3) In the treatment of myasthenia gravis, 10 mg of guanidine (NH-C(NH2)2) per kilogram of body weight is given. Nitrogen in a sample with a total mass of 7.50 g and containing 4 tablets is converted to ammonia by Kjeldahl decomposition. It is then distilled into 100 mL of 0.1750 M HCI. Performed analysis; titration of excess acid with 11.37 mL of 0.180 M NaOH solution. Accordingly, in which option is the number of tablets at the appropriate dose given for a 48 kg patient? (C-12.0 g/mol; H=1 g/mol; N = 14.0 g/mol; CI-35,5 g/mol) a) 3 b) 6 c) 9 d) 12 f) 15

3) In the treatment of myasthenia gravis, 10 mg of guanidine (NH-C(NH2)2) per kilogram of body weight is given. Nitrogen in a sample with a total mass of 7.50 g and containing 4 tablets is converted to ammonia by Kjeldahl decomposition. It is then distilled into 100 mL of 0.1750 M HCI. Performed analysis; titration of excess acid with 11.37 mL of 0.180 M NaOH solution. Accordingly, in which option is the number of tablets at the appropriate dose given for a 48 kg patient? (C-12.0 g/mol; H=1 g/mol; N = 14.0 g/mol; CI-35,5 g/mol) a) 3 b) 6 c) 9 d) 12 f) 15

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter16: Applications Of Neutralization Titrations

Section: Chapter Questions

Problem 16.37QAP

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3.) In the assay of NaHCO3, 3.0g of the solid is dissolved in 25mL water. What is the normality? How many mL of 1N H2SO4 will be required to neutralize this solution? From this volume of acid, compute the percent purity of NaHCO3.
3) 2.413 g sample contains Na CO̟, NaHCO and inert material. This sample was solved in water and diluted to 250.0 ml. 80 ml solution was taken and titrated with 0.09644 N HCl with the indicator of phenolftalein. 6.13 ml HCl was consumed. From a second solution, again 80 ml was taken and titrated with the same HCl solution with the indicator of methylorange. 15.4 ml HCl was consumed. Calculate the percentage of NaHCO¸ and 3 Na CO in sample (Na CO_=106.0 g/mol, NaHCO_=84.02 g/mol). 3
3) 2.413 g sample contains Na CO, NaHCO and inert material. This sample was solved in water and diluted to 250.0 ml. 80 ml solution was taken and titrated with 0.09644 N HCl with the indicator of phenolftalein. 6.13 ml HCl was consumed. From a second solution, again 80 ml was taken and titrated with the same HCl solution with the indicator of methylorange. 15.4 ml HCl was consumed. Calculate the percentage of NaHCO and Na CO in sample (Na_CO_=106.0 g/mol, NaHCO =84.02 g/mol). 2 2 3 3
A sample of meat scrap weighing 2.000 g is digested with concentrated sulfuric acid and a catalyst. The resulting solution is made alkaline with NaOH and the liberated ammonia distilled into 50.00 mL of 0.6700 N HCl. The excess acid then requires 30.10 mL of 0.6520 N NaOH for neutralization. What is the percentage of the protein in the meat? The Kjeldahl factor is 6.25. (pls answer thanku)
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The ascorbic acid, C,H;Os (176.124 g/mmol) content of a bottle of peach juice containing 2.50 L was determined by titration with a standard solution of potassium iodate, KIO3. The KIO; solution was prepared by dissolving 100.4 mg primary standard grade KIO; (214.001 mg/mmol) to a final volume of 250.0 mL. To a 200.00-mL aliquot of the sample, 10 mL of KI, 10 mL of HCl and 5 mL of starch solution were added and subsequently titrated, requiring 18.19 mL of the KIO; titrant. The relevant reactions are given below: KIO; + 5KI + 6H* → 3l2 + 6K* + 3H;0 CH;O, + l2→ CH,O, + 21- + 2H* a. How many millimoles of ascorbic acid is in the titrated sample? b. What is the mass of ascorbic acid per bottle of the peach juice?
The ethyl acetate concentration in an alcoholic solution was determined by diluting a 10.00-mL sample to 100.00 mL. A 19.00-mL portion of the diluted solution was refluxed with 40.00 mL of 0.04601 M KOH: CH3 СОО С2H; + ОН — СH3 COO + C2H; ОН After cooling, the excess OH was back-titrated with 3.02 mL of 0.05056 M H2 SO4. Calculate the amount of ethyl acetate (88.11 g/mol) in the original sample in grams. Amount of ethyl acetate =
Calculate the percentage CH3COOH in a sample of vinegar from the following data.Sample = 15.00 g, NaOH used = 43.00 ml ; 0.600 N H2SO4 used for back titration =0.250 ml ; 1.00ml NaOH is equivalent to 0.0315 g H2C2O4. 2H2O.
A 1.219-g containing (NH4)2SO4, NH4NO3, and nonreactive substances was diluted to 200 mL in a volumetric flask. A 50.00-mL aliquot was made basic with strong alkali, and the liberated NH3 was distilled into 30.00-mL of 0.08421 M HCl. The excess HCl required 10.17 mL of 0.08802 M NaOH. A 25-mL aliquot of the sample was made alkaline after the addition of Devarda’s alloy, and the NO3- was reduced to NH3. The NH3 from both the NH4+ and NO3- was then distilled into 30.00 mL of the standard acid and back titrated with 14.16 mL of base. Calculate the percentage of (NH4)2SO4 and NH4NO3 in the sample.
The arsenic in a 2.345g sample of a pesticide was converted to H 3 AsO4 by suitable treatment.The acid was then neutralized, and 60.00 ml of 0.06781M AgNO 3 was added to precipitate thearsenic quantitatively as Ag 3 AsO4. The excess Ag+ in the filtrate and washings from theprecipitate was titrated with 15.27 ml of 0.123 M KSCN; the reaction wasAg+ + SCN- → AgSCN(s)Calculate the percentage As 2 O 3 in the sample.
3. Analysis of a mixture consisting of NaOH + Na2CO3 + inert matter gives the following data: 10.00 g. Its aqueous solution is diluted to 250.0 mL and two separate 25.00 mL sample portions are titrated. With one portion, an end point with phenolphthalein is obtained in cold solution, with 44.52 mL of 0.5000 N HCI. The other portion requires 46.53 mL of the acid for an end point with methyl orange. Calculate the percentage composition of the original sample.