A metal oxide has empirical formula `M_(0.96)O_(1.00)` What will be the percentage of `M^(2+)` ion in the crystal ?

Answer

91.67, 8.33

Explanation

Let `M^(2+)` ions in the crystal be x so that `M^(3+)` ions in the crystal will be 0.96 - x. Total charge on the compound must be zero, so that
`+2 xx x + 3 (0.96 - x) - 2 = 0`
`2x - 2.88 - 3x - 2 = 0`
or `x = 0.88`
`:. % of M^(2+) = (0.88)/(0.96) xx 100 = 91.67`
% of `M^(3+) = 100 - 91.67 = 8.33`.