A solution of HNO, is standardized by reaction with pure sodium carbonate. +2 Na* + H₂O + CO₂ 2H+Na₂CO, A volume of 27.42 + 0.05 ml of HNO, solution was required for complete reaction with 0.8388 +0.0007 g of Na, CO,. (FM 105.988+0.001 g/mol). Find the molarity of the HNO, solution and its absolute uncertainty. [HNO,1- Note: Significant figures are graded for this problem. To avoid rounding errors, do not round your answers until the very end of your calculations. 0.576 1 Incorrect M 0.0026 At Incorrect M
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- 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) 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.
- Example 2: You prepared a 0.250 M NH3 solution by diluting 8.45 (±0.04) mL of 28.0 (10.5) 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.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.2H+ + Na2CO3⟶2Na+ + H2O + CO2 the volume of 28.30 ± 0.06 mL of HNO3 solution was required for complete reaction with 0.8450 ± 0.0009 g of Na2CO3, (FM 105.988 ± 0.001 g/mol). Please Find the molarity of the HNO3 solution along with its absolute uncertainty. 1. [HNO3] = ________________ M 2. ___ ± ____________ M
- 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.-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 choice1. (40 pts) We can measure the concentration of HCl solution by reaction with pure sodium carbonate: 2H + Na2CO3 →2Na+ + H₂O + CO₂ Complete reaction with 0.9674 +0.0009 g of Na2CO3 (FM 105.9884 +0.0007) required 27.35 0.04 mL of HCl. Find the molarity of the HCI and its absolute uncertainty.
- Q3/ A) 0.63 g of a sample containing Na,CO3, NaHCO, and inert impurities is titrated with 0.2 M HCI, requiring 17.2 mL to reach the phenolphthalein end point and a total of 43.5 mL to reach the modified methyl orange end point, How many grams NazCO3 and NaHCO, are in the mixture?P Question /// Q 10) Find the value of the equilibrium constant expression. Fe3+ SCN- FESCN?+ 1.3 x 10-3 1.3 x 10-3 C -1.80 x 10-4 -1.80 x 10-4 +1.80 x 10-4 1.1 x 10-3 1.1 x 10-3 +1.80 x 10-4 P Question //Q 11) For the spectrophotometry experiment, the student first makes a standard curve. The student uses a 0.1000 M solution of CuSO4(aq) to make three more(a) How many grams of nickel are contained in 10.0 g of a 10.2 wt% solution of nickel sulfate hexahydrate, NiSO4 ? 6H2O (FM 262.85)? (b) The concentration of this solution is 0.412 M. Find its density.