I want the best value for percent purity and how did you arrive at the best value TF.Commercial aspirinBLab synthesized aspirinBComment on the purity of each sample and discuss the result.Part Il-Synthesized AspirinTrial 1Trial 2Mass of aspirin (g).486 g485 g2.70 x 10^-3 mol2.69 x 10^-3 molTheoretical molesShow calculations for theoretical moles:trial 1:.486 g asp x 1.00 mol / 180.16 g asp = 2.70 x 10 ^~3trial 2 :0.485 g asp x 1.00 / 180.16 g asp = 2.69 x 10 ^-3Molarity of NaOH (mol/L).216 mol/LVolume of NaOH used (mL)trial 1: 11.85 mLtrial 2: 12.99 mLColor of Solutiontrial 1: medium/ dark pink colortrial 2: darker pink color than trial 1Moles of NaOH usedtrial 1:.026 moles NaOHtrial 2 : .028 moles NaOHShow calculations for moles NaOH:trial 1: .216 mol / 1.00 Lx.1185 L NAOH = .26 moles NaOHtrial 2: .216 mol /1.00 Lx .1299 NaOH = .28 moles NaOH%3DMacBook Air000000DD08F3F6F5F4232$7.8.3.5.E.K.H. Percent purity of aspirin (%)99.41Example Calculation:.4833 g asp/.4862 x 100 = 99.41%Best Value for % PurityHow did you arrive at the best value?Part III-Commercial AspirinTrial 1.371gMass of aspirin tablet (g)2.06x10^-3Theoretical moles in tablet

The best value is calculated from the average of the good data values.

Answered: Best Value for % Purity How did you…

EBK A SMALL SCALE APPROACH TO ORGANIC L

4th Edition

ISBN:9781305446021

Author:Lampman

Publisher:Lampman

Chapter3: Extraction

Section: Chapter Questions

Problem 1Q

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You have a chemical in a sealed glass container filled with air. The setup is sitting on a balance as shown below. The chemical is ignited by means of a magnifying glass focusing sunlight on the reactant. After the chemical has completely burned, which of the following is true? Explain your answer. a. The balance will read less than 250.0 g. b. The balance will read 250.0 g. c. The balance will read greater than 250.0 g. d. The scales reading cannot be determined without knowing the identity of the chemical.
The meat from one hazelnut has a mass of 0.985 g. (a) What is the mass of a millionth of a mole (106) of hazelnut meats? (A millionth of a mole is also called a micromole.) (b) How many moles are in a pound of hazelnut meats?
the label on an ocean spary cran-raspberry drink list 30g of surgar in 240mL of drink. I weighted 240mL of drink and found its mass to be 251g. what is the percent composition of surgar in the drink.
Commercial aqueous nitric acid has a density of 1.42 g/mLand is 16 M. Calculate the percent HNO3 by mass in thesolution.
An antacid tablet weighing 0.942g contained calcium carbonate as the active ingredient., in addition to an inert binder. When an acid solution weighing 56.413g was added to the tablet, carbon dioxide was released, producing fizz. The resulting solution weighted 57.136g. How many grams of carbon dioxide were produced?
Given the following data for the hydrate M(NO3)3 dot X H2O, where M is a metal with the atomic mass 90.97 g/mol, Mass of Crucible and Lid 34.0386 Mass of Crucible, Lid and Hydrate 39.4586 Mass of Crucible, Lid and Anhydrous Salt (3rd Heating) 37.3780 What was the mass percent of water in the hydrated salt, with the correct significant figures? Express units as %
Swimming pool water is often made safe for swimming by treating with chlorine in the form of sodium hypocholrite (NaOCI) solution. If a swimming pool contains 5.62×10^5L of water, what volume of 5.00% NaOCI (by mass) solution is required to produce a sodium hypoclorite concentrarion of 3.00×10^-7 mol /L? (assuume the density of water and the NaOCI solution is 1.00g/ml). Do not give handwriting solution.
a hydrated CuSO4 salt was heated and thus dehydrated. Determine the % H2O by weight in the hydrated CuSO4 salt. SHOW WORK TO RECEIVE FULL CREDIT mass of empty dish 43.571 gmass of dish + hydrated salt 44.326 gmass of dish + dehydrated salt 44.054 g 4. Using the data found in question number 3, determine the empirical formula for the hydrated CuSO4salt. What is the chemical name of this dehydrated salt? 5. Suppose that after your second heating, you were impatient and did not wait until your porcelain evaporating dish to cool. Instead, you weighed it while it was still hot. How would this specifically affect the calculated percentage of water in the compound?
1. A student collected the following data during Lab: Mass of MgCO3 hydrate = 0.9987 g. Constant mass of anhydrous MgCO3 = 0.4831 g How many moles of water were in the MgCO3 hydrate? 2. A student uses gravimetric determination to find the water of hydration of a hydrated sample of cobalt (II) sulfate. The student’s sample contained 0.0098459 moles of anhydrous cobalt(II) sulfate (CoSO4) and 0.068921 moles of water (H2O). What is the formula of the cobalt(II) sulfate hydrate? 3. A student has a sample of CaSO4 hydrate and it weighs 0.4813 grams. He heats it strongly to drive off the water of hydration, and after subsequent heatings, the student finds the anhydrous compound has a constant mass of 0.3750 grams. Find the formula of the hydrate.
How many moles of NaOCl would be present in 1 gallon of commercial bleach (density = 1.05 g/ml), which is 6.25% mass percent active ingredient. (1 L = 1.057 qt.)
Fluoride ion is poisonous in relatively low amounts: 0.2 g of F⁻ per 70 kg of body weight can cause death. Nevertheless,in order to prevent tooth decay, F⁻ ions are added to drinking water at a concentration of 1 mg of F⁻ion per L of water. How many liters of fluoridated drinking water would a 70-kg personhave to consume in one day to reach this toxic level? How manykilograms of sodium fluoride would be needed to treat a 8.50x10^7-gal reservoir?
2HCl + Na2CO3 > 2NaCl + CO2 + H2O mass of empty crucible and lid is 33.076 g grams of sodium carbonate = 0.575 g how many grams of sodium chloride should the person theoretically obtain from this experiment? Must show calculations

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Best Value for % Purity How did you arrive at the best value?