Calcium oxalate is a common component in kidney stones. It is also used as a primary standard in redox titrations. If 0.25 g of a kidney stone is dissolved in acid and titrated with 0.100 M KMnO4, it requires 5.70 mL of KMnO4
solution to oxidise the oxalate to CO2. Balance the equation below and
calculate the percentage of calcium oxalate in the kidney stone.
(C2O4)2- + (MnO4)- = Mn2+ + CO2

Question

Calcium oxalate is a common component in kidney stones. It is also used as a primary standard in redox titrations.  If 0.25 g of a kidney stone is dissolved in  acid  and  titrated  with  0.100  M  KMnO4,  it  requires  5.70  mL  of  KMnO4
solution  to  oxidise  the  oxalate  to  CO2.   Balance  the  equation  below  and 
calculate the percentage of calcium oxalate in the kidney stone. 
(C2O4)2- + (MnO4)- =>  Mn2+ + CO2

aaronq · Answer

have you balanced the equation?

anonymous · Answer

let me balance it

anonymous · Answer

i got this

2(MnO4)-  + 16H+  + 5C2O4 => 2(Mn)2+ + 8H2O + 10CO2

anonymous · Answer

911

aaronq · Answer

so find the moles of KMnO4 used, and equate those to the amount of CaC2O4

aaronq · Answer

this question is identical to the ones you've been recently posting

anonymous · Answer

then after finding the amount of CaC2O4, I must divide it by 025g? to find its percentage composition?