On the direct iodometric titration experiment, Standardization of Na2S2O3 with KIO3 standard solution, why is it better to replace with iodine solution and HCl(as a catalyst) to make safer solvent and auxiliaries( reduced toxic waste)? explain why should we use iodine solution and HCl(as a catalyst) instead of Na2S2O3 with KIO3 ?

On the direct iodometric titration experiment, Standardization of Na2S2O3 with KIO3 standard solution, why is it better to replace with iodine solution and HCl(as a catalyst) to make safer solvent and auxiliaries( reduced toxic waste)? explain why should we use iodine solution and HCl(as a catalyst) instead of Na2S2O3 with KIO3 ?

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter20: Applications Of Oxidation/reduction Titrations

Section: Chapter Questions

Problem 20.4QAP

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Similar questions

5. A 300.0 mg sample containing Na,CO3, NaHCO3 and NaOH and inert material either alone or in some combination was dissolved and titrated with 0.1000 M HCI the titration required 24.41 mL to reach the phenolphthalein endpoint. And an additional 8.67 mL to reach the methyl red endpoint. Determine the composition of the sample and calculate the percent of each titrated component.
5. A 300.0 mg sample containing Na,CO3, NaHCO, and NaOH and inert material either alone or in some combination was dissolved and titrated with 0.1000 M HCI the titration required 24.41 ml to reach the phenolphthalein endpoint. And an additional 8.67 mL to reach the methyl red endpoint. Determine the composition of the sample and calculate the percent of each titrated component.
6. The mass percent of KHP in an unknown salt sample was determined using both volumetric and gravimetric titration. Ten determinations using each method were performed: (You should be using Excel to solve for the required values) Volumetric (% KHP): 34.22 33.86 34.07 34.49 34.69 33.71 34.28 34.11 34.26 34.10Gravimetric (% KHP): 34.35 34.26 34.10 34.19 34.18 34.32 34.11 34.33 34.17 34.12 a) Do the two methods give similar standard deviations? b) Do the two methods give similar results for the mass percent of KHP at the 95% confidence level?
On the redox titration experiment, Standardization of Na2S2O3 with KIO3 standard solution, what can be replaced KIO3 to make safer solvent and auxiliaries( reduced toxic waste)? explain why?
A 50.00 ml aliquot of a solution containing Ca2+ and Mg2+ was buffered at pH 10 and titrated with 0.0474 M EDTA. The endpoint volume was 40.99 ml. A second aliquot of the same mixture was made strongly basic by the addition of NaOH – this causes the Mg2+ to precipitate as Mg(OH)2. The solution was then titrated with the 0.0474 M EDTA and the endpoint volume was found to be 30.04 ml.
A 50.00 mL aliquot of standard CaCO3 (0.3834g CaCO3 per liter) consumed 42.35 mL of EDTA solution. The same EDTA standard solution was used for the titration of a 3.00 mL water sample. This required 30.56 mL of the titrant. Calculate the molar concentration of EDTA standard solution. What is the total hardness of water sample (then after solving explain how it come up to the final answer.)
Standard oxylate solution used to standardize KMnO4 was prepared by dissolving 3.299g of Na2C2O4 in 1.000L of water containing H2SO4. add 25mL aliquot of the Na2C2O4 solution required 28.39 mL of KMnO4 for titration. A blank titration of 25mL of water containing H2SO4 required 0.03 mL of KMnO4. what is the molarity of the KMnO4 solution? 5C2O42-+2MnO4-+16H+ → 10CO2+2Mn2++8H2O
Coulometry consumes larger amount of analyte than voltammetry The answer is either true or false Electrodes of the second kind can respond to the activities of anions that form sparingly soluble precipitates The equivalence point is at the first quarter of 3 the steep part of the titration curve when the reaction stoichiometry is 1:1. In order to be useful in endpoint detection, a redox indicator's range of color change should be at least double the potential expected at the end of the titration Membrane indicator electrodes are 5 sometimes called p-ion electrodes because they measure the pH only The IR drop refers to the deviation of the electrode potential from the value predicted by the Nernst equation on the passage of 6 current
how to prepare this buffer TES (Sigma-Aldrich) infiltration buffer(10 mM TES, 10 mM MgCl2, pH 7.5) ? What should be the ratio of TES and MgCl2?
One of the following statements is incorrect: Titration error is the difference between equivalence point volume and end point volume Back-titration is required when the rate of the reaction slow Standardization is not required when the titrant solution molarity is approximate A standard solution should react completely with the analyte with a definite chemical equation A primary standard O should be highly pure, has atmospheric stability and absence of hydrated water
What is selective precipitation? What is confirmatory test and its significance? What are the products formed when Group 1 cations are allowed to react with KOH? Why is it necessary to have an acidic environment when separating Group 1 cations from other metal ions?
The Ksp of the salt MC204 was determined by titration with potassium permanganate. The balanced net ionic reaction for this titration reaction is shown below. 2MnO4 +5C₂04² + 16H* --> 2Mn²+ +10CO2 + 8H₂O If a 50.00 mL saturated solution of MC₂04 requires 1.49 mL of a 0.000520 M solution of potassium permanganate, what is the Ksp for MC₂04? Enter your answer using scientific notation like this: 10,000 = 1*10^4.