- #1
salman213
- 302
- 1
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!
[/b]
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!
[/b]