory Mr.Yahiya Al Moqbali wanted to prepare KCI solution. He has dissolved 2.634 (+0.002) g of KCI in a 250.00 (±0.08) mL volumetric flask. Calculate the molarity of the solution and express your answer with its absolute uncertainty and give reasonable number of significant figure. [The formula mass of KCI is 74.5513 (±0.001) amu] (Show your Calculation)
- (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.What is the absolute uncertainty and relative uncertainty of the molarity of the solution? M = = 0.078376462 = 0.078 M Pb2+(a) Standard Ag1 solution was prepared by dissolving 1.224 3 g of dry AgNO3 (FM 169.87) in water in a 500.0-mL volumetric flask. A dilution was made by delivering 25.00 mL of solution with a pipet to a second 500.0-mL volumetric flask and diluting to the mark. Find the concentration of Ag1 in the dilute solution. (b) A 25.00-mL aliquot of unknown containing Cl2 was titrated with the dilute Ag1 solution, and the equivalence point was reached when 37.38 mL of Ag1 solution had been delivered. Find the concentration of Cl2 in the unknown.