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Question

A2On is oxidized to AO−3 by KMnO4 in acidic medium. If 1.34 mmol of A2On requires 32.2 mL of 0.05 M acidified KMnO4 solution for complete oxidation, which of the following statement(s) is/are correct?


A

The value of n = 2

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B

Empirical formula of the oxide is AO

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C
1.0 mole of A2On would require 1.0 mole of acidified K2Cr2O7 solution
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D

'A' can be a metal from second group of the periodic table

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Solution

The correct options are
A

The value of n = 2


B

Empirical formula of the oxide is AO


C 1.0 mole of A2On would require 1.0 mole of acidified K2Cr2O7 solution

The oxidation reaction is: A2On2AO3
nfactor=102n
(102n)×1.34=32.2×0.05×5
n=2
n-factor = 10 - 4 =6
Thus, the molecular formula of the compound is A2O2 and the empirical formula is AO.
Since the n-factor is 6, 1.0 mole of A2On can be oxidized by using 1.0 mole of K2Cr2O7, which has the same n-factor.
'A' can't be a metal from the second group as it changes its oxidation state from +2 to +5.


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