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If 3 mL of 0.130 M KMnO4 was mixed with 6 mL of H2C2O4 and 6 mL of H2O, what would be the final concentration of KMnO4?

If 3 mL of 0.130 M KMnO4 was mixed with 6 mL of H2C2O4 and 6 mL of H2O, what would be the final concentration of KMnO4?

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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If 3 mL of 0.130 M KMnO4 was mixed with 6 mL of H2C2O4 and 6 mL of H2O, what would be the final concentration of KMnO4?

**Rate Law Determination** **Procedure:** **Determination 1:** 1. Dispense, from a buret, 5.00 mL of a 0.755 M \( \text{H}_2\text{C}_2\text{O}_4 \) solution into a clean, dry 20 x 150-mm test tube. 2. Dispense, from a buret, 6.00 mL of deionized water into a 125 mL flask. 3. Dispense, from a buret, 1.00 mL of a 0.100 M \( \text{KMnO}_4 \) solution into the flask containing the deionized water. Swirl the flask to mix the solution. 4. Quickly transfer the \( \text{H}_2\text{C}_2\text{O}_4 \) solution from the test tube into the flask containing the \( \text{KMnO}_4 \) solution, start the timer, and swirl continuously. 5. Stop the timer when the last trace of red disappears and the solution is yellow. Record on the Data Sheet: - Volume of each reactant - Volume of deionized water - Elapsed time 6. Repeat steps 1-5 until you can reproduce the elapsed time to within 10 s. Record on data sheet. 7. **Determinations 2 and 3:** Follow the same procedure as used in determination 1, using the quantities of reagents designated for determinations 2 and 3. See Procedure Table below. Record all elapsed times on Data Table. --- **Reagent Proportions:** | Reactants | Determination 1 | Determination 2 | Determination 3 | |------------------------|-----------------|-----------------|-----------------| | \( \text{H}_2\text{C}_2\text{O}_4 \) solution, mL | 5.00 | 10.00 | 5.00 | | \( \text{KMnO}_4 \) solution, mL | 1.00 | 1.00 | 2.00 | | Deionized \( \text{H}_2\text{O} \), mL | 6.00 | 1.00 | 5.
Transcribed Image Text:**Rate Law Determination** **Procedure:** **Determination 1:** 1. Dispense, from a buret, 5.00 mL of a 0.755 M \( \text{H}_2\text{C}_2\text{O}_4 \) solution into a clean, dry 20 x 150-mm test tube. 2. Dispense, from a buret, 6.00 mL of deionized water into a 125 mL flask. 3. Dispense, from a buret, 1.00 mL of a 0.100 M \( \text{KMnO}_4 \) solution into the flask containing the deionized water. Swirl the flask to mix the solution. 4. Quickly transfer the \( \text{H}_2\text{C}_2\text{O}_4 \) solution from the test tube into the flask containing the \( \text{KMnO}_4 \) solution, start the timer, and swirl continuously. 5. Stop the timer when the last trace of red disappears and the solution is yellow. Record on the Data Sheet: - Volume of each reactant - Volume of deionized water - Elapsed time 6. Repeat steps 1-5 until you can reproduce the elapsed time to within 10 s. Record on data sheet. 7. **Determinations 2 and 3:** Follow the same procedure as used in determination 1, using the quantities of reagents designated for determinations 2 and 3. See Procedure Table below. Record all elapsed times on Data Table. --- **Reagent Proportions:** | Reactants | Determination 1 | Determination 2 | Determination 3 | |------------------------|-----------------|-----------------|-----------------| | \( \text{H}_2\text{C}_2\text{O}_4 \) solution, mL | 5.00 | 10.00 | 5.00 | | \( \text{KMnO}_4 \) solution, mL | 1.00 | 1.00 | 2.00 | | Deionized \( \text{H}_2\text{O} \), mL | 6.00 | 1.00 | 5.
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