1. The problem statement, all variables and given/known data A student weighs by difference 0.1956 g of sodium oxalate into a 100 ml Volumetric flask and dilutes to the mark 10 ml of HCl and 90 ml of distilled water. Approximately how many ml's of 0.02 M KMnO4 would be required to reach the equivalence point of the titration? 2. Relevant equations 3. The attempt at a solution Please correct me if my reasoning is faulty. So, isn't the "end point" the point during the reaction in which the moles of sodium oxalate and potassium permanganate equal? And if this is so...then: 0.1956 g Na2C2O4 x 1 mol Na2C2O4 / 133.998 g/mol Na2C2O4 = 0.00146 mol Na2C2O4/0.1 L = 0.0146 M and then there is 0.02 mol KMnO4/L But I can't make the connection on how to find the information I'm asked....help? Thanks in advance!