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$0.0026 {MI}_{2}$ solution having unknown volume is reacted with excess of ferrous thiocynate solution to form ${Fe}_{2} O_{3}, {SO}_{4}^{2 -}, {CN}^{-}$ along with $I^{-}$ . If all the sulphate ions formed are precipitated using ${BaCl}_{2}$ such that $1.6776 gm$ of ${BaSO}_{4}$ is obtained, calculate volume of $I_{2}$ consumed in litre

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answer is 9.

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Detailed Solution

The reaction is,

$2 Fe ({SCN}_{2} + 13 I_{2} ⟶ {Fe}_{2} O_{3} + 4 {SO}_{4}^{2 -} + 4 {CN}^{-} + 26 I^{-}$

$= \frac{13}{4} \times 7.2 \times 10^{- 3} V$

So,

${BaCl}_{2} + {SO}_{4}^{2 -} ⟶ {BaSO}_{4} V = 9000 ml$

$Volume = 9 litre$ .

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