Potassium permanganate, KMnO4, reacts with oxalic acid, H2C2O4, in aqueous sulfuric acid according to the following equation:
2 KMnO4 (aq) + 5 H2C2O4 (aq) + 2 H2SO4 (aq) â 2 MnSO4 (aq) + 10 CO2 (g) + 8 H2O (l) + K2SO4 (aq)
How many milliliters of a 0.209 M KMnO4 solution are needed to react completely with 3.873 g of oxalic acid?
Potassium permanganate, KMnO4, reacts with oxalic acid, H2C2O4, in aqueous sulfuric acid according to the following equation:
2 KMnO4 (aq) + 5 H2C2O4 (aq) + 2 H2SO4 (aq) â 2 MnSO4 (aq) + 10 CO2 (g) + 8 H2O (l) + K2SO4 (aq)
How many milliliters of a 0.209 M KMnO4 solution are needed to react completely with 3.873 g of oxalic acid?
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Related questions
A volume of 60.0 mL of aqueous potassium hydroxide (KOH) was titrated against a standard solution of sulfuric acid (H2SO4). What was the molarity of the KOH solution if 11.7 mL of 1.50 M H2SO4 was needed? The equation is
2KOH(aq)+H2SO4(aq)âK2SO4(aq)+2H2O(l)
Express your answer with the appropriate units.
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Part B
Redox titrations are used to determine the amounts of oxidizing and reducing agents in solution. For example, a solution of hydrogen peroxide, H2O2, can be titrated against a solution of potassium permanganate, KMnO4. The following equation represents the reaction:
2KMnO4(aq)+H2O2(aq)+3H2SO4(aq)â3O2(g)+2MnSO4(aq)+K2SO4(aq)+4H2O(l)
A certain amount of hydrogen peroxide was dissolved in 100. mL of water and then titrated with 1.68 M KMnO4. What mass of H2O2 was dissolved if the titration required 17.8 mL of the KMnO4 solution?
Express your answer with the appropriate units.