A sample containing H 2 C 2 O 4 was dissolved and all of

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SUMMARY

The discussion focuses on calculating the mass of H2C2O4 in a sample that underwent a redox titration with 26.37 mL of 0.1420 M MnO4. The balanced redox reaction is 5 H2C2O4 (aq) + 2 MnO4- (aq) + 6 H+ (aq) -> 10 CO2 + 2 Mn2 + 8 H2O. To find the moles of MnO4 used, the formula moles = concentration (M) × volume (L) is applied, leading to the determination of the moles of H2C2O4 based on the stoichiometry of the reaction.

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  • Understanding of redox reactions and stoichiometry
  • Knowledge of molarity and volume calculations
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  • Calculate moles of MnO4 using the formula: moles = concentration × volume
  • Determine the moles of H2C2O4 based on the stoichiometric coefficients from the balanced equation
  • Convert moles of H2C2O4 to grams using its molar mass
  • Explore additional resources on redox titration calculations
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A sample containing H2C2O4 was dissolved and all of

A sample containing H2C2O4 was dissolved and all of it used in a redox titration. What mass of H2C2O4 was in the sample if it required 26.37 mL of 0.1420 M MnO4to react completely with H2C2O4? They interact according to the redox reaction below.

5 H2C2O4 (aq) + 2 (MnO4)- (aq) + 6 H+ (aq) -> 10 CO2 + 2 Mn2 + 8 H2O
 
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It looks like you got everything you need.

How many moles is 26.37 mL of 0.142 M MnO4?
 

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