A 4.912-g sample of a petroleum product was burned in a tube furnace, and the SO 2 produced was collected in 3 % H 2 0 2. Reaction: SO 2 (g) + H 20 2 → H 2 SO 4 A 25.00-mL portion of 0.00873M NAOH was introduced into the solution of H 2 SO 4 , following which the excess base was back-titrated with 15.17 mL of 0.01102 M HCl. Calculate the sulfur concentration in the sample in parts per million.

A 4.912-g sample of a petroleum product was burned in a tube furnace, and the SO 2 produced was collected in 3 % H 2 0 2. Reaction: SO 2 (g) + H 20 2 → H 2 SO 4 A 25.00-mL portion of 0.00873M NAOH was introduced into the solution of H 2 SO 4 , following which the excess base was back-titrated with 15.17 mL of 0.01102 M HCl. Calculate the sulfur concentration in the sample in parts per million.

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter4: Stoichiometry: Quantitative Information About Chemical Reactions

Section4.9: Spectrophotometry

Problem 2.1ACP: Excess KI is added to a 100.0-mL sample of a soft drink that had been contaminated with bleach,...

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6. The hydrogen sulfide in an 80.0-g sample of crude petroleum was removed by distillation and uncollected in a solution of CdCl2. The precipitated CdS was then filtered, washed, and ignited to CdSO4. Calculate the percentage of H2S in the sample if 0.125 g of CdSO4 was recovered. 7. A 0.2121-g sample of an organic compound was burned in a stream of oxygen, and the CO2 produced was collected in a solution of barium hydroxide. Calculate the percentage of carbon in the sample if 0.6006 g of BaCO3 was formed.
The ethyl acetate concentration in an alcoholic solution was determined by diluting a 10.00-mL sample to 100.00 mL. A 20.00-mL portion of the diluted solution was refluxed with 40.00 mL of 0.04672 M KOH. After cooling, the excess OH2 was back-titrated with 3.41 mL of 0.05042 M H2SO4. Calculate the amount of ethyl acetate (88.11 g/mol) in the original sample in grams.
The ethyl acetate concentration in a alcoholic solution was determined by diluting a 10.00 mL sample to 100.00 mL. A 20.00 mL portion of diluted solution was refluxed with 40.00 mL of 0.04672 M KOH. Ater cooling, the excess OH2 was back-titrated with 3.41 mL of 0.05042 M H2SO4. Calculate the amount of ethyl acetate (88.11 g mol) in the original sample in grams.
0.7050-g of pure KHP (FW = 204.2) was dissolved and titrated with 35.00mL of NaOH solution. The excess NaOH was backtitrated with 5.00mL of HCl solution. In a separate titration it was found that 30.00mL of NaOH will react with 28.00mL of HCl. Find the molarity of NaOH and HCl. Show all the solutions involved and round-off final answers to two decimal places except for Molarity. (Molar concentrations should be in four decimal places)
The solubility of borax, which is made up of sodium tetraborate (Na2B4O5(OH)4 8H2O), was analyzed. The dissolution of borax is: Na2B4O5(OH)4 • 8H2O(s) ⇌ 2 Na+(aq) + B4O5(OH)42–(aq) + 8 H2O(l) A 50 mL saturated solution was prepared. After filtration of solution, 5 mL aliquot was transferred to a flask and titrated using 0.432 M HCl. The endpoint was found to be 4.73 mL of the titrant. Tetraborate anion (B4O5(OH)42-) is a weak base which reacts with HCl like the following reaction: B4O5(OH)42–(aq) + 2 H+(aq) + 3 H2O(l) ⇌ 4 H3BO3(aq) What is Ksp expression for the dissolution? What is the tetraborate ions concentration in the filtrate? What is the molar solubility and Ksp of borax if the titration was done at room temperature (298 K)?
