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 DeterminationProcedure:Determination 1:Dispense, from a buret, 5.00 mL of a 0.755 M H2C2O4 solution into a clean,dry 20 x 150- mm test tube.1.2.Dispense, from a buret, 6.00 mL of deionized water into a 125 mL flask.Dispense, from a buret, 1.00 mL of a 0.100 M KMNO4 solution into the flaskcontaining the deionized water. Swirl flask to mix the solution.3.Quickly transfer the H2C2O4 solution from the test tube into the flask containing the KMNO4solution, start the timer, and swirl continuously.4.Stop the timer when the last trace of red disappears and the solution is yellow.Record on the Data Sheet:1. Volume of each reactant2. Volume of deionized water5.3. Elapsed timeRepeat steps 1-5 until you can reproduce the elapsed time to within 10 s. Recordon data sheet.6.7.Determinations 2 and 3:Follow the same procedure as used in determination 1, using the quantities ofreagents designated for determinations 2 and 3. See Procedure Table below.Record all elapsed times on Data Table.Reagent ProportionsReactantsDetermination 1Determination 2Determination 3H»C2O4 solution, mLKMNO4 solution, mLDeionized H2O, mL5.0010.005.001.001.002.006.001.005.00

In the given question we have to calculate final concentration of KMnO4 after mixing the oxalic acid…

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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?

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section11.1: Reaction Rate

Problem 11.2CE: Instantaneous rates for the reaction of hydroxide ion with Cv+ can be determined from the slope of...

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Chemical Reactions and Equations

When a chemical species is transformed into another chemical species it is said to have undergone a chemical reaction. It consists of breaking existing bonds and forming new bonds by changing the position of electrons. These reactions are best explained using a chemical equation.

Question

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:
Dispense, from a buret, 5.00 mL of a 0.755 M H2C2O4 solution into a clean,
dry 20 x 150- mm test tube.
1.
2.
Dispense, from a buret, 6.00 mL of deionized water into a 125 mL flask.
Dispense, from a buret, 1.00 mL of a 0.100 M KMNO4 solution into the flask
containing the deionized water. Swirl flask to mix the solution.
3.
Quickly transfer the H2C2O4 solution from the test tube into the flask containing the KMNO4
solution, start the timer, and swirl continuously.
4.
Stop the timer when the last trace of red disappears and the solution is yellow.
Record on the Data Sheet:
1. Volume of each reactant
2. Volume of deionized water
5.
3. Elapsed time
Repeat steps 1-5 until you can reproduce the elapsed time to within 10 s. Record
on data sheet.
6.
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
H»C2O4 solution, mL
KMNO4 solution, mL
Deionized H2O, mL
5.00
10.00
5.00
1.00
1.00
2.00
6.00
1.00
5.00

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