100 ml 0.1 M $K_{2} S O_{3}$ and 100 ml 0.1 M $K M n O_{4} / H^{+}$ are mixed and allowed for a complete redox change. Hence ______

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Newly formed $S O_{4}^{- 2}$ has 0.05 M concentration

0.02 M $M n^{+ 2}$ ions are present in the final solutions

Some $K M n O_{4}$ is left unreacted

$K_{2} S O_{3}$ is partially left unreacted

answer is A, B, D.

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Detailed Solution

$100 \times 0.2 = 20 m e q S O_{3}^{- 2};$

$100 \times 0.5 = 50 m e q M n O_{4}^{-}$

$∴ S O_{3}^{- 2}$ in limiting reagent

$M n O_{4}^{-} l e f t = 30 m e q$

$∴ [M n^{+ 2}] = \frac{20 / 5}{200} = 0.02 M$

$[S O_{4}^{- 2}] = \frac{20 / 2}{200} = 0.05 M$

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