[A_(2)O_(X)" is oxidised to "AO_(3)^(-)" by "MnO_(4)^(-)" in "],[" acidic medium.If "1.5times10^(-3)" mole of "A_(2)O_(x)],[" requires "40ml" of "0.03M-KMnO_(4)" solution "],[" in acidic medium.Find the value of "x.]

A_(2)O_(X) is oxidised to AO_(3)^(-) by MnO_(4)^(-) in acidic medium. If 1.5times10^(-3) mole of A_(2)O_(X) requires 40ml of 0.03M-KMnO_(4) solution in acidic medium. The value of x

An oxide X_(2)O_(n) is oxidised to XO_(3)^(-) by MnO_(4)^(-) in acidic medium.If 1.5times10^(-3) moles of X_(2)O_(n) requires 1.8times10^(-3) moles of MnO_(4)^(-) for complete oxidation.Assuming that oxidation state of oxygen is -2 in all compounds.The value of

The ion A^(n+) is oxidised to AO_(3)^(-) by MnO_(4)^(-) changing to Mn^(2+) in acid medium. Given that 2.68 xx10^(-3) mole of A^(n+) required 1.61 xx10^(-3) mole of MnO_(4)^(-) . What is the value of n.

A 3 mole mixture of FeSO_(4) and Fe_(2)(SO_(4))_(3) required 100 mL of 2M KMnO_(4) solution in acidic medium. Find the mole of FeSO_(4) in the mixture.

The number of moles of H_(2)O_(2) required to completely react with 400 ml of 0.5 N KMnO_(4) in acidic medium are

10mL of H_2O_2 solution (volume strength = x ) requires 10mL of N//0.56 MnO_4^(ɵ) solution in acidic medium. Hence x is

10mL of H_2O_2 solution (volume strength = x ) requires 10mL of N//0.56 MnO_4^(ɵ) solution in acidic medium. Hence x is