The concentration of H2S in wastewater samples was determined by coulometric titration using Kl as mediator and I3 as "titrant". H2S(ag) + 13 (ag) + 2H2Ou) --> 2H3O*(aq) + 31 (ag) + S(s) A 50 mL wastewater sample was placed in a coulometric cell, added with excess KI and starch indicator. Electrolysis was carried out at a constant current of 84.6 mA for 386 s to reach the end point of the titration. What is the concentration of H2S in the sample (in ppm)?

The concentration of H2S in wastewater samples was determined by coulometric titration using Kl as mediator and I3 as "titrant". H2S(ag) + 13 (ag) + 2H2Ou) --> 2H3O*(aq) + 31 (ag) + S(s) A 50 mL wastewater sample was placed in a coulometric cell, added with excess KI and starch indicator. Electrolysis was carried out at a constant current of 84.6 mA for 386 s to reach the end point of the titration. What is the concentration of H2S in the sample (in ppm)?

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 14.97QE: According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as...

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The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSiF6, 0.026 g/100 mL (contains SiF62- ions) (b) Ce(IO3)4, 1.5102 g/100 mL (c) Gd2(SO4)3, 3.98 g/100 mL (d) (NH4)2PtBr6, 0.59 g/100 mL (contains PtBr62- ions)
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When 85.0 mL of 0.250 M Ba(OH)2 solution is added to 85.00 mL of 0.250 M Al (NO3)3 solution, a white gelatinous precipitate of Al(OH)3; is formed. Assuming 100% yield, (a) what mass (in grams) of Al(OH)3 is formed? (b) what is the molarity of each of the ions Ba2+, OH-, Al3+, NO3- in the resulting solution?
Lead poisoning has been a hazard for centuries. Some scholars believe that the decline of the Roman Empire can be traced, in part, to high levels of lead in water from containers and pipes, and from wine that was stored in leadglazed containers. If we presume that the typical Roman water supply was saturated with lead carbonate, PbCO3 (Ksp = 7.4 1014), how much lead will a Roman ingest in a year if he or she drinks 1 L/day from the container?
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A solution was prepared by dissolving 435 mg of K3Fe(CN)6 in enough water to give 945 mL of solution. (a) Calculate the molar concentration of K+(aq) and Fe(CN)63-(aq). (b) The normality of K+(aq) and Fe(CN)63-(aq). c) Calculate the weight/volume percentage of K3Fe(CN)6. d) The concentration of K+(aq) and Fe(CN)63-(aq) in ppm.
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A solution of HClO4 was standardized by dissolving 0.4008 g ofprimary-standard-grade HgO in a solution of KBr: HgO(s) + 4Br- + H2O → HgBr4 2- + 2OH- The liberated OH2 consumed 43.75 mL of the acid. Calculate themolar concentration of the HClO4.
A 2.036 g of copper (II) salt was dissolved in a 250 mL volumetric flask. A 25 mL aliquot of the solution was analyzed by adding 1 g of potassium iodide and titrating the liberated iodine with 24.45 mL of 0.1664 M of sodium thiosulfate. Determine the percent by weight Cu in the sample. Cu2+ + + Cula + l3 l3 + S2O32 |- + S4O62- 19.05% 12.70% 6.35% O 25.40%
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