### Determination of Vitamin C Concentration via Redox Titration with Iodine Solution**Vitamin C (Ascorbic Acid, C₆H₈O₆, 176.12 g/mol) Quantification:**Vitamin C can be accurately measured through a redox titration process involving iodine solution. In this reaction, iodine (I₂) is reduced to iodide ions (I⁻), while ascorbic acid is oxidized to dehydroascorbic acid (C₆H₆O₆). Typically, the iodine solution is prepared in the presence of iodide ions, forming the more stable triiodide ion (I₃⁻). The overall reaction can be represented as:C₆H₈O₆(aq) + I₃⁻(aq) + H₂O(l) → C₆H₆O₆(aq) + 3I⁻(aq) + 2H⁺(aq)**Titration Process:**1. **Starch Presence:** - The titration is carried out in the presence of starch. Starch acts as an indicator because it forms a dark blue complex with excess iodine once the endpoint is reached. 2. **Standardization of Iodine Solution:** - To ensure the accuracy of the iodine solution concentration, ascorbic acid can be used as a standard. 3. **Example Calculation:** - **Sample Preparation:** A sample of 0.315 g of ascorbic acid is titrated with the iodine solution. - **Titration Endpoint:** 30.2 mL of the iodine solution are required to reach the endpoint. 4. **Calculation Task:** - **Objective:** Calculate the molar concentration of the I₃⁻ ion in the solution.Please ensure thorough understanding of the titration procedure and precise calculation techniques for accurate results in vitamin C quantification.**Graphs and Diagrams:**There are no graphs or diagrams in the image provided.

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Mail-Francesca A Tantillo-Out X Homepage-CHM150-251 Chen X Question 19 of 20 Vitamin C (ascorbic acid, C&H:06, 176.12 g/mol) can be measured by redox titration with iodine solution. lodine is reduced to iodide ion, while ascorbic acid is oxidized to dehydroascorbic acid (CHO). The iodine solution is usually made in the presence of iodide ion, forming the more stable triiodide ion, Is, giving the following overall reaction CeHsOc(aq) + Is (aq) + H₂O(1)→ CHOs(aq) +31-(aq) + 2H*(aq) The titration is carried out in the presence of starch, which forms a dark blue complex with the excess iodine when the endpoint is reached. Ascorbic acid can be used to standardize the iodine solution. A 0.315 g sample of ascorbic acid was titrated with iodine solution, requiring 30.2 mL to reach the endpoint. Calculate [ls], the molar concentration of Is ion in the solution. LO M Inbox (1,543)-ftantill@udeledu x ← C app.101edu.co Aktiv Chemistry 79°F Sunny + 4 7 +/- 2 5 8

Mail-Francesca A Tantillo-Out X Homepage-CHM150-251 Chen X Question 19 of 20 Vitamin C (ascorbic acid, C&H:06, 176.12 g/mol) can be measured by redox titration with iodine solution. lodine is reduced to iodide ion, while ascorbic acid is oxidized to dehydroascorbic acid (CHO). The iodine solution is usually made in the presence of iodide ion, forming the more stable triiodide ion, Is, giving the following overall reaction CeHsOc(aq) + Is (aq) + H₂O(1)→ CHOs(aq) +31-(aq) + 2H*(aq) The titration is carried out in the presence of starch, which forms a dark blue complex with the excess iodine when the endpoint is reached. Ascorbic acid can be used to standardize the iodine solution. A 0.315 g sample of ascorbic acid was titrated with iodine solution, requiring 30.2 mL to reach the endpoint. Calculate [ls], the molar concentration of Is ion in the solution. LO M Inbox (1,543)-ftantill@udeledu x ← C app.101edu.co Aktiv Chemistry 79°F Sunny + 4 7 +/- 2 5 8

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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