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?

Question

jfraser · Answer

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.

anonymous · Answer

What is the chemical equation for this reaction?

anonymous · Answer

i believe it may be H2C2O4+2KOH-->2H2O+K2C2O2

anonymous · Answer

thats what I got too. thanks!