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- When purifying a sample of aspirin that was produced in the lab, the impure aspirin sample should be dissolved in a very cold solvent, so that solid impurities can be filtered and analyzed the next day or the next week. True or False?50.00 cm3 of a 1.5784 mol.dm-3 solution of potassium hydroxide is transferred to an empty 700.00 cm3 volumetric flask. This flask is made up to the mark with distilled water and then shaken well. The concentration of the potassium hydroxide in this second flask is:The distillation flask is best completely filled with mixture as large as available never less than half empty about 70% full
- A student determined fluoride in a toothpaste sample using ion chromatography. A toothpaste sample of mass 0.100 g was dissolved in type I water and then quantitatively filtered through a Whatman #1 filter paper into a clean 100 ml volumetric flask. The flask was then made up to volume with type I water and mixed thoroughly.A portion of the solution was filtered through a 0.45 um filter into a sample vial for analysis. Analysis of the sample gave a fluoride concentration of 1.60 mg/l Calculate the % w/w fluoride in the original toothpaste sample. (Give your answer to 3 decimal places please)Assignment: This is an individual activity. After studying the lesson and watching all the videos, answer the following questions. Answer in not more than 3 sentences per question. 1. Discuss the a) direct method of weighing b) indirect weighing using the analytical balance. 2. Explain how suction filtration is carried out in the laboratory. Give the important points that must be observed in doing the process. 3. Explain why it is important to wash the precipitate. Can distilled water be used to wash all types of precipitates? 4. Discuss how to use a desiccator. When should a desiccant be replaced?An impure sample of 0.1002 g benzoic acid underwent purification by recrystallization. A mass of 0.0542 g of white solid benzoic acid was obtained. Calculate the % purity of the initial sample. Show calculations and report the result with correct number of significant figures. Hi there please answer all parts clearly and concisely with legible hand writting, thank you!
- i have hard time geting it stright even after I do the experiment can u help me with the one pls Material ChemicalsSealed NO2 tubes, KSCN solution (0.002 M), acidified Fe(NO3)3 solution (0.2 M), KSCN crystals, Fe(NO3)3 crystals, KOH (concentrated (8 M)), distilled waterApparatus:Bunsen burner, ring stand, wire gauze, matches, thermometer, dropper, test tubes, glass stirring rod, beaker tongs Procedure Part A: Fill a 600 mL beaker to the 3/4 mark with water. Bring to a boil using a Bunsen burner. In another 600 mL beaker, fill to the 1/2 mark with water; add ice in order to lower the temperature to about 0°C. Note the room temperature. Observe the NO2 thoroughly at room temperature. Place the sealed NO2 tube in the cold bath. Note your observations. Remove the test tube from the cold bath. Let the test tube stand until it reaches room temperature. Note your observations. Place the test tube in the hot bath. Note your observations. Remove the test tube from the hot bath. Let the test…Make a dilution series to get to 1:100. Start with making 1:10 dilution by adding 1mL of sample and 9mL of diluent, now continue the series to get to 1:100A student weighed approximately 1.5 g of an unknown solid acid and carefully placed the sample in a clean, but not necessarily dry, 250.0 mL volumetric flask. The student added deionized water to the flask, swirled the solution until the solid acid dissolved, then added sufficient deionized water to fill the flask to the fill line. A volumetric pipet was used to transfer 25.00 mL of the resulting solution to an Erlenmeyer flask, and 2 – 3 drops of phenolphthalein were added.The student filled the sodium hydroxide buret and titrated the acid solution with standardized 0.1000 M NaOH to the first permanent faint pink color, then repeated the titration a second time.Your instructor will provide the mass of unknown solid acid, as well as the initial and final buret readings for the two titrations. From this data and the information above, you will be able to calculate the molar mass of the unknown acid.The unknown solid acid is diprotic; that is, there are two moles of ionizable H+ ions per…
- A student weighed approximately 1.5 g of an unknown solid acid and carefully placed the sample in a clean, but not necessarily dry, 250.0 mL volumetric flask. The student added deionized water to the flask, swirled the solution until the solid acid dissolved, then added sufficient deionized water to fill the flask to the fill line. A volumetric pipet was used to transfer 25.00 mL of the resulting solution to an Erlenmeyer flask, and 2 – 3 drops of phenolphthalein were added.The student filled the sodium hydroxide buret and titrated the acid solution with standardized 0.1000 M NaOH to the first permanent faint pink color, then repeated the titration a second time.Your instructor will provide the mass of unknown solid acid, as well as the initial and final buret readings for the two titrations. From this data and the information above, you will be able to calculate the molar mass of the unknown acid.The unknown solid acid is diprotic; that is, there are two moles of ionizable H+ ions per…Stock iron(II) solution (200Ug mL-1 Fe) ferrous ammonium sulfate hexahydrate mass= 0.1437g, transfer it to a 100 ml beaker. add 15 ml approx of water and 15m1 'approx of dilute sulphuric acid (2M H2SO.). then transfer FeII to 100 ml flask makeup to the mark with water. calculate the moles of ferrous ammonium sulfate hexahydrate solution in unit ug/mL.An oil sample had its iodine number determined using the pyridinium tribromide method. The sample and reagents used are as follows: Oil sample: 0.20 mL, density: 0.958 g/mL Pyridinium tribromide: 0.486 g Na2S2O3: 0.1 M, endpoint = 42.17 mL How much pyridinium tribromide was in excess?