Stoichiometry of a RedOx Reaction

  • Thread starter salman213
  • Start date
  • #1
302
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1. Oxalic acid, H2C2O4, reacts with dichromate ion, in acidic solution to produce carbon dioxide and chromium(III) ion.
If exactly 50.0 mL of an oxalic acid solution is required to react completely with 25.0 mL of a 0.0100 M dichromate solution, what is the molarity of the oxalic acid solution?




2. Molarity = Moles/Lsolution




3. well the equation i got was
H2C2O4 + CrO7 (2-)---> Cr (3+) + CO2

I used oxidation method to balance it to

9H2C2O4 + CrO7 ---> Cr + 7H2O + 4H + 18CO2


then i found moles of CrO7

molarity x L solution = 0.01 x (25/1000) = 0.00025 mol CrO7

then moles of H2C2O4 = 0.00025 mol CrO7 x 9 moles/1 mole

= 0.00225 moles H2C2O4


using this i divide by L solution to get molarity?

M = 0.00225 / (50/1000)

=0.045 M

But according to my online assignment i put that in and its WRONG :(

Maybe i balanced incorrectly or im doing something else wrong
plz help!!







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Answers and Replies

  • #2
302
1
never mind i found my mistake i was using

CrO7 but obviously it is Cr2O7 :D::D:D thanks !
 

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