Approximately 0.10 g of KMnO4 was accurately weighed in a beaker. 200 cm3 of water was measured in a in a measuring cylinder. The water was transferred to the beaker with the KMnO4, and the mixture was stirred for a few seconds.
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0.10 g of KMnO4 was accurately weighed in a beaker. 200 cmÂł of water was measured in a measuring cylinder. The water was transported to a beaker with the KMnO4, and the mixture was stirred for a few seconds. 1. What is the solution color? 2. What is the resulting concentration (g/cmÂł)?
Ted G.
KMnO4 (Potassium permanganate) = 4.19% (m/m) H2O2 (Hydrogen peroxide) = 3% Mass % = mass of solute / mass of solution x 100% trial 1 Pipette with H2O2 before titration (g) 3.1036 Pipette with KMnO4 before titration (g) 3.1187 Pipette with H2O2 after titration (g) 2.5925 Pipette with KMnO4 after titration (g) 2.3835 Fill in the table below Trial 1 1. Reacted H2O2 Solution (g) 2. Titrated KMnO4 Solution (g) 3. Titrated KMnO4 (g) 4. Molar Mass KMnO4 (g/mol) 5. Moles KMnO4 Titrated
Shaiju T.
Potassium manganate(VII), KMnO4, oxidises potassium iodide, KI, to liberate iodine, I2. The iodine liberated can be titrated with aqueous sodium thiosulfate, Na2S2O3. From the results obtained, the concentration of potassium manganate(VII) solution can be calculated. The equations for the reactions are shown below. 16 H+ + 2 MnO4- + 10 I- -> 2 Mn2+ + 8 H2O + 5 I2 2 S2O3 2- + I2 -> S4O6 2- + 2 I- In the experiment, the iodine liberated from 25.0 cm3 of potassium manganate(VII) requires 26.20 cm3 of 0.500 mol dm-3 sodium thiosulfate for complete reaction. Using the equations and the titration results, calculate the concentration of the potassium manganate(VII) solution.
Madhur L.
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