A solution contaning `2.7 xx 10^(-3) mol of A^(2+) "ion required" 1.6 xx 10^(-3)mol of MnO_(4)^(2-)` for the oxidation of `A^(2+) "to" AO_(3)^(-)` the medium is:

A solution containing 2.7 xx 10^-3 mol of A^(2+) irons required 1.6 xx 10^(-3) mole of MnO_4^- for the oxidation of A^(2+) to AO_3^- the medium used is :

A solution containing 2.68 xx 10^(-3) mol of A^(n+) ions requires 1.61xx10^(-3) mol of MnO_(4)^(-) for the complete oxidation of A^(n+) " to "AO_3^(-) in acidic medium. What is the value of n ?

A solution containing 2.68 x 10^(-3) mol of a solution containing an A^(n+) ion requires 1.61x 10^(-3) mol of MnO_4 ^(-1) for the complete oxidation of A^(n+) to AO_3^(-) in acidic medium. What is the value of n ?

3.90xx10^(-3) moles of a solution containing an ion A^(n+) require 2.34xx10^(-3) moles of MnO_4^(-) for the oxidation of A^(n+) " to " AO_3^(-) in acidic medium . What is the value of n ?