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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?

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!!

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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