**Vitamin C (ascorbic acid, C₆H₈O₆, 176.12 g/mol) Measurement by Redox Titration**Vitamin C can be measured by redox titration with an iodine solution. In this process, iodine is reduced to the iodide ion, while ascorbic acid is oxidized to dehydroascorbic acid (C₆H₆O₆). The iodine solution is typically made in the presence of iodide ion, forming the more stable triiodide ion, I₃⁻, as shown in the following reaction:\[ \text{C}_6\text{H}_8\text{O}_6(\text{aq}) + \text{I}_3^-(\text{aq}) + \text{H}_2\text{O}(\text{l}) \rightarrow \text{C}_6\text{H}_6\text{O}_6(\text{aq}) + 3\text{I}^-(\text{aq}) + 2\text{H}^+(\text{aq}) \]The titration is conducted in the presence of starch, forming a dark blue complex with excess iodine at the endpoint. This method allows ascorbic acid to standardize the iodine solution. In the experiment, a 0.315 g sample of ascorbic acid was titrated using the iodine solution, requiring 29.2 mL to reach the endpoint.**Objective:**Calculate \([I_3^-]\), the molar concentration of the triiodide ion in the solution.**Input Area:**A mock-up of an input interface is shown, containing numeric buttons to enter the values and calculate the concentration using the provided data.

Given: mass of ascorbic acid = 0.315 g volume of I3- solution = 29.2 mL molar mass of ascorbic acid = 176.12 g/molBalanced chemical reaction between ascorbic acid and iodine solution is given by, C6H8O6(aq)+I3-(aq)+H2O(l)→C6H6O6(aq)+3I-(aq)+2H+(aq) Calculation for moles of ascorbic acid: moles=massmolar massmoles of C6H8O6=0.315 g176.12 g/molmoles of C6H8O6=0.00179 molCalculation for moles of I3- ions: 1 mole of C6H8O6 react with 1 moles of I3- ions. 0.00179 mole of C6H8O6 react with 0.00179 moles of I3- ions. Calculation for concentration of I3- ions: molarity=molesVolume (L)Concentration of I3- ions=0.00179 mol29.2×10-3 LConcentration of I3- ions=0.06125 mol/L≈0.0612 M

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Vitamin C (ascorbic acid, C&H&O6, 176.12 g/mol) can be measured by redox titration with iodine solution. Iodine is reduced to iodide ion, while ascorbic acid is oxidized to dehydroascorbic acid (C6H6O6). The iodine solution is usually made in the presence of iodide ion, forming the more stable triiodide ion, 5, giving the following overall reaction C6HSO6(aq) + Is-(aq) + H2O(I) → CsH&O6(aq) + 3l-(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 29.2 mL to reach the endpoint. Calculate [ls], the molar concentration of Is ion in the solution.

Vitamin C (ascorbic acid, C&H&O6, 176.12 g/mol) can be measured by redox titration with iodine solution. Iodine is reduced to iodide ion, while ascorbic acid is oxidized to dehydroascorbic acid (C6H6O6). The iodine solution is usually made in the presence of iodide ion, forming the more stable triiodide ion, 5, giving the following overall reaction C6HSO6(aq) + Is-(aq) + H2O(I) → CsH&O6(aq) + 3l-(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 29.2 mL to reach the endpoint. Calculate [ls], the molar concentration of Is ion in the solution.

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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

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Question

**Vitamin C (ascorbic acid, C₆H₈O₆, 176.12 g/mol) Measurement by Redox Titration**

Vitamin C can be measured by redox titration with an iodine solution. In this process, iodine is reduced to the iodide ion, while ascorbic acid is oxidized to dehydroascorbic acid (C₆H₆O₆). The iodine solution is typically made in the presence of iodide ion, forming the more stable triiodide ion, I₃⁻, as shown in the following reaction:

\[ \text{C}_6\text{H}_8\text{O}_6(\text{aq}) + \text{I}_3^-(\text{aq}) + \text{H}_2\text{O}(\text{l}) \rightarrow \text{C}_6\text{H}_6\text{O}_6(\text{aq}) + 3\text{I}^-(\text{aq}) + 2\text{H}^+(\text{aq}) \]

The titration is conducted in the presence of starch, forming a dark blue complex with excess iodine at the endpoint. This method allows ascorbic acid to standardize the iodine solution. In the experiment, a 0.315 g sample of ascorbic acid was titrated using the iodine solution, requiring 29.2 mL to reach the endpoint.

**Objective:**
Calculate \([I_3^-]\), the molar concentration of the triiodide ion in the solution.

**Input Area:**
A mock-up of an input interface is shown, containing numeric buttons to enter the values and calculate the concentration using the provided data.

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