A solution of sodium thiosulfate, Na2S₂O3, is 0.2657 M. 12.82 mL of this solution reacts with 38.74 mL of I₂ solution. What is the molarity of the I₂ solution? 2(Na₂S₂O3) + I2→→Na₂S406 + 2(Nal) Very similar to the other problems that you have been doing. Submit Answer Incorrect. 18.42 mL of the I₂ solution from above is required to titrate a sample containing As2O3. Calculate the mass of As2O3 (197.8 g/mol) in the sample. As2O3 + 5(H₂O) + 212 → 2(H3ASO4) + 4HI

A solution of sodium thiosulfate, Na2S₂O3, is 0.2657 M. 12.82 mL of this solution reacts with 38.74 mL of I₂ solution. What is the molarity of the I₂ solution? 2(Na₂S₂O3) + I2→→Na₂S406 + 2(Nal) Very similar to the other problems that you have been doing. Submit Answer Incorrect. 18.42 mL of the I₂ solution from above is required to titrate a sample containing As2O3. Calculate the mass of As2O3 (197.8 g/mol) in the sample. As2O3 + 5(H₂O) + 212 → 2(H3ASO4) + 4HI

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter4: Reactions In Aqueous Solution

Section: Chapter Questions

Problem 53QAP: The molarity of iodine in solution can be determined by titration with arsenious acid, H3AsO4. The...

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Vitamin C has the formula C6H8O6. Besides being an acid, it is a reducing agent. One method for determining the amount of vitamin C in a sample is to titrate it with a solution of bromine, Br2, an oxidizing agent. C6H8O6(aq) + Br2(aq) 2 HBr(aq) + C6H6O6(aq) A 1.00-g "chewable" vitamin C tablet requires 27.85 ml of 0.102 M Br2 for titration to the equivalence point. What is the mass of vitamin C in the tablet?
What volume of 0.250 M NaOH is required to react completely with 0.0100 moles of H2SO4? (a) 80.0 mL (b) 60.0 mL (c) 40.0 mL (d) 125 mL
What is the molar concentration of an H2SO4 solution if a 50.0-mL sample requires 9.65 mL of a 1.33 M solution of NaOH to reach the equivalence point?
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The molarity of iodine in solution can be determined by titration with arsenious acid, H3AsO4. The unbalanced equation for the reaction is H3AsO3(aq)+I2(aq)+H2O2 I(aq)+H3AsO4(aq)+2 H+(aq)A 243-mL solution of aqueous iodine is prepared by dissolving iodine crystals in water. A fifty-mL portion of the solution requires 15.42 mL of 0.134 M H3AsO3 for complete reaction. What is the molarity of the solution? How many grams of iodine were added to the solution?
A solution of sodium thiosulfate, Na2S2O3, is 0.2202 M. 21.62 mL of this solution reacts with 21.01 mL of I2 solution. What is the molarity of the I2 solution? 2(Na2S2O3) + I2↔Na2S4O6 + 2(NaI) 16.11 mL of the I2 solution from above is required to titrate a sample containing As2O3. Calculate the mass of As2O3 (197.8 g/mol) in the sample. As2O3 + 5(H2O) + 2I2 → 2(H3AsO4) + 4HI
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Determine the volume of 0.205 MM KOHKOH solution required to neutralize each sample of sulfuric acid. The neutralization reaction is:H2SO4(aq) + 2KOH(aq) → K2SO4(aq)+2H2O(l) A) 180 mL of 0.110 M H2SO4 Express your answer using three significant figures. B) 65 mL of 0.100 M H2SO4
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