`2.68xx10^(-3)` moles of solution containing anion `A^(n+)` require `1.61xx10^(-3)` moles of `MnO_(4)^(-)` for 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 ?

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 ?

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 ?

4 " mol of "a solution containing A^(n+) requried 1.6 mon of MnO_(4)^(ɵ) for the oxidation to A^(n+) to AO_(3)^(ɵ) in acidic medium. The value of n is