please need help woth this volume of olarity of Submit Hints My Answers Gave Up

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please need help woth this

volume of olarity of Submit Hints My Answers Gave Up Review Part Part B Redox titrations are used to determine the amounts of oxidizing and reducing agents in soution For example, a solution of hydrogen peroxide. H2 can be titrated against a solution of potassium permanganate, KMno1. The following equation represents the reantion: A certain amount cl hydrogen peroxide was dssolved in 100 mL of water and then titratod with 1,68 M What mass of Hao was dissolved if the titration requred 17.8 mL of the solution? Express your answer with the appropriate units. mass of H20, Value Submit Hints My Answers Gve up RevinwPart mistry

Explanation / Answer

Ans:
2KMnO4 (aq) + H2O2 (aq) +3H2SO4 (aq) -----> 3O2 (g) + 2MnSO4 (aq) + K2SO4 (aq) + 4H2O (l)

Number of moles = Molarity * Liters of solution

So, 1.68 * 0.0173 = 0.029064 mole of KMnO4

2 moles of KMnO4 reacts with 1 mole of H2O2 (from the balanced chemical equation),

So, 0.029064 mole of KMnO4 reacts with 1/2 x 0.029064 mole of H2O2

Mass of H2O2 = (1/2 x 0.029064 mole of H2O2 ) x (mass of 1 mole of H2O2 )

= 0.014532 moles x 34.02 g = 0.4940 g H2O2

So, mass of H2O2 required is 0.4940 g

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