Can anyone help me to explain how to solve the answer after working out how many mols reacted.
Ethanedioic acid, H2C2O4, is found in a number of plants and spices, including rhubarb, tea leaves and black pepper. The ‘gritty feeling’ experienced when drinking milk with a rhubarb dessert is caused by the precipitation of calcium ethanedioate.
In the body, ethanedioate ions combine with iron(II) ions to form a precipitate of iron(II) ethanedioate, FeC2O4. Some of the iron(II) ethanedioate remains in solution and is excreted in urine.
(a) The concentration of iron(II) ethanedioate in urine can be determined by back titration.
The iron(II) ethanedioate is oxidised by cerium(IV) ions, Ce4+.
Fe2+(aq) + Ce4+(aq) → Fe3+(aq) + Ce3+(aq)
C2O42− (aq) + 2Ce4+(aq) → 2CO2(g) + 2Ce3+(aq)
After this reaction, the excess cerium(IV) ions are titrated with a standard solution of sodium ethanedioate.
50.0 cm3 of 0.200 mol dm−3 cerium(IV) sulfate solution, Ce(SO4)2(aq), was added to 25.0 cm3 of a sample of urine. The excess cerium(IV) ions were reduced to cerium(III) ions by adding 30.00 cm3 of 0.100 mol dm−3 sodium ethanedioate.
Calculate the concentration, in mol dm−3, of the iron(II) ethanedioate in the sample of urine.
(5)
The correct answer is 0.0533 mol dm−3