Iodine titrations: Compounds containing iodine are widely used in titrations, commonly known as iodine titration. It is of two kinds: (i) lodometric titrations (ii) lodimetric titrations. (i) lodometric titrations : It is nothing but an indirect method of estimating the iodine. In this type of titration, an oxidising agent is made to react with excess of KI, in acidic medium or, basic medium in which I_2oxidises into L. Now the liberated I_2can be titrated with Na_(2)S_(2)O_3 .solution. KI overset("Oxidising Agent")rarrI_(2)overset(Na_(2).S_(2)O_(3)//H^(+))rarrI^(-)+Na_(2)S_(4)O_6Although solid I_2is black and insoluble in water, but it converts into soluble I_3ions underset("Black")(I_2(s))+IhArrunderset("Dark brown")(I_3^(-))Starch is used as indicator near the end point or equivalence point. Even small amount of I_2molecules, gives blue colour with starch. The completion of the reaction can be detected when blue colour disappears at the and point. In iodimetric titration, the strength of reducing agent is determined by reacting it with I_2A solution containing Cu^(+2) and C_(2)O_(4)^(-2) ions M which on titration with M/10 KMnO_4requires 50 mL. The resulting solution is neutralized with K_(2)CO_(3)then treated with excess of KI. M The liberated I_2required 25 mL M/10 Na_(2)S_(2)O_3in acidic solution, then what is the difference of the number of m mole of Cu^(+2) and C_(2)O_(4)^(-2)ions in the solution ?