### Standardizing Potassium Permanganate Solutions Using Sodium OxalatePotassium permanganate solutions utilized in oxidation-reduction titrations are regularly standardized against sodium oxalate, \(\text{Na}_2\text{C}_2\text{O}_4\), which serves as a primary standard. The chemical reaction involved in this process is:\[ 5\text{C}_2\text{O}_4^{2-}(\text{aq}) + 2\text{MnO}_4^{-}(\text{aq}) + 16 \text{H}^+(\text{aq}) \rightarrow 2\text{Mn}^{2+}(\text{aq}) + 8\text{H}_2\text{O}(l) + 10\text{CO}_2(\text{g}) \]In this experiment, a 0.2252 g sample of sodium oxalate is dissolved in 100 mL of an acid solution. The permanganate solution is then added slowly from a buret. The endpoint of the titration is indicated when 15.85 mL of the permanganate solution has been added.**Given Data and Information:**- Mass of sodium oxalate: \(0.2252 \text{ g}\)- Volume of permanganate solution at endpoint: \(15.85 \text{ mL}\)- Molar mass of sodium oxalate: \(134.00 \text{ g/mol}\)**Objective:**Calculate the molar concentration of the permanganate solution, represented as \([\text{MnO}_4^-]\).#### Steps for Calculation:1. **Determine the moles of sodium oxalate:**\[ \text{Moles of } \text{Na}_2\text{C}_2\text{O}_4 = \frac{0.2252 \text{ g}}{134.00 \text{ g/mol}} = 0.001681 \text{ mol} \]2. **Use stoichiometry to find moles of \(\text{MnO}_4^-\):**According to the reaction, 5 moles of \(\text{C}_2\text{O}_4^{2-}\) react with 2 moles of \(\text{MnO}_4^-\):\[ \text{

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Question 20 of 20 Potassium permanganate solutions used in oxidation-reduction titrations are often standardized against sodium oxalate, Na2C2O4, used as a primary standard. The reaction involved is 5C₂042 (aq) + 2MnO. (aq) + 16 H (aq) → 2Mn²+ (aq) + 8H₂O(l) + 10CO₂(g) A 0.2252 g sample of sodium oxalate is dissolved in 100 mL of acid solution, and the permanganate solution is added slowly from a buret. The endpoint is reached when 15.85 mL of the permanganate solution has been added. The molar mass of sodium oxalate is 134.00 g/mol. Calculate [MnO4], the molar concentration of the permanganate solution. 4 7 +/-

Question 20 of 20 Potassium permanganate solutions used in oxidation-reduction titrations are often standardized against sodium oxalate, Na2C2O4, used as a primary standard. The reaction involved is 5C₂042 (aq) + 2MnO. (aq) + 16 H (aq) → 2Mn²+ (aq) + 8H₂O(l) + 10CO₂(g) A 0.2252 g sample of sodium oxalate is dissolved in 100 mL of acid solution, and the permanganate solution is added slowly from a buret. The endpoint is reached when 15.85 mL of the permanganate solution has been added. The molar mass of sodium oxalate is 134.00 g/mol. Calculate [MnO4], the molar concentration of the permanganate solution. 4 7 +/-

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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