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loadsy
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Hey there, recently we just did a lab in Chemistry 101 on "Redox Titrations." I'm now working on the lab writeup but was hoping that someone may be able to help me with this question I am currently stuck on. It asks the following:
A sample of Au2(C2O4)3 is contaminated with Li2(C2O4). An acidified 0.2000g sample of this mixture requires 18.12mL of 0.02593mol/L KMnO4 to reach the equivalence point. In acidic solution, the oxalate ion is protonated and titrated with MnO4^- as in the laboratory experiment. Determine the mass percent of Li2(C2O4) in the sample.
Note: The metal ions are not oxidized by the permanganate ion. However, all of the oxalate bonded to the metals reacts completely with the permanganate ion.
Now I know you can start off the problem by finding the number of mols and then from that finding the molar mass of Li2(C2O4). But from there what do I do? Thanks a lot to anyone who can help me. :D
A sample of Au2(C2O4)3 is contaminated with Li2(C2O4). An acidified 0.2000g sample of this mixture requires 18.12mL of 0.02593mol/L KMnO4 to reach the equivalence point. In acidic solution, the oxalate ion is protonated and titrated with MnO4^- as in the laboratory experiment. Determine the mass percent of Li2(C2O4) in the sample.
Note: The metal ions are not oxidized by the permanganate ion. However, all of the oxalate bonded to the metals reacts completely with the permanganate ion.
Now I know you can start off the problem by finding the number of mols and then from that finding the molar mass of Li2(C2O4). But from there what do I do? Thanks a lot to anyone who can help me. :D