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Considering the 2 reactions occurring in your titration: 103 (aq) + 6H+ (aq) + 5 I¯ (aq) → 3 12 (aq) + 3 H₂O (1) S4062-(aq) + 21 (aq) 2 S₂O32- (aq) + 1₂ (aq) - -> If your titration uses 3.000 x 10-3 moles S₂O3²-, how many moles of 103 were present? 4.500 x 10-3 moles 103- 1.800 x 10-2 moles 103- 5.000 x 10-4 moles 103 1.500 x 10-3 moles 103-

Considering the 2 reactions occurring in your titration: 103 (aq) + 6H+ (aq) + 5 I¯ (aq) → 3 12 (aq) + 3 H₂O (1) S4062-(aq) + 21 (aq) 2 S₂O32- (aq) + 1₂ (aq) - -> If your titration uses 3.000 x 10-3 moles S₂O3²-, how many moles of 103 were present? 4.500 x 10-3 moles 103- 1.800 x 10-2 moles 103- 5.000 x 10-4 moles 103 1.500 x 10-3 moles 103-

Chemistry
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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### Titration Reactions and Calculation In the titration process, consider the following two reactions: 1. \( \text{IO}_3^- \, (\text{aq}) + 6\text{H}^+ \, (\text{aq}) + 5\text{I}^- \, (\text{aq}) \rightarrow 3\text{I}_2 \, (\text{aq}) + 3\text{H}_2\text{O} \, (\text{l}) \) 2. \( 2\text{S}_2\text{O}_3^{2-} \, (\text{aq}) + \text{I}_2 \, (\text{aq}) \rightarrow \text{S}_4\text{O}_6^{2-} \, (\text{aq}) + 2\text{I}^- \, (\text{aq}) \) **Problem:** If your titration uses \( 3.000 \times 10^{-3} \) moles of \( \text{S}_2\text{O}_3^{2-} \), how many moles of \( \text{IO}_3^- \) were present? **Options:** - \( 4.500 \times 10^{-3} \) moles \( \text{IO}_3^- \) - \( 1.800 \times 10^{-2} \) moles \( \text{IO}_3^- \) - \( 5.000 \times 10^{-4} \) moles \( \text{IO}_3^- \) - \( 1.500 \times 10^{-3} \) moles \( \text{IO}_3^- \) To calculate the moles of \( \text{IO}_3^- \), use the stoichiometry of the reactions provided.
Transcribed Image Text:### Titration Reactions and Calculation In the titration process, consider the following two reactions: 1. \( \text{IO}_3^- \, (\text{aq}) + 6\text{H}^+ \, (\text{aq}) + 5\text{I}^- \, (\text{aq}) \rightarrow 3\text{I}_2 \, (\text{aq}) + 3\text{H}_2\text{O} \, (\text{l}) \) 2. \( 2\text{S}_2\text{O}_3^{2-} \, (\text{aq}) + \text{I}_2 \, (\text{aq}) \rightarrow \text{S}_4\text{O}_6^{2-} \, (\text{aq}) + 2\text{I}^- \, (\text{aq}) \) **Problem:** If your titration uses \( 3.000 \times 10^{-3} \) moles of \( \text{S}_2\text{O}_3^{2-} \), how many moles of \( \text{IO}_3^- \) were present? **Options:** - \( 4.500 \times 10^{-3} \) moles \( \text{IO}_3^- \) - \( 1.800 \times 10^{-2} \) moles \( \text{IO}_3^- \) - \( 5.000 \times 10^{-4} \) moles \( \text{IO}_3^- \) - \( 1.500 \times 10^{-3} \) moles \( \text{IO}_3^- \) To calculate the moles of \( \text{IO}_3^- \), use the stoichiometry of the reactions provided.
Expert Solution
Step 1: Balanced chemical equation

Balanced chemical equation contain equal number of atoms of each elements on both sides of the reaction.

Balanced chemical equation can be used to determine the amount of reactant needed or product formed.


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