A solution of sodium thiosulfate was standardized by dissolving 0.1906 g KIO3 (214.00 g/mol) in water, adding a large excess of KI, and acidifying with HCI. The liberated iodine required 48.92 mL of the thiosulfate solution to decolorize the blue starch/iodine complex. Calculate the molar concentration of the Na2S2O3. Express your answer with 3 decimal places

A solution of sodium thiosulfate was standardized by dissolving 0.1906 g KIO3 (214.00 g/mol) in water, adding a large excess of KI, and acidifying with HCI. The liberated iodine required 48.92 mL of the thiosulfate solution to decolorize the blue starch/iodine complex. Calculate the molar concentration of the Na2S2O3. Express your answer with 3 decimal places

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Chapter21: Chemistry Of The Main-group Elements

Section: Chapter Questions

Problem 21.190QP

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KClO3 in a 0.1862 g sample of an explosive was determined by the reaction with 50.00 mL of Fe2+ 0.01162 M. ClO3- + 6 Fe2+ + 6H+ → Cl- + 3H2O + 6Fe3+ When the reaction was complete, the excess Fe2+ was back-titrated with 13.26 mL of Ce4+ 0.07654 M. Calculate the percentage of KClO3 in the sample.
Question 3 A solution of sodium thiosulfate was standardized by dissolving 0.1172 g KIO3 (214.00 g/mol) in water, adding a large excess of KI, and acidifying with HCI. The liberated iodine required 44.09 mL of the thiosulfate solution to decolorize the blue starch/iodine complex. Calculate the molar concentration of the Na2S2O3. Express your answer with 3 decimal places
If 3.00g ruthenium (III) chloride, RuCl3 is added to 75.0mL of a 3.00M sodium periodate, NaIO4 solution. What is the mass of RuO4 produced by the reaction? 8RuCl3+5NaIO4+12H2O=8RuO4+5NaI+24HCl.What is the reducing agent and what is the oxidizing agent?
A 3650-mg sample containing bromate and bromide was dissolved in sufficient water to give 250.0 mL. After acidification, silver nitrate was added to a 25.00 mL aliquot where the resulting precipitate was filtered, washed and then redissolved in an ammoniacal solution of potassium tetracyanonickelate(II) according to the reaction: Ni(CN), + 2 AgBr) → 2 Ag(CN), + Ni? + 2 Br The liberated nickel ion required 26.73 mL of 0.02089 M EDTA. The bromate ion in a 10.00 mL aliquot was reduced to bromide with As* prior to the addition of silver nitrate. The same procedure was followed and the released nickel ion was titrated with 21.94 mL of the EDTA solution. Calculate the percentage of impurity in the sample. Br (79.904) a. 24.45% b.34.38% c. 41.17% d. 65.62%
What is the full equation (not the net ionic equation) for the chemical reaction of 0.001 M Fe(NO3)3 plus 0.0002 M NaSCN diluted up to 10 mL with 0.1M HNO3? Please include the acid that is the diluent.
0.7120 g of iron ore was dissolved and the iron was reduced to Fe2+ with Jones's reagent. Fe(II) was titrated with 0.02086 M KMnO4 and consumed 39.21 mL. What is the iron content of iron ore? Report the concentration as percentage of iron (Fe%) and iron oxide (Fe2O3%).
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?
A 1.00 g sample of limonite iron ore, 2Fe203 · 3H20, is dissolved, reduced to Fe2+ and titrated with 20.00 mL of 0.20 M cerium (IV). Calculate the percentage of 2FE203 · 3H20, (FM: 373.38 g/mol) in the sample. Titration reaction: Fe2+ + Ce*+ → Fe3+ + Ce3+
5.3 A 0.1200 g sample of pure iron wire was dissolved in acid, reduced to +2 state and titrated with 23.00 mL of cerium (IV). Calculate the molar concentration of the Ce4+ solution.
Na2S2O3 was standardized using primary standard KIO3. A 0.1000 g sample of KIO3 (FW=214.00 g/mol) was dissolved in dilute HCl. 25.00 mL of water was added with an unmeasured excess of KI. The liberated iodine required 18.50 mL of Na2S2O3. What is the molar concentration of the titrant?
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