0.7050-g of pure KHP (FW = 204.2) was dissolved and titrated with 35.00mL of NaOH solution. The excess NaOH was backtitrated with 5.00mL of HCl solution. In a separate titration it was found that 30.00mL of NaOH will react with 28.00mL of HCl. Find the molarity of NaOH and HCl.
Five white, 500-mg uncoated ascorbic acid (AA) tablets with an average weight of 0.6152-g were pulverized in a mortar. A sample of the powdered ascorbic acid weighing 0.4700-g was placed in an iodine flask and was dissolved in 50-mL H2SO4 then 5-g of KBr was added to the resulting solution. The solution was titrated with 47.81-mL of 0.09640 N STD. KBrO3 to reach a faint yellow endpoint then 3-g KI and 5-mL Starch TS. The blue color solution is then titrated with 2.73-mL of 0.09123 N STD. Na2S2O3 to reach the disappearance of the blue iodostarch complex. MW: KBrO3 = 167.0 ; KIO3 = 214.0 ; Na2S2O3 = 158.11 ; C6H8O6 = 176.12 Compute the milligrams of pure AA per tablet from the assay. 293.3 mg 502.5 mg None of the choices 383.9 mg
Zhongli is a speleologist tasked to analyze the CaCO₃ content of a limestone stalactite. A 5.0000-g sample was dissolved in 25.00 mL of 1.350 M HCl, it was then heated to expel any CO₂ formed. The excess HCl was titrated to a phenolphthalein end point, it used 37.50 mL of 0.1200 M NaOH. What is the reaction for the digestion of the limestone sample A. 2 NaOH + CaCO₃ ⇌ Na₂CO₃ + Ca(OH)₂ B. CaCO₃ ⇌ CaO + CO₂ C. 2 HCl + CaCO₃ ⇌ CaCl₂ + H₂O + CO₂ D. NaOH + HCl ⇌ NaCl + H₂O
A 1.250 g sample of cheese was subjected to a Kjeldahl analysis to determine the amount of protein. The sample was digested, the nitrogen is oxidized to NH₄⁺, and was then converted to NH₃ with NaOH, and distilled into a collection flask containing 50.00 mL of 0.1050 M HCl. The excess HCl is back titrated with 0.1175 M NaOH, this required 21.65 mL to reach the bromothymol blue end point. A. How many moles of N is present in the cheese sample? B. Report the %N of the cheese sample. C. Report the %protein of the cheese sample, assuming that there are 6.4 grams of protein for every gram of nitrogen
A 1.250 g sample of cheese was subjected to a Kjeldahl analysis to determine the amount of protein. The sample was digested, the nitrogen is oxidized to NH₄⁺, and was then converted to NH₃ with NaOH, and distilled into a collection flask containing 50.00 mL of 0.1050 M HCl. The excess HCl is back titrated with 0.1175 M NaOH, this required 21.65 mL to reach the bromothymol blue end point. What is the reaction for the digestion of the limestone sample A. 2 NaOH + CaCO₃ ⇌ Na₂CO₃ + Ca(OH)₂ B. 2 HCl + CaCO₃ ⇌ CaCl₂ + H₂O + CO₂ C. CaCO₃ ⇌ CaO + CO₂ D. NaOH + HCl ⇌ NaCl + H₂O
A 1.250 g sample of cheese was subjected to a Kjeldahl analysis to determine the amount of protein. The sample was digested, the nitrogen is oxidized to NH₄⁺, and was then converted to NH₃ with NaOH, and distilled into a collection flask containing 50.00 mL of 0.1050 M HCl. The excess HCl is back titrated with 0.1175 M NaOH, this required 21.65 mL to reach the bromothymol blue end point. What is the reaction for the back titration for this analysis? a. NH₄⁺ + NaOH ⇌ NH₃ + H₂O + Na⁺ b. NaOH + HCl ⇌ NaCl + H₂O c. NH₃ + HCl ⇌ NH₄⁺ + Cl⁻ d. N₂ + 3 H₂ ⇌ 2 NH₃ How many moles of N is present in the cheese sample? a. 544 x 10⁻³ b. 706 x 10⁻³ c. 250 x 10⁻³ d. 794 x 10⁻³ Report the %N of the cheese sample. a. 851% b. 884% c. 033% d. 736%
The formaldehyde content of a pesticide was determined by weighing 0.9327 g of the liquid sample into a flask containing 50.0 mL of 0.08624 M NaOH and 50 mL of 3% H2O2. It was heated then cooled. After cooling, the excess base was titrated with 27.8 mL of 0.06325 M H2SO4. Calculate the percentage of HCHO in the sample.