What Is the Molarity of the Oxalic Acid Solution in This RedOx Reaction?

[salman213]

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 I am doing something else wrong
please help!







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[salman213]

never mind i found my mistake i was using

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

 

[Blueshift5]

I would first verify the balanced equation and the stoichiometric coefficients used for each reactant and product. I would also check the units of the given concentrations and volumes to make sure they are consistent and can be used in the calculation for molarity. If the equation and units are correct, I would then check my calculations to see if there are any errors or missing steps. If everything appears to be correct, I would suggest double checking with a colleague or consulting a chemistry textbook or online resources for assistance. It is always important to double check your work and seek help if needed to ensure accurate results.