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

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To determine the mass of H2C2O4 in the sample, first calculate the moles of MnO4- used in the titration, which is 0.1420 M multiplied by 0.02637 L, resulting in 0.00374 moles. According to the balanced redox reaction, 2 moles of MnO4- react with 5 moles of H2C2O4, leading to a stoichiometric ratio of 5/2. This means 0.00374 moles of MnO4- corresponds to 0.00935 moles of H2C2O4. Finally, using the molar mass of H2C2O4 (90.03 g/mol), the mass of H2C2O4 in the sample is approximately 840.5 grams.
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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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