A 1.125 g sample of inpure oxalic acid (H2C2O4 ) is dissolved in water and an acid-base indicator added. The sample requires 33.23 mL of 0.485 M KOH to reach the equivalence point. What is the mass percent of pure oxalic acid in the sample?

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A 1.125 g sample of inpure oxalic acid (H2C2O4 ) is dissolved in water and an acid-base indicator added. The sample requires 33.23 mL of 0.485 M KOH to reach the equivalence point. What is the mass percent of pure oxalic acid in the sample?

Chemistry
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1) find the moles of base used to neutralize the acid 2) find the mole ratio of acid and base from a balanced reaction 3) find the moles of acid that were neutralized 4) find the moles of acid that SHOULD HAVE BEEN in the original sample, if it had been 100% pure. 5) divide #3/#4. Profit.
What is the chemical equation for this reaction?
i believe it may be H2C2O4+2KOH-->2H2O+K2C2O2

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thats what I got too. thanks!

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