Iodometric titration of vitamic C with sodium thiosulfate Why was the known excess of iodine generated using iodate rather than weighing out a known excess of iodine?
Q: Why is rinsing of the burettes both with distilled water and solution a critical step in titration?
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Q: A multivitamin sample has a label claim of 500 mg ascorbic acid (176.12 g/mol). According to quality…
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Q: Determine the Weight f the Sample, if it Used 24.9ml of 0.1Normal Sodium Hydroxide of Titrant…
A: Solution- Data Given- 24.9ml of 0.1 Normal Sodium Hydroxide and 33.29% of Busulfan (C7H602
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Q: Why is the use of high-precision volumetric material essential for titration?
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Q: A multivitamin sample has a label claim of 500 mg ascorbic acid (176.12 g/mol). According to quality…
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Q: calculate the number of moles of sodium thiosulphate (vi) needed to react with iodine liberated…
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Q: Give six differences between tituration and levigation
A: Six differences between trituration and levigation- 1) Triturate is the continual rubbing of a solid…
Q: The Kjedahl procedure was used to analyze 256 µL of a solution containing 37.9 mg protein/mL. The…
A: NH3 + HCl = NH4Cl HCl + NaOH = H2O + NaCl Here, one mole of NH3 reacts with one of HCl and also…
Q: Determine the Weight f the Sample, if it Used 24.9ml of 0.1Normal Sodium Hydroxide of Titrant…
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Q: A multivitamin sample has a label claim of 500 mg ascorbic acid (176.12 g/mol). According to quality…
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A: Methyl orange is used as an indicator in this titration.
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Q: Why did the color of the solution in the conical flask change at the end of the titration?
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A: In which cases are the wet Electrostatic Precipitators used?
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Q: 2. What is the physical observation when the endpoint has been achieved during titration?
A: Endpoint: refers to the point at which the indicator changes color in an acid-base titration.
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Q: How would the calculated molar concentration of the analyte be affected if the burette is rinsed…
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Iodometric titration of vitamic C with sodium thiosulfate
Why was the known excess of iodine generated using iodate rather than weighing out a known excess of iodine?
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- The Merck Index indicates that 10 mg of guanidine,CH5N3, may be administered for each kilogram of bodymass in the treatment of myasthenia gravis. The nitrogenin a 4-tablet sample that had a total mass of 7.50 g wasconverted to ammonia by a Kjeldahl digestion, followedby distillation into 100.0 mL of 0.1750 M HCl. Theanalysis was completed by titrating the excess acid with11.37 mL of 0.1080 M NaOH. How many of thesetablets represent a proper dose for a patient who weighs(a) 100 lb, (b) 150 lb, and (c) 275 lb?Which of the following statement of neutralization titration experiment is correct? 1. OBromocresol green indıcator has yellow color in basic media O Sodium hydroxide was used for standardization phosphoric acid 3. Oredox titration involve acid-base reactions 4. OKHP is secondary standard material 5. OPhosphoric acid is analyte in this experimentWhich of the following is incorrect about direct titration? 1. OThe prepared solutions must be stable during titration 2. OStoichiometry of reaction between analyte and titrant should be known. 3. OReaction between titrant and analyte should be slow. 4. OReaction between titrant and analyte should be fast.
- 4. Determine the weight of pure urea in a 500 mg sample if 15.35 ml of 0.4967N NaOH were required in the titration after the ammonia from the sample had been distilled into 50.0 ml of 0.4861N H2SO4.The Kjeldahl procedure was used to analyze 244 µL of a solution containing 38.1 mg protein/mL. The liberated NH3 was collected in 5.00 mL of 0.0375 M HCl and the remaining acid required 5.98 mL of 0.00998 M NaOH for complete titration. What is the weight percent of nitrogen in the protein?An indicator was not used during potentiometric titration of a weak acid Is there a positive error, negative error, no effect, or error could not be determined In terms of the Computed pKa of the unknown weak acid?
- 5. A 300.0 mg sample containing Na,CO3, NaHCO3 and NaOH and inert material either alone or in some combination was dissolved and titrated with 0.1000 M HCI the titration required 24.41 mL to reach the phenolphthalein endpoint. And an additional 8.67 mL to reach the methyl red endpoint. Determine the composition of the sample and calculate the percent of each titrated component.Consider the data obtained from titration of HCl with NaOH to a phenolphthalein end point: MHCl = 0.37M, VHCl = 25.10mL, VNaOH = 36.45 mL.An unknown sample containing mixed alkal (NaOH NaHCO or Na,CO) was analyzed using the double flask method, A 250 mg sample was dissolved in 250 m CO3 free water. A 20.0 mL aliquot of this sample required 11.3 ml. of 0.009125 M HCl solution to reach the phenolphthalein end point. Another 29.0 ml aliquot of the sample was bitrated to the bromocresol green endpoint using 31.1 ml of the standard acid. How many millimoles of the components are there in the original solid sample) 0-928 mmol No. 0.0103 mmol NaOH 0078 m N.CO Cannot be determined 012 mol NaC0, 197 minol NaHCO 129 mmol NaOH, 097ml Najco
- A 100.00-mL sample of 0.2000M glycine, A+ form (see structure below), was titrated with 0.2000Mof NaOH. Ka1 of glycine = 3.16x10-3; Ka2 of glycine = 2.51x10-10 a) What is the pH after the addition of 100.00 mL of NaOH?(b) What is the pH after the addition of 180.00 mL of NaOHA 0.9092-g sample of a wheat flour was ana- lyzed by the Kjeldahl procedure. The ammonia formed was distilled into 50.00 mL of 0.05063 M HCI; a 7.46-mL back-titration with 0.04917 M NAOH was required. Calculate the percent- age of protein in the flour.5. A 300.0 mg sample containing Na,CO3, NaHCO, and NaOH and inert material either alone or in some combination was dissolved and titrated with 0.1000 M HCI the titration required 24.41 ml to reach the phenolphthalein endpoint. And an additional 8.67 mL to reach the methyl red endpoint. Determine the composition of the sample and calculate the percent of each titrated component.