The sulfur from 4.00g steel is evolved as dihydrogen sulfide gas and titrated with 1.60 mL of 0.0500N iodine solution. How many milliliters if iodine will be reduced by 40.00 mL of Na2S2O3 solution of which 1mL thiosulfate solution = 0.006354g Cu? H2S + 12 → S + 21- + 2H+ AsO33- + 2HCO3- + l2 → AsO43- + 21- + 2CO2 + H20 2Cu2+ + 41- → 2Cul + l2 103 + 61- + 6H+ → 312 + - 3H2O 4.0mL 2.0mL 80mL O 160mL

The sulfur from 4.00g steel is evolved as dihydrogen sulfide gas and titrated with 1.60 mL of 0.0500N iodine solution. How many milliliters if iodine will be reduced by 40.00 mL of Na2S2O3 solution of which 1mL thiosulfate solution = 0.006354g Cu? H2S + 12 → S + 21- + 2H+ AsO33- + 2HCO3- + l2 → AsO43- + 21- + 2CO2 + H20 2Cu2+ + 41- → 2Cul + l2 103 + 61- + 6H+ → 312 + - 3H2O 4.0mL 2.0mL 80mL O 160mL

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter15: Equilibria Of Other Reaction Classes

Section: Chapter Questions

Problem 10E: The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities...

See similar textbooks

Similar questions

A solid sample containing chloride and with a mass equal to 6.000 g was dissolved in water and transferred to a 100.0 ml flask. A 50.0 mL aliquot of this solution was diluted to 250.0 mL. In the titration of 20.0 mL of the diluted solution, 32.0 mL of 0.2000 mol L-1 AgNO3 standard solution were used. Calculate the % of impurities in the analyzed sample. Data: Cl = 35.45
A 100.0 mL water sample was mixed with 25.00 mL of 0.002517 M K₂Cr₂O7 (294.2 g/mol) to oxidize Fe² to Fe³+ The excess K₂Cr₂O7 was back-titrated with 5.30 mL of 0.00949 M Fe²+ on Calculate the concentration of Fe (55.8 g/mol) in the sample in parts per million. *+ Cr₂O7²- + 14H+ 6Fe³+ + 2Cr³+ + 7H₂O ( a. 113 b. 138 C 166 d. 183 e 160 1
The SO2 present in air is mainly responsible for the phenomenon of acid rain. The concentration of SO2 can be determined by titrating against a standard permanganate solution as follows: 5SO2 + 2MnO4- + 2H2O ---> 5SO42- + 2Ms2 + 4H+ Calculate the number of grams of SO2 in a sample of air if 4.90mL of 0.00700M KMnO4 solution are required for the titration. Be sure your answer has the correct number of significant digits.
A 10.00 mL sample containing 8.00 g/L of a mixture of KCI and NaCl was titrated with 0.10 M standard solution of AgNO3; where 5.6 mL was needed to reach the end-point. Calculate the mass of sample (in grams). 1. O0.0033 2. O0.0800 3. O0.0083 4. O0.0337
- Calculate the concerntration of NaOH in the solution provided.
2. A sample of pure sodium chloride (MW = EW = 58.44 ) weighing 0.2286 g is dissolved in water and exactly 50.00 mL of silver nitrate solution is added to precipitate AgCl. The excess Ag* is titrated with 12.56 mL of a 0.0986 N solution of KSCN. Calculate the normality of the AGNO3 solution.
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%
25.00 mL of a solution containing KIO4 is treated with excess potassium iodide. IO4- + 8H+ + 7I- → 4I2 + 4H2O The resulting solution is titrated with 0.15 M sodium thiosulfate pentahydrate. The average titre was 21.76 mL. I2 + 2S2O32- → 2I- + S4O62- What mass of KIO4 (in g) was dissolved in water to make the original solution?
A sample of unknown iron ore weighs 0.35 g. It is digested using dilute HCl. An SnCl2 solution is added to turn the solution yellow. Zimmermann–Reinhardt reagent is added, and the solution is diluted to 150mL. It is then titrated with 31.30 mL of 0.045 M potassium permanganate. a) How many moles of MnO4- were used to titrate the iron in the sample? b) How many moles of Fe2+ were in the sample? c) What is the mass of iron in the sample? d) What is the % w/w of Fe in the sample?
Sample containing arsenic weighing 0.800 are titrated with a standard iodine soluton. what should be the normality of the iodine in order that each ml of titrant represents 1/2% As2O3 in the sample (Answer: 0.0809 N show full solution please)
The concentration of H2S in wastewater samples was determined by coulometric titration using Kl as mediator and I3 as "titrant". H2S(as) + 13 (ag) + 2H2Ou) --> 2H3O*(aq) + 31 (ag) + S(s) A 50 ml wastewater sample was placed in a coulometric cell, added with excess Kl 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)?
Please show Given, Required, and Solution. Thank you very much! 2. Titration of 0.2121 g of pure Na2C2O4 (134.00 g/mol) required 43.31 mL of KMnO4. What is the molar concentration of the KMnO4 solution? The chemical reaction is