(adsbygoogle = window.adsbygoogle || []).push({}); Stoichiometry.... Did I work this problem correctly?

1. We dissolve 3.778 grams of a sample that contains some sodium oxalate, Na2C2O4, in water and acidify the solution with excess sulfuric acid. The sample requires 18.74 mL of 0.08395 M KMnO4, potassium permanganate, for complete reaction according to the reaction below. What is the percent Na2C2O4 in the sample? Assume that no other component reacts with the potassium permanganate.

8H2SO4 + 2KMnO4 + 5Na2C2O4 --> 8H2O + 2MnSO4 + 10CO2 + 5Na2SO4 + K2SO4

My solution:

.01874 L * 0.08395 M KMnO4 = 0.001573223 mols KMnO4

0.001573223 * (5 mols Na2C2O4/2 mols KMnO4)

= .0039330575 mols Na2C2O4

.0039330575 * (116.04 g) * (100/3.778 g) =12.08 %

(1 mol Na2C2O4 = 116.04 g)

I didn't round any numbers until the final answer. Does this look correct? If not where do you see an error? Thanks in advance for checking.....

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# Homework Help: Stoichiometry Did I work this problem correctly?

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