Synopsis of the work
We started using a 100ml volumetric flask to start the preliminary dilution after bringing all the necessary equipment. With a volumetric pipette, we add 10 ml of H2O2, dilute and stir the mixture until it is homogeneous. The diluted solution was then titrated by filling a 250 mL flask with 25 mL of distilled water, 2 mL of 1 M H2SO4 and stirring until complete homogenization. In the same way, we fill the flask with a diluted 10 mL H2O2 solution using a volumetric pipette. We place approximately 50 mL of the KMnO4 solution of concentration 0.1022 N in a 100 mL beaker, mark the outside and then pour it into a 25.00 mL burette.
A 250 mL beaker was used for the burette solution waste, and it was labeled "KMnO4 waste". We started the titration as soon as we realized there were no air bubbles.
When titrating, we continually stirred the solution from the burette into the Erlenmeyer flask until the first persistent pink color appeared. We then recorded the volume and repeated the operation twice more. After the task was over, we cleaned all the materials, finished the report, and disposed of the KMnO4 waste in the waste container that contained heavy metals.
Introduction
Hydrogen peroxide H202 serves as either an oxidant or a reductant in the titration we carried out between KMnO4 and H2O2. Given that potassium permanganate is a more powerful oxidant than hydrogen peroxide in this experiment, potassium permanganate functions as a reductant.
Manganeous ions, on the other hand, serve as a catalyst and speed up the titration process. When a pink tint results from a tiny excess of permanganate, the titration has reached its conclusion.
Findings and computations
KMnO4 concentration is 0.1022/5 = 0.02044 mol/C.
Then, the formula for the number of moles of KMnO4 is as follows: (No of mole of KMnO4 = C x V =0.02044 x 14.90 = 3.0455 x10-4
We are aware,
Two moles of KMnO4 > H202, 5 moles, 3.0445 x 10Amount: -4 moles of KMnO4 5/2 x3.0445 x10^7.614 x 104 moles of H2O2H2O2 at -4 moles
Concentration of Diluted H2O2 = 7.614 x 10-4/10 x 10-3 = 0.07614
Once more, Commercial H2O2 Concentration = 0.07614 x 10 = 0.7614 mol/L
The formula for H2O2's volume is 0.7614 x 11.2 = 8.5.
X̄ = 8.5 +8.5 /2 = 8.5
σ = √ (8.5 - 8.5)2/2 = 0.0
As a result, the peroxide concentration in hydrogen peroxide ("Volumes") is equal to (8.5 0.0).
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